Classification of Fungi based on the Host parasitic Relationship

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Classification of Fungi based on the Host parasitic Relationship

Based on the host parasitic relationship the fungi are grouped into three types.

a. Commensalism:

The fungus neither gets benefit nor harmed by the host parasitic relationship.

b. Mutualism:

The fungus benefited from the host parasitic relationship.

c. Parasitism:

The host is harmed by the fungus in host parasitic relationship.

Mycoses

Diseases caused by the medically important fungi are called Mycoses. Based on their wide spectrum of adaptability, fungi causing human mycoses can be categorized into:

a. Pathogenic fungi:

The ability of the fungi to adapt to skin flora and cause infection.

b. Opportunistic fungi:

When the immune status of the host is reduced, fungi will induce or cause infection.

c. Toxigenic fungi:

Toxins produced by fungi are responsible for the illness or death of patients after ingestion of the contaminated food.

d. Allergenic fungi:

Allergens are secreted by the fungi which cause allergic reaction in the human beings. Mycoses are classified according to the specific site of involvement.

a. Superficial Mycoses:

The infection is limited to the outer most layers of the skin and its appendages.

Example:
Malassezia and Piedra infection

b. Cutaneous Mycoses:

The infection extends deeper into the epidermis and it also invades hair and nails.

Example:
Dermatophytoses.

c. Sub cutaneous Mycoses:

The infection extends to dermis, subcutaneous tissue and muscles by any traumatic injury.

Example:
Mycetoma

d. Systemic Mycoses:

The infection originates from lungs and later spreads systemically to other organs. Systemic mycoses along with the opportunistic fungal infection are known as deep mycoses.

Example:
Cryptococcosis

e. Opportunistic Mycoses:

The infection occurs when the immune status of the individuals is altered. It is common among immune compromised and immune suppressed patients.

Example:
Candidiasis

Aeromycology

The Aeromycology is the study of air borne fungi, its types and the seasonal variations of allergenic fungal spores in the environment. There are certain fungal pathogens which cause infections associated with workers in mycological laboratories.

To avoid this safety procedures and equipments safety levels or bio safety levels (BSL) are used. BSL – 1 is used for low – risk microorganisms and BSL – 4 is used for highly risk pathogens.

Characteristics of Fungi

Fungi are heterotrophic organisms that exist as saprophytes, commensal or parasites. They are found on decaying vegetative matter and also in soil. Morphological features, cell structure, reproduction, nutritional requirement and thermal dimorphism in the pathogenic fungi are described as follows:

i. Morphological Features

Fungi are eukaryotic with well defined cell wall and intra cellular membrane bound organelles. The cell wall is composed of polysaccharides and chitin. Fungi vary in size and shape. They are broadly divided into two main groups.

a. Yeasts:

The yeasts are unicellular organisms which reproduce by asexual process known as budding or by fission. The cell develops a protuberance that enlarges and separates from the parental cell. The yeasts produce chains of elongated cells known as Pseudohyphae.

Some yeasts reproduce by sexual process Example: Cryptococcus neoformans. Germ tube is special morphology found in Candida albicans. Some are commensal without any medical significance.

b. Molds:

The molds grow by apical extension, forming an interwoven mass called as Mycelium, branching filaments known as hyphae. Hyphae that grow on the surface are called vegetative hyphae. They are responsible for the absorption of nutrients. The hyphae that project above the surface are called aerial hyphae and they produce specialized reproductive structures called as conidia.

Depending on cell morphology fungi are divided into four types, they are Yeasts: These are unicellular organisms that divide by budding (Figure 9.1 a & b). Example: Cryptococcus neoformans (Pathogenic), Saccharomyces cerevisiae (Non pathogenic).
Classification of Fungi based on the Medical Mycology img 1
Classification of Fungi based on the Medical Mycology img 1a

Yeast – like fungi:

These fungi reproduce by budding but fails to separate and hence elongation takes place forming pseudohyphae. Example: Candida species (Pathogenic).

Molds:

These fungi produce spores which germinate to form vegetative hyphae (Figure 9.2).
Classification of Fungi based on the Medical Mycology img 2

Example:
Dermatophytes, Aspergillus, Penicillium, Mucor.

Dimorphic fungi:
These Fungi exist in both yeast at 37°C and filamentous form at 25°C. This Phenomenon is known as Fungal dimorphism (Figure 9.3).
Classification of Fungi based on the Medical Mycology img 3

Example:
Histoplasma capsulatum, Blastomyces dermatitidis.

Phaeoid fungi:

Most of true pathogenic fungi are dimorphic fungi which are composed of darkly coloured hyphal form known as dematiaceous fungi. Some are yeast like and also known as black yeasts.

Vegetative Structures:

Several structures are formed by the vegetative mycelia that have no reproductive value but are important for the differentiation of fungi eg. Chlamydospores and Arthrospores. Chlamydospores are thick walled, resistant to adverse conditions and are larger than other cells. Arthrospores are rectangular spores which are thick walled that are disposed on maturity.

ii. Cell structure

a. Capsule:
Fungi produce an extra cellular polysaccharide in the form of capsule. Example: Cryptococcus.

b. Cell wall:
Fungi possess a multilayered rigid cell wall exterior to the plasma lemma. The cell wall is made up of chitin, a water insoluble, homopolymer of N-acetyl glucosamine. Chitin synthase is responsible for the bio synthesis of chitin.

c. Plasmalemma:
Cytoplasmic membrane or plasmalemma encloses complex cytosol. It is composed of glycoprotein, lipids and ergosterol.

d. Cytosol:
Cytosol comprises of mitochondria, microtubules, ribosomes, golgi apparatus, double membrane endoplasmic reticulum and Nucleus. The nuclei of the fungi are enclosed by a membrane and contain most of cellular DNA.

iii. Reproduction of fungi

Spores play a major role in reproduction. There may be asexual or sexual cell divisions.

a. Asexual Reproduction:

The asexual reproduction involves, budding or fission or mitosis. Fungi produce more than one type of asexual spores. They are microspores (microconidia) and macrospores (macroconidia).

Spores that are present inside sporangium are known as sporangiospores and those that are borne exogenously are called conidiospores (Figure 9.4). Based on the arrangement of conidia they are classified as Acropetal, Basipetal and Sympodial.
Classification of Fungi based on the Medical Mycology img 4

b. Sexual Reproduction:

The process of sexual reproduction typically consists of plasmogamy (cytoplasmic fusion), Karyogamy (union of two nuclei) and meiosis (haploid formation). Anamorphs and Telomorphs are the 2 phases of sexual reproduction.

c. Mycelia Sterile:

Mycelia sterile are fast growing molds that do not produce spores or conidia. They are medically significant fungi and are difficult to identify.

iv. Growth and nutrition

Fungi are ubiquitous in nature and grow readily in the presence of nitrogen and carbohydrates. Medically significant fungi are Mesophilic. The optimum temperature invitro for majority of the pathogenic fungi is between 25°C and 37°C.

The fungi prefer acidic pH; do not require light for their growth. All fungi are heterotrophs requiring organic nutrients. They absorb their nutrient and do not ingest food. Medically significant fungi are facultative
parasites, capable of causing disease or living on dead organic matter.

Ascaris Lumbricoides

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Ascaris Lumbricoides

Geographical Distribution

It is the most common of human helminthes and is distributed worldwide.

Habitat

The adult worms lives in the small intestine particularly in jejunum and in ileum.

Morphology

Adult worm Ascaris lumbricoides resembles and sometimes confused with the earthworm. Its specific name lumbricoides means earthworm in Latin. Male and Female worm of Ascaris lumbricoides are shown in Figure 8.15.
Ascaris Lumbricoides img 1

  1. They are large cylindrical worms with tapering ends. The anterior end being thinner than the posterior end. It is the largest intestinal nematode parasitizing man.
  2. The life – span of the adult worm is less than a year.

Male worm

  • The adult male worm is smaller than female worms.
  • The tail – end (Posterior end) of the male worm is curved ventrally to form a hook and 2 curved copulatory spicules.

Female worm

  • The adult female worm is larger (20-40 cm) and thicker (3-6 mm) than male worm.
  • The posterior end is conical and straight. The anus is in the sub terminal part and opens like a transverse slit on the ventral surface.
  • The vulva is situated mid – ventrally, near the junction of the anterior and middle thirds of the body. This part of the worm is narrow and is called the vulvar waist.
  • A single worm lays up to 200,000 eggs per day.

Egg:

Two types of eggs are passed in feces by the worms.

Fertilized Egg

  • The fertilized eggs are produced by fertilized females.
  • The eggs are round or oval in shape and measures 45 µm in length and 35 µm to 50µm in breadth.
  • They are bile – stained and appear as golden brown (brownish) in colour.
  • The egg is surrounded by a thick smooth shell with an outer albuminous coat (corticated eggs). Sometimes this outer coat is lost in few eggs. Those eggs are called as decorticated eggs (Figure 8.16).
  • Each egg contains a large unsegmented ovum with a clear crescentic area at each pole. The eggs float in saturated solution of common salt.
    Ascaris Lumbricoides img 2

Unfertilized egg

  • The female even not fertilized by male is capable of liberating eggs. These unfertilized eggs are narrower, longer and elliptical in shape.
  • These are heaviest of all the helminthic eggs – It measures about 80µm × 105µm in size.
  • The eggs have a thinner shell with an irregular coating of albumin (Figure 8.16).
  • These eggs do not float in saturated solution of common salt.

Life – Cycle

The life – cycle of A. lumbricoides is completed in a single host, human (Figure 8.17).

Infective form:

Ermbryonated eggs. The fertilized egg passed in feces is not immediately infective. It has to undergo a period of development in soil. The development usually takes from 10-40 days. The embryo moults twice during the time and becomes the infective rhabditiform larva.

Mode of transmission:

Man acquires the infection by ingestion of food, water or raw vegetables contaminated with embryonated eggs of the round worm. The ingested eggs reach the duodenum to liberate the larvae by hatching. These larvae then penetrate the intestinal wall and are carried by the portal circulation to the liver. They live in liver for 3 to 4 days. Then they are carried to the right side of the heart, then to lung. In the lung, they grow and moult twice.

After development in the lungs, in about 10-15 days, the larvae pierce the lung capillaries and reach the alveoli. Then they are carried up the respiratory passage to the throat and swallowed back to the small intestine.

In the small intestine, the larvae moult finally and develop into adults. They become sexually mature in about 6-12 weeks. The fertilized female start laying eggs which are passed in the faces to repeat the cycle.Ascaris Lumbricoides img 3

Pathogenesis

Infection of A. lumbricoides in human is known as ascariasis. The adult worm may produce its pathogenic effects in the following ways.

a. The spoliative or nutritional effects is usually seen when the worm burden is heavy. Presence of enormous numbers (sometime exceeds 500) often interferes with proper digestion and absorption of food. Ascariasis may contribute to protein – energy malnutrition and vitamin A deficiency.

b. The toxic effects is due to the metabolites of adult worm. Ascaris allergens produce various allergic manifestations such as fever, urticaria and conjunctivitis.

c. The mechanical effects are the most important manifestations of ascariasis. In heavy infections, adult worms can cause obstruction and inflammation of intestinal tract, particularly of the terminal ileum.

d. Ectopic ascariasis (Wander lust) is due to the adult male worms. They are restless wanderers. The wandering happens when the host temperature rises above 39°C. The worm may wander up or down along the gut. It may enter the biliary or pancreatic duct causing acute biliary obstruction or pancreatitis. It may enter the liver and lead to liver abscesses.

The worm may go up the esophagus and come out through mouth or nose. It may crawl into the trachea and the lung causing respirator obstruction or lung abscesses. Migrating downwards, the worm may cause obstructive appendicitis. The worm may also reach kidneys. “Larva migrans” is a term used when the larval sworms migrate to various parts of the body.

Clinical Manifestations

Incubation Period is 60-70 days. Clinical manifestations due to adult worm vary from asymptomatic to severe and even fatal infection. Clinical manifestation in ascariasis can be caused either by the migrating larvae or by the adult worms.

Symptoms due to the migrating larvae:

Leads to ascaris pneumonia and larvae may enter the general circulation, disturbances have been reported in the brain, spinal cord, heart and kidneys.

Symptoms due to the adult worms:

Diffuse or epigastric abdominal pain, abdominal cramping, abdominal swelling (especially in children), fever, nausea, vomiting and passing roundworms and their eggs in the stool.

Laboratory Diagnosis

Specimen collected: Stool, sputum and blood.

Detection of parasite

Adult worm:
It can be detected in stool or sputum of patient by naked eye. Pancreatic or biliary worms can be detected by ultra-sound and endoscope.

Larvae:
Larvae can be detected in sputum and often in gastric washings. Chest X – ray may show pulmonary infiltrates.

Eggs:
Detection is through demonstration of eggs in feces. Detection of both fertilized and unfertilized eggs are made after staining. Eggs may be demonstrative in the bile obtained by duodenal aspirates.

Blood Examination
Complete blood count may show eosinophilia in early stage of infection.

Serological tests
Ascaris antibody can be detected by IHA, IFA and ELISA

Treatment
Commonly used drugs are Albendazole and Mebendazole.

Prevention and Control

  • Proper health education should be given for improved sanitation and personal hygiene.
  • Avoid eating of uncooked green vegetable, food preparation and fruits that may contain faecal eggs.
  • Treating infected persons especially children. Deworming of school children have been found effective in control of ascariasis.

Haloalkanes and Haloarenes Class 12 Notes Chemistry Chapter 10

By going through these CBSE Class 12 Chemistry Notes Chapter 10 Haloalkanes and Haloarenes, students can recall all the concepts quickly.

Haloalkanes and Haloarenes Notes Class 12 Chemistry Chapter 10

Haloalkanes and Haloarenes Class 12 Notes Chemistry 1
In Haloalkanes X is attached to sp3 hybridized carbon atom, whereas it is attached to sp2 hybridized carbon atom in the aryl group.

Classification:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 2
(a) Alkyl halides or Haloalkanes (R-X) [sp3 C-X Bond]
General Formula: Cn H2n-1X
Haloalkanes and Haloarenes Class 12 Notes Chemistry 3
(b) Allylic halides: Here halogen atom is bonded to an sp3-hybridized carbon atom next to C = C, i.e., to an allylic carbon.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 4
(c) Benzylic halides: Halogen is bonded to sp3 carbon next to the aromatic ring.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 5
Compounds containing sp2 C-X Bond:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 6
Haloalkanes and Haloarenes Class 12 Notes Chemistry 7
Haloalkanes and Haloarenes Class 12 Notes Chemistry 8
IUPAC name:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 9
Common and IUPAC names of some halides:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 10

Structure Common name IUPAC name
CH2Cl2 Methylene chloride Dichloromethane
CHCl3 Chloroform Trichloromethane
CHBr3 Bromoform Tribromomethane
CCI4 Carbon tetrachloride Tetrachl or methane
CH3CH2CH2F n-Propyl fluoride 1-Fluoropropane

Nature of C-X bond: Due to the difference in electronegativity of C and X, the C-X bond is polarised; carbon bears a partial positive charge whereas the halogen atom bears a partial negative charge.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 11
Carbon-halogen bond length increases from C-F to C-I as the size of the halogen atom increases.

Methods of Preparation:
1. From alcohols
Haloalkanes and Haloarenes Class 12 Notes Chemistry 12
The order of reactivity of alcohols with a given haloacid is 3° > 2° > 1°.

2. From hydrocarbons:
1. By Free radical halogenation: It gives a complex mixture of isomeric mono and polyhaloalkanes which is difficult to separate.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 13
2. By electrophilic Substitution: Aryl chlorides and bromides can be easily prepared by electrophilic substitution of arenes with chlorine and bromine respectively in the presence of Lewis acid catalysts like iron or iron (III) chloride.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 14
The ortho and para isomers can be easily separated due to large differences in their melting points.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 15
3. Sandmayer’s reaction:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 16
4. From alkenes: (a) Addition of hydrogen halides
Haloalkanes and Haloarenes Class 12 Notes Chemistry 17
Addition to unsymmetric alkenes is as per Markovnikov’s Rule
Haloalkanes and Haloarenes Class 12 Notes Chemistry 18
(b) Addition of Halogens
Haloalkanes and Haloarenes Class 12 Notes Chemistry 19
5. Halogen Exchange: Finkelstein Reaction
R-X + Nal → R-I + NaX
X = Cl, Br

Swartz Reaction: This method is used to prepare alkyl fluorides by heating an alkyl chloride/bromide in the presence of AgF/Hg2F2.
H3C-Br + AgF → H3C-F + AgBr

Physical Properties:

  1. Alkyl halides are colorless when pure. However, bromides and iodides develop color when exposed to light.
  2. Melting & b.Pts: Lower members are gases at room temperature. Higher members are liquids or solids.

Due to the polar character of the C-X bond and higher molecular mass as compared to the parent hydrocarbon, the intermolecular forces of attraction (dipole-dipole and van der Waals) are stronger in halogen derivatives. That is why boiling points of chlorides, bromides, and iodides are considerably higher than those of the hydrocarbons of comparable molecular mass.

For the same alkyl group, the boiling points increase from RF to RI in the order RF < RCl < RBr < RI.
For isomeric haloalkenes, the b.pts decrease with an increase in branching (lesser the surface area)
Haloalkanes and Haloarenes Class 12 Notes Chemistry 20
B. pts of isomeric di-halogens are very nearly the same. However, para isomers are higher melting as compared to their ortho and meta isomers. It is due to the symmetry of para isomers that fits in the crystal lattice better as compared to ortho and meta isomers.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 21
3. Density: Bromo, iodo, and poly-chloro derivatives of hydrocarbons are heavier than water. The density increases with an increase in the number of carbon atoms, halogen atoms, and atomic mass of halogens.

4. Solubility: The haloalkanes are only very slightly soluble in water. However, they tend to dissolve in organic solvents.

Chemical Reactions:
A. Reactions of haloalkanes:

  1. Nucleophilic substitution reactions (SN)
  2. Elimination reactions
  3. Reactions with metals.

1. Nucleophilic Substitution reactions: A nucleophile (Nu 🙂 reacts with haloalkane (the substrate) which has a polar C-X bond.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 22
Haloalkanes and Haloarenes Class 12 Notes Chemistry 23
Haloalkanes and Haloarenes Class 12 Notes Chemistry 24
Such reactions in which a stronger nucleophile displaces a weaker nucleophile are called Nucleophilic Substitution (SN) reactions and the halide ion which departs with its bonding pair of electrons is called the leaving group. The better the leaving group, the more facile is the nucleophile substitution reaction. It follows the order
I > Br > Cl > F
∴ The order of reactivity of haloalkanes follows the sequence Iodoalkanes > Bromoalkanes > chloroalkanes > fluoroalkanes.

Types of Nucleophilic Substitution reactions:

  1. SN2 [Substitution, nucleophilic, bimolecular]
  2. SN1 [Substitution, nucleophilic, unimolecular]

1. Substitution nucleophilic bimolecular (SN2): The reaction between CH3Cl and hydroxide ion to yield methanol and chloride ion follows second-order kinetics, i.e., the rate depends upon the concentration of both reactants.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 25
rate of reaction ∝ [Base] [R-X]

Since the rate of the reaction depends upon the concentration of both the reactants, it is a bimolecular nucleophilic displacement reaction.

There occurs a complete stereochemical inversion of the configuration. The order of reactivity of the alkyl halides is Primary halide > Secondary halide > Tertiary halide.

In the SN2 reaction, the attack of the nucleophile (OH above) occurs from the backside, and the halide ion leaves from the front side. This inversion of configuration is called Walden Inversion. As far as the ease of departure of halide ion is concerned, the order of reactivity is RI > RBr > RCl > RF.

2. Substitution, nucleophilic, unimolecular (SN1) – SN1 reactions are generally carried out in polar protic solvents (like water, alcohol, acetic acid, etc). The reaction between tert-butyl bromide and hydroxide ion yields tert-butyl alcohols and follows first-order kinetics.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 26
This reaction is independent of the concentration of the base. The rate law suggests the reaction proceeds in two steps.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 27
This step is slow and hence is the rate-detaining step.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 28
This step, being fast, does not affect the rate of reaction. If the alkyl halide is optically active, then the product is a racemic mixture.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 29
Allylic and benzylic halides show high reactivity towards SN1 reaction

The carbocation gets stabilized through resonance as shown below:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 30
For a given alkyl group, the reactivity of the halide, R-X, follows the same order in both mechanisms.
R-I > R-Br > R-Cl > > R-F.

Stereochemical aspects of nucleophilic substitution reactions: An SN2 reaction proceeds with complete stereochemical inversion of configuration while an SN1 reaction proceeds with racemization.

Optical Activity: Certain compounds exhibit the property of rotating the plane polarised light when it passed through their solutions. Such compounds are called Optically Active compounds arid this phenomenon is called Optical Activity.

If the compound rotates the plane-polarised light to the right, i.e., in a clockwise direction, it is called dextro-rotatory or the d-form and is indicated by placing a positive (+) sign before the degree of rotation. If the light is rotated towards the left (anticlockwise), the compound is said to be laevorotatory or the /-form and a negative sign (-) is placed before the degree of rotation. Such (+) and (-) isomers of a compound are called Optical Isomers and this phenomenon is termed Optical Isomerism.

All the physical properties of compounds showing optical activity are the same like refractive index solubility, density, m.pts, b.pts, etc. Even the extent of rotation is the same. They differ from each other only in the direction of rotation.
If all the substituents attached to the C atom are different, such a carbon atom is called asymmetric carbon or stereocentre.

The resulting molecule would lack symmetry and is referred to as asymmetric or ‘dissymmetric molecule. This asymmetry of the molecule is responsible for the optical activity in such organic compounds. Such molecules are non-superimposable on their mirror image (as the left hand is non-superimposable on the right hand) and are said to be Chiral. This property of non-super imposibility of the mirror image on the object is called Chirality. The objects which are superimposable on their mirror image are called Achiral.

Butan-2-ol has 4 different groups attached to the tetrahedral carbon atom and is Chiral. The mirror image of Butan-2-ol non-superimposable onbutan-2-ol
Haloalkanes and Haloarenes Class 12 Notes Chemistry 31
Other chiral molecules are Bromochloroiodimethane (BrCl CHI), 2-chlorobutanol, 2, 3-dihydroxypropanal (OHC- CHOH-CH2OH), lactic acid (CH3CH(OH)COOH). The stereoisomers related to each other as non-superimposable are also called Enatiomers and the concept Enantiomerism.

A mixture containing two enantiomers in equal proportions will have zero optical rotation, as the rotation due to one isomer will be canceled by the rotation due to the other isomer. Such a mixture is called Racemic Mixture or Racemic Modification. It is represented by prefixing dl or (±) before the name, e.g., (±) butan-2-ol. The process of conversion of enantiomer into a racemic mixture is known as Racemisation.

Retention: Retention of configuration is the preservation of the integrity of the spatial arrangement of bonds to an asymmetric center during a chemical reaction or transformation. It is also the configurational correlation when a chemical species XCabc is converted into the chemical species YCabc having the same relative configuration.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 32
Inversion, retention, and racemization: These are three possibilities for a reaction to occur at an asymmetric carbon atom.

Consider the replacement of a group X and Y in the following reaction:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 33
If (A) is the only compound obtained, the process is called retention of configuration.
If (B) is the only compound obtained, the process is called inversion of configuration.
If a 50: 50 mixture of (A) and (B) is obtained, the process is called racemization and the product is optically inactive.

Thus during an SN2 reaction involving an optically active alkyl halide, the reactant undergoes inversion of configuration.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 34
In the case of optically active alkyl halides, SN1 reactions are accompanied by racemization. Consider hydrolysis of optically active 2-romobutane, which results in the formation of(±) butan-2-oI.

Step I:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 35
Haloalkanes and Haloarenes Class 12 Notes Chemistry 36
2. Elimination Reactions: When a haloalkane with a β-hydrogen atom is heated with an alcoholic solution of potassium hydroxide, there is an elimination of hydrogen atom from β-carbon and a halogen atom from the a-carbon atom.

An alkene is formed as a result. Since the β-hydrogen atom is involved in elimination, it is often called β-elimination.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 37
If there is the possibility of the formation of more than one alkene due to the availability of more than one β-hydrogen atom, usually one alkene is formed as the major product. These form part of a pattern first observed by Russian Chemist Alexander Zaitsev (also pronounced as Saytzeff) who in 1875 formulated a rule which can be summarised as in dehydrohalogenation reactions, the preferred product is that alkene which has the greater number of alkyl groups attached to the doubly bonded carbon atoms.” Thus, 2-bromopentane gives pent-3-ene as the major product.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 38
An alkyl halide with β-hydrogen atoms when reacted with a base or a nucleophile has two competing routes: substitution (SN1 and SN2) and elimination. The route to be taken up depends upon the nature of alkyl halide, strength and size of base/nucleophile, and reaction conditions.

Thus, a bulky nucleophile abstracts a proton rather than approaches a tetravalent C atom (steric hindrance). Similarly, a primary alkyl halide will prefer an SN2 reaction, a secondary halide SN2 or elimination depending upon the strength of base/nucleophile, and a tertiary halide: SN1 or elimination depending upon the stability of carbocation or the more substituted alkene.

3. Reaction With Metals: Most organic chlorides bromides and iodides react with certain metals to give compounds containing carbon-metal bonds. Such compounds are known as organometallic compounds.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 39
In the Grignard reagent, the C-Mg bond is covalent but highly polar, the MgX bond is essentially ionic.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 40
The Grignard reagent is highly reactive. Even H2O reacts with it.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 41
Wurtz Reaction: Alkyl halides react with sodium in dry ether to give hydrocarbons containing double the number of carbon atoms present in the reaction. This reaction is known as the Wurtz reaction.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 42
Reactions of Haloarenes:
1. Nucleophilic Substitution: Alkyl halides are extremely dull/ loss reactive towards SN reactions due to the following reasons.
1. Resonance effect: In haloarenes, the electron pairs on halogen atom are in conjugation with π-electrons of the ring as given below:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 43
C-Cl bond a partial double bond character due to one. As a result difficult to break the C-X bond and therefore less reactive towards SN1
2. Different hybridization of Carbon atom in C-X bond: In haloalkanes, the C is sp3 hybridized while in haloarenes, the carbon attached to has is sp2 hybridized.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 44
The sp2 hybridized carbon with \(\frac{1}{3}\) s-character is more electronegative and can hold the electron pair of C-X bond more tightly than sp3-hybridized carbon in haloalkane ‘With s-character. Thus

The C-Cl bond length in haloalkane is 177 pm while in haloarene it is 169 pm. Since it is difficult to break a shorter bond than a longer bond, therefore, haloarenes are less reactive than haloalkanes towards SN reactions.

3. Instability of phenyl cation: In the case of haloarenes, the phenyl cation formed as a result of self-ionization will not be stabilized by resonance and, therefore, the SN1 mechanism is ruled out.

4. Because of the possible repulsion, it is less likely for the electron-rich nucleophile to approach electron-rich arenes.
Replacement by hydroxyl group:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 45
The presence of an electron-withdrawing (-NO2) at ortho and para position increases the reactivity of haloarenes.
The effect is pronounced when the (-NO2) group is introduced at ortho and para positions. However, no effect on the reactivity of haloarenes is observed by the presence of an electron-withdrawing group at meta-position. Mechanism of the reaction is as depicted
Haloalkanes and Haloarenes Class 12 Notes Chemistry 46
The effect is pronounced when (—NO2 the) group is introduced at ortho and para positions. However, no effect on the reactivity of haloarenes is observed by the presence of an electron-withdrawing group at the meta position. The mechanism of the reaction is as depicted:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 47
Haloalkanes and Haloarenes Class 12 Notes Chemistry 48
Haloalkanes and Haloarenes Class 12 Notes Chemistry 49
The presence of a nitro group at ortho- and para- position withdraws the electron density from the benzene ring and thus facilitates the attack of the nucleophile on haloarene.

The carbanion thus formed is stabilized through resonance. The negative charge appeared at ortho- and para- positions with respect to the halogen substituent is stabilized by -NO2 group while in the case of mcfa-nitrobenzene, none of the resonating structures bear the negative charge on carbon atom bearing the -NO2 group.

Therefore, the presence of a nitro group of meta-position does not stabilize the negative charge and no effect on reactivity is observed by the presence of the -NO2 group of meta-position.

2. Electrophilic Substitution Reactions: Haloarenes undergo the usual electrophilic reactions of the benzene ring such as halogenation, nitration, sulphonation, and Friedel-Crafts reactions. Halogen atom besides being slightly deactivating is o, p-directing, therefore, further 1 substitution occurs at ortho- and para-positions with respect to the halogen atom.

The o, p-directing; therefore, further substitution occurs at ortho- and para-positions with respect to the halogen atom. The o, p-directing influence of halogen atom can be easily understood if we consider the resonating structures of halobenzene as shown:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 50
Due to resonance, the electron density increases more at ortho- and para-positions than at mcia-positions. Further, the halogen atom because of its-I effect has some tendency to withdraw electrons from the benzene ring. As a result, the ring gets somewhat deactivated as compared to benzene and hence the electrophilic substitution reactions in haloarenes occur slowly and require more drastic conditions as compared to those in benzene.
1. Halogenation:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 51
2. Nitration:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 52
3. Sulphonation:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 53
4. Friedel-Crafts reaction:
Haloalkanes and Haloarenes Class 12 Notes Chemistry 54
Haloalkanes and Haloarenes Class 12 Notes Chemistry 55
3. Reaction with metal:
Wurtz-Fitting Reaction: It is between an alkyl and aryl halide.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 56
→ Polyhalogen Compounds: Carbon compounds containing more than one halogen atom are usually referred to as polyhalogen compounds.

→ Dichloromethane (Methylene chloride CH2Cl3: It is widely used as a solvent in paint remover, as a propellant in aerosols, and as a process solvent in the manufacturing of drugs. It harms the human central nervous system.

→ Trichloromethane (Chloroform CHCl3): It is used as a solvent for fats, alkaloids, iodine, waxes, rubbers, plastics, etc. It was used as a general anesthetic in surgery.

Chloroform is slowly oxidized to carbonyl chloride (phosgene) by air in the presence of light. It is extremely poisonous in nature.
Haloalkanes and Haloarenes Class 12 Notes Chemistry 57
It is therefore stored in colored bottles to cut off light and in well- stoppered fully filled bottles to cut off air.

→ Triiodomethane (Iodoform CHI33): It was used as an antiseptic, but the antiseptic properties are due to the liberation of free iodine and not due to the iodoform itself.

→ Tetrachloromethane (Carbon Tetrachloride CCl4): It is used for the synthesis of chlorofluorocarbons and as a solvent. There is some evidence that exposure to CCl4 causes liver cancer in humans. It causes dizziness, nausea, and vomiting which can cause permanent damage to nerve cells. The chemical may irritate the eyes on contact. It depletes the ozone layer when released into the air.

→ Freons: Chlorofluorocarbon compounds of methane and ethane are collectively known as freons. They are extremely stable, unreactive, non-toxic, non-corrosive, and easily liquefiable gases, Freon 12 (CCl2F2) is one of the most common freons in industrial use. Most freon, even that used in refrigeration, eventually makes its way into the atmosphere where it diffuses into the stratosphere where it is able to imitate radical change reactions that can upset the natural ozone balance.

→ p, p’-Dichlorodiphenyltrichloroethane (DDT): The use of DDT was effectively used against the mosquito that spreads malaria and lice that carry typhus. Many species of insects developed resistance to DDT, and DDT was also discovered to have a high degree of toxicity towards fish. The chemical stability of DDT and its fat solubility compounded the problem. The use of DDT was banned in the USA in 1973, although it is still in use in some parts of the world. Its chemical formula is
Haloalkanes and Haloarenes Class 12 Notes Chemistry 58
Many out of these polyhalogen compounds cannot be easily decomposed and cause of depletion of the ozone layer and are proving environmental hazards.

Plasmodium Falciparum and P. vivax (Sporozoa – Plasmodium)

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Plasmodium Falciparum and P. vivax (Sporozoa – Plasmodium)

Protozoan parasites characterised by the production of spore – like oocysts containing sporozoites were known as sporozoa. The parasites belonging to this group of protozoa do not possess any special organs of locomotion, such as flagella or cilia. The medically important parasite of this class that is given in the
text is malarial parasite.

Malaria

It is the disease condition with seasonal intermittent fevers, chills and shivering. The name malaria (Mal: bad, aria: air) was given in the 18th century in Italy. The specific agent of malaria was discovered in RBC’s of a patient in 1880 by Alphonse Laveran.

In 1897, Ronald Ross identified the developing stages of malarial parasites in mosquitoes in Secunderabad, India. This led to various measures for the control and possible eradication of malaria by mosquito control. Both Ross (1902) and Laveran (1907) won the Nobel Prize for their discoveries in malaria.

Causative agents of human malaria:

The organisms: Four species of Plasmodium cause malaria in humans.

  • Plasmodium vivax: (Benign Tertian malaria)
  • Plasmodium falciparum: (Malignant tertian malaria)
  • Plasmodium malaria: (Benign Quartan malaria)
  • Plasmodium ovale: (Benign tertian malaria)

The two most common species are P. vivax and P. falciparum, WHO reports (2018) that falciparum being the most pathogenic of all.

Geographical Distribution

Malarial parasites are found in all countries. In India, malaria continues to be a major public health threat.

Habitat

The malarial parasites infecting man, after passing through a developmental phase in the parenchyma cells of the liver, reside inside the red blood corpuscles and are carried by the circulating blood to all the organs.

Vectors

Human malaria is transmitted by over 60 species of female Anopheles mosquito.

Human malarial parasite – Plasmodium falciparum

Of all the human malaria parasites, P. falciparum is the most highly pathogenic and responsible for malignant tertian malaria. This is a form of disease which runs an acute course in non-immune patients and is frequently fatal if untreated.

Life Cycle

The malaria parasite passes its life cycle in two different hosts and comprises of two phase as follows,

Definitive host:

Female Anopheles mosquito (a sexual phase of parasite occurs).

Intermediatehost:

Human (an asexual phase of parasite occurs). Thus, life cycle of malaria parasite show alternation of generations – asexual and sexual generation in two different hosts (Figure 8.12).
Plasmodium Falciparum and P. vivax (Sporozoa - Plasmodium) img 1

Human Cycle (Asexual Phase – Schizogony)

Human infection occurs when the sporozoites (the infective forms of the parasite are present in the salivary gland of the mosquito) are injected into blood capillaries when the mosquito feeds on blood after piercing the skin. The malarial parasite multiplies by division and the process designated as Schizogony (schizo: to split, gone: generation).

Sporozoites are minute thread-like curved organisms with tapering ends. Measuring 9-12µ in length with a central elongated nucleus while, the cytoplasm reveals no pigment as seen with a light microscope. In human, schizogony occurs in two locations. One in the red blood cells (erythrocytic schizogony) and other
in the liver cells (pre – or exoerythrocytic schizogony).

A. Pre-erythrocytic or Exoerythrocytic schigony

  • Sporozoites do not directly enter the RBC’s to initiate erythrocytic schizogony, but undergo developmental phase in other human tissues.
  • This cycle lasts for about 8 days in Plasmodium vivax, 6 days in P. falciparum and 9 days in P. ovale.
  • This pre-erythrocytic schizogony occurs within parenchymal cells of the liver.
  • The Sporozoites, which are elongated spindle – shaped bodies, become rounded inside the liver cells.
  • They enlarge in size and undergo repeated nuclear division to form several daughter nuclei, each of which is surrounded by cytoplasm.
  • This stage of the parasite is called the pre-erythrocytic or exoerthrocytic schizont or merozoites.
  • The heptocyte is distended by the enlarging schizont and the liver cell nucleus is pushed to the periphery.
  • Mature liver stage schizonts are spherical multinucleate and contain 2000-50,000 uninucleate merozoites.
  • These normally rupture in 6-15 days and release thousands of merozoites into the blood stream.
  • They do not return from red blood cells to liver cells.

Plasmodium vivax and P. ovale – parasites in liver tissue are called hypnozoites.

B. Erythrocyticstage

  • The merozoites released by pre-erythrocytic schizonts invade the red blood cells (Parasitaemia).
  • Merozoites are pear – shaped bodies, about 1.5 µm in length.
  • In the erythrocyte, the merozoite loses its internal organelles and appears as rounded body having a vacuole in the center with the cytoplasm pushed to the periphery and the nucleus at one pole. These forms are called ring forms or young trophozoites.
  • The parasite feeds on the hemoglobin of the erythrocyte. They incompletely metabolize hemoglobin therefore, hematin – globin pigment or haemozoin pigment is left behind.
  • The malaria pigment released when the parasitized cells rupture is taken up by recticuloendothelial cells.
  • The ring form develops and becomes irregular in shape and shows amoeboid motility. This is called the amoeboid form.
  • When the amoeboid form reaches a certain stage of development, its nucleus starts dividing by mitosis followed by a division of cytoplasm to become mature schizonts or merozoites.
  • A mature schizont contains 8-32 merozoites and haemozoin. The mature schizont bursts releasing the merozoites into the circulation.
  • The merozoites invade fresh erythrocytes within which they go through the same process of development. This cycle is called erythrocytic schizogony.
  • The rupture of the mature schizont releases large quantities of pyrogens. This is responsible for the febrile paroxysms characterising malaria.
  • In P. falciparum, erythrocytic schizogony always takes place inside the capillaries and vascular regions of internal organs. Therefore, in these infections, schizonts and merozoites are usually not seen in the peripheral blood.

C. Gametogony

  • Some of the merozoites, after a few erythrocytic cycles do not develop into trophozoites and schizonts but they undergo sexual differentiation to develop into the gametocytes.
  • Development of gametocytes takes place within the internal organs and only the mature forms appear in circulation.
  • The mature gametocytes in P. falciparum are crescent shaped.
  • Female gametocytes are generally more numerous and larger.
  • Male gametocytes and female gametocytes are called micro gametocytes and macro gametocytes respectively.
  • Gametocyte appears in 10-12 days in P. falciparum.
  • The gametocytes do not cause any clinical illness in the host, but are essential for transmission of the infection.
  • A person who harbors the gametocytes is referred to as a carrier or reservoir.

Mosquito Cycle (Sexual Cycle – Sporogony)

  • A Female Anopheles mosquito during its blood – meal from an infected person, sucks up both the sexual and asexual forms of parasite. But, only the mature sexual forms develop and the rest die.
  • The gametocytes are set free in the midgut (stomach) of mosquito and undergo further development.
  • The nuclear material and cytoplasm of the male gametocyte divides to produce long, actively motile, whip – like forms of 8 microgametes. This process is called exflagellation of male gametocytes.
  • The Exflagellation is completed within 15-30 minutes for P. falciparum.
  • The female gametocyte does not divide but maturation involves by condensation of nucleus to become the female gamete.
  • Female gamete is fertilized by one of the microgametes to produce the zygote. The zygote is formed in 20-120 minutes after the blood meal. The zygote is initially is a non – motile round body, but within 18-24 hours, it gradually elongates into a vermicular motile form. This is called the ookinete.
  • Ookinete penetrates the epithelial lining of stomach wall. Their anterior end comes in close contact to the cell membrane by secretion of some proteolytic substances which causes lysis of cell membrane. Later, the ookinete come to lie just beneath the basement membrane.
  • It becomes rounded into a sphere with an elastic membrane. This stage is called the oocyst. The oocyst increase in size and undergo numerous nuclear multiplication which develops a large number of sickle shaped bodies known as sporozoites.
  • Number of oocysts in the stomach wall varies from a few to over a hundred.
  • Around the 10th day of infection the oocyst ruptures, releasing sporozoites in the body cavity of the mosquitos.
  • The sporozoites are distributed through the circulating fluid into various organs and tissues of the mosquito except the ovaries.
  • The sporozoites have a special affinity towards the salivary glands. The mosquito at this stage is capable of transmitting infection to man.

Pathogenesis

In malaria, typical pathological changes are seen primarily in the spleen, liver, bone marrow, lungs, kidney and brain.

Liver:
The liver is enlarged. The organ becomes more firm and pigmented. Pigments are found in parenchymal cells.

Spleen:
The spleen is markedly enlarged. If the infection lasts over a long period, the spleen is usually grayish, dark brown or even black and is commonly known as ‘ague cake’. Bone marrow, Lungs, Kidneys and Brain are enlarged and pigmented. They are filled with parasitized erythrocytes.

Anemia is caused by destruction of large number of red cells by complement mediated and autoimmune hemolysis. It is also due to the increased clearance of both parasites and parasitized RBCs by the spleen.

Clinical Manifestations

The incubation period is generally 9-14 days but, it can be as short as 7 days. The most malignant form of malaria is caused by P. falciparum hence, variable clinical syndromes are associated with falciparum malaria. That include,

1. Prodromal (initial indication of the onset of disease) period:

Non – specific symptoms such as malaise (condition of general weakness or discomfort), myalgia
(severe muscle pain) headache and fatigue (feeling of tiredness) are usually seen during the prodromal period.

2. Malarial paroxysm (sudden onset of disease):

It is the classical manifestation of acute malaria. It is characterised by fever, chill and rigor (sudden feelings of cold with shivering).The fever is caused by rupture of red blood cells that contain malarial parasites. The fever occurs every 48 hours in falciparum malaria.

3. Anemia (A condition in which the blood does not have enough healthy Red Blood cells) and

4. Hepatosplenomegaly (simultaneously enlargement of both the liver and the spleen)

The symptoms are non – specific with headache, pains in back and limbs, anorexia, nausea and a feeling of chill rather than a distinct cold phase. Hyponatremia (A condition that occurs when the level of Sodium in the blood is too low) occur in both uncomplicated and severe malaria.

Complications of Severe

Falciparum Malaria

1. Black water fever

The syndrome is the manifestation of repeated infections of falciparum malaria, which were inadequately treated with quinine. The condition is associated with haemoglobinaemia (excess of hemoglobin in the blood plasma) and haemoglobinuria (excretion of free haemoglobin in the urine).

The syndrome is known as black water fever due to the dark red to brown – black appearance of the urine in this condition (Figure 8.13). It is dark due to presence of free haemoglobin as methaemoglobin or oxyhaemoglobin in it. Kidney failure is the immediate cause of death.
Plasmodium Falciparum and P. vivax (Sporozoa - Plasmodium) img 2

2. Cerebral malaria

Cerebral malaria is the most common presentation of severe malaria in adult. Cerebral malaria may be sudden in onset. Clinically, the condition manifests with fever for 4-5 days, slowly lapsing into coma, with or without convulsions.

It is marked by a severe headache, high fever even above 180°F, and changes in mental
status. Death may occur within few hours. Algid malaria and septicemic malaria are also other serious complication of falciparum malaria.

3. Pernicious malaria

The term pernicious malaria is referred to as a series of phenomena that occur during the course of an in treated P. falciparum infection within 1 to 3 days.

Anaemia:

An individual suffering from an attack of malaria, after a few paroxysms becomes temporarily anaemic. The reduction in red blood cells is greater in P. falciparum infection than in infection with P. vivax and P. malariae. This is because P. falciparum invades young and mature erythrocytes and the infection rate
of red blood cells is also greater.

Recrudescence

In P. falciparum and P. malariae infections after the primary attack, sometimes there is a period of latency, during which there is no clinical illness. But some parasites persist in some erythrocytes and gradually increase in numbers.

Fresh malarial attacks then develop. It appears after a period of latency usually within weeks after the primary attacks. Persistence of the erythrocytic cycle of the parasites are called recrudescences. In P. falciparum infections, recrudescences are seen for 1-2 years, while in P. malariae infection, they may last for long periods, even upto 50 years.

Plasmodium vivax

P. vivax shows a similar life cycle in humans and mosquitoes like that of P. falciparum. Except in P. vivax, a latent tissue stage, the hypnozoites present in the liver parenchyma. Relapse in vivax malaria is caused by these hypnozoites. Hypnozoites are the dormant stages of the parasites.

These are single – nucleated parasites measuring 4µm-6µm in diameter. These become active and develop into tissue schizonts after a short period of dormancy. This relapse may occur at intervals up to 3 years or more after the first attack. P. vivax merozoites invade only young erythrocytes and the reticulocytes.

Clinical Manifestations

P. vivax is the most wide spread species causing malaria in man. However, unlike falciparum malaria, vivax malaria, is less severe and death from the condition relatively is less common. Table 8.2 describes the comparison of course of infection in Falciparum malaria with Vivax malaria

Stage

P.falciparum

P.vivax

Pre-erythrocytic schizogony Stage lasts for 6 days. Each Schizont produces about 40,000 merozoites approximately. Lasts for 8 days. Each Schizont produces about 12,000 approximately
Erythrocytic schizogony Each cycle lasts for 36–48
hours. First temperature peak occurs by 12th day of infection. Primary attack last for 10-14 days
Each cycle lasts for 48 hours. First fever peak occur by 16th day of infection. Primary attack lasts for 3-4 weeks.
Gemotogony Gametocytes in peripheral blood may be seen on 21st day of infection Gametocytes in peripheral
blood may be seen on 16th day of infection.
Exo – erythrocytic schizogony Absent. Relapses do not occur Present. Can continue for up to 3 years. Relapses often occur.

Laboratory Diagnosis

Diagnosis of malaria includes:

  • Parasitic diagnosis
  • Serodiagnosis, and
  • Molecular diagnosis

Parasitic diagnosis – Demonstration of parasite by microscopy

Specimen:
Blood

Conventional light microscopy of stained blood smear is the gold standard for confirmation of malaria.

Two types of smears are prepared from the peripheral blood. They are thin and thick smears (Figure 8.14). Ring forms and gametocytes are most commonly seen in the peripheral blood smear. They are thin and thick smears (Figure 8.14). Ring forms and gametocytes are most commonly seen in the peripheral blood smear.
Plasmodium Falciparum and P. vivax (Sporozoa - Plasmodium) img 3

Thin smear They are prepared from capillary blood of fingertip and spread over a good quality slide by a second slide (spreader slide) held at an angle of 30°-45° from the horizontal such that a tail is formed. Thin smears thus prepared are air dried, fixed in alcohol and stained by one of the Romanowsky stains such as Leishman, Giemsa or JSB (Jaswant singh and Bhattacharjee) stain.

Thin smears are used for:

  • Detecting parasites, and
  • For determining the species of the infecting parasite.

Thick smear

They are prepared usually with 3 drops of blood spread over a small area of about 10mm. The thick film is dried. This smears consist of a thick layer of dehemoglobinized (lysed) red blood cells. It is not fixed in methanol. Thick film is stained similar to thin film. Thick smears have the advantage of concentrating the parasites and therefore increase the sensitivity of diagnosis. Thick smears are used for:

  • Defecting parasites,
  • Quantitating parasitaemia, and
  • Demonstrating malarial pigments.

Fluoroscence microscopy

The method is mainly used for mass screening in field laboratory. Fluorescent dyes like acridine orange is used to stain the blood smears. It stains DNA as fluorescent green and cytoplasmic RNA as red.

QBC (Quantitative Buffy coat smear)

This is a sensitive method for detection of malaria parasites. In this method, blood is collected in a capillary tube coated with fluorescent dye and is subjected to centrifugation. After centrifugation, the Buffy coat in the centrifuged capillary tubes is examined under a fluorescent microscope. Acridine orange – stained
malaria parasites appear brilliant green.

Serodiagnosis

It is not helpful in clinical diagnosis. It is used mainly for epidemiological survey and to identify the infected donors in transfusion malaria. The test used are indirect haemagglutination (IHA), Indirect fluorescent antibody (IFA) and Enzyme – linked immunosorbent assay (ELISA) for the detection of serum antibodies.

Rapid Antigen detection tests kits are available commercially like the dipstick, card and cassette bearing monoclonal antibody. These tests are based on the detection of antigens using immune chromatographic methods. These tests can detect plasmodium in 15 minutes.

Molecular diagnosis

DNA probe and PCR are highly sensitive methods for the diagnosis of malaria. It is more sensitive than that of thick blood smear. It is highly species specific. Other tests includes the measurement of hemoglobin, total WBC and platelet count in severe falciparum malaria, urine can be tested for free hemoglobin, if black water fever is suspected. Blood urea and serum creatinine has to be monitored for renal failure.

Treatment

The most commonly used drugs are Chloroquine, Quinine, Pyrimethamine and Doxycycline.

Prevention and Control

The preventive measures to control malaria mainly depend on treatment of infected individuals and reducing the transmission of malaria. The control measures include the use of insecticides such as DDT (Di chlorodiphenyl tri chloromethane) or Malathion for controlling the populations of adult mosquitoes.

Proper use of mosquito nets, wearing protective clothings and use of mosquito repellants can prevent the mosquito bite.

Introduction to Helminths

General characteristics of Helminthic parasite:

  1. Helminths are multicellular worms. They are bilaterally symmetrical animals having 3 germ layers and belong to the kingdom Metazoa.
  2. They are invertebrates characterised by elongated, flat or round bodies.
  3. Helminths develop through egg, larval and adult stages. Flowchart 8.1 describes the classification of helminthes.

Tissue Flagellates – Leishmania Donovani

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Tissue Flagellates – Leishmania Donovani

The genus is named after the scientist Leishman, who first described the parasite in London in May 1903.

Geographical Distribution:

Leishmania species is found in the Mediterranean, the Middle East, Africa and Asia including India.

Habitat:

Leishmania donovani is an obligate intracellular parasite of human and other mammalian hosts. They are always found as intracellular amastigotes in the reticuloendothelial cells of the spleen, bone marrow, liver, intestinal mucosa and mesenteric lymph nodes of hosts.

Morphology:

The parasite exists in two forms:

Amastigote:

It is the form found in human and other mammalian hosts. They are found inside monocytes, polymorphonuclear leucocytes or endothelial cells. They are small, round to oval bodies measuring 2-3µm in length (Figure 8.8). They are also known as LD (Leishman donovan) bodies.
Tissue Flagellates - Leishmania Donovani img 1

Promastigote:

These forms are found in the mid-gut of sand fly and in the culture media. The fully developed promastigotes are long, slender and spindle – shaped. They measure 15µm to 25µm in length and 1.5µm to 3.5µm in breadth. A single nucleus is situated at the centre. The kinetoplast lies near the anterior end. The flagellum is single, delicate and measures 15µm-28µm (Figure 8.8).
Tissue Flagellates - Leishmania Donovani img 1

Life – Cycle of Leishmania donovani

Leishmania donovani completes its life cycle in two different hosts. The complete life cycle is given in Figure 8.9.
Tissue Flagellates - Leishmania Donovani img 2

Host

Forms

Human and other mammals
(Example: Dogs)
Amastigote
Sandfly of Genus Phlebotomus Promastigote

Development in Human

The parasite is transmitted to human and other vertebrate hosts by the bite of blood sucking female sandfly. During the blood meal, the sandfly deposists promastigotes on surface of the skin. These promastigotes are immediately phagocytosed by fixed macrophages of the host, in which they are transformed into amastigotes. The amastigotes multiply by binary fission within the macrophages.

As many as 50 to 200 amastigotes may be present inside the enlarged cell. These are called LD bodies. The rupture of cell releases amastigotes in large numbers which inturn are free to infect other cells. Free amastigotes are subsequently carried by circulation. These forms invade monocytes of the blood and macrophages of the spleen, liver, bone marrow, lymph nodes and other tissues of the reticuloendothelial cells.

Development in sandfly

Female sandfly during a blood meal ingest free, as well as intracellular amastigotes in the blood. In the mid gut of the sandfly, the amastigotes are transformed within 72 hours to flagellated promastigotes. These promastigotes multiply by binary fission. After a period of 6 to 9 days, these forms migrate from the midgut to the pharynx and buccal cavity of sandfly. Bite of the infected sandfly transmits infection to susceptible persons and the life – cycle is repeated.

Pathogenesis

Leishmania donovani causes visceral Leishmaniasis. The disease is also known as Dum – Dum fever, Asian fever, Assam fever, or infantile splenomegaly. Leishmaniasis is a disease of the reticuloendothelial system. Proliferation and destruction of reticuloendothelial cells of the internal organs are responsible for the pathological changes in visceral leishmaniasis.

Spleen, liver and lymphnodes are enlarged in this condition. Bone marrow is dark red in colour and shows extensive proliferation of reticuloendothelial cells. Kidney shows cloudy swelling and is invaded by macrophages parasitized by amastigotes.

Clinical Features

Incubation period:
It is usually 3-6 months but can be months or years.

Visceral Leishmaniasis is a serious and fatal systemic disease. In India, the disease is called Kala – azar meaning “black disease”. The disease is characterized by the presence of fever, hepatosplenomegaly (Figure 8.10) (the simultaneous enlargement of both liver and the spleen), hypergammaglobulinemia (a condition in which increased levels of a certain immunoglobulin in blood serum), Leucopenia, Thrombocytopenia (deficiency of platelets in the blood), Cachexia (a condition that causes extreme weight loss) with marked anemia, emaciation and loss of weight.

Epistaxis (bleeding from nose) and bleeding from gums are common. In Indian patients, the skin on the hands, feet, abdomen, around the mouth and fore – head becomes grayish and dark coloured. This hypo – pigmentation of the skin is unique in Indian patients giving the disease name Kala – azar.
Tissue Flagellates - Leishmania Donovani img 3

Post kala – azar dermal leishmaniasis

(PKDL):
It is a non – ulcerative lesion of the skin, which is seen after completion of treatment of the kala – azar. This condition is characterized by multiple, hypopigmented, erythematous macules involving the face and trunk (Figure 8.11).
Tissue Flagellates - Leishmania Donovani img 4
In Indian forms, PKDL appears after a latent period of 2 years and may even persist as long as 20years, creating a persistent human reservoir of infection.

Laboratory diagnosis

Specimens:
Aspiration from spleen, bone marrow, lymph node, liver biopsy and peripheral blood.

Methods of examination:
This includes, microscopy and culture

1. Direct microscopy

The amastigotes of Leishmania donovani (known as LD bodies) can be demonstrated in the smears of spleen, bone marrow, liver, lymph node and peripheral blood stained in Leishman, Giemsa or wright stains. Splenic aspiration is the most sensitive method to detect LD bodies. Examination of peripheral blood smear and buffy coat smear is more commonly used to find LD bodies in the circulating monocytes.

2. Culture

Promastigotes are found in the culture media. Tissue samples and aspirates are inoculated in the NNN (Novy-MacNeal-Nicolle) medium for demonstration of promastigotes. Laboratory diagnosis of kala – azar is briefly discussed in Flowchart 8.5.
Tissue Flagellates - Leishmania Donovani img 5

Treatment:
Pentavalent antimonials are the drugs of choice. Pentamidine, Amphotericin B and Miltefosine (oral drug) are recommended.

Prevention and Control

Integrated insecticidal spraying (DDT and Malathion) to reduce sandfly population. Reduction of reservoir by killing all the infected dogs. Personal prophylaxis by using anti – sandfly measures like using thick clothes, bed nets, window mesh or insect repellants and keeping the environment clean. No vaccine is available against kala – azar.

Giardia Lamblia of Medical Parasitology

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Giardia Lamblia of Medical Parasitology

(Also known as Giardia duodenalis, Giardia intestinalis)

Geographical Distribution

It is the most common protozoan pathogen and is worldwide in distribution. The diseaseis very high in areas with low sanitation, especially tropics and subtropics.

Habitat

Giardia lamblia lives in the duodenum and upper jejunum of human. It is the only protozoan parasite found in the lumen of the human small intestine.

Morphology

It exists in two forms

  • Trophozoite and
  • Cyst

Trophozoite

The trophozoite is in the shape of a tennis or badminton racket. It is rounded anteriorly and pointed posteriorly. The size of the trophozoite is 14 µ long by 7µ broad. Dorsally, it is convex and ventrally, it has a concave sucking disc which helps in its attachment to the intestinal mucosa.

It is bilaterally symmetrical. All the organs of the body are paired. Trophozoite of Giardia possess,

  • 1 pair of nuclei
  • 4 pairs of flagella
  • Parabasal body (Blepharoplast), from which the flagella arise (4 pairs)
  • 1 pair of axostyles, running along the midline
  • Two sausage – shaped parabasal or median bodies lying transversely posterior to the sucking disc
  • The trophozoite is motile, with a slow oscillation about its long axis, often resembling falling leaf (Figure 8.6a).

Giardia Lamblia of Medical Parasitology img 1

Cyst

It is the infective form of the parasite. The cyst is small and oval, measuring 12 µm × 8 µm and is surrounded by a hyaline cyst wall.

Its internal structure includes 2 pairs of nuclei grouped at one end. A young cyst contains 1 pair of nuclei. The axostyle lies diagnonally, forming a dividing line within cyst wall (Figure 8.6b).
Giardia Lamblia of Medical Parasitology img 2

Life Cycle:
Giardia Life Cycle in Host (Human)

Infective form:
Mature cyst

Mode of transmission:

Human acquires infection by ingestion of cyst in contaminated water and food. Direct person – to person transmission occurs in children. Transmission occurs through oral-anal and oral-genital route in sexually active homosexual males. Within half an hour of ingestion, the cyst hatches out into two trophozoites, which multiply by binary fission and colonize in the duodenum.

The trophozoites live in the duodenum and upper part of jejunum, feeding by pinocytosis. When conditions in duodenum are unfavourable, encystment occurs, usually in large intestine. Cysts are passed in stool and remain viable in soil and water for several weeks (Figure 8.7).
Giardia Lamblia of Medical Parasitology img 3

Pathogenicity

Giardia lamblia does not invade the tissue, but remains attached to intestinal epithelium by means of the sucking disc. It causes a disturbance of intestinal function leading to malabsorption of fat.

Clinical Manifestations

Incubation period is variable, but is usually about 2 weeks.

The disease is asymptomatic, but in some cases it may lead to abdominal cramps, flatulence, looseness of bowels, foul smelling stool and mild steatorrhoea (passage of yellowish and greasy stools in which there is excess of fat). The stool contains excess mucus and fat but no blood and pus.

Children may develop chronic diarrhoea, malaise (discomfort), nausea, anorexia (loss of appetite for food), malabsorption of fat, vitamin A and protein. Occasionally, Giardia may colonize the gall bladder causing biliary colic and jaundice.

Laboratory Diagnosis

Specimens:
Stool and blood

Examination of stool sample:
Giardiasis can be diagnosed by identification of cysts of Giardia lamblia in the formed stools and the trophozoites and cyst of the parasite in diarrhoeal stools.

Macroscopic examination of stool:
Fecal specimens containing Giardia lamblia may have an offensive odor. It is pale coloured with fatty substance floating in water.

Microscopic examination of stool:
Cysts and trophozoites can be found in diarrheal stools by saline and iodine wet preparations (Figure 8.8).

Serodiagnosis:
Immuno chromatographic strip tests and indirect immunofluorescence (IIF) tests are readily available. For antigen and antigen detection ELISA, Commercially available ELISA kits detects Giardia – Specific antigen.

Molecular methods:
DNA probes and polymerase chain reaction (PCR) have been used to demonstrate parasitic genome in the stool specimen.

Treatment

Metronidazole and Tinidazole are the drugs of choice.

Prevention and Control

Giardiasis can be prevented and controlled by,

  • Proper disposal of human faeces, maintenance of food and personal hygiene and health education.
  • After using the bathroom and before eating, the hands should be washed thoroughly with soap and warm water. Boiling of water is the best and effective method in killing the viable cysts.
  • To reduce the risk of venereal transmission, patients should avoid risky sexual behavior.
  • No vaccine or effective chemo prophylactic drug is available for prevention of Giardiasis.

Life Cycle of Entamoeba Histolytica

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Life Cycle of Entamoeba Histolytica

Geographical Distribution

It is Worldwide in distribution they are more common in the tropics than elsewhere. It is found wherever sanitation is poor.

Habitat

Trophozoites of E.histolytica live in the mucous and submucous layers of the large intestine of human.

Morphology

E. histolytica occurs in 3 forms as Trophozoite, Precyst and Cyst.

Trophozoite:

It is the growing or feeding stage of the parasite. It is the only form present in tissues. It has no fixed shape. They vary in size from 18 to 40µ, average being 20 to 30µ. The cytoplasm is usually described as outer ectoplasm and inner endoplasm (Figure 8.1). The endoplasm contains nucleus, food vacuoles, erythrocytes, occasionally leucocytes and tissue debris.

The nucleus is characterised by evenly arranged chromatin on the nuclear membrane and the presence of a small, compact, centrally located karoyosome (It is a DNA containing body, situated peripherally or centrally within the nucleus). Trophozoites exhibits active crawling or gliding motility by forming finger-like projections called Pseudopodia.

The trophozoite reproduce by binary fission in every 8 hours. Trophozoites survives upto 5 hours at 37°C and are killed by heat, drying and chemical sterilization. Even if live trophozoites from freshly passed stools are ingested, they are rapidly destroyed in stomach and cannot initiate infection. Therefore, the infections is not
usually transmitted by trophozoites.

Precyst

Trophozoites undergo encystment in the intestinal lumen. Encystment does not occur in the tissue or in feces outside the body. Precyst is smaller in size about 10 – 20 µm in size. It is round or oval in shape. The endoplasm is free of red blood cells and other ingested food particles (Figure 8.1). The nuclear structure retains the characteristics of the trophozoite.

Cyst

Precyst secretes a highly refractive cyst wall around it and becomes a cyst. A mature cyst is a quadrinucleate spherical body. The cyst begins as a uninucleate body but soon divides by binary fission and develops into binucleate and quadrinucleate bodies (Figure 8.1).
Life Cycle of Entamoeba Histolytica img 1

The cytoplasm of the cyst is clear and hyaline (translucent) and the nuclear structure retain the characteristic of the trophozoites. The mature quadrinucleate cyst, passed in the stool, does not undergo any further development and remain alive for several months in the soil or in environment where they were deposited. The mature quadrinucleate cysts are the infective forms of the parasite.

Life – Cycle of Entamoeba histolytica

E. histolytica passes its life cycle only in one host, the human.

Infective form:
Mature quadrinucleate cyst.

Mode of transmission:
Ingestion of food and water contaminated with cyst.

The cysts that are swallowed along with food and water enter into the alimentary canal. The cyst wall is resistant to action of gastric juice. The cysts pass through the stomach undamaged and enters the small intestine (Figure 8.2).
Life Cycle of Entamoeba Histolytica img 2

When the cyst reaches caecum or lower part of the ileum, due to alkaline medium, the cyst wall is damaged by trypsin leading to excystation.

The cytoplasm gets detached from the cyst wall and an amoeboid movement appear causing a tear in the cyst wall, through which quadrinucleate amoeba is liberated. This stage is called the metacyst.

The nuclei in the metacyst immediately undergo division to form 8 nuclei, each of which gets surrounded by its own cytoplasm to become 8 small amoebulae or metacystic trophozoites.

These metacystic trophozoites are carried to the caecum and colon. They invade the tissues and lodge in the submucous tissue of the large intestine which is their normal habitat.

Trophozoite grow and multiply by binary fission. The trophozoite phase of the parasite is responsible for producing the characteristic lesion of amoebiasis.

Some of the trophozoites in colon develop into precystic forms and cysts, which are passed in feces to repeat the cycle.

Pathogenesis

E. histolytica causes intestinal and extra intestinal amoebiasis (Flowchart 8.3).

E. histolytica can live in the intestine without causing symptoms. But, they can also cause severe disease. These amoebas may invade the wall of the intestine leading to amoebic dysentery, an illness that causes intestinal ulcers, bleeding, increased mucus production and diarrhoea. The ulcers are strictly confined to the large intestine being most numerous in the caecum and next in the sigmoid-rectal regions.

The lesions may be generalized or localised. A typical amoebic ulcer varies from pin’s head to one inch or more in diameter in size. The shape of ulcer may be round or oval.

On vertical section, the ulcer appears like flask, with mouth and neck being narrow and base being large and rounded (Figure 8.3 shows the flask – shaped ulcer). The base of ulcer is generally formed by the muscular coat and filled up by the necrotic material. The ulcers generally do not extend deeper than submucosal layer.
Life Cycle of Entamoeba Histolytica img 3

Clinical Features

Incubation period is highly variable, but is generally 4 to 5 days. A wide spectrum, from asymptomatic infection (luminal amoebiasis), to invasive intestinal amoebiasis (dysentery, colitis, appendicitis, toxic mega colon, amoebomas), to invasive extraintestinal amoebiasis occurs. Flowchart 8.4 classifies the clinical
outcomes of infection with Entamoeba histolytica. Only about 10% to 20% of people who are infected with E. histolytica become sick from the infection.
Life Cycle of Entamoeba Histolytica img 4

The typical manifestation of intestinal amoebiasis is amoebic dysentery. The symptoms are often quite mild and can include loose feaces, stomach pain and stomach cramping. In acute amoebic dysentery, the symptoms include abdominal pain, bloody stool, fever, tenderness, rectal tenesmus and hepatomegaly (enlargement of liver).

People affected may develop anemia due to loss of blood. On clinical and laboratory ground, amoebic dysentery should be differentiated from bacillary dysentery. A Table 8.1 shows the difference between the stools of amoebic and bacillary dysentery. Table 8.1: Difference between the stools of amoebic and bacillary dysentery.
Life Cycle of Entamoeba Histolytica img 5

Extra intestinal amoebiasis

1. Hepatic amoebiasis:

This is the most common form of extra intestinal invasive amoebiasis. Liver abscess may be multiple or more often solitary, usually located in the upper right lobe of the liver (Figure 8.4). Amoebic liver abscess (ALA) contains an odour less and thick chocolate brown pus called anchovy sauce pus.

ALA is associated with an abrupt onset of high fever, right upper abdominal pain and tenderness. Anorexia (loss of appetite for food), nausea (the sensation to vomit), vomiting, fatigue (extreme tiredness) and weight loss are also frequent.

2. Pulmonary Amoebiasis:

It is very rare, but this may occur by direct hematogenous spread from the colon. The patient presents with severe chest pain and have dyspnoea (shortness of breath). The sputum of patient is chocolate brown. Amoebic trophozoites may be demonstrated in the sputum.

3. Cerebral amoebiasis:

The condition is unusual. In cerebral amoebiasis, the abscess is single, small and is located in the cerebral hemisphere. The patient may die of rupture or involvement of cerebellam within 12-72 hours. Biopsy of the brain shows the amoebic trophozoites.

4. Cutaneous amoebiasis:

It can be caused by perforation of an amoebic abscess or surgical wound infected with amoebae. It is less frequent condition.

5. Genitourinary Amoebiasis:

This condition includes amoebiasis of the kidney and genital organs. Amoebiasis of the genital organs is a rare condition. Lesions of amoebiasis is shown in Figure 8.5.
Life Cycle of Entamoeba Histolytica img 6

Laboratory Diagnosis

Specimens:
Stool is the specimen of choice. Other specimens collected includes blood, rectal exudates and rectal ulcer tissue collected from the base by endoscopies.

Methods in examination of stool

A. Direct wet mount examination of stool:

Demonstration of mature quadrinucleate cysts or trophozites in stool is diagnostic of intestinal amoebiasis. The wet mount of stool is prepared in the saline, iodine or lacto phenol cotton blue.

B. Examination of stool after concentration:

Demonstration of amoebic cysts by Formalin – ether is the method of choice.

C. Examination of stained stool smears:

Staining by iron haematoxylin, Periodic Acid – Schiff (PAS) stains demonstrate the presence of both trophozoites and cyst.

Amoebic liver abscess (ALA):
Demonstration of amoebic trophozoites in the aspirated liver pus establishes the diagnosis of ALA.

Serology:
Detection of amoebic antigens in the serum by Enzyme Linked Immunosorbent Assay (ELISA).

Molecular diagnosis:
PCR (Polymerase chain reaction) is employed to detect amoebic genome in the aspirated liver pus for the diagnosis of ALA.

Imaging methods:
X – Ray magnetic resonance imaging (MRI) scan and computerized Axial Tomography (CAT) Scan are the imaging methods used.

Treatment:
Eradication of amoebae by the use of amoebicidal drugs and replacement of fluid and electrolyte is the treatment for amoebiasis. Listed below the drugs used in the treatment for amoebiasis.

  • Paramomycin and iodoquinol acts in the intestinal lumen but not in tissues.
  • Emetine, chloroquine are effective in systemic infection. They act only on trophozoites.

Metronidazole is the drug of choice which acts as both luminal and tissue amoebicides. It is low in toxicity and is effective against intestinal as well as extra -intestinal amoebic infections.

Prevention and Control

  • Proper sanitation is the key to avoid amoebiasis. Washing hands with soap and water after using the bathrooms and before handling food.
  • Drinking safe and boiled water.
  • Avoid eating unwashed fruits and vegetables.
  • Prevention of water supplies from faecal contamination.
  • Early rapid detection of diseased people and subsequent treatment with amoebicidal drugs. No vaccine is available yet against amoebiasis in humans.

Medical Parasitology of Parasite and Host

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Medical Parasitology of Parasite and Host

Parasites are living organisms, which depend on living host for their nourishment and survival. They multiply or undergo development in the host. Host is defined as an organism, which harbors the parasite, provides nourishment and gives shelter to parasite. Host is relatively larger than the parasite.

Association between Host and Parasite

The relationship between host and the parasite can be of the following types:

  • Symbiosis
  • Commensalism, and
  • Parasitism.

Flowchart 8.1 describes the types of host – parasite relationshipMedical Parasitology of Parasite and Host img 1

Types and Classification of Parasite

According to the nature of the host – parasite interaction and the environmental factors, the parasite may be one of the following,

Ectoparasite:

These parasites live on the outer surface or in the superficial tissues of the host (Example: Lice). The infection by these parasites is called infestation.

Endoparasite:

The parasite which lives within the host is called Endoparasite. Invasion by the parasite is called Infection. Most of the protozoan and helminthic parasites causing human diseases are endoparasites.

Endoparasites can be further classified as:

Obligate parasite:
This parasite is completely dependent on its host and cannot survive without it.

Example:
Hookworms.

Facultative parasite:
This parasite may either live as free living form or as a parasite when the opportunity arises.

Example:
Naegleria fowleri.

Opportunistic parasite:
This parasite is capable of producing disease in an immune deficient host (like AIDS and cancer patients).

Example: Toxoplasma gondii.

Zoonotic Parasite:
This parasite primarily infects animals and is transmittable to humans.

Example:
Fasciola species.

Accidental parasite:
This parasite infect an unusual host are known as accidental parasites.

Example:
Echinococcus granulosus infects man accidentally.

Wandering or Aberrant parasites:

Parasites which infect a host migrate to the site where it cannot live or develop further are called aberrant parasites.

Example:
Dog roundworm infecting humans.

Types of Host

Definite host:

The host which harbour the adult parasites or in which parasites undergo sexual method of reproduction is referred to as a definite host. The definite host may be a human or any other living organism. Example: Mosquito acts as a definite host for Plasmodium spp. in Malaria.

Intermediate host:

The host in which the larval stages of the parasite live or in which asexual reproduction of parasite takes place is called the intermediate host.

Example:
Man acts as an intermediate host for Plasmodium spp. in Malaria.

Reservoir host:

The host which harbour the parasite and acts has an important source of infection to other susceptible hosts is known as reservoir host. It is also called temporary host.

Example:
Dog is the reservoir host for disease kala azar.

Natural host:
The host which is naturally infected with a certain species of parasite, is called natural host.

Example:
Pig is the natural host of Balantidium coli.

Paratenic host or transport host:

some parasites enter a host in which they do not undergo any development but remains alive till they gain entry into the definitive host or intermediate host. Such a host is termed as paratenic host or transport host or carrier host.

Classification of Medical Parasitology

The most acceptable taxonomic classification of human parasites includes Endoparasites and Ectoparasite. Endoparasites are subclassified into protozoan parasite (unicellular organisms) and helminthic parasite (multicellular organism). Parasites of medical Importance come under the Kingdom called Protista and Animalia. Protista includes the microscopic single – celled eukaryotes known as protozoa.

In contrast, helminths are microscopic, multicellular worms possessing well differentiated tissues and complex organs belonging to the kingdom Animalia. Classification of medically important parasites is given in Flowchart 8.2.

Life Cycle of Parasites

Direct life cycle

The life cycle of parasite that requires only single host to complete its development, is called direct life cycle.

Example:
Entamoeba histolytica requires only human host to complete its life cycle.

Indirect life cycle

The life cycle of parasite that requires two or more species of hosts to complete its development, the life cycle is called as indirect life cycle.

Example:
Malarial parasite (Plasmodium spp.) requires both human host and mosquito to complete its life cycle.

Transmission of Parasites

It depends upon Source or reservoir of infection, and mode of transmission.

1. Sources of infection

A. Human:

Human is the source or reservoir for a majority of parasitic infection. The condition in which the infection is transmitted from one infected human to another human is called anthroponoses.

B. Animals:

Animals act as the source of infection in many parasitic diseases. The condition where infection is transmitted from animals to humans is called zoonoses.

2. Mode of transmission

A. Oral transmission:

This is through ingestion of contaminated food, water, vegetables, soiled fingers or fomites contaminated by faeces that contain the infective stage of parasite. This mode of transmission is referred to as faecal-oral route. Example: Cysts of Entamoeba histolytica.

B. Skin transmission:

This is another important route. The infective larvae of hookworm enter the skin of persons walking bare footed on contaminated soil.

C. Vector transmission:

It could be a biological or a mechanical means. Many parasitic diseases are transmitted by insect bite.

Example:
sandfly is vector for Leishmania.

D. Direct transmission by person to person contact. Frequently, Entamoeba, Giardia andTrichomonas are transmitted by sexual contact among homosexuals.

E. Vertical transmission:

It is the transmission from mother to fetus.

Example:
Toxoplasmosis.

So far, we have learnt about the general introduction and classification of parasites. Now, let us learn a few important human parasites in detail.

Introduction to Protozoa

General characteristics of protozoa:

  1. They are microscopic unicellular eukaryotes.
  2. The single cell has a relatively complex internal structure and it performs various complex metabolic activities such as digestion, reproduction, respiration and excretion.
  3. Each cell consists of nucleus and cytoplasm.
  4. A protozoa parasite during its life cycle may exist in two stages such as trophozoite and cyst.

Amoebae

Amoebae are structurally simple protozoans which have no fixed shape. The cytoplasm of amoeba is bounded by a membrane and can be differentiated into an outer ectoplasm and inner endoplasm. Pseudopodia (false foot) are formed by the amoebae by throwing out ectoplasm followed by endoplasm. These are employed for locomotion and engulfment of food by phagocytosis.

Reproduction occurs by fission and budding. Amoebae are classified as either free living or intestinal amoebae.

Coordination Compounds Class 12 Notes Chemistry Chapter 9

By going through these CBSE Class 12 Chemistry Notes Chapter 9 Coordination Compounds, students can recall all the concepts quickly.

Coordination Compounds Notes Class 12 Chemistry Chapter 9

Coordination Compounds or complex compounds are usually formed by the transition metals ¡n which the metal atoms or ions are bound to a number of anions or neutral molecules Chlorophyll, haemoglobin and vitamin B12 are coordination compounds of magnesium, iron and cobalt respectively.

Wernet’s Theory of Coordination Compounds:
Alfred Werner, a Swiss chemist proposed the concept of a primary valence and a secondary valence for a metal ion. Werner in 1998 propounded his theory of coordination compounds.

The main postulates are:

  1. In coordination compounds metals show two types of linkages (valences) primary and secondary.
  2. The primary valences are normally ionisable and are satisfied by negative ions.
  3. The secondary valences are non-ionizable. These are satisfied by neutral molecules or negative ions. The secondary valence is equal to the coordination number and is fixed for a metal.
  4. The ion.s/groups bound by the secondary linkages to the metal have characteristic spatial arrangements corresponding to different numbers.

Such spatial arrangement is called coordination polyhedra. The species within the square bracket are coordination entities or complex part and the ions outside the coordination entities or complex part are called counter ions.

Werner further postulated that octahedral, tetrahedral, and square planar geometrical shapes are more common in coordination compounds of transition metal.

[CO(NH3)6]3+, [Cr(H2O)6]3+, [Cr Cl (NH3)5]2+, [COCl2(NH3)4]+ are octahedral complexes [NiCO)4] and [PtCl4]2- are tetrahedral and square planar respectively.

Difference between a double salt and a complex: Both double salts, as well as coordination compounds, are formed by the combination of two or more stable compounds in a stoichiometric ratio.

  1. KCl + MgCl2 + 6 H2O → KCl. MgCl2. 6H20 (carnallite)
  2. FeSO4 + (NH4)2SO4 + 6 H2O → FeSO4. (NH4)2 SO4. 6H2O (Mohr’s salt)
  3. 4 KCN + Fe (CN)2 → K4[Fe(CN)6]
  4. CoCl3 + 6 NH3 → [Co(NH3)6]Cl3

1 and 2 are examples of double salts
3 and 4 are examples of coordination compounds.

Double salts lose their identity in aqueous solutions. They dissociate into simple ions completely when dissolved in water.

Coordinate complexes retain their identity both in the solid-state and in aqueous solutions. For example [Fe (CN)6]4- does not dissociate into Fe2+ and CN ions.

→ Coordination Sphere: The central atom/ion and the ligands attached to it are enclosed in a square bracket is collectively called the Coordination sphere. For example in K4[Fe (CN)6], [Fe(CN)6]4- is coordination sphere and ionisable group K+ written outside the coordination group is called Counterion.

→ Coordination Polyhedron: The spatial arrangement of the ligand atoms which are directly attached to the central atom/ion defines polyhedron about the central atom/ion [Co(NH3)6]3+, [Ni (CO)4] and [Pt Cl]2- are respectively octahedral, tetrahedral and square planar coordination polyhedra.
Coordination Compounds Class 12 Notes Chemistry 1
(Shapes of different coordination polyhedra. M = Central metal/ ion and L = a unidentate ligand)

→ Oxidation Number of Central Atom: The oxidation number of the central atom in a complex is defined as the charge it would carry if all the ligands are removed along with the electron pairs that are shared with the central atom. Oxidation no. of copper in [Cu (CN)4]3- is + 1 and it is written as Cu (I).

→ Coordination Entity/Complexion: A coordination entity constitutes a central metal atom or ion bonded to a fixed number of ions or molecules. For example, [CoCl (NH3)3] is a coordination entity in which the cobalt ion is surrounded by three ammonia molecules and three chloride ions. Other examples are [Ni (CO)4], [PtCl, (NH3)2], [Fe (CN)6]3-, [CO(NH3)6]3+.

→ Central atom/ion: In a coordination entity, the atom/ion to which a fixed number of ions/ groups are bound in a definite geometrical arrangement around it, is called the central atom or ion. For example, the central atom/ion in the coordination entities: [NiCl2 (H2O)4], [COCl(NH3)5]2+, [Fe(CN)6]3- are Ni2+, CO3+ and Fe3+, respectively. These central atoms/ions are also referred to as Lewis acids.

→ Ligands: The ions or molecules bound to the central atom/ion in the coordination entity are called ligands. These may be simple ions such as Cl, small molecules such as H2O or NH3, larger molecules such as H2NCH2CH2NH2 or N (CH2 CH2 NH2)3 or even macromolecules, such as proteins. When a ligand is bound to a metal ion through a single donor atom, as with Cl, H2O or NH3, the ligand is said to be unidentate.

When a ligand can bind itself through two donor atoms as in H2NCH2CH2NH2 (ethane-1,2-diamine) or C2O42- (oxalate), the ligand is said to be bidentate, and when several donor atoms are present in a single ligand as in N (CH2CH2NH2)3, the ligand is said to be polydentate. Ethylenediaminetetracetate ion (EDTA4-) is an important hexadentate ligand. It can bind through two nitrogen and four oxygen atoms to a central metal ion.
Coordination Compounds Class 12 Notes Chemistry 2
When a di- or polydentate ligand uses its two or more donor atoms to bind a single metal ion, it is said to be a chelate ligand. The number of such ligating groups is called the denticity of the ligand. Such complexes,
called chelate complexes tend to be more stable than similar complexes containing unidentate ligands. The ligand, which can ligate through two different atoms is called ambidentate ligand. Examples of such ligands are the NO2 and SCN ions. NO2 ion can coordinate either through v nitrogen or through oxygen to a central metal atom/ion
Coordination Compounds Class 12 Notes Chemistry 3
→ Coordination Number: The coordination number (CN) of a metal ion in a complex can be defined as the number of ligand donor atoms to which the metal.is directly bonded. For example, in the complexions, [PtCl6]2+ and [Ni(NH3)4]2+ the coordination number of Pt and Ni are 6 and 4 respectively. Similarly, in the complexions, [Fe(C2O4)3]2- and [Co(en)3]3+, the coordination number of Fe and Co both is 6 because C2O42- and en (ethane-1, 2-diamine) are bidentate ligands.

It is important to note here that the coordination number of the central atom/ ion is determined only by the number of sigma bonds formed by the ligand with the central atom/ion. Pi bonds, if formed between the ligand and the central atom/ion, are not counted for this purpose.

Homoleptic and Heteroleptic Complexes [Co(NH3)6]3+ in which metal is bound to only one kind of donor group, i.e., NH3 is called homoleptic complex. [Co(NH3)4 Cl2]+ complex in which a metal is bound to more than one kind of donor groups is called heteroleptic complex.

→ Nomenclature of Coordination Compounds: The formulae and names for coordination entities are based on the recommendations of the International Union of Pure and Applied Chemistry (IUPAC).

Formulae of Mononuclear Coordination Entities:
The following rules are applied while writing the formulae:

  1. The central atom is listed first.
  2. The ligands are then listed in alphabetical order. The placement of ligand in the list does not depend upon its charge.
  3. Polydentate ligands are also listed alphabetically. In the case of abbreviated ligand. The first letter of the abbreviation is used to determine the position of the ligand in alphabetical order.
  4. The formula for the entire coordination entity, whether charged or not, is enclosed in square brackets. When ligands are polyatomic, their formulae are enclosed in square brackets. When ligands are polyatomic their formulae are enclosed in parenthesis. Ligand abbreviations are also enclosed in parenthesis.
  5. There should be no space between the names of the ligands and the metal within a coordination sphere.
  6. When the formula of a charged coordination entity is to be written without that of the counter ion, the charge is indicated outside the square brackets as a right superscript with the number before the sign. For example, [Co(CN)6]3-, [Cr (H2O)6]3+ etc.
  7. The charge of the cations is balanced by the charge of the anions.

Note: The 2004 IUPAC draft recommends that ligands will be sorted alphabetically, irrespective of the charge.

The naming of Mononuclear Coordination Compounds Rules:

  1. The cation is named first.
  2. The ligands are named in alphabetical order before the name of the central atom/ion.
  3. Names of the anionic ligands end in – O. No special ending for neutral ligands .and cationic ligands. Aqua for H20, amine for NH3, carboxyl for CO and nitrosyl for NO, cyano for CN, Oxo for O2-.
  4. Prefixes mono, di, tri etc. are used to indicate the number of individual ligands in the coordination entity. When the names of the ligands include a number, then the terms bis, tris takes are used, the ligand to which they refer is placed in parenthesis. For example, [NiCl2 (P Ph3)] is named as dichloro bis (triphenylphosphine) nickel (II).
  5. The oxidation number/state of the metal in cation, anion or neutral coordination entity is indicated by a Roman numeral in parenthesis.
  6. If the complexion is an anion, the name of the metal ends with -ate. For example Cr in [Cr(CN)6]3- is chromate,
  7. The neutral complex molecule is named the same as that of the complex cation.

Note: The 2004IUPAC draft recommends that anionic ligands will end with – ido so that chloro would become chloride, etc.

Examples:

  1. Cr [(NH3)3 (H2O)3]Cl3: triamine tri aqua chromium (III) chloride.
  2. [Co (H2N CH2CH2NH2)3]2 (SO4)3: tris (ethane -1,2 di-ammine) Cobalt (III) sulphate.
  3. [Cr(H2O)6] Cl3: Hexaaquachromium (111) chloride.
  4. [Ag(NH3)2] [Ag(CN)2]: diammine silver (I) dicyano argentate (I).

→ Isomerism in Coordination Compounds: Isomers are two or more compounds that have the same chemical formula, but different arrangements of atoms.
1. Stereoisomerism:
(a) Geometrical isomerism,
(b) Optical isomerism.

2. Structural Isomerism:
(a) Linkage isomerism,
(b) Coordination isomerism,
(c) Ionisation isomerism,
(d) Solvate isomerism.

Stereoisomers have the same chemical formula and chemical bonds but they have different special arrangements. Structural isomers have different bonds.

→ Geometrical Isomerism: It arises in heteroleptic complexes due to different possible geometric arrangements of the ligands. If in square planar complex [MX2L2], the two ligands X are on the same side and two ligands L are on the other, it is called CIS-isomer. If the two ligands X and L are opposite to each other, it is called a Trans-Isomer.
Coordination Compounds Class 12 Notes Chemistry 4
Example: [Pt (NH3)2 Cl2]: diammine dichloroplatinum (II)

Octahedral complexes [CO(NH3)4Cl2]+ and [Co{en)2Cl2]+ exist as cis and trans isomers.
Coordination Compounds Class 12 Notes Chemistry 5
2. Optical isomerism: The isomers which rotate the plane polarised light equally but in opposite directions are called optical isomers. The isomer which rotates the plane polarised light to right is called dextrorotatory (designated as d-) while the one which rotates the plane of polarised light to the left is called laevorotatory (designated as 1). The main requirement for optical activity is that the molecule/ion should not have a plane of symmetry.

For example, complexes such as [Co(en)3]3+ and [Cr(ox)3]3- exist as optical isomers.
Coordination Compounds Class 12 Notes Chemistry 6
Another example of the optical isomers is shown by the complex [Co(en)2 Cl2]+.
Coordination Compounds Class 12 Notes Chemistry 7
2. Structural Isomerism: They are further divided into:
1. Linkage Isomerism: It arises in a coordination compound containing ambidentate ligand. The complex [CO(NH3)5(NO2)]Cl2 exists in two forms: the red form in which the nitrite ligand is bound through oxygen (- ONO) and the yellow form in which nitrate is bound through nitrogen (-NO2). ,

2. Coordination Isomerism: It arises due to the interchange of ligands between cationic and anionic entities of different metal ions present in a complex. For example
[CO(NH3)6] [Cr (CN)6] and [Cr (NH3)6] [CO(CN)6]

3. Ionisation Isomerism: This isomerism arises when the counter ion m a complex salt is itself a potential ligand and can displace a ligand which can then become the counter ion.
(a) [CO(NH3)4O2]NO2 gives NO2 ions in solution and [CO(NH3)4 Cl(NO2)]Cl which gives Cl ions in solution.

(b) [CO(NH3)5 SO4] Br which gives a ppt. with AgNO3 [of AgBr] and [Co (NH3)Br[ SO4 which gives ppt. with Bad2 solution.

4. Solvate or Hydrate Isomerism: It is similar to ionisation isomerism with the only difference that water (H2O) is involved as a \ solvent. For example aqua complex Cr[(H2O)6]Cl3 – violet and its solvate isomer [Cr(H2O)5 Cl] Cl2. H2O – grey-green.

Bonding in Coordination Compounds:
There are two theories,
1. Valence Bond Theory for Bonding in Coordination Compounds: This theory was developed by Linus Pauling in 1930.
The basic assumptions of the theory are:
(a) The central metal atom in the complex must make available a number of empty orbitals equal to its coordination number for accommodating the electrons from ligands.
(b) The appropriate atomic orbitals (s, p, d) of the metal hybridise to give a new set of equivalent hybrid orbitals which are directed towards the ligand sites.
(c) The d orbitals used for hybridization may be either inner (n – 1)d orbitals or outer nd orbitals.
(d) The hybrid orbitals of the metal overlap with the filled orbitals of\the ligands to form coordinate bonds.

Thus, With the help of V.B. theory, the geometry of the complex can be predicted if the number of unpaired electrons is known. Alternatively, the number of unpaired electrons can be predicted from the known geometry of the complex.

The common types of geometries and hybrid orbitals used are:
Coordination Compounds Class 12 Notes Chemistry 8
The theory may be illustrated by two important examples:
1. [CO(NH3)6]3+ and [COF6]3-. In these complexes, Co (III) has six d- electrons. The first complexion is diamagnetic and the second has paramagnetic character due to four unpaired electrons. In the [CO(NH3)6]3+ complex, the two 3d electrons get paired up with the other two leaving two vacant orbitals and these vacant orbitals get d2sp3 hybridized. In the second [COF6]3- complexes, the 3d electrons are not disturbed and the outer 4d orbitals are used for hybridization.
Coordination Compounds Class 12 Notes Chemistry 9
Coordination Compounds Class 12 Notes Chemistry 10
[CO(NH3)6]3+ is called an inner orbital or low spin or spin paired complex. The paramagnetic octahedral complex [COF6]3- is failed outer orbital or high spin or spin-free complex.

In a tetrahedral complex one s and three p-orbitals are hybridized to form four equivalent orbitals oriented tetrahedrally, e.g., [Ni Cl4]2-.
Coordination Compounds Class 12 Notes Chemistry 11
It is paramagnetic. (High spin complex).

In the square planar complexes, the hybridisation involved is dsp2. An example is [Ni(CN)4]2-. Here nickel is in a + 2 oxidation state and has the electronic configuration 3d8.
Coordination Compounds Class 12 Notes Chemistry 12
It is a diamagnetic complex.

Magnetic properties of Coordination Compounds: For metal ions with up to three electrons in the d-orbitals like Ti3+ (d); V3+ (d2); Cr3+ (d3) two vacant d orbitals are available for octahedral hybridisation with 4s and 4p orbitals. The magnetic behaviour of these free ions and complex is similar.

When more than three 3d electrons are present, the required pair of 3d orbitals for octahedral hybridisation is not directly available (as a consequence of Hund’s rule). Thus, for d4 (Cr2+, Mn3+), d5 (Mn2+, Fe3+), d6 (Fe2+, CO3+) cases, a vacant pair of d orbitals results only by the pairing of 3d electrons which leaves two, one and zero unpaired electrons respectively.

The magnetic data agree with maximum spin pairing in many cases, especially with coordination compounds containing d6 ions. However, with species containing d4 and d5 ions, there are complications. [Mn (CN)6]3- has a magnetic moment of two unpaired electrons while [MnCl6]3- has a paramagnetic moment of four unpaired electrons. [Fe(CN)6]3- has a magnetic moment of a single unpaired electron while [FeF6]3- has a paramagnetic moment of five unpaired electrons. [COF6]3- is paramagnetic with four unpaired electrons while [Co(C2O4)3]3- is diamagnetic.

This apparent anomaly is explained by valence bond theory in terms of the formation of inner orbital and outer orbital coordination entities. [Mn(CN)6]3-, [Fe(CN)6]3- and [Co(C2O4)3]3- are inner orbital complexes involving d2 sp3 hybridisation, the former two complexes are paramagnetic and the latter diamagnetic. On the other hand, [MnCl]3-/ [FeF6]3- and [COF6]3- are outer orbital complexes involving sp3d2 hybridisation and are paramagnetic corresponding to four, five and four unpaired electrons.

Limitations of Valence Bond Theory:

  1. It involves a no. of assumptions.
  2. It does not give a quantitative interpretation of magnetic data.
  3. It does not explain the colour shown by coordination compounds.
  4. It does not explain the thermodynamic or kinetic stabilities of co-ordinate compounds.
  5. It does not make exact predictions regarding the tetrahedral and square planar structures of 4-coordination complexes.
  6. It does not distinguish between weak and strong ligands.

2. Crystal Field Theory: This theory envisages the metal ligand to be purely ionic arising.from electrostatic interactions between the metal and ligand. Ligands are treated as point charges in case of anions or dipoles in case of neutral molecules. The five d orbitals in an isolated gaseous metal atom/ion have the same energy, i.e., they are degenerate.

On the arrival of the ligands, these d-orbitals split up. Those orbitals which lie on the direct path of the ligands are repelled more than those which lie away from the path of approaching ligands. This pattern of splitting depends upon the nature of the crystal field.

A. Crystal Field splitting into Octahedral Coordination Entities: In an octahedral complex when the six ligands approach the metal atom/ ion, out of five d-degenerate orbitals, three-d orbitals (dxy, dyz, dzx) which lie away from the path of the approaching ligands (∵ they lie in between the axes) are repelled less than those two d-orbitals (dx2y2 and dz2) which lie on the direct path [they lie in between the axes].

Thus the degeneracy of the five d-orbitals are lost and these d-orbitals split up. This splitting gives two sets of orbitals -12 set of three orbitals of lower energy and eg set of two orbitals (dx2y2 and dz2) of higher energy. It is called Crystal Field Splitting and the difference of energy is denoted by Δ0 (o -for octahedral complex). The energy of two eg orbitals is raised by \(\frac{3}{5}\) Δ0 and that of the three t2g will decrease by \(\frac{2}{5}\) Δ0.

The crystal field splitting, Δ0, depends upon the field strength of the ligands which is in the order:
I < Br < SCN < Cl < S2- < F < OH < C2O42- < H2O < NCS < edta4- < NH3 < en < CN < CO such a series is called spectrochemical series.

In d1 complexes, the single d-electron occupies the lower t2g orbital. In d2 and d3 coordination entities, the d-electrons occupy the three t2g orbitals singly in keeping with Hund’s Rule.

For d4 ions, two different patterns are possible:

  1. the 4th electron could either enter the lower energy t2g level and pair with an existing electron, or
  2. it could occupy the higher energy e2g level. It depends upon two factors:
    (a) The magnitude of crystal field splitting energy Δ0.
    (b) The pairing energy P [energy required for electron pairing in a single orbital).

1. If Δ0 < P, the 4th electron enters one of the eg orbitals. Ligands for which Δ0 < P is known as Weak field ligands and form high spin complexes.
Coordination Compounds Class 12 Notes Chemistry 13
Crystal Field Splitting of d-orbitals in an Octahedral complex

2. If Δ0 > P, the 4th electron occupies a lower energy t2g orbital. Ligands producing this effect are known as strong field ligands and form low spin complexes.

Calculations show that d4 to d7 coordination entities are more stable for the strong field as compared to weak field cases.

B. Crystal Field Splitting into Tetrahedral Coordination Entities: In tetrahedral complexes, splitting of d-orbitals is such that it is opposite to that of octahedral complexes. The eg set of d-orbitals of the metal ion is lower in energy and the t2g set has higher energy. Moreover, the value of Δt [t for tetrahedral complex] is smaller than Δ0 (Δt = \(\frac{4}{9}\) Δ0) for the same ligands and metal-ligand distances. Consequently, the orbital splitting energies are not sufficiently large for forcing pairing of electrons, i.e., electrons prefer to remain unpaired and thus low spin complexes are rarely observed in tetrahedral complexes.
Coordination Compounds Class 12 Notes Chemistry 14
d-orbitals splitting in tetrahedral crystal field

Colour in Coordination Compounds: Formation of coloured complexes is .the characteristic property of transition elements. It can be explained readily on the basis of crystal field theory, taking an example of an octahedral complex of [Ti (H2O)6]3+ in which the metal ion Ti3+ is a 3d1 system.

The t2g set is lower in energy and the eg set is higher in energy. The rotary 3d1 electron prefers to remain in t2g set in the ground state. If the light corresponding to a yellow-green region of white light is absorbed by this complex, it will excite the electron from the t2g set to the next available eg
set[t2g eg° → t°2g eg1 ]. Thus the complex appears violet.
Coordination Compounds Class 12 Notes Chemistry 15
The transition of an electron in [Ti(H2O)6]3+ complex

The colour of the complexes is explained by crystal field theory due to the d-d transition of the electron. Removal of the ligands does not cause crystal field splitting and hence the complex becomes colourless,
e.g., where CuSO4.5H20 [Complex: [Cu (H2O)4]2+. SO42-. H2O] is blue in colour due to absorption of the red region of white light, anhydrous CuSO4 s white. Removal of water from [Ti(H2O)6]Cl3 on heating renders it colourless.

The influence of the ligand on the colour of a complex may be illustrated by considering the [Ni (H2O)6]2+ complex, which forms when nickel (II) chloride is dissolved in water. If the identity ligand, ethane- 1, 2-diamine (en) is progressively added in the molar ratios en: Ni, 1:1, 2:1,3:1 the following series of reactions with associated colour changes occur.
Coordination Compounds Class 12 Notes Chemistry 16
Limitations of Crystal Field Theory:

  1. As ligands are assumed to be point charges, anionic ligands are expected to have a greater splitting effect. However, actually, they are found to be at the lower end of the spectrochemical series.
  2. It does not take into account the covalent character of bonding between the ligand and the central atom/ion.
  3. Though OH ion in the spectrochemical series lies below H2O and NH3, yet it produces a greater splitting effect.

→ Bonding in Metal Carbonyls: The homoleptic carbonyls (compounds containing carbonyl ligands only) are formed by most of the transition metals. Tetracarbonylnickel (o), viz., [Ni (CO)4] is tetrahedral, Penta carbonyl iron (o) is trigonal bipyramidal while Hexa carbonyl chromium (o) is octahedral.
Coordination Compounds Class 12 Notes Chemistry 17
Stability of Coordination Compounds: Consider the reaction
M + 4 L → ML4
Stability constant (on Equilibrium constant)
K = \(\frac{\left[\mathrm{ML}_{4}\right]}{\left[\mathrm{M} \mid[\mathrm{L}]^{4}\right.}\)

The numerical value of the stability constant is a measure of the stability of the complex in the solution.

Importance And Applications of Coordination Compounds: These compounds are widely present in the mineral, plant and animal world. They play important functions in analytical chemistry, metallurgy, biological systems, industry and medicine.
1. Hardness of water is estimated by simple titration with Na2 EDTA. The Ca2+ and Mg2+ ions present in hard water make stable complexes with EDTA.

2. Metallurgical extraction of silver and gold make use of complex formations. Gold can be extracted from [Au (CN)2] complex by the addition of zinc.

3. Purification of Nickel can be achieved by Mond’s process by converting impure nickel to complex [Ni (CO)4] which decomposes to yield pure nickel.

4. Chlorophyll, the green pigment present in plants responsible for photosynthesis, is a coordination compound of Magnesium. Haemoglobin, the red blood pigment of blood that acts as an oxygen carrier is a coordination compound of iron. Vitamin B12, Cyanocobalamin, the anti-pernicious anaemia factor, is a cord in. m compound of cobalt.

5. Coordination comp us are used as catalysts for many industrial processes. Rhodium complex [(Ph3P) RhCl]. a Wilkinson catalyst is used for the hydrogenation of alkenes.

6. Articles can be electroplated with silver and gold much more smoothly and evenly from a solution of complexes Ag (CN)2] and [Au (CN)2] than from a solution of simple metal ions.

7. In black and white photography, the developed film is fixed by washing with hypo solution which dissolves the under-composed AgBr to form a complex io,n [ Ag (S2O3)2]3-.

8. Cis-platin is used for the treatment of cancer. Excess of copper and iron are removed by the chelating ligands D-penicillamine and desferrioxamine B via the formation of coordination compounds. EDTA is used in the treatment of lead poisoning

The d-and f-Block Elements Class 12 Notes Chemistry Chapter 8

By going through these CBSE Class 12 Chemistry Notes Chapter 8 The d-and f-Block Elements, students can recall all the concepts quickly.

The d-and f-Block Elements Notes Class 12 Chemistry Chapter 8

Transition Elements: d-Block. elements are called transition elements. They are placed in between the s-block on their left and the p-block on their right. They are called transition elements because they have properties intermediate between those of s- and p-block elements and represent a change from the most electropositive s-block elements to the least electropositive elements.

This element has partly filled (n -1) d-subshell in their atomic or ionic state. They are called d-block elements since in them 3d, 4d, 5d and 6d subshells are incomplete and the last electron enters (n -1) d subshell, i.e., penultimate (last but one) shell.

General Electronic Configuration:
The outermost shell: Their general electronic configuration is (n – 1) d1-10 ns0-2 where n is the outermost shell. Filling of 3d, 4d, 5d and 6d subshells leads to first transition series [4th period], 2nd transition series [5th period], 3rd transition series [6th period] and 4th incomplete transition series [7th period] respectively.

1st Transition Series or 3d series: Starts from Sc (At. No. 21) and ends at Zinc (Zn; atomic no. = 30).

Their configuration is 3d1-10 ns1-2.

  • Scandium (Sc) = 21 = [Ar]18 3d1 4s2.
  • Titanium (Ti) = 22 = [Ar]18 3d2 4s2
  • Vanadium (V). = 23 = [Ar]18 3d3 4s2
  • Chromium (Cr) = 24 = [ Ar]18 3d5 4s1
  • Manganese (Mn) = 25 = [Ar]18 3d6 4s2
  • Iron (Fe) = 26 = [Ar]18 3d6 4s2
  • Cobalt (Co) = 27 = [Ar]18 3d7 4s2
  • Nickel (Ni) = 28 = [Ar]18 3d8 4s2
  • Copper (Cu) = 29 = [Ar]18 3d10 4s1
  • Zinc (Zn) == 30 = [Ar]18 3d10 4s2

It may be noted that the electronic configuration of chromium and copper given above are exceptional. They have a single electron in the 4s-orbital. It is due to the extra-stability of 3d5 and 3d10 (half-filled and completely filled) orbitals. They consist up of 10 elements.

2nd Transition Series or 4d Series: Starts from the element Ytterium (Y) [Z = 39] and ends of cadmium (Cd; Z = 46). Their electronic configuration is 4d0-10 5s1-2. Palladium (Pd; Z = 46) has exceptional configuration of 4d10 5s°. They consists up of ten elements.
The d-and f-Block Elements Class 12 Notes Chemistry 1
Third Transition Series or 5d series: Corresponds to filling of 5d sub-level. They consist up of ten elements La (Z = 57), H/(Z = 72), Ta, W, Re, Os, Ir, Pt, Au and Hg(Z = 80).

The electronic configuration of 3rd transition elements in the inner and valence shell is given below:
The d-and f-Block Elements Class 12 Notes Chemistry 2
Fourth Transition Series or 6d Series: Corresponds to tire filling up of 6d Sub level and starts with Actinium (Ac; Z = 89), Rf (earlier Ku, Z = 104), Db, Sg, Bh, Hs, Mt, Ds, Rg and ends at Uub (Z = 112).
The d-and f-Block Elements Class 12 Notes Chemistry 3
The fundamental difference in the electronic configuration of Representative Elements and Transition Elements: In the representative elements (s- and p-block elements), the valence electrons are present only in the outermost shell while in the transition elements, the valence electrons are present in the outermost shell as well as d- orbitals of the penultimate shell.

Zinc (Zn), Cadmium (Cd) and mercury (Hg) are misfits according to the definition of transition elements as they have 3d10, 4d10, 5d10 (completely filled inner d-orbitals) in the ground state of their atoms or in one of the common oxidation states (dipositive ions: Zn2+, Cd2+, Hg2+) respectively. They do not show properties of transition elements to any appreciable extent, except for their ability to form complexes.

The d-block of the periodic table contains the elements of Groups 3-12 in which the d-orbitals progressively filled in each of the four long periods.

General Properties of Transition Elements:
(a) Metallic character: All the elements of d block are metals. This is due to the fact that they have low ionisation energy values and have only one dr two s-electrons in the outermost shell. The transition elements exhibit good mechanical properties i.e., they are hard, malleable and ductile. Except for Zn, Cd and Hg, they have high m. and b.pts. They have thermal and electrical conductivity and metallic lustre.

(b) Variable oxidation states: The transition elements exhibit a variety of oxidation states in their compounds. This is due to the fact that (n -1) d orbitals are of comparable energy to ns orbitals and therefore some or all of the (n -1) d electrons can be used along with ns electrons in compounds formation. Some common oxidation states exhibited by elements of the first transition series are listed below:
The d-and f-Block Elements Class 12 Notes Chemistry 4
(The value in parentheses are less common oxidation states.)

(c) Coloured compounds: Most of the compounds of transition elements are coloured. The d orbitals in transition metal compounds are not of equal energy. In transition elements, the d-orbital are partly filled and electron may be promoted from one d level to another d level by absorbing visible light. Consequently, the compound has the colour complement to the absorbed light. For example, Cu2 absorbs red light and transmitted light contains an excess of the other colours of the spectrum and appears to be blue.

The ions Zn2+, Cu+, Ti4+, Sc3+ are white because they have either completely empty or completely filled d-subshell.

(d) Magnetic properties: Most of the transition metals and their compounds are paramagnetic i.e., they are attracted by the magnetic field. This, the property is due to the presence of unpaired electrons in the d orbitals of their atoms. The elements like iron, nickel and cobalt have appreciable paramagnetism and are called ferromagnetic substances. The magnetic moment of compounds of d-block elements are determined by spin only values which may be related to the number of impaired electrons (n) as

Spin magnetic moment (μs) = \(\sqrt{n(n+2)}\)

The agreement between the observed and calculated values is quite good for most of the elements. However, for the latter half of the series, the contribution from orbital magnetic moments is observed.

(e) Complex formation: The transition elements have a great tendency to form complexes.

This is because of:

  • their small cation size
  • high effective nuclear charge and
  • presence of empty d-orbitals of appropriate energy for bonding to the ligands.

It has been noticed that

  1. In each transition series, the stability of complexes increases with an increasing atomic number of the element and in a particular oxidation state with decreasing size of its atoms.
  2. In the case of metal atoms that show more than one oxidation state, the complexes of greater stability are formed with the metal ions of the highest charge.

(f) Catalytic properties: Many transition metals and their compounds show catalytic properties e.g., Fe, Pt, V2O5, Ni etc. This property may be due to either the use of the d-orbitals or from the formation of transient intermediate compounds to absorb and activate the reacting substances.

(g) Alloy Formation: Transition metals mix freely with each other in the molten state and on cooling a solution of different transition metals to form alloys. For example, chromium dissolves in nickel to form Cr-Ni alloy; manganese dissolves in iron to form manganese steel. They take part in alloy formation because their atoms can exchange lattice sites of each other. Such alloys are formed by atoms with metallic radii that are within about 15 per cent of each other.

(h) Formation of Interstitial Compounds: Interstitial compounds are those which are formed when small atoms like H, C or N are trapped inside the crystal lattices of metals. They are usually non-stoichiometric and are neither typically ionic nor covalent. Many of the transition metals form interstitial compounds particularly with small non-metal atoms such as hydrogen, boron, carbon and nitrogen.

These small atoms enter into the voids sites between the packed atoms of the crystalline metal, e.g., TiC, Mn4N, Fe3M and TiH2 etc. The formulae quoted do not, of course, correspond to any normal oxidation state of the metal and often non-stoichiometric material is obtained with such composition as VH056 and TiH17. Because of the nature of their composition, these compounds are referred to as interstitial compounds.

The principal physical and chemical characteristics of these compounds are as follows:

  1. They have high melting points, higher than those of pure metals.
  2. They are very hard, some borides approach diamond in hardness.
  3. They retain metallic conductivity.
  4. They are chemically inert.

Some Important Compounds of Transition Metals:
Oxides: Transition metal oxides are formed by the action of oxygen with transition metals at high temperature. The general formulas of the oxides of transition metals are MO, M2O3, M3O4, MO2, M2O5 and MO3.

It has been observed that:

  • the oxides in which the metals are in a lower oxidation state are basic in nature.
  • the oxides in which the metal is in a higher oxidation state are acidic in nature.
  • the oxides in which the metal exhibits intermediate oxidation states are amphoteric.

For example, among the oxides of manganese, MnO is basic, Mn2O3, Mn3O4 and MnO2 are amphoteric while Mn2O7 is acidic.

Oxides Of 3d Metals:
The d-and f-Block Elements Class 12 Notes Chemistry 5
Chemical Reactivity and E° Values: Transition metals vary widely in their chemical reactivity. Many of them are sufficiently electropositive to dissolve in mineral acids, although a few are ‘noble’: that is, they are unaffected by simple acids.

The metals of the first series with the exception of copper are relatively more reactive and are oxidised by 1M H+, though the actual rate at which these metals react with oxidising agents like hydrogen ion (H+) is sometimes slow. For example, titanium and vanadium, in practice, are passive to dilute non-oxidising acids at room temperature. The Ee values for M2+/M indicate a decreasing tendency to form divalent cations across the series.

This general trend towards less negative Ee values is related to the increase in the sum of the first and second ionisation enthalpies. It is interesting to note that the Ee values for Mn, Ni, and Zn are more negative than expected from the general trend. Whereas the stabilities of half-filled d subshell (d5) in Mn2+ and completely filled d subshell (d10) in zinc are related to their Eθ values; for nickel, Eθ value is related to the highest negative enthalpy of hydration.

An examination of the Eθ values for the redox couple M3+/M2+ shows that Mn3+ and CO3+ ions are the strongest oxidising agents in aqueous solutions. The ions Ti2+, V2+ and Cr2+ are strong reducing agents and will liberate hydrogen from a dilute acid. e.g.
2 Cr2+(aq) + 2 H+(aq) → 2 Cr3+(aq) + H2(g)

Trends in Stability of Higher oxidation states as exhibited in the oxides and halides of 3d-Series:
The table below shows the stable halides of the 3d series of transition metals. The highest oxidation numbers are achieved in Ti tetrahalides, VF5 and CrF6. The +7 state for Mn is not represented but MnOF3 is known and beyond Mn, no metal has a trihalide except Fe and COF3.

The ability of F to stabilize the higher oxidation state is due to either higher lattice energy of the higher compound as in the case of COF3 or higher bond energy terms for the higher covalent compounds e.g. VF5 and CrF6.

Table: Formulae of halides of groups 4 to 12:
The d-and f-Block Elements Class 12 Notes Chemistry 6
Halides: Transition metals react with halogens at high temperature to form transition metal halides. The order of reactivity of halogens is F > Cl > Br > I. The halides of higher oxidation states are the fluorides because metals can be oxidised to higher oxidation states with only fluorine which is most reactive. Bonding in fluorides is mainly ionic. In chlorides, bromides and iodides, the ionic character decrease with the atomic mass of halogen.

The ability of O to stabilize the higher oxidation state is also demonstrated in the oxohalides. Although Vv is represented only by VF5, the oxohalides VOX3 are known where X = F, Cl or Br. Another feature of fluorides is their instability in the low oxidation states e.g., VX2 (X = Cl, Br or I) and the same applies to CuX. On the other hand, all Cu11 halides are known except the iodide, in this case, Cu2+ oxidises I to I2:
Cu2+ + 2I→ CuI(S) + \(\frac{1}{2}\) I2

However Cul is unstable in solution and undergoes disproportionation.
2Cu+ → Cu2+ + Cu

The stability of Cu2+ (aq) rather than Cu+ (aq) is due to the much more negative Ah d H ° of Cu2+ (aq) than Cu+ (aq), which more than compensates for the 2nd IE of Cu.

The highest oxidation number in the oxides (Table) coincides with the group number and is attained in Sc2O3, to Mn2O7. Beyond Group 7, no higher oxides of Fe above Fe2O3, are known, although ferrates (VI):(FeO4)2- are formed in alkaline media they readily decompose to Fe2O3 and O2. Besides the oxides, oxidations stabilise Vv as VO2+, Vlv VO2+ and TiIV as TiO2+.

The ability of O to stabilise these high oxidation states exceeds F in this regard. Thus the highest Mn fluoride is MnF4 whereas the highest oxide is Mn2O7. The ability of oxygen to form multiple bonds to metals explains its superiority. In the covalent oil Mn2O7, each Mn is tetrahedrally surrounded by O’s including an Mn-O-Mn bridge. The tetrahedral [MO4]n- ions are known for Vv, CrvI, Mnv, MnvI and MnvII.

Comparison of the First Row Transition Metals Through The d-EIectron Configuration:
In the d° configuration of the simple ions, only Sc3+ is known to have this configuration. This configuration then occurs for those metals in which the formal oxidation states equal the total no. of 3d and 4s electron. This is true for Ti (IV), V (V), Cr (VI) and Mn (VII).

→ The d1 Configuration: Except Vanadium (IV), all others with this configuration are either reducing or undergo disproportionation. For .example, disproportionation occurs for Cr (V) and Mn (VI)
3 CrO43- + 8H+ → 2 CrO4 + Cr3+ + 4 H2O
3 MnO42- + 4H+ → 2 MnO4 + MnO + 2H20

→ The d2 Configuration: This configuration ranges from Ti11 which is very strongly reducing, to FeVI which is very strongly oxidizing. Vanadium (III) is also reducing.

→ The d3 configuration is shown by Chromium (III). It is quite stable and takes part in complex formation.

→ The d4 Configuration: There are really no stable species with the configuration Cr (II) is strongly reducing. ,

→ The d5 Configuration: The two important species with this configuration are Mn2+ and Fe3+, the latter may, however, be reduced to Fe2+.

→ The d6 Configuration: Iron (II) and Cobalt (III) are important species with this configuration. Iron (II) is quite stable although a mild reducing agent and cobalt (III) are stable in the presence of strong complexing reagents.

→ The d7 Configuration: The species with this configuration is cobalt (II) which is stable in aqueous solutions but gets oxidized to form CO (III) complexes in the presence of strong ligands.

→ The d8 Configuration: Nickel (II) is the most important species with this species.

→ The d9 Configuration: This configuration is found in Cu2+ compounds. It is by far the most important in the chemistry of copper.

→ The d10 Configuration: The two species Cu+ and Zn2+ are important with this configuration. Whereas Copper (I) is easily oxidized to copper (II), zinc (II) is the only state known for zinc.

General Group Trends in the Chemistry of the d-Block Metals:
Group 4:
The titanium group of transition metals consists up of the elements titanium, zirconium and hafnium. The most important member of this group is titanium. It is extremely strong, has a high melting point and is resistant to corrosion. It is in great demand as a structural material. Zirconium and hafnium are silvery-white metals. The most stable oxidation state for the elements of this group is +4.

The titanium also possesses a + 3 oxidation state. The typical compounds of these elements are chlorides, TiCl4, ZrCl4, HfCl4 and oxides TiO2, ZrO2 and HfO2, ZrO2 is a refractory material. Zirconium and hafnium occur together and exhibit similar properties.

Their atomic radii (Zr = 160 pm, Hf = 159 pm) are almost equal. This is due to the reason that usually increases in size down the group is cancelled by the lanthanide contraction. Zirconium and hafnium are both important for the generation of nuclear energy.

The vanadium group (Group 5): consists of vanadium, niobium and tantalum. The most stable oxidation state for this group is + 5. Vanadium is used as an additive to steel. The most important compound of vanadium is its pentoxide, V2O5, which is used as a catalyst in many reactions. Niobium alloys are used in jet engines, Tantalum is very resistant to corrosion and is used for making apparatus in chemical plants. It is also used in surgery, as for bone pins.

The chromium group (Group 6): contains the elements, chromium, molybdenum and tungsten. The most important oxidation states for chromium are + 3 and + 6, and for molybdenum and tungsten are + 5 and + 6. The zero oxidation states for these elements arise in metal carbonyls such as Cr (CO)6.

These elements have very high melting and boiling points. Tungsten is the metal with the highest melting point. These metals are also very hard. Chromium is unreactive or passive at low temperatures because of the formation of a surface coating of oxide. It is due to this passive behaviour that chromium is used for electroplating iron to prevent rusting.

The metals of this group are very useful. Chromium is used in many ferrous alloys such as stainless steel, chrome steel, etc. It is also used for electroplating iron or some other metals to prevent corrosion. K2Cr2O7 is a very important and useful compound of chromium.

Molybdenum and tungsten form very hard alloys with steel and are used in making cutting tools. Tungsten is also used as filament in electric bulbs. Molybdenum disulphide, MoS2 acts as a lubricant because it has a layer lattice.

Group 7: the manganese group: consist of the elements manganese, technetium and rhenium. These elements exhibit all the oxidation states from 0 to + 7, the most important being + 2, + 4 and + 7 for manganese and + 4 and + 7 for technetium and rhenium.

The elements of this group have quite a high melting and boiling points.

Manganese is obtained from its oxide ores by reduction with carbon or aluminium. Manganese metal does not have any use as such but is used in the manufacture of alloys such as ferromanganese (Fe + Mn) and manganese bronze (Mn + Cu + Zn). KMnO4 is an important compound of Mn which is used as an oxidizing agent and finds so many other applications. Manganese dioxide is used as a catalyst. Rhenium is used in electronic filaments, high-temperature thermocouples and in flashbulbs.

The metals of group 8,9 and 10 are known as iron group metals: These elements are:
The d-and f-Block Elements Class 12 Notes Chemistry 7
The first triad comprising of iron, cobalt and nickel is known as ferrous metals. These metals are ferromagnetic. Iron and cobalt exhibit oxidation states of + 3 and + 2 in their compounds while nickel compounds are generally in the + 2 oxidation state.

The elements of the second and third triad, ruthenium, rhodium, palladium, osmium, iridium and platinum are collectively known as platinum metals. These elements are relatively less abundant and exhibit a wider range of oxidation states. They are inert and serve as good catalysts.

The copper group (group 11): includes the elements copper, silver and gold. These metals are known as coinage metals. They form alloys with many metals. The most stable oxidation state for copper is + 2. For silver and gold, the oxidation state of + 1 is relatively more stable. The metals of this group have the highest electrical and thermal conductivities.

The zinc group (group 12): consists of the elements zinc, cadmium and mercury. The elements of this group show none of the characteristic properties of transition metals. The metals of this group are moderately electropositive and exhibit an oxidation state of + 2. Since their ionization energy is very high none of these metals possesses an oxidation state higher than + 2. Mercury, due to metal-metal bond also shows a formal oxidation state of +1. The elements of this group are diamagnetic. Mercury is the only metal that exists as a liquid.

Potassium Dichromate (K2Cr2O7):
Preparation: Chromite ore is fused with sodium or potassium carbonate in free access of air when the following reaction occurs.
The d-and f-Block Elements Class 12 Notes Chemistry 8
The yellow solution of sodium chromate (Na2CrO4) is filtered and acidified with a calculated amount of sulphuric acid from which orange sodium dichromate Na2Cr2O7. 2H2O can be crystallised.
2 Na2CrO4 + 2H+ → Na2Cr2O7 + 2Na+ + H2O

Potassium dichromate is prepared by treating the solution of sodium dichromate with a calculated amount of potassium chloride.
Na2Cr2O7 + 2 KCl → K2Cr2O7 + 2 NaCl.

Orange crystals of potassium dichromate crystallise out. The dichromate and chromate are interconvertible in an aqueous solution depending upon the pH of the solution.
2 CrO42- + 2 H+ → Cr2O72- + H2O.
Cr2O72- + 2 OH → 2 CrO42- + H2O.

The structures of chromate ionCrO42-, and dichromate ion, Cr2O72- and shown below. Whereas CrO42- is tetrahedral sharing one comer with Cr-O-Cr bond angle of 126°.
The d-and f-Block Elements Class 12 Notes Chemistry 9
In acidic solution, both sodium and potassium dichromates are strong oxidizing agents, the former has a greater solubility in water.
Cr2O72- + 14 H+ + 6e → 2 Cr3+ + 7 H2O [E° = 1.33 V]

→ Acidified solution oxidizes
1. iodides to iodine
6I → 3I2 + 6e

2. sulphides to sulphur
3 H2S → 6 H+ + 3 S + 6e

3. tin (II) to tin (IV)
3 Sn2+ → 3 Sn4+ + 6e

4. iron (II) salts to iron (III)
6 Fe2+ → 6 Fe3+ + 6e
The full ionic equation may be obtained by adding the two half-reactions. e.g.,
Cr2072- + 14 H+ + 6 Fe2+ → 2 Cr3+ + 6 Fe3+ + 7 H2O.

Potassium Permanganate, KMn04:
Preparation:
1. KMnO4 is prepared by fusion of MnO, and KOH with an oxidizing agent like KNO3.
The d-and f-Block Elements Class 12 Notes Chemistry 10
Potassium manganate (K2MnO4) gives KMnO4 in a neutral/acidic solution.
3 MnO42- + 4H) → 2 MnO4 + MnO2 + 2H2O

2. Comfnercially, KMnO4 is prepared from MnO2 by electrolytic oxidation.
The d-and f-Block Elements Class 12 Notes Chemistry 11
KMnO4 forms dark purple crystals. It is not very soluble in water. When heated it decomposes at 240°C.
The d-and f-Block Elements Class 12 Notes Chemistry 12
KMnO4 shows weak temperature-dependent paramagnetism. It arises due to the coupling of the diamagnetic ground state of MnO4 ion with paramagnetic excited states under the influence of the magnetic field.

The manganate and permanganate ions are tetrahedral. The green MnO42- is paramagnetic with one unpaired electron, but MnO4 is diamagnetic.
The d-and f-Block Elements Class 12 Notes Chemistry 13
Permanganic acid (HMnO4) can be obtained by low-temperature evaporation of its aqueous solution. It is a strong oxidizing agent and in a pure state, it is explosive above 0°C.

→ Acidified KMnO4 is a strong oxidizing agent:
MnO4 + e → MnO42-
[Reduction half reaction]; E° = + 0.56 V

MnO4 + 4H+ + 3e → MnO2 + 2H2O
[Reduction half reaction]; E° = + 1.69 V.

MnO4 + 8H+ + 5e → Mn2+ + 4 H2O
[Reduction half reaction]; E° = + 1.52 V.

A few important oxidizing reactions of KMnO4 are given below.
1. In acid solutions:
(a) Iodine is liberated from potassium iodide:
10I + 2MnO4 + 16H+ → 2Mn2+ + 8H20 + 5I2

(b) Fe2+ ion is converted to Fe3+:
5Fe2+ + MnO4 + 8H+ → Mn2+ + 4H2O + 5Fe3+
The green iron (II) solution changes to yellow iron (III) solution.

(c) Oxalate ion or oxalic acid is oxidized at 60°C:
5 C2O42- + 2MnO4+ 16H+ → 2Mn2+ + 8H2O + 10CO2

(d) Hydrogen sulphide is oxidized, sulphur being precipitated:
H2S + 2H+ → + S2-
5S2- + 2MnO4 + 16H+ → 2Mn2+ + 8H2O + 5S

(e) Sulphurous acid or sulphite is oxidized to a sulphate or sulphuric acid:
5 SO32- + 2MnO4 + 6H+ → 2Mn2+ + 3H2O + 5SO42-

(f) Nitrite is oxidized to nitrate:
5NO2 + 2MnO4 + 6H+ → 2Mn2+ + 5NO3 + 3H2O

2. In neutral or faintly alkaline solution:
(a) A notable reaction is the oxidation of iodide to iodate:
2MnO4 + H2O + I → 2MnO2 + 2OH + IO3

(b) Thiosulphate: s oxidised almost quantitatively to sulphate, a trace of thionate being formed
8MnO4 + 3S2O32- + H2O → 8MnO2 + 6SO42- + 2OH

(c) Manganous salt is oxidised to MnOz; the presence of zinc sulphate or zinc oxide catalyses the oxidation:
2MnO4 + 3Mn2+ + 2H2O → 5MnO2 + 4H+

Note: Permanganate titrations in presence of hydrochloric acid are unsatisfactory since hydrochloric acid is oxidised to chlorine.

Uses: Besides its use in analytical chemistry, potassium permanganate is used as a favourite oxidant in preparative organic chemistry. Its uses for the bleaching of wool, cotton, silk and other textile fibres and for the decolourisation of oils are also dependent on its strong oxidising power.

→ The Inner Transition Elements (f-Block): It consists up of two series of elements.
1. Lanthanoids (58-71) which follow lanthanum (57) in the periodic table. are fourteen in number. Because La (57) closely resembles the lanthanoids, it is usually included in the study of lanthanoids and the general symbol Ln is often used.

2. Actinoids [the fourteen elements (90-103)] which follow actinium (89). A discussion of actinoids also includes actinium (Ac), besides the 14 elements.

In the case of lanthanoids, 4f orbitals/are filled up and in the case of actinoids, 5f orbitals are filled up. That is why they are called Inner Transition Elements as the last electron (also called differentiating electron) enters the antepenultimate energy level, ie.., (n – 2) f-orbitals: inner to the penultimate energy level and they form a transition series within the transition series (d-block elements)

Lanthanides or Landhanoids or Lanthanoness: In these elements, the last electron enters the 4f-orbitals and is also referred to as the first inner transition series. Earlier they were called rare earth.

Actinides or Actinoids or Actions: In these elements, the last electron enters one of the 5f-orbitals and is also required as the second inner transition series.

The study of lanthanoids is easier because they show only one stable oxidation state (+ 3). On the other hand, the chemistry of actinoids is much more complicated partly because they show a wide range of oxidation states and partly because they are radioactive.

→ Electronic Configuration: General E.C. of lanthanoids and actinoids is (n – 2) f1-14 (n – 1) d0-1 ns2. Thus they have three incomplete shells, viz., (n – 2), (n – 1) and nth. Their electronic config. is given below.
The d-and f-Block Elements Class 12 Notes Chemistry 14
Trends in Ionic Radii of Trivalent Lanthanoids

Table: Electronic configurations and radii of lanthanum and lanthanoids:
The d-and f-Block Elements Class 12 Notes Chemistry 15
Only electrons outside [Xe] core are indicated.

The overall decrease in atomic and ionic radii from lanthanum to lutetium (the lanthanoid contraction) is a unique feature in the tire chemistry of lanthanoids. It is due to the imperfect shielding of one 4f electron from another 4f electron due to the highly diffused shape of f-orbitals. With the increase in nuclear charge, there is a fairly regular decrease in their sizes.

The cumulative effect of the contraction of the lanthanoid series called lanthanoid contraction causes the radii of the third transition series to be very similar to those of the correspond ing members of the 2nd series. As a.result Zr (160 pm) and Hf (159 pm) have identical radii and so exist together.

Thus Zr and Hf face difficulty in their separation.
Colour and Paramagnetism: Many trivalent lanthanoids are coloured both in the solid-state and in aqueous solutions. It is due to the presence of f-electrons. Neither Lu3+ ion (f°) nor Lu3+ (f14) shows any colour. All others (having f1 to f13 arrangement) show colour. The lanthanoid ions other than f° (La3+, Ce4+) type and the f14 type (Yb2+, Lu3+) are all paramagnetic due to the presence of unpaired electrons. Paramagnetism is maximum in neodymium.

→ Ionisation Enthalpies: The IE1 and IE2 are around 600 kJ mol-1 and 1200 kJ moH comparable with those of calcium. The values of IE3 indicate that the exchange energy considerations impart a degree of stability to empty, half-filled and completely filled f-level (f°, f7, f14). It is evident from the abnormally low values of IE3 of lanthanum, gadolinium and lutetium.

→ Oxidation States: All the lanthanoids show a + 3 oxidation state which is most significant: Some of them show + 2 and + 4 oxidation states also as ions in solution or in solid compounds. This irregularity arises mainly from the extra stability of empty, half-filled or completely filled f-subshell. CeIV [16Rn-noble gas] is formed easily, but it is a strong oxidant reverting to the common oxidation state of + 3.
Ce4+ + e → Ce3+] Reduction half reaction
E° for the above is = + 1.74 V

If can oxidise water, but the reaction rate is slow. Pr, Nd, Tb and Dy also exhibit + 4 states in oxides MOr Eu2+ is formed by losing the two s-electrons (F). However, Eu2+ is a strong reducing agent changing to the common oxidation state + 3.
EU2+ → EU3+ + e

Similarly Yb2+ [f14] is a reductant. Tb (IV) [f7] is an oxidant.
Tb4+ + e- → Tb3+

Samarium also shows oxidation states of + 2 and + 3 like Eu.

Properties and Uses:
1. All the lanthanides are silvery-white soft metals and tarnish rapidly in the air. Hardness increases with increasing atomic number, Samarium is steel hard.

2. M.Pts are in the range of 1000 to 1200 K, but Sm melts at 1623 K

3. They have a metallic structure.

4. They are good conductor of heat and electricity.

5. In their chemical behaviour, lanthanoids are generally similar to calcium (Ca = 20), but with increasing atomic number, they behave more like aluminium.

6. Values for E° for the reduction half-reaction.
Ln3+ (aq) + 3e → Ln (s) are in the range of – 2.2 to – 2.4 V except for Ln = Eu, for which it is – 2.0 V,

7. The metals combine with hydrogen when heated gently.
2 Ln + 3 H2 → 2 Ln H3

8. When heated in carbon, carbides of the type Ln3C, Ln2C3 and LnC2 are formed.

9. They liberate H2 gas from dilute acids.
2 Ln + 6HCl (dil.) → 2 LnCl3 + 3H2I

10. They bum in halogens to form halides.
2 Ln + 3X2 → 2 LnX3

11. They form oxides and hydroxides of the type M2O3 and M (OH)3. They are basically like alkaline earth metal oxides and hydroxides. A summary of the chemical reactions of lanthanoids are given below:
The d-and f-Block Elements Class 12 Notes Chemistry 16
The best use of the lanthanoids is for the production of alloy steels for plates and pipes. A well-known alloy is Misch Metall which consists of a lanthanoid metal (~ 95%) and iron (~ 5%) and traces of S, C, Ca and Al. It is used to produce bullets, shell and lighter flint. Mixed oxides are used as catalysts in cracking. Some Ln oxides are used as phosphors in TV screens.

→ The Actinoids: The elements which follow actinium (89) in the periodic table are called actinoids [Starting from Th – 90 to Lr – 103.]

→ Actinoids are radioactive elements. Earlier members have relatively long half-lives and later ones from day to 3 minutes for Lr. This makes their study difficult.

→ Electronic Configuration: All the actinoids have a 7s2 electron configuration and variable occupancy of the 5f and 6d subshells. The irregularities in the electronic configuration of actinoids like those in lanthanoids are related to the stabilities of 5f°, 5f7 and 5f14. 5f orbitals participate in bonding to a greater extent.

→ Oxidation states: There is a greater range of oxidation states shown by actinoids due to the comparable energies of 5f, 6d and 7s levels.

The electronic configurations and oxidation states of actinoids are in the following tables.
The d-and f-Block Elements Class 12 Notes Chemistry 17
Table: Oxidation states of actinium and actinoids:
The d-and f-Block Elements Class 12 Notes Chemistry 18
Unlike 4f orbitals of lanthanoids which are buried, 5f orbitals of actinoids participate in bonding to a far greater extent. In addition to showing an oxidation state of + 3 like lanthanoids, actinoids also show oxidation states of + 4, + 5, + 6 and + 7. Actinoids which show several oxidation states [Np, Pu, Am] make it difficult to review their chemistry.

Physical and Chemical reactivity of actinoids

  • Actinoids are all silvery-white metals.
  • They are highly reactive metals, especially when finely divided.
  • Boiling water reacts with them to give a mixture of oxides, hydrides.

Some applications of d-Block elements

  1. Iron and Steel are the most important construction materials.
  2. Compounds like TiO are prepared for use in the pigment industry.
  3. Mn02 is used in dry battery cells. The battery industry also requires Zn and Ni/Cd.
  4. Cu, Ag and Au are coinage metals.
  5. Many of the metals and their compounds find use as catalysts like finely divided Ni, V2O5, TiCl4, Fe etc.
  6. PdCl2 is used in the Wacker process for the oxidation of ethyne to ethanol
  7. Ni-complexes are used in the polymerisation of alkynes and other organic compounds like benzene.
  8. AgBr is used in the photographic industry.

An Overview of Leptospira Interrogans

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An Overview Leptospira Interrogans

Spirochaetes of the genus Leptospira are actively motile, delicate and possess numerous closely wound spirals with characteristic hooked ends. Several Leptospires are saprophytes, while many are potential pathogens of rodents, domestic animals and humans. The genus Leptospira consists of two important
species, which are Leptospira interrogans and Leptospira biflexa.

Leptospira interrrogans is the causative agent of leptospirosis, a zoonotic disease. The word Leptospira is derived from Latin word ‘Leptos’ = fine or thin and ‘spira’ = Coil and interrogans = Question mark (The shape of this spirochete accounts for its name)

Morphology

  • They are spiral bacteria (5-20µm × 0.1µm) with numerous closely set coils. Their ends are hooked and resemble umbrella handles.
  • They are actively motile by rotatory movements. They cannot be seen under light microscope due to its thinness, best observed by dark fieldmicroscopy (Figure 7.24), phase contrast and electron microscope.
  • They stain poorly with aniline dyes, it may be stained with giemsa stain or silver impregnation techniques.

Leptospira Interrogans img 1

Antigenic Structure

Leptospires show considerable antigenic cross reaction.

  1. Genus – Specific somatic antigen – It is present in all members of the genus.
  2. Surface antigens – This antigen is used to classify Leptospira into serogroups and serotypes.

Pathogenicity

Source of infection:

Contaminated water

Route of entry:

Through cuts or abrasions on skin or mucosa

Incubation period:

6-8 days

  • Leptospira interrogans causes a zoonotic disease named Leptospirosis. It is transmitted to humans by direct or indirect contact with water, contaminated by urine of carrier animals (rat and dog).
  • Leptospira enter the body through cuts or abrasions on skin or through mucous membranes of the mouth, nose or conjunctiva.
  • After an incubation period of 6-8 days. There is onset of febrile (related to fever) illness with Leptospira in blood (Septicemic phase) which lasts for 3-7 days.
  • The organisms disappear from the blood and invades liver, kidney, spleen, meninges producing meningeal irritation such as headache, vomiting.
  • The pathogen persists in the internal organs and most abundantly in the kidney. Severe Leptospirosis (Weil’s disease) is associated with Fever, conjunctivitis (inflammation of conjunctiva), albuminuria (presence of albumin in the urine), jaundice and hemorrhage. It is a fatal illness with hepatorenal (Kidney failure with severe liver damage).

Clinical manifestations

  • In severe cases, vomiting, headache, irregular fever and intense infection of the eyes.
  • Jaundice, Albuminuria (The presence of protein Albumin in the urine) and purpuric hemorrhages sometimes occur on skin and mucosa.

Laboratory Diagnosis

The diagnosis of Leptospirosis is made by the following ways

  • Direct microscopy of blood or urine
  • Isolation of pathogen by culture
  • Serological tests.

Direct Microscopy

Blood:

Leptospira can be observed in the blood by dark – filed microscope. Blood examination is useful in first week as Leptospira disappear from blood after 8 days.

Urine:

Leptospira may be present in urine in the 22nd week of the disease and intermittently thereafterup to 6 weeks. Centrifuged deposit of urine may be observed by Dark filed microscopy.

Culture:

Blood (1st week) and urine (22nd – 6  week) can be cultured in Korthof ’s medium. Media are incubated at 37°C for 2 days and then left at room temperature for 2 weeks. Culturesare examined every third day for the presence of Leptospira under DFM.

Serological tests

It is very useful method of diagnosis two types of serological tests are used, which are,

a. Screening tests:

These tests are genus – specific and done using reactive genus specific antigen (non – pathogenic L. biflexapatoc I strain).

Screening test includes – CFT, ELISA, SEL, HAT indirect IF these tests are capable to detect IgM and IgG leptospiral antibodies.

b. Serotype specific tests:

These tests identify the infecting serovar by demonstrating specific antibodies.

  • Macroscopic agglutination test
  • Microscopic agglutination test

Treatment and Preventions

  • Leptospira are sensitive to penicillin and tetracycline.
  • Preventive measures include rodent control, disinfection of water.