ISC class 12th Latest CHEMISTRY Syllabus after Cutoff

              CHEMISTRY 

               CLASS XII

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1.. Solid State

Solids: their classification based on different 

binding forces such as: ionic, covalent 

molecular; amorphous and crystalline solids 

(difference), metals. Type of unit cell in 

Two dimensional and three dimensional lattices,

number of atoms per unit cell (all types).

Calculation of density of unit cell, packing 

 In solids, packing efficiency, point defects,

electrical and magnetic properties.

Band theory of metals. Conductors,

semiconductors (n and p type) and insulators.

(i) Crystalline and amorphous solids.

(ii) Definition of crystal lattice, unit cell; types of 

unit cell (scc, fcc, bcc); calculation of the 

number of atoms per unit cell; relationship 

between radius, edge length and nearest 

neighbour distance. Calculation of 

density Of unit cell, formula of the compound –

numericals based on it; packing in 3 – D, 

packing fraction in scc, fcc, bcc with 

derivation.

(iii) Characteristics of crystalline solids; ionic 

(NaCl), metallic (Cu), atomic (diamond and 

graphite).

(iv) Point defects: Stoichiometric, non-

stoichiometric and impurity defects 

(F- centres).

(v) Electrical properties: Conductors, 

semiconductors (n & p types) and insulators.

(vi) Magnetic properties: diamagnetic, 

paramagnetic.

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2. Solutions 

Study of concentration of solutions of solids in 

liquids, liquid in liquid, solubility of gases in

liquids, Colligative properties - Raoult's law of 

relative lowering of 

vapour pressure elevation of boiling point,

depression of freezing 

point, osmotic pressure. Use of colligative 

properties in determining molecular masses of 

solutes, abnormal molecular mass association and 

dissociation, van't Hoff factor.

Normality, molality, molarity, mole fraction, as 

measures of concentration. Definition of the 

above with examples. Simple problems based on 

the above.

(i) Solubility of gases in liquids – Henry’s Law, 

simple numericals based on the above.

(ii) Raoult’s Law for volatile solutes and non-

volatile solutes, ideal solution, non-ideal 

solution. Azeotropic mixtures – definition, 

types.

(iii) Colligative properties – definition and 

examples, and its use in determination of 

molecular mass.

(a) Relative lowering of vapour pressure: 

Definition and mathematical expression 

of Raoult’s Law. Determination of 

relative molecular mass by measurement 

of lowering of vapour pressure. 

(b) Depression in freezing point: molal 

depression constant (cryoscopic 

constant) – definition and mathematical 

expression (derivation included).

(c) Elevation in boiling point method: molal 

elevation constant (ebullioscopic 

constant) definition and mathematical 

expression (derivation included). 

(d) Osmotic pressure: definition and 

explanation. Natural and chemical 

semipermeable membranes, reverse 

osmosis, isotonic, hypotonic and 

hypertonic solutions. Comparison 

between diffusion and osmosis. 

Application of osmotic pressure in the 

determination of relative molecular 

mass.

 van’t Hoff- Boyle’s Law, van’t Hoff –

Charles’ Law, van’t Hoff - Avogadro’s 

law. 

(e) Abnormal molecular mass: Dissociation 

and Association with suitable examples

(f) van’t Hoff factor for the electrolytes 

which dissociate and the molecules 

which associate in solution. 

Modification of the formula of colligative 

properties based on van’t Hoff factor. 

Simple problems. Calculation of degree 

of dissociation and association. 

Experimental details not required.

Numerical problems based on all the above 

methods. Experimental details not required.

3. Electrochemistry

Electrolytic and electrochemical cells. Redox 

reactions in electrochemical cells.

Electromotive Force (emf) of a cell, standard 

electrode potential, Nernst equation and its 

application to chemical cells. Relation between 

Gibbs energy change and emf of a cell. 

Conductance in electrolytic solutions, specific, 

equivalent and molar conductivity, variations of 

conductivity with concentration. Kohlrausch's 

Law of electrolysis and Faraday’s Laws of

electrolysis.

(i) Electrochemical cells: introduction, redox 

reactions (principle of oxidation and 

reduction in a cell). 

(ii) Galvanic cells - introduction; 

representation, principle – oxidation 

reduction. Mechanism of production of 

electric current in a galvanic cell. 

(iii) Measurement of potential. Single electrode 

potentials. 

Standard hydrogen electrode - definition, 

preparation, application and limitations. 

Standard electrode potential (Eo

) -

Measurement of standard electrode potential 

of Zn ++ / Zn, Cu ++ / Cu, half cell (using 

standard hydrogen electrode).

Cell notation – representation. 

Factors affecting electrode potential with 

explanation - main emphasis on the 

temperature, concentration and nature of the 

electrode.

(iv) Electrochemical series. Its explanation on 

the basis of standard reduction potential.

 Prediction of the feasibility of a reaction.

(v) Nernst equation and correlation with the free 

energy of the reaction with suitable 

examples. 

Prediction of spontaneity of a reaction based 

on the cell emf. 

Numericals on standard electrode potential 

of half-cells, cell emf, relationship between 

free energy and equilibrium constant, 

standard electrode potential and free energy.

(vi) Comparison of metallic conductance and 

electrolytic conductance. Relationship 

between conductance and resistance. Specific 

resistance and specific conductance. 

Cell constant: Calculation of cell constant. 

Meaning of equivalent conductance. 

Meaning of molar conductance. General 

relationship between specific conductance, 

molar conductance and equivalent 

conductance.

Units, numericals.

Molar conductance of a weak electrolyte at a 

given concentration and at infinite dilution. 

Kohlrausch’s Law – definition, applications 

and numericals.

(vii) Faraday’s laws of Electrolysis.

Faraday’s First Law of electrolysis. 

Statement, mathematical form. Simple 

problems. 

Faraday’s Second Law of electrolysis: 

Statement, mathematical form. Simple 

problems.

Relation between Faraday, Avogadro’s 

number and charge on an electron. F = NAe 

should be given (no details of Millikan’s 

experiment are required).

4. Chemical Kinetics

Meaning of Chemical Kinetics – slow and fast 

reactions. Rate of a reaction - average and 

instantaneous rate (graphical representation). 

Factors affecting rate of reaction: surface area, 

nature of reactants, concentration, temperature, 

catalyst and radiation. Order and molecularity 

of a reaction, rate law and specific rate constant. 

Integrated rate equations and half-life (only for 

first order reactions), concept of collision 

theory (elementary idea, no mathematical 

treatment). Concept of threshold and activation 

energy, Arrhenious equation.

(i) Meaning of chemical kinetics, Scope and 

importance of Kinetics of the reaction, slow 

and fast reactions – explanation in terms of bonds.

(ii) Rate of Reaction: definition, representation

of rate of reaction in terms of reactants and 

products, determination of rate of reactions 

graphically, instantaneous and average rate 

of reaction. Factors affecting rate of 

reaction.

(iii)Law of mass Action: statement and meaning 

of active mass. Explanation with an example 

– general reactions.

(iv) Effect of concentration of reactants on the 

rate of a reaction: Qualitative treatment, 

based on the law of mass Action, statement of 

rate law, General rate equation – 

Rate = k(concentration of the reactant)n

, 

where k is rate constant and n is the order of 

the reaction, relationship between the rate of 

the reaction with rate constant with respect 

to various reactants.

(v) Order of a reaction: meaning, relation 

between order and stoichiometric coefficients 

in balanced equations, order as an 

experimental quantity, rate equation,

mathematical derivation of rate equation for 

first order reaction, characteristics of first 

order reaction – rate constant is independent 

of the initial concentration, units to be 

derived, definition of half-life period, 

derivation of expression of half-life period 

from first order rate equation.

 Problems based on first order rate equation 

and half-life period.

(vi) Molecularity of the reaction: Meaning –

physical picture, Relation between order, 

molecularity and the rate of a reaction, 

Differences between order and molecularity 

of a reaction.

(vii) The concept of energy: Exothermic and 

endothermic reactions, concept of energy 

barrier, threshold and activation energy, 

formation of activated complex, effect of 

catalyst on activation energy and reaction 

rate.

(viii)Collision Theory: Condition for a chemical 

change – close contact, particles should

collide. Collisions to be effective – optimum 

energy and proper orientation during 

collision. Energy barrier built-up when the 

collision is about to take place, Activated 

complex formation, difference in energy of 

the reactant and the product – exothermic

and endothermic reactions with proper 

graphs and labelling.

(ix)Mechanism of the reaction: meaning of 

elementary reaction, meaning of complex 

and overall reaction, explanation of the 

mechanism of the reaction, slowest step of 

the reaction. Relationship between the rate 

expression, order of reactants and products 

at the rate-determining step, units of rate 

constant – explanation with suitable 

examples.

(x) Effect of temperature on the rate constant of 

a reaction: Arrhenius equation – K=Ae-Ea/RT, 

Meaning of the symbols of Arrhenius 

equation, related graph, evaluation of Ea and 

A from the graph, meaning of slope of the 

graph, conversion from exponential to log 

form of the equation, relationship between 

the increase in temperature and the number 

of collisions. Numerical based on Arrhenius 

equation.

5. Surface Chemistry

Absorption and Adsorption - physisorption and

chemisorption, factors affecting adsorption of

gases on solids and liquids. Catalysis; 

homogenous and heterogenous, activity and 

selectivity.

Colloidal state distinction between true solutions, 

colloids and suspension; lyophilic, lyophobic

multi-molecular, macromolecular and associated 

colloids; properties of colloids; Brownian

movement, Tyndall effect, coagulation and 

electrophoresis. Emulsion - types ofemulsions.

(i) Difference between absorption and 

adsorption: definition of physisorption and

chemisorption and their differences. 

Factors affecting adsorption of gases on 

solids.

(ii)Catalysis: definition, types of catalysts –

positive and negative, homogeneous and 

heterogeneous catalyst based on the state of 

the reactant and the catalyst, Elementary 

treatment of intermediate compound 

formation theory with examples; adsorption 

Theory, effect of catalyst on the rate of 

reaction – the change in the energy of 

activation in the activation energy curve. 

Characteristics of a catalyst; specificity, 

activity, surface area of a catalyst. Promoter and poison.

(iii)Colloidal State: Thomas Graham classified 

the substances as crystalloid and colloid, 

classification of substances on the basis of 

the particle size i.e. true solution, sol and 

suspension, colloidal system is 

heterogeneous. lyophilic and lyophobic 

colloid; classification of colloidal solutions 

as micro, macro and associated colloids. 

Preparation of lyophilic colloids. 

Preparation of lyophobic colloids by colloid 

mill, peptization, Bredig’s arc method, 

oxidation, reduction, double decomposition 

and exchange of solvent method, purification 

of colloids (dialysis, ultra-filtration, and 

ultracentrifugation). 

Properties of colloidal solutions: Brownian 

movement, Tyndall effect, coagulation, 

electrophoresis (movement of dispersed 

phase), Protection of colloids, Gold number 

and Hardy- Schulze rule. Emulsions, 

surfactants, micelles (only definition and 

examples).

Application of colloids and emulsions in 

daily life.

6. General Principles and Processes of Isolation 

ofElements

Metals: metallurgy, ores, principles and 

methods of extraction - concentration, 

oxidation, reduction, electrolytic refining. 

Occurrence and principles of extraction of

aluminium, copper, zinc, iron and silver.

Definition of minerals, ores and metallurgy; 

principle ores of aluminium, iron, copper, zinc 

and silver. 

Methods of concentration of ores: hydraulic 

washing, magnetic separation, froth floatation 

method, leaching.

Extraction of metal from concentrated ore –

calcination, roasting and thermal reduction.

Metallurgy of aluminium, iron, copper, zinc and 

silver. 

Refining of metals - distillation, liquation, 

electrolysis, vapour phase refining (nickel), zone 

refining.

7. p-Block Elements

Group-15 Elements

Position in the periodic table, occurrence, 

electronic configuration, oxidation states, trends 

in physical and chemical properties. Nitrogen: 

preparation properties and its uses; compounds 

of nitrogen: nitric acid – preparation and 

properties. Phosphorus - compounds of

phosphorus: preparation and properties of

phosphine.

(i) General introduction, electronic 

configuration, occurrence, oxidation states. 

Trends in physical properties; chemical 

properties with hydrogen, oxygen and 

halogens.

(ii) Nitrogen - Laboratory preparation, 

decomposition (ammonium dichromate). 

Properties and uses.

(iii) Nitric Acid - Preparation and manufacture. 

Properties: reaction with copper (dilute and 

concentrated HNO3), carbon and sulphur. 

Uses.

(iv) Phosphine – preparation from phosphorus 

and properties: reaction with halo acids.

 Group-16 Elements

Position in the periodic table, occurrence, 

electronic configuration, oxidation states,

trends in physical and chemical properties. 

Ozone – methods of preparation.

Compounds of sulphur: preparation, 

properties and uses of sulphur-dioxide, 

sulphuric acid (industrial process of

manufacture). 

(i) Electronic configuration, oxidation 

states, occurrence. Trends in physical 

properties; chemical properties with 

hydrogen, oxygen and halogens.

(ii) Ozone: manufacture by Siemen’s 

ozoniser, thermal decomposition of 

ozone, its oxidising nature – reaction 

with lead sulphide, potassium iodide and 

mercury, its uses.

(iii) Sulphur dioxide: laboratory and

industrial preparation from sulphites and 

sulphide ores, reaction of sulphur dioxide with NaOH, Cl2, KMnO4.

(iv) Sulphuric Acid: manufacture by Contact 

Process (equations, conditions and 

diagram), properties - acidic nature, 

mode of dilution, oxidising action, 

dehydrating nature and uses of sulphuric 

acid in industry.

 Group-17 Elements

Position in the periodic table, occurrence,

electronic configuration, oxidation states,

trends in physical and chemical properties; 

Preparation, properties and uses of chlorine. 

Interhalogen compounds.

(i) General introduction, electronic 

configuration, oxidation states. Trends in 

physical properties and chemical 

properties (hydrogen, oxygen, halogens 

and metals).

(ii) Chlorine – preparation from MnO2 and 

HCl, from NaCl, MnO2 and conc. H2SO4

(only equations), reactions of chlorine 

with H2S, NH3, cold, dilute NaOH and 

hot, concentrated NaOH.

(iii)Interhalogen compounds – structure, 

hybridisation and shapes: XX′, XX′3, 

XX′5, XX′7.

Group-18 Elements

Position in the periodic table, occurrence, 

electronic configuration, trends in physical and 

chemical properties, inert nature, uses.

(i) General introduction, electronic 

configuration, occurrence, trends in

physical; chemical properties, state and low 

reactivity. 

(ii) Formation of xenon compounds with fluorine 

and oxygen (equations only), hybridisation, 

shape and structure of compounds. 

(iii) Uses of noble gases.

8. d and f Block Elements

Position in the periodic table, occurrence, 

electronic configuration and characteristics of 

transition metals, general trends in properties of 

the 3d-series of transition metals - metallic 

character, ionisation enthalpy, oxidation states, 

ionic radii, colour of ions, catalytic property, 

magnetic properties, preparation and properties

of K2Cr2O7 and KMnO4.

Lanthanoids and actinoids.

(i) d-Block: 3d, 4d and 5d series

Study in terms of metallic character, atomic 

and ionic radii, ionisation enthalpy, 

oxidisation states, variable valency, 

formation of coloured compounds, formation 

of complexes, alloy formation.

(ii) f-Block: 4f and 5f series 

Electronic configuration, atomic and ionic 

radii, oxidisation states, formation of 

coloured compounds, formation of 

complexes. Lanthanoid contraction and its

consequences. Chemical reactivity – with 

oxygen, hydrogen, halogen, sulphur, 

nitrogen, carbon and water.

Actinoids - oxidation states and comparison

with lanthanoids.

(iii)Potassium permanganate: structure, shape, 

equation of extraction from pyrolusite ore, its 

oxidising nature in acidic, basic and neutral 

medium, use in redox titration.

Oxidising nature in acidic [FeSO4, 

(COOH)2.2H2O, KI], basic (KI) and neutral 

(H2S) mediums to be done.

(iv) Potassium dichromate: structure, shape, 

equation of extraction from chromite ore and 

its use in titration. Oxidising nature in acidic, 

basic and neutral medium, use in redox 

titration. 

9. Coordination Compounds

Concept of complexes, definition of ligands,

coordination number, oxidation number. IUPAC

nomenclature of mononuclear coordination

compounds. Isomerism (structural and stereo). 

Bonding, Werner's theory, VBT. Colour, 

magnetic properties and shapes. Importance of 

coordination compounds (in qualitative analysis, 

extraction of metals and biologicalsystem). 

(i) Definition of coordination compounds / 

complex compounds, differences with a 

double salt, study of ligands – mono-, bi-, tri-

, tetra-, penta-, hexa- and polydentate, 

chelating ligands, definition of coordination 

number, its calculation for a complex 

coordination sphere, study of oxidation state of an element in a complex, its calculation, 

IUPAC rules of nomenclature of 

coordination compounds. 

(ii) Isomerism – structural, stereo types and 

examples.

(iii)Valence bond theory of coordination 

compounds – examples of formation of inner 

orbital and outer orbital complexes (high 

and low spin, octahedral, tetrahedral and 

square planar), prediction of magnetic 

character.

(iv) Importance and uses.

10. Haloalkanes and Haloarenes.

Haloalkanes: General formula, nomenclature 

and classification. Nature of C–X bond, 

physical and chemical properties, mechanism 

of substitution reactions, opticalrotation.

Haloarenes: Basic idea, nature of C–X bond, 

substitution reactions (directive influence of 

halogen in monosubstituted compounds only).

Nature of C-X bond

Naming the halogen derivatives of alkanes by 

using common system and IUPAC system for 

mono, di and tri-halo derivatives.

Preparation of haloalkanes from:

- Alkane and halogen.

- Alkene and hydrogen halide.

- Alcohols with PX3, PCl5 and SOCl2.

- Halide exchange method (Finkelstein and 

Swarts)

- Silver salt of fatty acids (Hunsdiecker).

Physical properties: State, melting point, boiling

point and solubility. 

Chemical properties: nucleophilic substitution 

reactions (SN1, SN2 mechanism in terms of 

primary, secondary and tertiary halides) 

Reaction with: sodium hydroxide, water, sodium 

iodide, ammonia, primary amine, secondary 

amine, potassium cyanide, silver cyanide, 

potassium nitrite, silver nitrite, silver salt of fatty 

acid and lithium-aluminium hydride. 

Elimination reaction (Saytzeff’s rule) / β 

elimination.

Reaction with metals: sodium and magnesium 

(Wurtz’s reaction, Grignard’s reagent 

preparation).

Chloroform and iodoform: preparation and 

properties.

Preparation of haloarenes by Sandmeyer’s and 

Gattermann’s reaction, by electrophilic 

substitution.

Physical properties: State, melting point, boiling

point and solubility.

Chemical properties:

- Electrophilic substitution (chlorination 

nitration and sulphonation).

- Nucleophilic substitution (replacement of 

chlorine with -OH, -NH2).

- Reduction to benzene. 

- Wurtz-Fittig reaction.

- Fittig reaction. 

- Addition reaction with magnesium 

(formation of Grignard reagent).

11. Alcohols, Phenols and Ethers

Alcohols: Classification, general formula, 

structure and nomenclature. Methods of 

preparation, physical and chemical properties 

(of primary alcohols only), identification of 

primary, secondary and tertiary alcohols, uses 

with special reference to methanol andethanol.

(i) Classification into monohydric, dihydric and 

polyhydric alcohols, general formulae, 

structure and nomenclature of alcohols. 

Difference between primary, secondary and 

tertiary alcohols in terms of structure, 

physical properties and chemical properties.

(ii) Methods of preparation: 

- Hydration of Alkenes – direct hydration, indirect hydration,

hydroboration  oxidation 

- From Grignard’s reagent.

- Hydrolysis of alkyl halides.

- Reduction of carbonyl compounds.

- From primary amines.

* Properties:

- Acidic nature of alcohols: 

- Reaction with sodium.

- Esterification.

- Reaction with hydrogen halides.

- Reaction with PCl3, PCl5, and SOCl2.

- Reaction with acid chlorides and acid anhydrides.

- Oxidation.

- Dehydration.

 Uses of alcohols.

(iii) Conversion of one alcohol into another.

(iv) Distinction between primary, secondary and 

tertiary alcohols by Lucas’ Test.

Phenols: Classification and nomenclature. 

Methods of preparation, physical and chemical 

properties, acidic nature of phenol, electrophilic 

substitution reactions, uses ofphenols.

Preparation of phenol from diazonium salt, 

chlorobenzene (Dow’s process) and from 

benzene sulphonic acid.

Manufacture from Cumene.

Physical properties: state and solubility.

Chemical properties: 

- Acidic character of phenol.

- Reaction with sodium hydroxide. 

- Reaction with sodium. 

- Reaction with zinc. 

- Reaction with acetyl chloride and acetic 

anhydride. 

- Reaction with phosphorus penta chloride. 

- Bromination, nitration and sulphonation 

(Electrophilic substitution reactions). 

- Kolbe’s reaction (formation of salicylic 

acid). 

- Reimer – Tiemann reaction

- Test for phenol – FeCl3 test, azo dye test.

Aliphatic Ethers: General formula, structure and 

nomenclature. Methods of preparation, physical

and chemical properties, uses.

Ethers: structure of ethereal group.

Preparation from alcohol (Williamson’s 

synthesis). 

Physical properties: state, miscibility.

Chemical properties: 

- Reaction with chlorine.

- Oxidation (peroxide formation). 

- Reaction with HI. 

- Reaction with PCl5.

12. Aldehydes, Ketones and Carboxylic Acids

Aldehydes and Ketones: Nomenclature, 

structure of methods of preparation of 

aldehydes and ketones, physical and chemical 

properties, mechanism of nucleophilic addition, 

reactivity of alpha hydrogen in aldehydes and

uses.

Preparation:

• From alcohol.

• From alkenes (ozonolysis).

• From alkynes (hydration).

• From acid chlorides (Rosenmund’s 

reduction, reaction with dialkyl cadmium).

• From calcium salt of carboxylic acids.

• From nitriles (Stephen reaction, Grignard’s 

reagent). 

• From esters.

Physical properties – state and boiling point.

Chemical properties:

• Nucleophilic addition reactions with 

mechanism (ammonia and its derivatives, 

HCN, NaHSO3 and Grignard’s reagent). 

• Oxidation reactions, iodoform reaction.

• Reduction: reduction to alcohol and alkanes 

(Clemmensen’s reduction, Wolff-Kishner 

reduction, Red phosphorus and HI).

• Base catalysed reactions: Aldol 

condensation, cross Aldol condensation, 

Cannizzaro’s reaction.

Tests: difference between formaldehyde and 

acetaldehyde; aldehydes and ketones.

Uses of aldehydes and ketones.

Aromatic aldehyde (Benzaldehyde)

Lab preparation from toluene by oxidation with 

chromyl chloride. 

Physical properties: state and stability.

Chemical properties:

• Oxidation and reduction.

• Nucleophilic addition reaction (hydrogen cyanide and sodium bisulphite).

• Reactions with ammonia and its derivatives 

(hydroxyl amine, hydrazine and phenyl 

hydrazine).

• Reaction with phosphorus pentachloride.

• Cannizzaro reaction.

• Benzoin condensation.

• Perkin’s reaction.

• Electrophilic substitution - halogenation, 

nitration and sulphonation.

Test: distinction between aromatic and aliphatic 

aldehydes. 

Uses of benzaldehyde.

Carboxylic Acids: Classification, general 

formula and structure of carboxylic group. 

Nomenclature, acidic nature, methods of 

preparation, physical and chemical properties 

and uses.

Classification of mono and di carboxylic acids 

with examples. 

Preparation of aliphatic and aromatic carboxylic 

acid:

- From alcohols, aldehydes.

- From nitriles.

- From Grignard’s reagent.

Physical properties: state, boiling point and 

solubility.

Chemical properties:

- Acidic character: (aliphatic, aromatic 

carboxylic acids with the effect of 

substituents on the acidic character – to be 

dealt with in detail) 

- Reaction with active metals, alkalies, 

carbonates and bicarbonates,

- Formation of acid derivatives.

- Decarboxylation (chemical and Kolbe’s 

electrolytic reaction).

- HVZ reactions.

- Substitution of benzene ring (meta directive 

effect of carboxylic acid group) nitration and 

sulphonation. 

Tests for acids: formic acid, acetic acid and 

benzoic acid. 

Uses of formic acid, acetic acid and benzoic acid. 

13. Organic compounds containing Nitrogen

Aliphatic Amines: General formula and, 

classification of amines. Structure of the amino 

group, nomenclature. Methods of preparation, 

physical and chemical properties, uses,

identification of primary, secondary and tertiary

amines.

• Amines 

Nomenclature, classification with examples, 

structure, general formula. 

Methods of preparation:

- From alcohol.

- From alkyl halide.

- From cyanide.

- From amide (Hofmann’s degradation).

- From nitro compounds.

- Gabriel phthalimide Synthesis.

Physical properties: comparison between 

primary, secondary and tertiary amines in 

terms of – state, solubility, boiling point 

(hydrogen bonding), comparison with 

alcohols. 

Chemical properties: 

- Basic character of amines – comparison

between primary, secondary and tertiary 

alkyl amines/ ammonia/ aniline. 

Effect of substituents on the basic strength of aniline.

- Alkylation and acylation with 

mechanism.

- Reaction with nitrous acid.

- Carbylamine reaction.

Distinction between primary, secondary 

and tertiary amines (Hinsberg’s Test).

Aniline

Preparation reduction of nitrobenzene. 

Physical properties – state, solubility and boiling point.

Chemical properties:

- Reaction with HCl and H2 SO4  

- Acetylation, alkylation. 

- Benzoylation.

Carbylamine reaction.

- Diazotisation.

- Electrophilic substitution (bromination, 

nitration and sulphonation). 

Tests for aniline.

Uses of aniline.

Diazonium salts: Preparation, chemical 

reactions and importance in synthetic organic

chemistry.

Preparation from aniline; 

Properties: Sandmeyer’s reaction, Gattermann 

reaction, replacement of diazo group by – H, -

OH, -NO2, coupling reaction with phenol and 

aniline.

12. Biomolecules

Carbohydrates – Definition, Classification 

(aldoses and ketoses), monosaccahrides (glucose

and fructose), D-L configuration 

oligosaccharides (sucrose), polysaccharides 

(starch, cellulose); Importance of carbohydrates.

Carbohydrates: definition, classification - mono 

(aldose, ketose), oligo (di, tri, tetra saccharides) 

and polysaccharides with examples: reducing 

sugars and non-reducing sugars – examples and 

uses. 

Heating with HI, reaction with hydroxylamine, 

bromine water and nitric acid.

Test for glucose and fructose (bromine water test 

with equation).

Disaccharides – structure of sucrose (glycosidic 

linkage).

Polysaccharides – starch, cellulose, glycogen.

Proteins – structural units of proteins. Basic

idea of - amino acids, peptide bond,

polypeptides, proteins, denaturation of proteins. 

Enzymes, hormones - elementary idea only. 

Proteins: Amino acids – general structure, 

classification and zwitter ion formation. 

Isoelectric point. 

Classification of proteins on the basis of 

molecular shape; denaturation of proteins. 

(Definitions only. Details and diagrams are not 

required).

Vitamins - Classification and functions.

Vitamins A, B, C, D, E and K: classification 

(fat soluble and water soluble), deficiency 

diseases. (Chemical names and structures are not 

required).

Nucleic Acids - DNA and RNA.

Nucleic acids: basic unit – purine and 

pyrimidine, DNA – structure (double helical), 

RNA (No chemical structure required).

Differences between DNA and RNA.

13. Polymers

Definition and classification on different 

parameters. Methods of polymerisation 

(addition and condensation), copolymerisation, 

and some important polymers: natural and 

synthetic like polythene, nylon polyesters,

bakelite, rubber. Biodegradable and non-

biodegradable polymers.

Classification based on source, on structure, on 

mode of polymerisation, on molecular forces, on 

growth

Preparation of important addition polymers -

Polythene, polypropene, PVC, PTFE, 

polystyrene.

Rubber – natural and synthetic (Buna-N and 

Buna-S), vulcanisation of rubber.

Preparation of important condensation polymers 

- polyester, Nylon 66, Nylon 6, Bakelite, 

melamine (to be learnt in terms of monomers). 

Biodegradable polymers – PHBV, Nylon 2 -

Nylon 6.

Uses.

14. Chemistry in Everyday life

Chemicals in medicines - analgesics, 

tranquilizers antiseptics, disinfectants,

antimicrobials, antifertility drugs, antibiotics, 

antacids,antihistamines.

In medicine: antipyretics, analgesics, 

tranquillisers, antiseptics, disinfectants, 

anti-microbials, anti-fertility drugs, 

antihistamines, antibiotics, antacids.

Definition, common examples, uses.

Differences between antiseptics 

 and disinfectants. 

Structure not required.

Chemicals in food - preservatives, artificial

sweetening agents, elementary i

Idea of antioxidants.

Preservatives: role, example (Sodium benzoate). 

Artificial sweetening agents: role, examples 

(aspartame, saccharine, sucralose and alitame).