CHEMISTRY - Pustakkosh

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CHEMISTRY

3rd EDITION YEAR 2020-21

I SBN “978-93-5423-043-1”

SYLLABUS

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CONTENTSl Latest Further Reduced Syllabus issued by CISCE for Academic Year 2020 - 21 9 - 19l Topics found difficult by the Candidates 20 - 21l Concepts in which Candidates got Confused 22 - 23l Suggestions for the Students 24 - 24

qMind Maps 1 - 16qOn Tips Notes 17 - 59q Sample Question Papers (Solved) Sample Question Paper - 1 (Examination Paper - 2020) 60 - 76 With Topper's Answer Sample (Specimen - 2018) Question Paper - 2 77 - 87 With Solutions Sample Question Paper - 3 88 - 91 Sample Question Paper - 4 92 - 95 Sample Question Paper - 5 96 - 99

q Self Assessment Papers* Self Assessment Paper - 1 100 - 103 Self Assessment Paper - 2 104 - 107 Self Assessment Paper - 3 108 - 111 Self Assessment Paper - 4 112 - 115 Self Assessment Paper - 5 116 - 119 Self Assessment Paper - 6 120 - 123 Self Assessment Paper - 7 124 - 127 Self Assessment Paper -8 128 - 131 Self Assessment Paper -9 132 - 135 Self Assessment Paper -10 136 - 139

q Solutions Sample Question Paper - 3 140 - 146 Sample Question Paper - 4 147 - 154 Sample Question Paper -5 155 - 162

q Hints of Self Assessment Papers 1-10 163 - 167

qq

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Further Reduced Syllabus for Academic Year 2020-21

CHEMISTRYCLASS 12

There will be two papers in the subject. Paper I: Theory 3 hours..... 70 marks Paper II: Practical : 3 hours ... 15 marks Project Work ... 10 marks Practical File .... 5 marks

PAPER I (THEORY) - 70 Marks There will be no overall choice in the paper. Candidates will be required to answer all questions. Internal choice will be available in two questions of 2 marks each, two questions of 3 marks each and all the three questions of 5 marks each.

S.No. UNIT TOTAL WEIGHTAGE

1. Solid State

Physical Chemistry

25 Marks

2. Solutions

3. Electrochemistry

4. Chemical Kinetics

5. Surface Chemistry

6. General Principles and Processes of Isolation ofElementsInorganic Chemistry

20 Marks

7. p- Block Elements

8. d- and f-Block Elements

9. Coordination Compounds

10. Haloalkanes and Haloarenes

Organic Chemistry

25 Marks

11. Alcohols, Phenols and Ethers

12. Aldehydes, Ketones and Carboxylic Acids

13. Organic Compounds containing Nitrogen

14. Biomolecules

15. Chemistry in Everyday Life

Total 70 Marks

PAPER I –THEORY – 70 Marks1. 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.

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.

Normality, molality, molarity, mole fraction, as measures of concentration. Definition of the above with examples. Simple problems based on the above.

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

numericals based on the above.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.

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 (E0) - 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).

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...contd.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 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) 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.

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...contd. Properties of colloidal solutions: Brownian movement,

Tyndall effect, coagulation, electrophoresis (movement

of dispersed phase), Protection of colloids, 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 of

Elements

Metals: metallurgy, ores, principles and methods

of extraction - concentration, oxidation, reduction,

electrolytic refining. Occurrence and principles of

extraction of copper, zinc, iron and silver.

Definition of minerals, ores and metallurgy; principle ores

of 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.

Extraction of metal from concentrated ore – calcination,

roasting and thermal reduction.

Metallurgy of iron, copper, zinc and silver.

Refining of metals - distillation, liquation, electrolysis.

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 (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.

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.


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.


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.

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...contd. (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, properties of

K2Cr2O7 and KMnO4.

Lanthanoids and actinoids.

(i) 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; 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; 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, optical rotation.

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.

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...contd.

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) with mechanism.

- 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.


- 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.


- Reaction with chlorine.

- Oxidation (peroxide formation).

- Reaction with HI.

- Reaction with PCl5.

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...contd.

12. Aldehydes, Ketones and CarboxylicAcids

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:

l From alcohol.

l From alkenes (ozonolysis).

l From alkynes (hydration).

l From acid chlorides (Rosenmund’s reduction, reaction

with dialkyl cadmium).

l From calcium salt of carboxylic acids.

l From nitriles (Stephen reaction, Grignard’s reagent).

l From esters.

Physical properties – state and boiling point.


l Nucleophilic addition reactions with mechanism

(ammonia and its derivatives, HCN, NaHSO3 and

Grignard’s reagent).

l Oxidation reactions, iodoform reaction.

l Reduction: reduction to alcohol and alkanes

(Clemmensen’s reduction, Wolff-Kishner reduction,

Red phosphorus and HI).

l Base catalysed reactions (with mechanism): 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.


l Oxidation and reduction.

l Nucleophilic addition reaction (hydrogen cyanide and

sodium bisulphite).

l Reactions with ammonia and its derivatives (hydroxyl

amine, hydrazine and phenyl hydrazine).

l Reaction with phosphorus pentachloride.

l Cannizzaro reaction.

l Benzoin condensation.

l Perkin’s reaction.

l 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.


- 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.

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...contd.

l 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.


- 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.


- 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.

14. 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).

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.

15. 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.

(17)

...contd.

Chemicals in food - preservatives, artificial

sweetening agents, elementary idea of antioxidants.

Preservatives: role, example (Sodium benzoate).

Artificial sweetening agents: role, examples (aspartame,

saccharine, sucralose and alitame).

PAPER II

PRACTICAL WORK – 15 Marks

Candidates are required to complete the following

experiments:

1. Titrations

Oxidation-reduction titrations: potassium manganate

(VII) / ammonium iron (II) sulphate; potassium manganate (VII) / oxalic acid.

The candidate may be required to determine the percentage purity of a compound and the number

of molecules of water of crystallization in hydrated

salts. In such experiments sufficient working details including recognition of the end point will be given.

Candidates will be required to calculate:

l Molarity

l Concentration in grams L-1 / molecular mass

l Number of molecules of water of crystallisation/

percentage purity.

NOTE: Molarity must be calculated upto 4 decimal

places at least, in order to avoid error.

OBSERVATION TABLE

S. No. (A) (B) (B – A)

Initial burette reading

(ml)

Final burette reading

(ml)

Difference (ml)

1

2

3

l Concordant reading is to be used for titre value.

Concordant reading is two consecutive values which are exactly the same. Average will not be accepted as

titre value.

l The table is to be completed in ink only. Pencil is not

to be used.

l Overwriting will not be accepted in the tabular

column.

Observations:

l Pipette size (should be same for all the candidates at the centre).

l Titre value (concordant value).

2. Study of the rate of reaction

The candidates will be required, having been given

full instructions, to carry out an experiment on

the rate of reaction, e.g. reaction between sodium

thiosulphate and hydrochloric acid (using different

concentrations for either), magnesium and dil. sulphuric acid/ dil. hydrochloric acid (using different

concentrations).

l Graph of volume vs. time and its interpretation.

l Relationship between concentration and rate, volume and

rate and time and rate.

3. Identification of the following compounds and

functional groups based on observations

l Alcoholic group - glycerol

l Aldehyde group- formaldehyde

l Ketonic group – acetone

l Carboxylic group – benzoic acid

l Amino group - aniline

*Please Note: Carbylamine and acrolein tests should not be performed.

The student should learn to differentiate between colours,

solution, ring and precipitate.

4. Characteristic tests of carbohydrates and proteins

l Carbohydrates – glucose

l Proteins – powdered milk

Identification should be of ‘Carbohydrate’ and ‘Protein’ not

of individual substances.

5. Qualitative analysis

Qualitative analysis: identification of single salt containing one anion and one cation:

Anions: CO32-, NO2

-, S2-, SO32-, SO4

2-, NO3-,

CH3COO-, Cl-, Br-, I-, C2O42-, PO4

3-.

Cations: NH4+, Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Mn2+ ,

Ni2+, Co2+, Ba2+, Sr2+, Ca2+, Mg2+.

(18)

...contd. ...contd.NOTE:

Chromyl chloride test not to be performed.

For wet test of anions, sodium carbonate extract

must be used (except for carbonate).

(Insoluble salts such as lead sulphate, barium

sulphate, calcium sulphate, strontium sulphate will

not be given).

Anions: Dilute acid group – CO32-, NO2

-, S2-, SO32-

Concentrated Acid Group – NO3-, Cl-, Br-, I-,

CH3COO-.

Special Group - SO42-, PO4

, C2O42-.

Cations: Group Zero: NH4+

Group I: Pb2+

Group II: Cu2+, Pb2+

Group III: Al3+, Fe3+

Group IV: Zn2+, Mn2+, Ni2+, Co2+

Group V: Ba2+, Sr2+, Ca2+

Group VI: Mg2+

NOTE:

l Formal analytical procedure is required for

Qualitative Analysis.

l Specific solvent for O.S. to be used;

l Before adding Group III reagents to the filtrate of

Group II, H2S must be removed followed by

boiling with conc. Nitric acid.

l The right order for buffer (NH4Cl and NH4OH)

must be used.

l The flame test with the precipitate obtained in

Group V for Ba2+, Sr2+, Ca2+ will also be accepted

as a confirmatory test.

For wet test of anions, sodium carbonate extract must be

used (except for carbonate).

PATTERN OF CHEMISTRY

PRACTICAL PAPER

Questions in the practical paper will be set as follows:

Question 1 Volumetric Analysis

Question 2 Any one or a combination of the following experiments:

• Study of the rate of reaction.

• Identification of the organic compounds and functional groups based on observations.

• Characteristic tests of carbohy-drates and proteins.

Question 3 Qualitative Analysis (single salt).

PROJECT WORK AND PRACTICAL FILE -

15 Marks

Project Work – 10 Marks

The project work is to be assessed by a Visiting Examiner

appointed locally and approved by the Council.

The candidate is to creatively execute one project/

assignment on an aspect of Chemistry. Teachers may assign or students may select a topic of their choice.

Following is only a suggestive list of projects.

Suggested Evaluation criteria for Project Work:

l Introduction / purpose

l Contents

l Analysis/ material aid (graph, data, structure, pie

charts, histograms, diagrams, etc.)

l Presentation

l Bibliography

Suggested Assignments:

1. Amino acids: Peptides, structure and classification, proteins structure and their role in the growth of

living beings.

2. Nucleic Acid: DNA and RNA – their structure. Unique nature. Importance in evolution and their

characteristic features.

3. Carbohydrates and their metabolism, Blood -

haemoglobin and respiration.

4. Vitamins and hormones

5. Simple idea of chemical evolution.

6. Natural polymers (any five) - structure,

characteristics, uses. Synthetic polymers (any five) - method of preparation, structure, characteristics

and uses.

7. Types of Dyes - methods of preparation,

characteristics and uses.

(19)

...contd. 8. Chemicals in medicines: antiseptics, antibiotics,

antacids, etc. and their uses.

9. Preparation of soap, nail polish, boot polish, varnish,

nail polish remover, shampoo and perfumes.

10. Chemicals and chemical processes in forensic studies.

11. Insecticides, pesticides and chemical fertilisers.

12. Ancient Indian medicines and medicinal plants.

13. Organic Chemistry in Nutrition, Food Science and

Biotechnology.

14. Effect of Green House Gases.

15. How Plastics have changed the world, both socially

and economically.

Practical File – 5 Marks

The Visiting Examiner is required to assess students on

the basis of the Chemistry Practical file maintained by

them during the academic year.

NOTE: According to the recommendation of International Union of Pure and Applied Chemistry (IUPAC), the groups

are numbered from 1 to 18 replacing the older notation of groups IA ….. VIIA, VIII, IB …… VIIB and 0. However, for

the examination both notations will be accepted.

Old notation IA IIA IIIB IVB VB VIB VIIB VIII IB IIB IIIA IVA VA VIA VIIA 0

New notation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18

qq

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Examination Paper 2019

l Rate law equation, order of reaction and numerical problems based on half-life period.l Numerical problems based on depression in freezing point, calculation of degree of association,

determination of molecular mass using colligative properties. Faraday’s laws of electrolysis, calculation of e.m.f. using Nernst equation and free energy change (ΔG) of the cell.

l Role of chemicals/substances in the extraction of aluminium, silver and iron. •Nomenclature of coordination compounds, hybridisation and magnetic behaviour.

l Surface chemistry, definition of certain terms related to colloidal state.l Name of organic reactions, conversion of organic compounds, chemical tests to distinguish the

organic compounds.l Name and structure of monomers and the type of polymerisation.l Types of vitamins, fat soluble and water soluble. Diseases caused by their deficiency.l Reasoning questions of p- and d-blocks.


l The packing efficiency of different type of unit cells. Imperfection in solids. l Numerical problem based on elevation of boiling point, depression in freezing point, l Van't Hoff factor and degree of dissociation. l Numerical problem related to Arrhenius equation. l Rate Law expression order of reaction and half-life period. l Nernst equation, electrochemical series, equivalent and molar conductance corrosion of metals. l Surface chemistry, application of colloids, purification of colloids. l Coordination compounds nomenclature, isomerism hybridisation of coordination compounds. l Chemical equations of inorganic compounds, extraction of copper, chemical equations of K2

Cr2 O7 and KMnO4. l Named organic reactions, conversion of organic compounds reasoning type of questions of

organic chemistry. l Polymers, Biodegradable Polymers and their examples. l Use of chemicals in Food Industry, antiseptics and disinfectants.

Examination Paper 2017l Concepts of molarity based on (grams/litre)/ molecular weight for pure substances and morality

based on titre value.l Difference between precipitate and solution.l Principles of formal group analysis.


l Numerical problems of relative molecular mass and mole, Van't Hoff factor and its relation with molecular weight, calculation of degree of dissociation

l Anisotropic nature of graphite, calculation of edge length (a) and radius (r) of unit cell l Chemical equilibrium, Le Chatelier's principle l Electrolytic conductance, calculation of emf of the cell and cell representation, Nernst equation l Ionic equilibria, calculation of pH value, solubility and solubility product l Bronsted-Lowry's concept for acid and base. Buffer action of basic buffer l Preparation of inorganic compounds l General electronic configuration of inner transition elements l Conversion of organic compounds, balancing of equations and named organic reactions l Chemical tests to distinguish between organic compounds

Topics found Difficult by Candidates

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l Relative molecular mass and mole (numerical problems), abnormal molecular weights.l Solid state, voids and defects in solid state.l Ionic equilibria (numerical problems) concept of solubility product, ionic product and common

ion effect.l Electrolytic conductance, electrode potential and Nernst equation.l Nomenclature, isomerism, hybridization and geometry of coordination compounds.l Balancing of equations for inorganic compounds.l Organic conversions, named reactions and balancing of equations.l Bio molecules.l Polymers.


l Relative molecular mass and molel Chemical kineticsl Chemical equilibriuml Electrolyte conductancel Coordination compoundsl Preparation of inorganic compoundsl Ionic equilibrial Organic conversions and balanced equationsl Named organic reactions (Balz-Schiemann’s reaction)

....contd. Topics found Difficult by Candidates

(22)

Examination Paper 2019l Relation between elevation of boiling point and number of moles of solute in solution.l Increasing order of acidic strength of the oxoacid and inductive effect.l The ionic size of La3+ and Lu3+.l Diamagnetic and paramagnetic nature of complex ions.l Peptisation, electrophoresis and dialysis in colloidal state.l Difference between ΔG and ΔGo.l Specific conductance and Kohlrausch’s Law.l Reactions of inorganic compounds and their balanced equations.Examination Paper 2018l Isomerism of coordination compounds (linkage and geometrical) and nomenclature of

coordination compounds. l Relationship between E°cell and standard free energy change (D G°). l Purines and pyrimidines present in RNA and DNA. l Colloidal solution and their applications. l Reactions of inorganic compounds with balanced equation. l Tests to distinguish organic compounds. Examination Paper 2017l Certain colours like buff precipitate. l Solubility of mixture or preparation of original solution for group separation. l Use of neutralized sodium carbonate extract for confirmatory test of anion. l Identification of gases. l Systematic analysis from group zero to IV and reporting absence and presence of groups. Examination Paper 2016l Van't Hoff factor and molecular weight l Anisotropic and isotropic l Common ion effect and solubility product l Total number of particles in bcc and fcc unit cell and their relationship l Paramagnetic and diamagnetic l Edge length (a) and radius (r) of various types of cubic unit cell and their relationship l Buffer action of acidic and basic buffer l Concept of oxidation and reduction of SO2 l Gibb's free energy and emf of cell in terms of spontaneity l Types of polymerization and polymer Examination Paper 2015l Van't Hoff factor, calculation of degree of dissociation.l Azeotropic mixtures, ideal and non-ideal solutions.l Order and molecularity of reaction, calculation of time period for the decomposition of

radioactive elements by Ist order kinetics.l Le Chatelier’s principle, change in equilibrium with change in pressure and temperature.

l Electrolytic conductance, numerical problems, calculation of Ecello

and Ecell by using Nernst equation.

l Calculation of solubility from solubility product, common ion effect and buffer solution.

Concepts in which Candidates got Confused

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l Nomenclature, isomerism, hybridization and geometry of coordination compounds.l Conversion of organic compounds, conditions and catalyst, named organic reactions.l Polymerisation, biomolecules.Examination Paper 2014l Van't Hoff factor and colligative properties lRaoult’s Law and elevation of boiling point

l Calculation of activation by using slope of the graph

l Unit in numerical l Le Chatelier’s principle

l Isomerism and hybridization in coordination compounds

l Organic conversions l Named reactions l Biomolecules

...contd.

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ðBe regular and systematic in your studies.ðUtilise the additional reading time given to read the question paper.ðRead the question carefully and comprehend what is required before attempting the question.ðAvoid selective study. Give equal importance to all the topics as questions are asked from every unit/chapter.ðLearn to write balanced chemical equations with the conditions/reagents/catalysts used in that reaction (inorganic

and organic chemistry).ðSolve numerical problems following the proper steps i.e. formula, substitution (take all the physical quantities in

same system of unit), calculation and answer with proper/required unit.ðWrite neatly and legibly.ðWrite the correct question numbers as mentioned in the question paper. ðLearn to write the key words in the answer.ðDo not waste time in attempting additional questions given as internal choices.ðKeep enough time for rechecking and avoid careless mistakes.ðPractice IUPAC nomenclature and isomerism of the coordination compounds.ðAvoid selective study - questions are asked from every chapter. ðName organic compounds preferably using the IUPAC Nomenclature. ðAlways solve the numerical problems stepwise i.e., (a) formula (b) substitution (c) calculation (d) answer with

correct unit. ðPractice adequate number of numerical problems. ðAlways write balanced chemical equations with the essential conditions. ðLearn both positive and negative chemical tests of organic compounds. ðIn each topic, learn the definitions with keywords with proper understanding. Write the keyword in your answer. ðRead the full chapter according to the topic given in the scope of syllabus. ðDo not waste time in attempting extra questions given as internal choice. ðStress upon clarifying the concepts of each topic to answer the reasoning type of questions. ðRead questions carefully and understand what is required before attempting the question. ðPractice numerical problems regularly, solve the numerical stepwise with correct formula and write the answer

with correct unit. ðLearn complete and balanced equations along with the conditions, in inorganic and organic compounds ðAvoid selective study. ðPractice writing the IUPAC names for coordination compounds as well as organic compounds. ðLearn both positive and negative chemical tests in organic reactions. ðLearn the shapes and hybridization of molecules with diagram. ðWhile solving numerical problems, proper steps should be followed, i.e. formula, substitution and correct answer

with units. ðAvoid selective study, give equal importance to all the topics.ðPractice more numerical problems. Solve the problems step-wise with correct formula and units.ðLearn both positive and negative chemical tests in organic reactions as it will help in distinguishing between

organic compounds.ðLearn the reactions both organic and inorganic with proper conditions. Always write the correct balanced

equations.ðDo not give dual statements for any answer.ðLearn to write the key words in the answer.ðNumericals should be practiced regularlyðPractice organic conversions with correct conditions. Write the correct balanced chemical equations.

ðRead the question carefully and understand what is required before attempting the answers.

ðStudy chemical tests to distinguish between organic compounds.

ðWrite the formula then substitute the values and calculate the answers with correct units.

Suggestions for Students

CHEMISTRY - Pustakkosh

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