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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
*Solutions can be downloaded from www.oswaalbooks.com or by Scanning the QR Code inside.
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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.
(10)
...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).
(11)
...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.
(12)
...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.
(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.
(13)
...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.
(14)
...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.
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.
(15)
...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.
Chemical properties:
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.
Chemical properties:
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.
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.
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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.
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.
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.
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...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
(20)
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.
Examination Paper 2018
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.
Examination Paper 2016
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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Examination Paper 2015
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.
Examination Paper 2014
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
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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