ISC Class 12 Syllabus 2024 Chemistry

ISC
Syllabus

2024

Revised

Syllabus

CHEMISTRY (862)

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

PAPER I (THEORY) - 70 Marks

S.No. UNIT TOTAL WEIGHTAGE

1. Solutions
Physical Chemistry
2. Electrochemistry
25 Marks
3. Chemical Kinetics

4. d -and f -Block Elements Inorganic Chemistry

5. Coordination Compounds 14 Marks

6. Haloalkanes and Haloarenes
7. Alcohols, Phenols and Ethers
Organic Chemistry
8. Aldehydes, Ketones and Carboxylic Acids
31 Marks
9. Organic Compounds containing Nitrogen
10. Biomolecules
Total 70 Marks

1

PAPER I –THEORY – 70 Marks van’t Hoff- Boyle’s Law, van’t Hoff –
Charles’ Law, van’t Hoff - Avogadro’s
1. Solutions
law.
Study of concentration of solutions of solids in
(e) Abnormal molecular mass: Dissociation
liquids, liquid in liquid, solubility of gases in
and Association with suitable examples
liquids, solid solutions, Colligative properties -
Raoult's law of relative lowering (f) van’t Hoff factor for the electrolytes
of vapour pressure (1st & 2nd), elevation of which dissociate and the molecules
which associate in solution.
boiling point, depression of freezing
Modification of the formula of colligative
point, osmotic pressure. Use of colligative properties based on van’t Hoff factor.
properties in determining molecular masses of Simple problems. Calculation of degree
solutes, abnormal molecular mass association and of dissociation and association.
dissociation, van't Hoff factor. Experimental details not required.
Normality, molality, molarity, mole fraction, Numerical problems based on all the above
ppm, as measures of concentration. Definition of methods. Experimental details not required.
the above with examples. Simple problems based
on the above. 2. Electrochemistry
(i) Solubility of gases in liquids – Henry’s Law, Electrolytic and electrochemical cells. Redox
simple numericals based on the above. reactions in electrochemical cells.
(ii) Raoult’s Law for volatile solutes and non- Electromotive Force (emf) of a cell, standard
volatile solutes, ideal solution, non-ideal electrode potential, Nernst equation and its
solution. Azeotropic mixtures – definition, application to chemical cells. Relation between
types, graphical representation, fractional Gibbs energy change and emf of a cell.
distillation with examples. Conductance in electrolytic solutions, specific,
(iii) Colligative properties – definition and equivalent and molar conductivity, variations of
examples, and its use in determination of conductivity with concentration, graphs;
molecular mass. Kohlrausch's Law of electrolysis and Faraday’s
(a) Relative lowering of vapour pressure: Laws of electrolysis. Dry cell and lead
Definition and mathematical expression accumulator, fuel cells, corrosion.
of Raoult’s Law. Determination of (i) Electrochemical cells: introduction, redox
relative molecular mass by measurement reactions (principle of oxidation and
of lowering of vapour pressure.
reduction in a cell).
(b) Depression in freezing point: molal
depression constant (cryoscopic (ii) Galvanic cells - introduction;
constant) – definition and mathematical representation, principle – oxidation
expression (derivation included). reduction. Mechanism of production of
(c) Elevation in boiling point method: molal electric current in a galvanic cell.
elevation constant (ebullioscopic (iii) Measurement of potential. Single electrode
constant) definition and mathematical potentials.
expression (derivation included). Standard hydrogen electrode (Eo) -
(d) Osmotic pressure: definition and definition, preparation, application and
explanation. Natural and chemical limitations.
semipermeable membranes, reverse
osmosis, isotonic, hypotonic and Standard electrode potential - Measurement
hypertonic solutions. Comparison of standard electrode potential of Zn ++ / Zn,
between diffusion and osmosis. Cu ++ / Cu, half cell (using standard
Application of osmotic pressure in the hydrogen electrode).
determination of relative molecular Cell notation – representation.
mass.
Factors affecting electrode potential with
explanation - main emphasis on the

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temperature, concentration and nature of the (ix) Corrosion: Concept, mechanism of
electrode. electrochemical reaction, factors affecting it
(iv) Electrochemical series. Its explanation on and its prevention.
the basis of standard reduction potential. 3. Chemical Kinetics
Prediction of the feasibility of a reaction. Meaning of Chemical Kinetics – slow and fast
(v) Nernst equation and correlation with the free reactions. Rate of a reaction - average and
energy of the reaction with suitable instantaneous rate (graphical representation).
examples. Factors affecting rate of reaction: surface area,
Prediction of spontaneity of a reaction based nature of reactants, concentration, temperature,
on the cell emf. catalyst and radiation. Order and molecularity
of a reaction, rate law and specific rate constant.
Numericals on standard electrode potential Integrated rate equations and half-life (only for
of half-cells, cell emf, relationship between zero and first order reactions), concept of
free energy and equilibrium constant, collision theory (elementary idea, no
standard electrode potential and free energy. mathematical treatment). Concept of threshold
(vi) Comparison of metallic conductance and and activation energy, Arrhenious equation.
electrolytic conductance. Relationship (i) Meaning of chemical kinetics, Scope and
between conductance and resistance. Specific importance of Kinetics of the reaction, slow
resistance and specific conductance. and fast reactions – explanation in terms of
Cell constant: Calculation of cell constant. bonds.
Meaning of equivalent conductance. (ii) Rate of Reaction: definition, representation
Meaning of molar conductance. General of rate of reaction in terms of reactants and
relationship between specific conductance, products, determination of rate of reactions
molar conductance and equivalent graphically, instantaneous and average rate
conductance (units and graphs). of reaction. Factors affecting rate of
Units, numericals. reaction.
Molar conductance of a weak electrolyte at a (iii) Law of mass Action: statement and meaning
given concentration and at infinite dilution. of active mass. Explanation with an example
Kohlrausch’s Law – definition, applications – general reactions.
and numericals. (iv) Effect of concentration of reactants on the
(vii) Faraday’s laws of Electrolysis. rate of a reaction: Qualitative treatment,
based on the law of mass Action, statement of
Faraday’s First Law of electrolysis. rate law, General rate equation –
Statement, mathematical form. Simple Rate = k(concentration of the reactant)n,
problems. where k is rate constant and n is the order of
Faraday’s Second Law of electrolysis: the reaction, relationship between the rate of
Statement, mathematical form. Simple the reaction with rate constant with respect
problems. to various reactants.
Relation between Faraday, Avogadro’s (v) Order of a reaction: meaning, relation
number and charge on an electron. F = N A e between order and stoichiometric coefficients
should be given (no details of Millikan’s in balanced equations, order as an
experiment are required). experimental quantity, rate equation for zero
order reaction and its unit, mathematical
(viii) Batteries: Primary and Secondary Cells:
derivation of rate equation for first order
Leclanche cell, mercury cell, Lead storage
reaction, characteristics of first order
battery and fuel cell – structure, reactions
reaction – rate constant is independent of the
and uses.
initial concentration, units to be derived,
definition of half-life period, derivation of
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expression of half-life period from first order transition metals, general trends in properties of
rate equation. the 3d-series of transition metals - metallic
character, ionisation enthalpy, oxidation states,
Problems based on first order rate equation
ionic radii, colour of ions, catalytic property,
and half-life period.
magnetic properties, interstitial compounds,
(vi) Molecularity of the reaction: Meaning – alloy formation, preparation and properties of
physical picture, Relation between order, K 2 Cr 2 O 7 and KMnO 4 .
molecularity and the rate of a reaction,
Lanthanoids and actinoids.
Differences between order and molecularity
of a reaction. (i) d-Block: 3d, 4d and 5d series
(vii) The concept of energy: Exothermic and Study in terms of metallic character, atomic
endothermic reactions, concept of energy and ionic radii, ionisation enthalpy,
barrier, threshold and activation energy, oxidisation states, variable valency,
formation of activated complex, effect of formation of coloured compounds, formation
catalyst on activation energy and reaction of complexes, alloy formation.
rate.
(ii) f-Block: 4f and 5f series
(viii)Collision Theory: Condition for a chemical
Electronic configuration, atomic and ionic
change – close contact, particles should
radii, oxidisation states, formation of
collide. Collisions to be effective – optimum
coloured compounds, formation of
energy and proper orientation during
complexes, alloy formation. Lanthanoid
collision. Energy barrier built-up when the
contraction and its consequences. Chemical
collision is about to take place, Activated
reactivity – with oxygen, hydrogen, halogen,
complex formation, difference in energy of
sulphur, nitrogen, carbon and water.
the reactant and the product – exothermic
and endothermic reactions with proper Actinoids - oxidation states and comparison
graphs and labelling. with lanthanoids.
(ix)Mechanism of the reaction: meaning of (iii) Potassium permanganate: structure, shape,
elementary reaction, meaning of complex equation of extraction from pyrolusite ore, its
and overall reaction, explanation of the oxidising nature in acidic, basic and neutral
mechanism of the reaction, slowest step of medium, use in redox titration.
the reaction. Relationship between the rate Oxidising nature in acidic [FeSO 4 ,
expression, order of reactants and products (COOH) 2 .2H 2 O, KI], basic (KI) and neutral
at the rate-determining step, units of rate (H 2 S) mediums to be done.
constant – explanation with suitable
examples. (iv) Potassium dichromate: structure, shape,
equation of extraction from chromite ore and
(x) Effect of temperature on the rate constant of its use in titration. Oxidising nature in acidic,
a reaction: Arrhenius equation – K=Ae-Ea/RT, basic and neutral medium, use in redox
Meaning of the symbols of Arrhenius titration. Interconversion of chromate and
equation, related graph, evaluation of E a and dichromate ion (effect of pH).
A from the graph, meaning of slope of the
graph, conversion from exponential to log 5. Coordination Compounds
form of the equation, relationship between
the increase in temperature and the number Concept of complexes, definition of ligands,
of collisions. Numerical based on Arrhenius coordination number, oxidation number. IUPAC
equation. nomenclature of mononuclear coordination
compounds. Isomerism (structural and stereo).
4. d and f Block Elements Bonding, Werner's theory, VBT and CFT.
Position in the periodic table, occurrence, Colour, magnetic properties and shapes.
electronic configuration and characteristics of Importance of coordination compounds (in

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qualitative analysis, extraction of metals and - Alkene and hydrogen halide.
biological system).
- Alcohols with PX 3 , PCl 5 and SOCl 2 .
(i) Definition of coordination compounds /
- Halide exchange method (Finkelstein and
complex compounds, differences with a
Swarts)
double salt, study of ligands – mono-, bi-, tri-
, tetra-, penta-, hexa- and polydentate, - Silver salt of fatty acids (Hunsdiecker).
chelating ligands, definition of coordination Physical properties: State, melting point, boiling
number, its calculation for a complex point and solubility.
coordination sphere, study of oxidation state
of an element in a complex, its calculation, Chemical properties: nucleophilic substitution
IUPAC rules of nomenclature of reactions (S N 1, S N 2 mechanism in terms of
coordination compounds. primary, secondary and tertiary halides)
Reaction with: sodium hydroxide, water, sodium
(ii) Isomerism – structural, stereo types and iodide, ammonia, primary amine, secondary
examples. amine, potassium cyanide, silver cyanide,
(iii) Valence bond theory of coordination potassium nitrite, silver nitrite, silver salt of fatty
compounds – examples of formation of inner acid and lithium-aluminium hydride.
orbital and outer orbital complexes (high Elimination reaction (Saytzeff’s rule) / β
and low spin, octahedral, tetrahedral and
elimination.
square planar), prediction of magnetic
character. Reaction with metals: sodium and magnesium
(Wurtz’s reaction, Grignard’s reagent
(iv) Crystal field theory – crystal field splitting in
preparation).
tetra and octahedral systems. Explanation of
colour and magnetic character. Chloroform and iodoform: preparation and
properties.
(v) Stability of coordination compounds (explain
stability on the basis of magnitude of K) as Structure of freons.
mentioned above). Preparation of haloarenes by Sandmeyer’s and
(vi) Importance and uses. Gattermann’s reaction, by electrophilic
substitution.
6. Haloalkanes and Haloarenes. Physical properties: State, melting point, boiling
Haloalkanes: General formula, nomenclature point and solubility.
and classification. Nature of C–X bond, Chemical properties:
physical and chemical properties, mechanism
of substitution reactions, optical rotation. - Electrophilic substitution (chlorination
nitration and sulphonation) with mechanism.
Haloarenes: Basic idea, nature of C–X bond,
substitution reactions (directive influence of - Nucleophilic substitution (replacement of
halogen in monosubstituted compounds only). chlorine with -OH, -NH 2 ) with mechanism.
Uses and environmental effects of - - Reduction to benzene.
dichloromethane, trichloromethane, tetra- - Wurtz-Fittig reaction.
chloromethane, iodoform, freons and DDT.
- Fittig reaction.
Nature of C-X bond
- Addition reaction with magnesium
Naming the halogen derivatives of alkanes by (formation of Grignard reagent).
using common system and IUPAC system for
mono, di and tri-halo derivatives. - Structure of DDT.
Preparation of haloalkanes from:
- Alkane and halogen.

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7. Alcohols, Phenols and Ethers Phenols: Classification and nomenclature.
Methods of preparation, physical and chemical
Alcohols: Classification, general formula,
properties, acidic nature of phenol, electrophilic
structure and nomenclature. Methods of
substitution reactions, uses of phenols.
preparation, physical and chemical properties
(of primary alcohols only), identification of Preparation of phenol from diazonium salt,
primary, secondary and tertiary alcohols, chlorobenzene (Dow’s process) and from
mechanism of dehydration, uses with special benzene sulphonic acid.
reference to methanol and ethanol.
Manufacture from Cumene.
(i) Classification into monohydric, dihydric and
Physical properties: state and solubility.
polyhydric alcohols, general formulae,
structure and nomenclature of alcohols. Chemical properties:
Difference between primary, secondary and
- Acidic character of phenol.
tertiary alcohols in terms of structure,
physical properties and chemical properties. - Reaction with sodium hydroxide.
(ii) Methods of preparation: - Reaction with sodium.
- Hydration of Alkenes – direct hydration, - Reaction with zinc.
indirect hydration, hydroboration - Reaction with acetyl chloride and acetic
oxidation. anhydride.
- From Grignard’s reagent. - Reaction with phosphorus penta chloride.
- Hydrolysis of alkyl halides. - Bromination, nitration and sulphonation
- Reduction of carbonyl compounds. (Electrophilic substitution reactions).
- From primary amines. - Kolbe’s reaction (formation of salicylic
acid).
Manufacture of methanol by Bosch process
and ethanol by fermentation of - Reimer – Tiemann reaction
carbohydrates, chemical equations required - Test for phenol – FeCl 3 test, azo dye test.
(only outline of the method of manufacture,
detail not required). Aliphatic Ethers: General formula, structure and
nomenclature. Methods of preparation, physical
Properties: and chemical properties, uses.
- Acidic nature of alcohols: Ethers: structure of ethereal group.
- Reaction with sodium. Preparation from alcohol (Williamson’s
- Esterification with mechanism. synthesis).
- Reaction with hydrogen halides. Physical properties: state, miscibility.
- Reaction with PCl 3, PCl 5 , and SOCl 2 . Chemical properties:
- Reaction with acid chlorides and acid - Reaction with chlorine.
anhydrides - Oxidation (peroxide formation).
- Oxidation. - Reaction with HI.
- Dehydration with mechanism. - Reaction with PCl 5 .
Uses of alcohols. Aryl ethers
(iii) Conversion of one alcohol into another. Physical properties – state and solubility.
(iv) Distinction between primary, secondary and Chemical properties – preparation of anisole
tertiary alcohols by Lucas’ Test. (Williamson’s synthesis), electrophilic
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substitution (halogenation, nitration and Chemical properties:
Friedel-Crafts reaction.)
• Oxidation and reduction.
Uses of ether.
• Nucleophilic addition reaction (hydrogen
8. Aldehydes, Ketones and Carboxylic Acids cyanide and sodium bisulphite).

Aldehydes and Ketones: Nomenclature, • Reactions with ammonia and its derivatives
structure of methods of preparation of (hydroxyl amine, hydrazine and phenyl
aldehydes and ketones, physical and chemical hydrazine).
properties, mechanism of nucleophilic addition, • Reaction with phosphorus pentachloride.
reactivity of alpha hydrogen in aldehydes and
uses. • Cannizzaro reaction.
Preparation: • Benzoin condensation.
• From alcohol. • Perkin’s reaction.
• From alkenes (ozonolysis). • Electrophilic substitution - halogenation,
nitration and sulphonation.
• From alkynes (hydration).
Test: distinction between aromatic and aliphatic
• From acid chlorides (Rosenmund’s aldehydes.
reduction, reaction with dialkyl cadmium).
Uses of benzaldehyde.
• From calcium salt of carboxylic acids.
Carboxylic Acids: Classification, general
• From nitriles (Stephen reaction, Grignard’s formula and structure of carboxylic group.
reagent). Nomenclature, acidic nature, methods of
• From esters. preparation, physical and chemical properties
and uses.
Physical properties – state and boiling point.
Classification of mono and di carboxylic acids
Chemical properties: with examples.
• Nucleophilic addition reactions with Preparation of aliphatic and aromatic carboxylic
mechanism (ammonia and its derivatives, acid:
HCN, NaHSO 3 and Grignard’s reagent).
- From alcohols, aldehydes.
• Oxidation reactions, iodoform reaction.
- From nitriles.
• Reduction: reduction to alcohol and alkanes - From Grignard’s reagent.
(Clemmensen’s reduction, Wolff-Kishner
reduction, Red phosphorus and HI). Physical properties: state, boiling point and
solubility.
• Base catalysed reactions (with mechanism):
Aldol condensation, cross Aldol Chemical properties:
condensation, Cannizzaro’s reaction. - Acidic character: (aliphatic, aromatic
Tests: difference between formaldehyde and carboxylic acids with the effect of
acetaldehyde; aldehydes and ketones. substituents on the acidic character – to be
dealt with in detail)
Uses of aldehydes and ketones.
- Reaction with active metals, alkalies,
Aromatic aldehyde (Benzaldehyde) carbonates and bicarbonates,
Lab preparation from toluene by oxidation with - Formation of acid derivatives.
chromyl chloride.
- Decarboxylation (chemical and Kolbe’s
Physical properties: state and stability. electrolytic reaction).

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- HVZ reactions. Aniline
- Substitution of benzene ring (meta directive Preparation reduction of nitrobenzene.
effect of carboxylic acid group) nitration and Physical properties – state, solubility and boiling
sulphonation. point.
Tests for acids: formic acid, acetic acid and Chemical properties:
benzoic acid. - Reaction with HCl and H 2 SO 4 .
Uses of formic acid, acetic acid and benzoic acid. - Acetylation, alkylation.
- Benzoylation.
9. Organic compounds containing Nitrogen
- Carbylamine reaction.
Aliphatic Amines: General formula and,
classification of amines. Structure of the amino - Diazotisation.
group, nomenclature. Methods of preparation, - Electrophilic substitution (bromination,
physical and chemical properties, uses, nitration and sulphonation).
identification of primary, secondary and tertiary Tests for aniline.
amines.
Uses of aniline.
• Amines
Cyanides and Isocyanides
Nomenclature, classification with examples, Methods of preparation:
structure, general formula.
Cyanides:
Methods of preparation:
- From alkyl halide.
- From alcohol. - From amide.
- From alkyl halide. Isocyanides:
- From cyanide. - From alkyl halide.
- From amide (Hofmann’s degradation). From primary amines
- From nitro compounds. Diazonium salts: Preparation, chemical
reactions and importance in synthetic organic
- Gabriel phthalimide Synthesis. chemistry.
Physical properties: comparison between Preparation from aniline;
primary, secondary and tertiary amines in Properties: Sandmeyer’s reaction, Gattermann
terms of – state, solubility, boiling point reaction and Balz – Scheimann reaction,
(hydrogen bonding), comparison with replacement of diazo group by – H, -OH, -NO 2 ,
alcohols. coupling reaction with phenol and aniline.
Chemical properties:
10. Biomolecules
- Basic character of amines – comparison
between primary, secondary and tertiary Carbohydrates – Definition, Classification
alkyl amines/ ammonia/ aniline. Effect of (aldoses and ketoses), monosaccahrides (glucose
substituents on the basic strength of and fructose), D-L configuration
aniline oligosaccharides (sucrose, lactose, maltose),
polysaccharides (starch, cellulose, glycogen);
- Alkylation and acylation with Importance of carbohydrates.
mechanism.
Carbohydrates: definition, classification - mono
- Reaction with nitrous acid. (aldose, ketose), oligo (di, tri, tetra saccharides)
- Carbylamine reaction. and polysaccharides with examples: reducing
sugars and non-reducing sugars – examples and
Distinction between primary, secondary uses.
and tertiary amines (Hinsberg’s Test).
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Establishment of structures for glucose and The candidate may be required to determine the
fructose (open and cyclic) heating with HI, percentage purity of a compound and the number
reaction with hydroxylamine, bromine water, of molecules of water of crystallization in
acetic anhydride, nitric acid and phenyl hydrated salts. In such experiments sufficient
hydrazine. working details including recognition of the end
point will be given.
Test for glucose and fructose (bromine water test
with equation). Candidates will be required to calculate:
Disaccharides – structures of sucrose, maltose • Molarity
and lactose (glycosidic linkage). • Concentration in grams L-1 / molecular mass
Polysaccharides – starch, cellulose, glycogen. • Number of molecules of water of
Proteins – structural units of proteins. Basic crystallisation/ percentage purity.
idea of - amino acids, peptide bond, NOTE: Molarity must be calculated upto 4
polypeptides, proteins, structure of proteins - decimal places at least, in order to avoid error.
primary, secondary, tertiary structure and
OBSERVATION TABLE
quaternary structures (qualitative idea only),
denaturation of proteins. Enzymes, hormones - S. (A) (B) (B – A)
elementary idea only. No.
Proteins: Amino acids – general structure, Initial Final Difference
classification and zwitter ion formation. burette burette (ml)
Isoelectric point. reading reading
(ml) (ml)
Classification of proteins on the basis of 1
molecular shape; primary, secondary, tertiary 2
and quaternary, structures of proteins, 3
denaturation of proteins. (Definitions only.
Details and diagrams are not required). • Concordant reading is to be used for titre value.
Vitamins - Classification and functions. Concordant reading is two consecutive values
which are exactly the same. Average will not be
Vitamins A, B, C, D, E and K: classification accepted as titre value.
(fat soluble and water soluble), deficiency
diseases. (Chemical names and structures are not • The table is to be completed in ink only. Pencil is
required). not to be used.

Nucleic Acids - DNA and RNA. • Overwriting will not be accepted in the tabular
column.
Nucleic acids: basic unit – purine and Observations:
pyrimidine, DNA – structure (double helical),
RNA (No chemical structure required). • Pipette size (should be same for all the
Differences between DNA and RNA. candidates at the centre).
• Titre value (concordant value).
PAPER II
2. Study of the rate of reaction
PRACTICAL WORK – 15 Marks The candidates will be required, having been
Candidates are required to complete the following given full instructions, to carry out an experiment
experiments: on the rate of reaction, e.g. reaction between
sodium thiosulphate and hydrochloric acid
1. Titrations (using different concentrations for either),
Oxidation-reduction titrations: potassium magnesium and dil. sulphuric acid/ dil.
manganate (VII) / ammonium iron (II) sulphate; hydrochloric acid (using different
potassium manganate (VII) / oxalic acid. concentrations).

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• Graph of volume vs. time and its 7. Qualitative analysis
interpretation. Qualitative analysis: identification of single salt
• Relationship between concentration and rate, containing one anion and one cation:
volume and rate and time and rate.
Anions: CO 3 2-, NO 2 -, S2-, SO 3 2-, SO 4 2-, NO 3 -,
3. Identification of the following compounds and CH 3 COO-, Cl-, Br-, I-, C 2 O 4 2-, PO 4 3-.
functional groups based on observations
Cations: NH 4 +, Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Mn2+
• Alcoholic group - glycerol , Ni2+, Co2+, Ba2+, Sr2+, Ca2+, Mg2+.
• Aldehyde group- formaldehyde
NOTE:
• Ketonic group – acetone
Chromyl chloride test not to be performed.
• Carboxylic group – benzoic acid
For wet test of anions, sodium carbonate
• Amino group - aniline extract must be used (except for carbonate).
*Please Note: Carbylamine and acrolein tests (Insoluble salts such as lead sulphate, barium
should not be performed. sulphate, calcium sulphate, strontium sulphate
The student should learn to differentiate between will not be given).
colours, solution, ring and precipitate.
Anions: Dilute acid group – CO 3 2-, NO 2 -, S2-,
4. Characteristic tests of carbohydrates and SO 3 2-
proteins
Concentrated Acid Group – NO 3 -, Cl-,
• Carbohydrates – glucose Br-, I-, CH 3 COO-.
• Proteins – powdered milk Special Group - SO 4 2-, PO 4 3-, C 2 O 4 2-.
Identification should be of ‘Carbohydrate’ and
Cations: Group Zero: NH 4 +
‘Protein’ not of individual substances.
5. Experiments related to pH change using pH Group I: Pb2+
paper or universal indicator. Group II : Cu2+, Pb2+
• Determination of pH of some solutions Group III: Al3+, Fe3+
obtained from fruit juice, solutions of known Group IV: Zn2+, Mn2+, Ni2+, Co2+
and varied concentrations of acids, bases and
salts. Group V: Ba2+, Sr2+, Ca2+
• Comparison of pH of the solutions of strong Group VI: Mg2+
and weak acids of the same concentration. NOTE:
Use of universal indicator/pH paper must be • Formal analytical procedure is required for
taught to the students. Qualitative Analysis.
6. Electrochemistry
• Specific solvent for O.S. to be used;
Setting up a simple voltaic cell.
• Before adding Group III reagents to the
Variation of cell potential in Zn/Zn2+//Cu2+/Cu filtrate of Group II, H 2 S must be removed
with change in concentration of electrolyte followed by boiling with conc. Nitric acid.
(CuSO 4 , ZnSO 4 ) at room temperature.
• The right order for buffer (NH 4 Cl and
NH 4 OH) must be used.
• 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).

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PATTERN OF CHEMISTRY Suggested Assignments:
PRACTICAL PAPER 1. Amino acids: Peptides, structure and
Questions in the practical paper will be set as classification, proteins structure and their role in
follows: the growth of living beings.
Question 1 Volumetric Analysis 2. Nucleic Acid: DNA and RNA – their structure.
Question 2 Any one or a combination of the Unique nature. Importance in evolution and their
following experiments: characteristic features.
• Study of the rate of reaction. 3. Carbohydrates and their metabolism, Blood -
• Identification of the organic haemoglobin and respiration.
compounds and functional groups 4. Vitamins and hormones
based on observations. 5. Simple idea of chemical evolution.
• Characteristic tests of carbohydrates
6. Natural polymers (any five) - structure,
and proteins.
characteristics, uses. Synthetic polymers (any
• Experiments related to pH
five) - method of preparation, structure,
determination using pH paper or
characteristics and uses.
universal indicator.
• Electrochemistry. 7. Types of Dyes - methods of preparation,
Question 3 Qualitative Analysis (single salt). characteristics and uses.
8. Chemicals in medicines: antiseptics, antibiotics,
PROJECT WORK AND PRACTICAL FILE - antacids, etc. and their uses.
15 Marks 9. Preparation of soap, nail polish, boot polish,
Project Work – 10 Marks varnish, nail polish remover, shampoo and
The project work is to be assessed by a Visiting perfumes.
Examiner appointed locally and approved by the 10. Chemicals and chemical processes in forensic
Council. studies.
The candidate is to creatively execute one 11. Insecticides, pesticides and chemical fertilisers.
project/assignment on an aspect of Chemistry. 12. Ancient Indian medicines and medicinal plants.
Teachers may assign or students may select a topic of
their choice. Following is only a suggestive list of 13. Organic Chemistry in Nutrition, Food Science
projects. and Biotechnology.
14. Effect of Green House Gases.
Suggested Evaluation criteria for Project Work:
15. How Plastics have changed the world, both
• Introduction / purpose socially and economically.
• Contents Practical File – 5 Marks
• Analysis/ material aid (graph, data, structure, pie
The Visiting Examiner is required to assess students
charts, histograms, diagrams, etc.)
on the basis of the Chemistry Practical file
• Presentation maintained by them during the academic year.
• Bibliography

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 IA IIA IIIB IVB VB VIB VIIB VIII IB IIB IIIA IVA VA VIA VIIA 0
notation
New 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
notation

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