ISC Class 12 Syllabus 2027 Chemistry

ISC YEAR 2027

INDIAN SCHOOL CERTIFICATE
EXAMINATION

CHEMISTRY
(862)

February 2025
____________________________________________________________________________________________

© Copyright, Council for the Indian School Certificate Examinations
All rights reserved. The copyright to this publication and any part thereof solely vests in the Council for the Indian
School Certificate Examinations. This publication and no part thereof may be reproduced, transmitted, distributed or
stored in any manner whatsoever, without the prior written approval of the Council for the Indian School Certificate
Examinations.

Council for the Indian School Certificate Examinations (CISCE)

MISSION STATEMENT

The Council for the Indian School Certificate
Examinations is committed to serving the nation's
children, through high quality educational
endeavours, empowering them to contribute towards
a humane, just and pluralistic society, promoting
introspective living, by creating exciting learning
opportunities, with a commitment to excellence.

ETHOS OF CISCE

Trust and fair play.
Minimum monitoring.
Allowing schools to evolve their own niche.
Catering to the needs of the children.
Giving freedom to experiment with new ideas
and practices.
Diversity and plurality - the basic strength for
evolution of ideas.
Schools to motivate pupils towards the
cultivation of:
Excellence - The Indian and Global
experience.
Values - Spiritual and cultural - to be the bedrock
of the educational experience.
Schools to have an 'Indian Ethos', strong roots in
the national psyche and be sensitive to national
aspirations.

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

11

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 - (f) van’t Hoff factor for the electrolytes
Raoult's law of relative lowering which dissociate and the molecules
of vapour pressure (1st & 2nd), elevation of 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 2. Electrochemistry
on the above.
Electrolytic and electrochemical cells. Redox
(i) Solubility of gases in liquids – Henry’s Law,
reactions in electrochemical cells.
simple numericals based on the above.
Electromotive Force (emf) of a cell, standard
(ii) Raoult’s Law for volatile solutes and non- electrode potential, Nernst equation and its
volatile solutes, ideal solution, non-ideal application to chemical cells. Relation between
solution. Azeotropic mixtures – definition,
Gibbs energy change and emf of a cell.
types, graphical representation, fractional
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 (ii) Galvanic cells - introduction;
depression constant (cryoscopic representation, principle – oxidation
constant) – definition and mathematical reduction. Mechanism of production of
expression (derivation included). electric current in a galvanic cell.
(c) Elevation in boiling point method: molal
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 Standard electrode potential - Measurement
osmosis, isotonic, hypotonic and of standard electrode potential of Zn ++ / Zn,
hypertonic solutions. Comparison Cu ++ / Cu, half cell (using standard
between diffusion and osmosis. hydrogen electrode).
Application of osmotic pressure in the
determination of relative molecular Cell notation – representation.
mass. Factors affecting electrode potential with
explanation - main emphasis on the

12

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,

13

definition of half-life period, derivation of 4. d- and f- Block Elements
expression of half-life period from first order
Position in the periodic table, occurrence,
rate equation.
electronic configuration and characteristics of
Problems based on first order rate equation transition metals, general trends in properties of
and half-life period. the 3d-series of transition metals - metallic
character, ionisation enthalpy, oxidation states,
(vi) Molecularity of the reaction: Meaning –
ionic radii, colour of ions, catalytic property,
physical picture, Relation between order,
magnetic properties, interstitial compounds,
molecularity and the rate of a reaction,
alloy formation, preparation and properties of
Differences between order and molecularity
K 2 Cr 2 O 7 and KMnO 4 .
of a reaction.
Lanthanoids and actinoids.
(vii) The concept of energy: Exothermic and
endothermic reactions, concept of energy (i) d-Block: 3d, 4d and 5d series
barrier, threshold and activation energy,
Study in terms of metallic character, atomic
formation of activated complex, effect of
and ionic radii, ionisation enthalpy,
catalyst on activation energy and reaction
oxidisation states, variable valency,
rate.
formation of coloured compounds, formation
(viii)Collision Theory: Condition for a chemical of complexes, alloy formation.
change – close contact, particles should
(ii) f-Block: 4f and 5f series
collide. Collisions to be effective – optimum
energy and proper orientation during Electronic configuration, atomic and ionic
collision. Energy barrier built-up when the radii, oxidisation states, formation of
collision is about to take place, Activated coloured compounds, formation of
complex formation, difference in energy of complexes, alloy formation. Lanthanoid
the reactant and the product – exothermic contraction and its consequences. Chemical
and endothermic reactions with proper reactivity – with oxygen, hydrogen, halogen,
graphs and labelling. sulphur, nitrogen, carbon and water.
(ix)Mechanism of the reaction: meaning of Actinoids - oxidation states and comparison
elementary reaction, meaning of complex with lanthanoids.
and overall reaction, explanation of the (iii) Potassium permanganate: structure, shape,
mechanism of the reaction, slowest step of equation of extraction from pyrolusite ore, its
the reaction. Relationship between the rate oxidising nature in acidic, basic and neutral
expression, order of reactants and products medium, use in redox titration.
at the rate-determining step, units of rate
constant – explanation with suitable Oxidising nature in acidic [FeSO 4 ,
examples. (COOH) 2 .2H 2 O, KI], basic (KI) and neutral
(H 2 S) mediums to be done.
(x) Effect of temperature on the rate constant of
a reaction: Arrhenius equation – K=Ae-Ea/RT, (iv) Potassium dichromate: structure, shape,
Meaning of the symbols of Arrhenius equation of extraction from chromite ore and
equation, related graph, evaluation of E a and its use in titration. Oxidising nature in acidic,
A from the graph, meaning of slope of the basic and neutral medium, use in redox
graph, conversion from exponential to log titration. Interconversion of chromate and
form of the equation, relationship between dichromate ion (effect of pH).
the increase in temperature and the number
of collisions. Numerical based on Arrhenius 5. Coordination Compounds
equation. Concept of complexes, definition of ligands,
coordination number, oxidation number. IUPAC
nomenclature of mononuclear coordination

14

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

15

- Addition reaction with magnesium (iii) Conversion of one alcohol into another.
(formation of Grignard reagent).
(iv) Distinction between primary, secondary and
- Structure of DDT. tertiary alcohols by Lucas’ Test.
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.

16

Aryl ethers Aromatic aldehyde (Benzaldehyde)
Physical properties – state and solubility. Lab preparation from toluene by oxidation with
chromyl chloride.
Chemical properties – preparation of anisole
(Williamson’s synthesis), electrophilic Physical properties: state and stability.
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,
reactivity of alpha hydrogen in aldehydes and • Reaction with phosphorus pentachloride.
uses. • Cannizzaro reaction.
Preparation: • Benzoin condensation.
• From alcohol. • Perkin’s reaction.
• From alkenes (ozonolysis). • Electrophilic substitution - halogenation,
• From alkynes (hydration). nitration and sulphonation.

• From acid chlorides (Rosenmund’s Test: distinction between aromatic and aliphatic
reduction, reaction with dialkyl cadmium). aldehydes.

• From calcium salt of carboxylic acids. Uses of benzaldehyde.

• From nitriles (Stephen reaction, Grignard’s Carboxylic Acids: Classification, general
reagent). formula and structure of carboxylic group.
Nomenclature, acidic nature, methods of
• From esters. preparation, physical and chemical properties
Physical properties – state and boiling point. and uses.

Chemical properties: Classification of mono and di carboxylic acids
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
(Clemmensen’s reduction, Wolff-Kishner - From Grignard’s reagent.
reduction, Red phosphorus and HI). Physical properties: state, boiling point and
• Base catalysed reactions (with mechanism): solubility.
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
Uses of aldehydes and ketones. dealt with in detail)

17

- Reaction with active metals, alkalies, - Alkylation and acylation with
carbonates and bicarbonates, mechanism.
- Formation of acid derivatives. - Reaction with nitrous acid.
- Decarboxylation (chemical and Kolbe’s - Carbylamine reaction.
electrolytic reaction).
Distinction between primary, secondary
- HVZ reactions. and tertiary amines (Hinsberg’s Test).
- Substitution of benzene ring (meta directive Aniline
effect of carboxylic acid group) nitration and Preparation reduction of nitrobenzene.
sulphonation.
Physical properties – state, solubility and boiling
Tests for acids: formic acid, acetic acid and point.
benzoic acid.
Chemical properties:
Uses of formic acid, acetic acid and benzoic acid. - Reaction with HCl and H 2 SO 4 .
9. Organic compounds containing Nitrogen - Acetylation, alkylation.
- Benzoylation.
Aliphatic Amines: General formula and,
classification of amines. Structure of the amino - Carbylamine reaction.
group, nomenclature. Methods of preparation, - Diazotisation.
physical and chemical properties, uses,
- Electrophilic substitution (bromination,
identification of primary, secondary and tertiary
nitration and sulphonation).
amines.
Tests for aniline.
• Amines
Uses of aniline.
Nomenclature, classification with examples,
Cyanides and Isocyanides
structure, general formula.
Methods of preparation:
Methods of preparation:
Cyanides:
- From alcohol.
- From alkyl halide.
- From alkyl halide. - From amide.
- From cyanide. Isocyanides:
- From amide (Hofmann’s degradation). - From alkyl halide.
- From nitro compounds. From primary amines
- Gabriel phthalimide Synthesis. Diazonium salts: Preparation, chemical
reactions and importance in synthetic organic
Physical properties: comparison between chemistry.
primary, secondary and tertiary amines in
Preparation from aniline;
terms of – state, solubility, boiling point
(hydrogen bonding), comparison with Properties: Sandmeyer’s reaction, Gattermann
alcohols. reaction and Balz – Scheimann reaction,
replacement of diazo group by – H, -OH, -NO 2 ,
Chemical properties: coupling reaction with phenol and aniline.
- Basic character of amines – comparison
between primary, secondary and tertiary 10. Biomolecules
alkyl amines/ ammonia/ aniline. Effect of Carbohydrates – Definition, Classification
substituents on the basic strength of (aldoses and ketoses), monosaccahrides (glucose
aniline and fructose), D-L configuration

18

oligosaccharides (sucrose, lactose, maltose), PAPER II
polysaccharides (starch, cellulose, glycogen);
Importance of carbohydrates. PRACTICAL WORK – 15 Marks
Candidates are required to complete the following
Carbohydrates: definition, classification - mono experiments:
(aldose, ketose), oligo (di, tri, tetra saccharides)
and polysaccharides with examples: reducing 1. Titrations
sugars and non-reducing sugars – examples and Oxidation-reduction titrations: potassium
uses. manganate (VII) / ammonium iron (II) sulphate;
potassium manganate (VII) / oxalic acid.
Establishment of structures for glucose and
fructose (open and cyclic) heating with HI, The candidate may be required to determine the
reaction with hydroxylamine, bromine water, percentage purity of a compound and the number
acetic anhydride, nitric acid and phenyl of molecules of water of crystallization in
hydrazine. hydrated salts. In such experiments sufficient
working details including recognition of the end
Test for glucose and fructose (bromine water test point will be given.
with equation).
Candidates will be required to calculate:
Disaccharides – structures of sucrose, maltose
and lactose (glycosidic linkage). • Molarity
• 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,
polypeptides, proteins, structure of proteins - NOTE: Molarity must be calculated upto 4
primary, secondary, tertiary structure and decimal places at least, in order to avoid error.
quaternary structures (qualitative idea only), OBSERVATION TABLE
denaturation of proteins. Enzymes, hormones -
elementary idea only. S. (A) (B) (B – A)
No.
Proteins: Amino acids – general structure,
Initial Final Difference
classification and zwitter ion formation.
burette burette (ml)
Isoelectric point.
reading reading
Classification of proteins on the basis of (ml) (ml)
molecular shape; primary, secondary, tertiary 1
and quaternary, structures of proteins, 2
denaturation of proteins. (Definitions only. 3
Details and diagrams are not required).
Vitamins - Classification and functions. • Concordant reading is to be used for titre value.
Concordant reading is two consecutive values
Vitamins A, B, C, D, E and K: classification which are exactly the same. Average will not be
(fat soluble and water soluble), deficiency accepted as titre value.
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
Nucleic acids: basic unit – purine and column.
pyrimidine, DNA – structure (double helical), Observations:
RNA (No chemical structure required).
Differences between DNA and RNA. • Pipette size (should be same for all the
candidates at the centre).
• Titre value (concordant value).

19

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

20

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 antacids, etc. and their uses.
FILE - 15 Marks 9. Preparation of soap, nail polish, boot polish,
varnish, nail polish remover, shampoo and
Project Work – 10 Marks
perfumes.
The project work is to be assessed by a Visiting 10. Chemicals and chemical processes in forensic
Examiner appointed locally and approved by the studies.
Council.
11. Insecticides, pesticides and chemical fertilisers.
The candidate is to creatively execute one
project/assignment on an aspect of Chemistry. 12. Ancient Indian medicines and medicinal plants.
Teachers may assign or students may select a topic of 13. Organic Chemistry in Nutrition, Food Science
their choice. Following is only a suggestive list of and Biotechnology.
projects. 14. Effect of Green House Gases.
Suggested Evaluation criteria for Project Work: 15. How Plastics have changed the world, both
socially and economically.
• Introduction / purpose
• 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

21