Chapter 17 Co-Ordination Compounds - JEE Main Chemistry

17 Co-Ordination Compounds

Introduction to co-ordination compounds, Werner’s theory; ligands, coordination number, denticity,
chelation; IUPAC nomenclature of mononuclear coordination compounds, isomerism; Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of coordination compounds (in qualitative analysis, extraction of metals and in biological systems).


Questions

1. Which of the following exists as covalent crystals in the solid state ?
(1) Iodine (2) Silicon (3) Sulphur (4) Phosphorus  (2013)

Answer (2)
 Silicon exists as covalent crystals in the solid state.




Introduction to Coordination Compounds

Redox Reactions And Electrochemistry - JEE Main Chemistry Chapter 8

8 Redox Reactions And Electrochemistry


Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning
oxidation number, balancing of redox reactions. Eectrolytic and metallic conduction, conductance in
electrolytic solutions, specific and molar conductivities and their variation with concentration: Kohlrausch’s law and its applications.
Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half - cell and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator; Fuel cells.


Redox Reactions - Bozeman Science
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Khan Academy - Redox Reactions
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JEE Main Chemistry - Chapter 12. General Principles And Processes Of Isolation Of Metals

12 General Principles And Processes Of Isolation Of Metals

Modes of occurrence of elements in nature, minerals, ores;
Steps involved in the extraction of metals - concentration, reduction (chemical and electrolytic
methods) and refining with special reference to the extraction of Al, Cu, Zn and Fe;
Thermodynamic and electrochemical principles involved in the extraction of metals.


Self Reduction of Copper
Carbon Reduction Method
Electrolytic reduction method

JEE Main Chemistry 2015 Syllabus

JEE Main Chemistry Syllabus Study Plan and Revision Notes:

Basic Concepts of Chemistry,

Study Guide -  Notes

States of Matter,

Study Guide -  Notes

Atomic Structure,

Class XI Portion Study Guide -  Notes

Chemical Bonding and Molecular Structure,

Study Guide -  Notes

Chemical Thermodynamics,

Study Guide -  Notes

Solutions,

Study Guide -  Notes

Equilibrium,

Study Guide -  Notes

Redox Reactions and Electrochemistry

Study Guide -  Notes

Chemical Kinetics,

Study Guide -  Notes

Surface Chemistry,

Study Guide -  Notes

Classification of Elements and Periodicity in Properties,

Study Guide -  Notes

General Principles and Process of isolation of Metals,

Study Guide -  Notes

Hydrogen,

Study Guide -  Notes

S, P, D and F Block Elements,

Study Guide -  Notes

Co-ordination Compounds,

Study Guide -  Notes

Environmental Chemistry,

Study Guide -  Notes

Purification and characteristics of organic compounds,
some basic principles of organic chemistry,

Study Guide -  Notes

Hydrocarbons,

Study Guide -  Notes

Organic Compounds Containing Halogens,

Study Guide -  Notes

Organic Compounds containing oxygen,

Study Guide -  Notes

Polymers,

Study Guide -  Notes

Bio-molecules,

Study Guide -  Notes

Chemistry in Daily Life  and Principles related to piratical chemistry.

Study Guide -  Notes




Detailed Syllabus

JEE MAIN 2015 DETAILED SYLLABUS FOR CHEMISTRY:

Section A: Physical Chemistry

1 Some Basic Concepts in Chemistry

Matter and its nature, Dalton’s atomic theory; Concept of atom, molecule, element and compound; Physical quantities and their measurements in Chemistry, precision and accuracy, significant figures, S.I. Units, dimensional analysis; Laws of chemical combination; Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae; Chemical equations and stoichiometry.

2 States of Matter

Classification of matter into solid, liquid and gaseous states
Gaseous State: Measurable properties of gases; Gas laws - Boyle’s law, Charle’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation; Kinetic theory of gases (only postulates); Concept of average, root
mean square and most probable velocities; Real gases, deviation from Ideal behaviour, compressibility factor and van der Waals equation.

Liquid State: Properties of liquids - vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).

Solid State: Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Bragg’s Law and its applications; Unit cell and lattices, packing in solids (fcc, bcc and hcp lattices), voids, calculations involving unit cell parameters, imperfection in solids; Electrical, magnetic and dielectric properties.

3 Atomic Structure
Thomson and Rutherford atomic models and their limitations; Nature of electromagnetic radiation,
photoelectric effect; Spectrum of hydrogen atom, Bohr model of hydrogen atom - its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model; Dual nature of matter, de-Broglie’s relationship, Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features, concept of atomic orbitals as one electron wave functions; Variation of y and y 2 , with r for
1s and 2s orbitals; various quantum numbers (principal, angular momentum and magnetic quantum numbers) and their significance; shapes of s, p and d - orbitals, electron spin and spin quantum number; Rules for filling electrons in orbitals – aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.

4 Chemical Bonding And Molecular Strucure


Kossel - Lewis approach to chemical bond formation, concept of ionic and covalent bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds;
calculation of lattice enthalpy. Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules.
Quantum mechanical approach to covalent bonding:

Valence bond theory – Its important features, concept of hybridization involving s, p and d orbitals; Resonance.
Molecular Orbital Theory - Its important features, LCAOs, types of molecular orbitals (bonding,
antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, concept of bond order, bond length and bond energy. Elementary idea of metallic bonding. Hydrogen bonding and its applications


5 Chemical Thermodynamics Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.
First law of thermodynamics - Concept of work, heat internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s law of constant heat summation; Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution.
Second law of thermodynamics; Spontaneity of processes; DS of the universe and DG of the system as criteria for spontaneity, DG0 (Standard Gibbs energy change) and equilibrium constant.

6 Solutions

Different methods for expressing concentration of solution - molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of
solutions and Raoult’s Law – Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and nonideal solutions; Colligative properties of dilute solutions - relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, van’t Hoff factor and its significance.


7 Equilibrium

Meaning of equilibrium, concept of dynamic equilibrium. Equilibria involving physical processes: Solid -liquid, liquid - gas and solid – gas equilibria, Henry’s law, general characterics of equilibrium involving physical processes.
Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of DG and DGo in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chatelier’s principle.
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Brnsted - Lowry and Lewis) and their ionization, acid - base equilibria (including multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, solubility of sparingly soluble salts and solubility products, buffer solutions.

8 Redox Reactions And Electrochemistry


Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning
oxidation number, balancing of redox reactions. Eectrolytic and metallic conduction, conductance in
electrolytic solutions, specific and molar conductivities and their variation with concentration: Kohlrausch’s law and its applications.
Electrochemical cells - Electrolytic and Galvanic cells, different types of electrodes, electrode potentials including standard electrode potential, half - cell and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation and its applications; Relationship between cell potential and Gibbs’ energy change; Dry cell and lead accumulator; Fuel cells.


9 Chemical Kinetics

Rate of a chemical reaction, factors affecting the rate of reactions: concentration, temperature, pressure and catalyst; elementary and complex reactions, order and molecularity of reactions, rate law, rate constant and its units, differential and integral forms of zero and first order reactions, their characteristics and half - lives, effect of temperature on rate of reactions – Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no
derivation).


10 Surface Chemistry

Absorption- Physisorption and chemisorption and their characteristics, factors affecting absorption of gases on solids - Freundlich and Langmuir absorption isotherms, absorption from solutions.
Colloidal state - distinction among true solutions, colloids and suspensions, classification of colloids -
lyophilic, lyophobic; multi molecular, macromolecular and associated colloids (micelles), preparation and properties of colloids - Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation and flocculation; Emulsions and their characteristics.


Section – B : Inorganic Chemistry


11 Classificaton Of Elements And Periodicity  In Properties


Modem periodic law and present form of the periodic table, s, p, d and f block elements, periodic trends in properties of elements atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity

12 General Principles And Processes Of Isolation Of Metals

Modes of occurrence of elements in nature, minerals, ores;
Steps involved in the extraction of metals - concentration, reduction (chemical and electrolytic
methods) and refining with special reference to the extraction of Al, Cu, Zn and Fe;
Thermodynamic and electrochemical principles involved in the extraction of metals.


13 Hydrogen

Position of hydrogen in periodic table, isotopes, preparation, properties and uses of hydrogen; Physical and chemical properties of water and heavy water; Structure, preparation, reactions and uses of hydrogen peroxide; Hydrogen as a fuel.


14.  S - Block Elements (Alkali And Alkaline Earth Metals)
Group - 1 and 2 Elements
General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships. Preparation and properties of some important compounds - sodium carbonate and sodium hydroxide; Industrial uses of lime, limestone, Plaster of Paris and cement; Biological significance of Na, K, Mg and Ca.


15. P - Block Elements Group - 13 to Group 18 Elements

General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.
Groupwise study of the p – block elements

Group – 13
Preparation, properties and uses of boron and aluminium; properties of boric acid, diborane, boron
trifluoride, aluminium chloride and alums.

Group – 14
Allotropes of carbon, tendency for catenation; Structure & properties of silicates, and zeolites.

Group – 15
Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus; Preparation, properties, structure and uses of ammonia, nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of phosphorus.

Group – 16
Preparation, properties, structures and uses of ozone; Allotropic forms of sulphur; Preparation, properties, structures and uses of sulphuric acid (including its industrial preparation); Structures of oxoacids of sulphur.

Group – 17
Preparation, properties and uses of hydrochloric acid; Trends in the acidic nature of hydrogen halides;
Structures of Interhalogen compounds and oxides and oxoacids of halogens.

Group –18
Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.


16.  d – and f – Block Elements Transition Elements


General introduction, electronic configuration, occurrence and characteristics, general trends in
properties of the first row transition elements - physical properties, ionizationenthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties and uses of K2Cr 2O7 and KmnO4.
Inner Transition Elements
Lanthanoids - Electronic configuration, oxidation states and lanthanoid contraction.Actinoids - Electronic configuration and oxidation states.

17 Co-Ordination Compounds

Introduction to co-ordination compounds, Werner’s theory; ligands, coordination number, denticity,
chelation; IUPAC nomenclature of mononuclear coordination compounds, isomerism; Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of coordination compounds (in qualitative analysis, extraction of metals and in biological systems).


18 Environmental Chemistry

Environmental pollution - Atmospheric, water and soil.
Atmospheric pollution - Tropospheric and Stratospheric Tropospheric pollutants – Gaseous pollutants: Oxides of carbon, nitrogen and sulphur, hydrocarbons; their sources, harmful effects and prevention; Green house effect and Global warming; Acid rain;

Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects and prevention.
Stratospheric pollution- Formation and breakdown of ozone, depletion of ozone layer - its mechanism and effects.

Water Pollution - Major pollutants such as, pathogens, organic wastes and chemical pollutants; their harmful effects and prevention.
Soil pollution - Major pollutants such as: Pesticides (insecticides,herbicides and fungicides), their harmful effects and prevention. Strategies to control environmental pollution.

Section-C: Organic Chemistry


19 Purification And Characterisation Of Organic Compounds


Purification - Crystallization, sublimation, distillation, differential extraction and chromatography - principles and their applications.
Qualitative analysis - Detection of nitrogen, sulphur, phosphorus and halogens.
Quantitative analysis (basic principles only) - Estimation of carbon, hydrogen, nitrogen, halogens,
sulphur, phosphorus. Calculations of empirical formulae and molecular formulae; Numerical problems in organic quantitative analysis.


20 Some Basic Principles Of Organic Chemistry

Tetravalency of carbon; Shapes of simple molecules - hybridization (s and p); Classification of organic compounds based on functional groups: - C = C - , - C h C – and those containing halogens, oxygen, nitrogen and sulphur; Homologous series; Isomerism - structural and stereoisomerism.
Nomenclature (Trivial and IUPAC) Covalent bond fission - Homolytic and heterolytic: free radicals,
carbocations and carbanions; stability of carbocations and free radicals, electrophiles and nucleophiles.
Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance and
hyperconjugation


21 Hydrocarbons

Classification, isomerism, IUPAC nomenclature, general
methods of preparation, properties and reactions.
Alkanes - Conformations: Sawhorse and Newman
projections (of ethane); Mechanism of halogenation of
alkanes.
Alkenes - Geometrical isomerism; Mechanism of
electrophilic addition: addition of hydrogen, halogens,
water, hydrogen halides (Markownikoff’s and peroxide
effect); Ozonolysis and polymerization.
Alkynes - Acidic character; Addition of hydrogen,
halogens, water and hydrogen halides; Polymerization.
Aromatic hydrocarbons - Nomenclature, benzene -
structure and aromaticity; Mechanism of electrophilic
substitution: halogenation, nitration, Friedel – Craft’s
alkylation and acylation, directive influence of functional
group in mono-substituted benzene


22 Organic Compounds Containing Halogens


General methods of preparation, properties and
reactions; Nature of C-X bond; Mechanisms of
substitution reactions.Uses; Environmental effects of
chloroform & iodoform.


23 Organic Compounds Containing Oxygen

General methods of preparation, properties, reactions
and uses.
Alcohols, Phenols And Ethers Alcohols: Identification
of primary, secondary and
tertiary alcohols; mechanism of dehydration.
Phenols: Acidic nature, electrophilic substitution
reactions: halogenation, nitration and sulphonation,
Reimer - Tiemann reaction.Ethers: Structure.
Aldehyde and Ketones: Nature of carbonyl
group;Nucleophilic addition to >C=O group, relative
reactivities of aldehydes and ketones; Important
reactions such as – Nucleophilic addition reactions
(addition of HCN, NH3 and its derivatives), Grignard
reagent; oxidation; reduction (Wolff Kishner and
Clemmensen); acidity of - hydrogen, aldol condensation,
Cannizzaro reaction, Haloform reaction; Chemical tests
to distinguish between aldehydes and Ketones.
Carboxylic Acids Acidic strength and factors affecting it


24 Organic Compounds Containing Nitrogen


General methods of preparation, properties, reactions
and uses. Amines: Nomenclature, classification,
structure, basic character and identification of primary,
secondary and tertiary amines and their basic character.
Diazonium Salts: Importance in synthetic organic
chemistry.
25 Polymers General introduction and classification of polymers,
general methods of polymerizationaddition
and condensation, copolymerization; Natural and
synthetic rubber and vulcanization; some important
polymers with emphasis on their monomers and uses -
polythene, nylon, polyester and bakelite.

26 Biomolecules

General introduction and importance of biomolecules.
Carbohydrates - Classification: aldoses and ketoses;
monosaccharides (glucose and fructose) and constituent
monosaccharides of oligosacchorides (sucrose, lactose
and maltose).
Proteins - Elementary Idea of - amino acids, peptide
bond, polypeptides; Proteins: primary, secondary,
tertiary and quaternary structure (qualitative idea only),
denaturation of proteins, enzymes.
Vitamins - Classification and functions.
Nucleic Acids - Chemical constitution of DNA and RNA.
Biological functions of nucleic
acids.

27 Chemistry

In Everyday Life Chemicals in medicines - Analgesics, tranquilizers,
antiseptics, disinfectants, antimicrobials, antifertility
drugs, antibiotics, antacids, antihistamins – their
meaning and common examples.Chemicals in food - Preservatives, artificial sweetening
agents - common examples.
Cleansing agents - Soaps and detergents, cleansing
action

28 Principles Related To Practical Chemistry

• Detection of extra elements (N,S, halogens) in organic
compounds; Detection of the following functional groups:
hydroxyl (alcoholic and phenolic), carbonyl (aldehyde
and ketone), carboxyl and amino groups in organic
compounds.
• Chemistry involved in the preparation of the following:
Inorganic compounds: Mohr’s salt, potash alum. Organic
compounds: Acetanilide, pnitroacetanilide, aniline
yellow, iodoform.
• Chemistry involved in the titrimetric excercises - Acids
bases and the use of indicators, oxalic-acid vs KMnO4,
Mohr’s salt vs KMnO4
• Chemical principles involved in the qualitative salt
analysis:
· Cations - Pb2+ , Cu2+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+,
Ba2+, Mg2+, NH4+.
· Anions- CO3 2-, S2-, SO4 2-, NO2-, NO3-, CI -, Br, I.
· (Insoluble salts excluded).
• Chemical principles involved in the following
experiments:
1. Enthalpy of solution of CuSO4
2. Enthalpy of neutralization of strong acid and strong
base.
3. Preparation of lyophilic and lyophobic sols.
4. 4. Kinetic study of reaction of iodide ion with hydrogen
peroxide at room temperature.

JEE Revision - Atomic structure - Basics

Thomson Model

J.J. Thomson studied the properties of cathode rays. Cathode rays were observed in tubes with gas at low pressures when electric charge was applied. The gas starts conducting electricity at low pressure and rays appear. During these studies, Thomson discovered electrons in 1897.

The experiments led to the conclusion that the particles comprising cathode rays were the same irrespective of the material of the cathode and the gas used in discarge tubes, The particles had the same mass and charge. Hence it was concluded that electrons are universal constituents of all matter.


Subsequently proton was also discovered. Rutherford's name can be mentioned in the case of proton as an important researcher.

Thomson proposed that the positive charge is spread over a sphere in which the electrons are embedded. This make the atom neutral. The model was also called Thomson's plum pudding model.

Rutherford model


In 1913, Niels Bohr proposed a model of the atom. He proposed that the electrons in an atom could only be in certain orbits, or energy levels, around the nucleus. Refinement of Bohr theory led to the modern theory of atomic structure based on quantum mechanics.

Wave mechanical model

Magnesium - Chemistry

Magnesium occupies sixth position in order of the abundance on earth.

Magnesium is greyish white metal.

Magnesium is the lightest metal used in industry and it has a density less than two thirds of aluminium. Magnesium is an important alloying metal.

Uses:

Some of the alloys of magnesium containing more than 90% magnesium and 2 to 9% of Aluminium and 1% zinc are used in automobile engines, in aircrafts and in making balances.
Up to 5% magnesium is added to most commercial aluminium alloys (duralumin, magnalium) to improve its resistance to corrosion, mechanical properties and weldability.

Magnesium is used as a reducing agent in metallurgy for the production of metals such as Titanium (Ti), Zirconium (Zr) and Hf.

Magnesium power is used in fireworks.

It is part of alkyl magnesium halide (RMgX), the Grignard reagent and it is useful for making number of organic compounds.

Magnesium hydroxide and magnesium carbonate are used in making toothpastes.

Magnesium hydroxide (milk of magnesia) is used as an antacid. It neutralises excess of acid in stomach and thus it is used as medicine.

Ores of Magnesium

1. Carnallite
2. Magnesite
3. Dolomite
4. Epsom salt or epsomite
5. Langbeinite
6. Asbestos

Extraction of Magnesium from Its Ores

Magnesium is finally extracted by the electrolysis of its molten anhydrous salts.

From Magnesite
The ore MgCO3 is calcined to form the oxide MgO.
The oxide is mixed with carbon and heated in a current of Cl2 gas to form magnesium chloride.
Magnesium chloride is subjected to electrolysis.

Electrolysis of Magnesium chloride

Magnesium chloride is with a mixture of sodium chloride and calcium chloride and heated to 973 K - 1023 K. The mixture melts at this temperature and the electrolysis in carried out in an iron vessel which serves as the cathode.  A graphite rod serves as anode. During the electrolysis an inert gas such as coal gas is passed through the cell to check the oxidation of magnesium. At cathode magnesium will emerge in molten state and at anode chlorine gas will be released. The liquid magnesium (m.p. 924K) is removed from time to time from the top of the vessel.

Magnesium is a s-Block element.

JEE (Advanced) 2013 Chemistry Syllabus

Physical Chemistry

General topics: Concept of atoms and
molecules; Dalton’s atomic theory; Mole
concept; Chemical formulae; Balanced
chemical equations; Calculations (based on
mole concept) involving common oxidation reduction, neutralisation, and displacement
reactions; Concentration in terms of mole
fraction, molarity, molality and normality.

Gaseous and liquid states: Absolute scale of
temperature, ideal gas equation; Deviation
from ideality, van der Waals equation; Kinetic
theory of gases; Average, root mean square
and most probable velocities and their relation
with temperature; Law of partial pressures;
Vapour pressure; Diffusion of gases.
Atomic structure and chemical bonding:
Bohr model, spectrum of hydrogen atom,
quantum numbers; Wave-particle duality, de
Broglie hypothesis; Uncertainty principle;
Qualitative quantum mechanical picture of
hydrogen atom, shapes of s, p and d orbitals;
Electronic configurations of elements (up to
atomic number 36); Aufbau principle; Pauli’s
exclusion principle and Hund’s rule; Orbital
overlap and covalent bond; Hybridisation
(involving s, p and d orbitals only); Orbital
energy diagrams for homonuclear diatomic
species; Hydrogen bond; Polarity in
molecules, dipole moment (qualitative aspects
only); VSEPR model and shapes of molecules
(linear, angular, triangular, square planar,
pyramidal, square pyramidal, trigonal
bipyramidal, tetrahedral and octahedral).
Energetics: First law of thermodynamics;
Internal energy, work and heat, pressurevolume work; Enthalpy, Hess’s law; Heat of
reaction, fusion and vapourization; Second law
of thermodynamics; Entropy; Free energy;
Criterion of spontaneity.

Chemical equilibrium: Law of mass action;
Equilibrium constant, Le Chatelier’s principle
(effect of concentration, temperature and
pressure); Significance of ΔG and ΔGo in
chemical equilibrium; Solubility product,
common ion effect, pH and buffer solutions;
Acids and bases (Bronsted and Lewis
concepts); Hydrolysis of salts.

Electrochemistry: Electrochemical cells and
cell reactions; Standard electrode potentials;
Nernst equation and its relation to ΔG;
Electrochemical series, emf of galvanic cells;
Faraday’s laws of electrolysis; Electrolytic
conductance, specific, equivalent and molar
conductivity, Kohlrausch’s law; Concentration
cells.
Chemical kinetics: Rates of chemical
reactions; Order of reactions; Rate constant;
First order reactions; Temperature dependence
of rate constant (Arrhenius equation).
Solid state: Classification of solids, crystalline
state, seven crystal systems (cell parameters
a, b, c,α,β,γ ), close packed structure of solids
(cubic), packing in fcc, bcc and hcp lattices;
Nearest neighbours, ionic radii, simple ionic
compounds, point defects.

Solutions: Raoult’s law; Molecular weight
determination from lowering of vapour
pressure, elevation of boiling point and
depression of freezing point.

Surface chemistry: Elementary concepts of
adsorption (excluding adsorption isotherms);
Colloids: types, methods of preparation and
general properties; Elementary ideas of
emulsions, surfactants and micelles (only
definitions and examples).

Nuclear chemistry: Radioactivity: isotopes
and isobars; Properties of α,β andγ rays;
Kinetics of radioactive decay (decay series
excluded), carbon dating; Stability of nuclei
with respect to proton-neutron ratio; Brief
discussion on fission and fusion reactions.

Inorganic Chemistry

Isolation/preparation and properties of the
following non-metals: Boron, silicon,
nitrogen, phosphorus, oxygen, sulphur and
halogens; Properties of allotropes of carbon
(only diamond and graphite), phosphorus and
sulphur.

Preparation and properties of the following
compounds: Oxides, peroxides, hydroxides,
carbonates, bicarbonates, chlorides and
sulphates of sodium, potassium, magnesium
and calcium; Boron: diborane, b
and calcium; Boron: diborane, boric acid and
borax; Aluminium: alumina, aluminium chloride
and alums; Carbon: oxides and oxyacid
(carbonic acid); Silicon: silicones, silicates and
silicon carbide; Nitrogen: oxides, oxyacids and
ammonia; Phosphorus: oxides, oxyacids
(phosphorus acid, phosphoric acid) and
phosphine; Oxygen: ozone and hydrogen
peroxide; Sulphur: hydrogen sulphide, oxides,
sulphurous acid, sulphuric acid and sodium
thiosulphate; Halogens: hydrohalic acids,
oxides and oxyacids of chlorine, bleaching
powder; Xenon fluorides.

Transition elements (3d series): Definition,
general characteristics, oxidation states and
their stabilities, colour (excluding the details of
electronic transitions) and calculation of spinonly magnetic moment; Coordination
compounds: nomenclature of mononuclear
coordination compounds, cis-trans and
ionisation isomerisms, hybridization and
geometries of mononuclear coordination
compounds (linear, tetrahedral, square planar
and octahedral).

Preparation and properties of the following
compounds: Oxides and chlorides of tin and
lead; Oxides, chlorides and sulphates of Fe2+,
Cu2+ and Zn2+; Potassium permanganate,
potassium dichromate, silver oxide, silver
nitrate, silver thiosulphate.

Ores and minerals: Commonly occurring ores
and minerals of iron, copper, tin, lead,
magnesium, aluminium, zinc and silver.

Extractive metallurgy: Chemical principles
and reactions only (industrial details excluded);
Carbon reduction method (iron and tin); Self
reduction method (copper and lead);
Electrolytic reduction method (magnesium and
aluminium); Cyanide process (silver and gold).
Principles of qualitative analysis: Groups I to
V (only Ag+, Hg2+, Cu2+, Pb2+, Bi3+, Fe3+,
Cr3+, Al3+, Ca2+, Ba2+, Zn2+, Mn2+ and
Mg2+); Nitrate, halides (excluding fluoride),
sulphate and sulphide.

Organic Chemistry

Concepts: Hybridisation of carbon; Sigma and
pi-bonds; Shapes of simple organic molecules;
Structural and geometrical isomerism; Optical
isomerism of compounds containing up to two
asymmetric centres, (R,S and E,Z
nomenclature excluded); IUPAC nomenclature
of simple organic compounds (only
hydrocarbons, mono-functional and bifunctional compounds); Conformations of
ethane and butane (Newman projections);
Resonance and hyperconjugation; Keto-enol
tautomerism; Determination of empirical and
molecular formulae of simple compounds (only
combustion method); Hydrogen bonds:
definition and their effects on physical
properties of alcohols and carboxylic acids;
Inductive and resonance effects on acidity and
basicity of organic acids and bases; Polarity
and inductive effects in alkyl halides; Reactive
intermediates produced during homolytic and
heterolytic bond cleavage; Formation,
structure and stability of carbocations,
carbanions and free radicals.

Preparation, properties and reactions of
alkanes: Homologous series, physical
properties of alkanes (melting points, boiling
points and density); Combustion and
halogenation of alkanes; Preparation of
alkanes by Wurtz reaction and decarboxylation
reactions.

Preparation, properties and reactions of
alkenes and alkynes: Physical properties of
alkenes and alkynes (boiling points, density
and dipole moments); Acidity of alkynes; Acid
catalysed hydration of alkenes and alkynes
(excluding the stereochemistry of addition and
elimination); Reactions of alkenes with KMnO4
and ozone; Reduction of alkenes and alkynes;
Preparation of alkenes and alkynes by
elimination reactions; Electrophilic addition
reactions of alkenes with X2, HX, HOX and
H2
O (X=halogen); Addition reactions of
alkynes; Metal acetylides.

Reactions of benzene: Structure and
aromaticity; Electrophilic substitution reactions:
halogenation, nitration, sulphonation, FriedelCrafts alkylation and acylation; Effect of o-, mand p-directing groups in monosubstituted
benzenes.

Phenols: Acidity, electrophilic substitution
reactions (halogenation, nitration and
sulphonation); Reimer-Tiemann reaction, Kolbe
reaction.
Characteristic reactions of the following
(including those mentioned above): Alkyl
halides: rearrangement reactions of alkyl
carbocation, Grignard reactions, nucleophilic
substitution reactions; Alcohols: esterification,
dehydration and oxidation, reaction with
sodium, phosphorus halides,
ZnCl2/concentrated HCl, conversion of
alcohols into aldehydes and ketones; Ethers:
Preparation by Williamson’s Synthesis;

Aldehydes and Ketones: oxidation, reduction,
oxime and hydrazone formation; Aldol
condensation, Perkin reaction; Cannizzaro
reaction; Haloform reaction and nucleophilic
addition reactions (Grignard addition);
Carboxylic acids: formation of esters, acid
chlorides and amides, ester hydrolysis;

Amines: basicity of substituted anilines and
aliphatic amines, preparation from nitro
compounds, reaction with nitrous acid, azo
coupling reaction of diazonium salts of
aromatic amines, Sandmeyer and related
reactions of diazonium salts; carbylamine
reaction; Haloarenes: nucleophilic aromatic
substitution in haloarenes and substituted
haloarenes (excluding Benzyne mechanism
and Cine substitution).

Carbohydrates: Classification; mono- and disaccharides (glucose and sucrose); Oxidation,
reduction, glycoside formation and hydrolysis
of sucrose.

Amino acids and peptides: General structure
(only primary structure for peptides) and
physical properties.
Properties and uses of some important
polymers: Natural rubber, cellulose, nylon,
teflon and PVC.

Practical organic chemistry: Detection of
elements (N, S, halogens); Detection and
identification of the following functional groups:
hydroxyl (alcoholic and phenolic), carbonyl
(aldehyde and ketone), carboxyl, amino and
nitro; Chemical methods of separation of
mono-functional organic compounds from
binary mixtures.

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