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About JEE Main Chemistry Exam

JEE Mains Chesmistry is part of the JEE entrance exam which is used to measure a student's capability in Sciences, mathematics and/or architecture. Students are granted admission into the prestigous IITs and other institutions in fields related to science and arrchitecture on the basis of their senior secondary scores and JEE advanced exam scores.


JEE Main Chemistry marking scheme

The exam is now conducted on computers. The stuudents have to answer a mix of multiple choice questions and numerical answer questions in each of the three sections (physics, chemistry and mathematics). 4 marks will be awarded for each correct answer. Every incorrect answer wil incur a penalty of -1 mark.

Marks subject
100 Chemistry
100 Physics
100 Maths

The Exam


The JEE Main Chemistry exam has 2 sections

Section I - 20 questions.

MCQs are either discreet questions or sets of question, Questions are based on the knowledge of Chemistry and Science practices outlined in JEE Main Chemistry course. These questions are a mix of theoretical and numerical questions ranging from eassy to moderate difficulty. The MCQs also form the bulk of the total questions in each subject, thereby being the quickest source of marks for each student.


Section II - 10 questions

The student has to answer 5 questions out of these 10 questions

This section contains questions with numerical answers that the student must input. Usually these questions are time consuming and difficult to solve. Answering nomenclature (such as number of decimal places, rounding of numbers allowed) is often provided with these questions.

JEE Exam Calculator Policy

Calculators are not permitted in in the JEE Chemistry exam. Any attempt to use calculator will be considered as cheating and the student's exam will be terminated immediately. Thus, we highly recommend memorizing formulas, values and basic calculations beforehand.



JEE Main Chemistry Exam Course Content

Section A - Physical Chemistry


UNIT I: SOME BASIC CONCEPTS IN CHEMISTRY.

1.1 Matter and its Nature and Classification of matter into solid, liquid and gaseous states.

1.2 Dalton's Atomic Theory.

1.3 Concept of Atom, Molecule, Element And Compound .

1.4 Physical Quantities And their Measurements in Chemistry and S.I. Units.

1.5 Precision, Accuracy and Types of Errors.

1.6 Scientific Notations and Rounding off Rules.

1.7 Significant Figures.

1.8 Dimensional Analysis.

1.9 Fundamental Laws of Chemical Combination.

1.10 Average Atomic Masses and Molecular Masses.

1.11 Mole Concept and Molar mass.

1.12 Percentage Composition, Empirical and Molecular formulae.

1.13 Types of Equations and Balancing Different types of Chemical equations.

1.14 Measuring Concentrations of Solutions --Molarity, Molality ,Mole Fraction, Percent by Mass ,Ppm,Ppb and percent by Polume.

1.15 Stoichiometry.

1.16 Limiting reactant and excess reactant.

1.17 Theoretical yield, Actual and percent yield.


UNIT 2: STATES OF MATTER


2.1 Gaseous State.
2.1.1- Measurable properties of gases and their units.

2.1.2- Gas laws -Boyle's Law, Charle’s law,Avogadro's law, Gay Lusaacc's law,Combined gas laws and Concept of Absolute scale of temperature.

2.1.3- Dalton's law of Partial Pressure.

2.1.4- Ideal gas Equation and its Application.

2.1.5- Kinetic Theory of Gases (Only Postulates) with reasoning.

2.1.6- Maxwell Boltzmann Distribution Curves for Kinetic Energy and Velocities.

2.1.7- Concept of Average, Root Mean Square and most Probable Velocities.

2.1.8- Effusion, Diffusion and Graham’s law,.

2.1.9- Deviation from Ideal Behaviour and Real gases.

2.1.10- Compressibility Factor and Van der Waals Equation.


2.2 Liquid State:

2.2.1- Properties of Liquids - Vapour Pressure.

2.2.2- Relation Between Vapour Pressure and Boiling Point.

2.2.3- Viscosity and Surface Tension.

2.2.4- Effect of Temperature on Properties of Liquids - (Qualitative Treatment only).


2.3-Solid State:

2.3.1- Classification of solids on the basis of interparticle attractive forces- Molecular solids, Ionic solids, Covalent network of solids, Metallic solids.

2.3.2- Amorphous and Crystalline Solids (Elementary idea).;

2.3.3- Bragg's Law and its Applications.

2.3.4- Unit cell and lattices.

2.3.5- Packing in solids (fcc, bcc and hcp lattices) and voids

2.3.6- Calculations Involving Unit cell Parameters.

2.3.7- An Kmperfection in Solids.

2.3.8- Electrical and Magnetic Properties of Solids.


UNIT 3: ATOMIC STRUCTURE


3.1 Thomson and Rutherford Atomic Models and Their Limitations.

3.2 Nature of Electromagnetic Radiation.

3.3 Photoelectric Effect.

3.4 Spectrum of the Hydrogen atom, Emission and Absorption Spectrum.

3.5 Bohr model of a hydrogen atom – its Postulates.

3.6 Derivation of the Relations for the Energy of the Electron and radii of the different orbits.

3.7 Limitations of Bohr's model.

3.8 Dual nature of matter.

3.9 De Broglie's Relationship.

3.10 Heisenberg Uncertainty Principle.

3.11 Elementary Ideas of qQuantum Mechanics, Quantum Mechanics.

3.12 The Quantum Mechanical Model of the Atom and its Important features.

3.13 Concept of atomic Orbitals as one-Electron wave functions.

3.14 Variation of ψ1 and ψ 2 with r for 1s and 2s orbitals.

3.15 Four quantum numbers (Principal, Angular Momentum and Magnetic quantum numbers) and their significance.

3.16 Shapes of s, p and d - Orbitals, Electron spin and Spin Quantum number

3.17 Rules for filling electrons in orbitals – Aufbau principle.

3.18 Pauli's Exclusion Principle and Hund's rule.


3.19 Electronic Configuration of Elements.

3.20 Extra stability of half-filled and completely filled orbitals.


3.21 Electronic configuration of ions.


UNIT 4: CHEMICAL BONDING


4.1 -MOLECULAR STRUCTURE
4.1.1- Kossel - Lewis’s approach to chemical bond formation.

4.1.2- The Concept of ionic and Covalent Bonds..


4.2 -Ionic Bonding:

4.2.1- Formation of ionic bonds.

4.2.2- Factors Affecting the formation of ionic bonds.

4.2.3- Calculation of lattice enthalpy. .


4.3-Covalent Bonding:

4.3.1- Concept of electronegativity.

4.3.2- Fajan’s rule.

4.3.3- Dipole moment.

4.3.4- Formal charges.

4.3.5- Valence Shell Electron Pair Repulsion (VSEPR ) theory,.

4.3.6- Shapes of simple molecules.

4.3.7- Polarity of molecules.

4.3.8- Types of Intermolecular forces of attractions.

4.3.9- Hydrogen bonding and its applications.


4.4-Quantum mechanical approach to covalent bonding:

4.4.1- Valence bond theory -its important features.

4.4.2- The concept of hybridization involving s, p and d orbitals.

4.4.3- Sigma and pi-bonds.

4.4.4- Bond length and bond energy,

4.4.5- Resonance.


4.5-Molecular Orbital Theory –

4.5.1- LCAOs-Its important features.

4.5.2- Types of Molecular Orbitals (Bonding, Antibonding).

4.5.3- Molecular Orbital Electronic Configurations of homonuclear diatomic molecules.

4.5.4- The concept of bond order.


4.6. Metallic bonding –

4.6.1- Elementary idea of metallic bonding.

4.6.2- Strength of metallic bonding.

4.6.3- Alloys and types of alloys.


UNIT 5: CHEMICAL THERMODYNAMICS


5.1 -Fundamentals of thermodynamics:
5.1.1- System and surroundings.

5.1.2- Sign convention in thermochemistry.

5.1.3- Extensive and intensive properties.

5.1.4- Meaning of standard state in thermochemistry.

5.1.5- State functions.

5.1.6- Types of processes.

5.1.7- Exothermic and endothermic processes.


5.2-The first law of thermodynamics -

5.2.1- Concept of work, heat and internal energy.

5.2.2- Enthalpy and enthalpy of reactions.

5.2.3- Specific heat capacity, heat capacity and molar heat capacity.

5.2.4- Cup calorimeter and bomb calorimeter.

5.2.5- Hess’s law of constant heat summation.

5.2.6- Meaning of Enthalpies of bond dissociation, combustion, formation, atomization, sublimation, phase transition, hydration, ionization and solution.

5.2.7- Born Haber’s Cycle.


5.3-The second law of thermodynamics -

5.3.1- Spontaneous and non-spontaneous process.

5.3.2- Entropy of the universe.

5.3.3- Gibbs free energy.

5.3.4- Relation between Gibbs free energy , enthalpy and entropy with temperature as the only variable.

5.3.5- ∆G0 of the system as criteria for spontaneity.

5.3.6- Relation between ∆G0(Standard Gibbs energy change) and equilibrium constant.

5.3.7- Relation between ∆G0(Standard Gibbs energy change) and cell potential.


UNIT 6: SOLUTIONS


6.1 Different methods for expressing the concentration of solution - molality,molarity, mole fraction, percentage (by volume and mass both),

6.2 the vapour pressure of solutions .

6.3 Raoult's Law -Ideal and non-ideal solutions, .

6.4 Vapour pressure - composition, plots for ideal and non-ideal solutions.

6.5 Meaning of Colligative properties of dilute solutions.

6.6 Relative lowering of vapour pressure.

6.7 Depression of freezing point.

6.8 The elevation of boiling point n.

6.9 Osmotic pressure.

6.10 Depression of freezing point.

6.11 Abnormal value of molar mass.

6.12 Van’t Hoff factor and its significance.


UNIT 7: EQUILIBRIUM


7.1 Meaning of Equilibrium.

7.2 The Concept of Dynamic Equilibrium.


7.1-Equilibria involving physical processes:

7.1.1- Solid-liquid, Liquid - Gas and Solid-gas Equilibria.

7.1.2- Henry's Law and its Applications.

7.1.3- General Characteristics of Equilibrium Involving Physical processes.


7.2-Equilibrium involving chemical processes:

7.2.1- Law of Chemical Equilibrium.

7.2.2- Equilibrium Constants (Kp and Kc) and their.

7.2.3- Significance.

7.2.4- The Significance of ∆G and ∆Go in chemical equilibrium.

7.2.5- Le-Chatelier’s principle-factors affecting equilibrium constant.
(a)Concentration.
(b)Pressure.
(c)Temperature.
(d)The effect of catalyst.


7.3-Ionic equilibrium: -

7.3.1- Weak and strong electrolytes and ionization of electrolytes.

7.3.2- Various concepts of acids and bases
(a) Arrhenius.
(b) Bronsted - Lowry.
(c) Lewis.

7.3.3- Strength of acids and bases and their ionization.

7.3.4- Acid-base equilibria (Including multistage ionization).

7.3.5- Ionization constants and ionization constant Ka , Kb.

7.3.6- Auto ionization of water and ionization constant of water -Kw.

7.3.7- PH scale, pOH ,Pka ,PKb and pKw and their relationship.

7.3.8- Common ion effect.

7.3.9- Hydrolysis of Salts and pH of their solutions.

7.3.10- The Solubility of Sparingly soluble salts and.

7.3.11- Solubility Products.

7.3.12- Buffer Solutions and their pH.


UNIT 8: REDOX REACTIONS AND ELECTROCHEMISTRY


8.1 Electronic concepts of oxidation and reduction and redox reactions.

8.2 Oxidation number, rules for assigning oxidation number.

8.3 Balancing of redox reactions.
(a)Half reaction method.
(b)Oxidation number method. .

8.4 Electrolytic and Metallic Conduction,Conductance in Electrolytic solutions.

8.5 Molar Eonductivities and their Variation with Concentration.

8.6 Kohlrausch’s law and its Applications.

8.7 Electrochemical cells –
(a)Electrolytic.
(b)Galvanic cells.

8.8 Different types of electrodes and electrode potentials including standard electrode potential.

8.9 Half - cell and cell reactions.

8.10 Emf of a Galvanic cell and its measurement.

8.11 Nernst equation and its applications.

8.12 Relationship between cell potential and Gibbs' energy change.

8.13 Dry cell and lead accumulator.

8.14 Fuel cells.


UNIT 9: CHEMICAL KINETICS


9.1 Rate of a chemical reaction.

9.2 Factors affecting the rate of reactions,
(a) Concentration.
(b) Temperature.
(c) Pressure.
(d) Surface area.
(e) Catalyst. .

9.3 Elementary and complex reactions.

9.4 Order and molecularity of reactions.

9.5 Rate law, rate constant and its units.

9.6 Ddifferential and integral forms of zero and first-order reactions, their characteristics and half-lives.

9.7 The effect of temperature on the rate of reactions.

9.8 Arrhenius theory, activation energy and its calculation.

9.9 Collision theory of bimolecular gaseous reactions (no derivation).


UNIT 10: SURFACE CHEMISTRY



10.1 Adsorption- Physisorption and chemisorption and their characteristics.

10.2 Factors affecting adsorption of gases on solids – .

10.3 Freundlich and Langmuir adsorption isotherms.

10.4 Adsorption from solutions.

10.5 Catalysis - Homogeneous and Heterogeneous.

10.6 Activity and Selectivity of Solid Catalysts.

10.7 Enzyme catalysis and its mechanism.

10.8 Colloidal state- Distinction among true Solutions, Colloids and suspensions
(a) Classification of colloids.
(b) Lyophilic.
(c) Lyophobic.
(D) Multimolecular.
(E) Macromolecular.
(F) Associated colloids (micelles).

10.9 Preparation and properties of colloids.

10.10 Tyndall effect. And Brownian movement.

10.11 Electrophoresis and dialysis.

10.12 Coagulation and flocculation.

10.13 Emulsions and their characteristics.


Section B - Inorganic Chemistry

UNIT 11: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

11.1 Modem periodic law.

11.2 General electronic configuration of groups and present form of the periodic table, s, p. d and f block elements.

11.3 Periodic trends in properties of elements
(a) Atomic and ionic radii.
(b) Ionization enthalpy.
(c) Electron gain enthalpy.
(d) Valence electrons.
(e) Oxidation states.
(f) Metallic and non metallic nature.
(g) Chemical reactivity of elements.
(h) Acidic oxides and basic oxides.


UNIT 12: GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF METALS


12.1 Modes of occurrence of elements in nature,
(a) Minerals.
(b) Ores.

12.2 Steps involved in the extraction of metals –
(a) Concentration.
(b) Reduction (chemical and electrolytic methods)
(c) Refining with special reference to the extraction of Al. Cu, Zn and Fe.

12.3 Thermodynamic and electrochemical principles involved in the extraction of metals.-Ellingham’s diagram.


UNIT 13: HYDROGEN


13.1 Position of hydrogen in periodic table.

13.2 Isotopes of hydrogen.

13.3 Preparation of hydrogen gas.

13.4 Properties of Hydrogen gas.

13.5 Uses of hydrogen gas.

13.6 Classification of hydrides –
(a) Ionic.
(b) Covalent.
(c) And interstitial. .

13.7 Hydrogen as a fuel.


13.1 Water-

13.1.1- Physical properties of water and heavy water.

13.1.2- Chemical properties of water and heavy water.


13.2 Hydrogen peroxide

13.2.1- Structure of Hydrogen Peroxide.

13.2.2- Preparation Hydrogen Peroxide.

13.2.3- Reactions Hydrogen Peroxide.

13.2.4- Uses of hydrogen Peroxide.

UNIT 14: S -BLOCK ELEMENTS (ALKALI AND ALKALINE EARTH METALS)


Group -1 and 2 Elements
14.1 General introduction and electronic configuration.

14.2 General trends in physical properties.

14.3 General trends chemical properties of elements.

14.4 Anomalous properties of the first element of each group.

14.5 Diagonal relationships.

14.6 Preparation and properties of some important compounds –
(a) Sodium carbonate.
(b) Sodium hydroxide and.
(c) Sodium hydrogen carbonate.

14.7 Industrial uses of
(a) lime.
(b) limestone.
(c) Plaster of Paris.
(d) cement.

14.8 Biological significance of
(a) Na
(b) K
(c) Mg
(d) Ca


UNIT 15: P- BLOCK ELEMENTS

15.1 Group -13 to Group 18 Elements
15.1.1- General Introduction and Electronic configuration

15.1.2- General trends across the periods and down the groups in
(a) physical properties
(b) Chemical properties of elements

15.1.3- Unique behaviour of the first element in each group.


15.2 Groupwise study of the p - block elements Group -13

15.2.1- Preparation, properties and uses of boron.

15.2.2- Preparation, properties and uses of aluminium.

15.2.3- Structure, properties and uses of
(a) Borax.
(b) Boric acid.
(c) Diborane.
(d) Boron.
(e) Trifluoride.
(f) Aluminium chloride.
(g) Alums.


15.3 Group -14

15.3.1- The tendency for catenation;

15.3.2- Structure,properties and uses of
(a) Allotropes and.
(b) Oxides of carbon.
(c) Silicon tetrachloride.
(d) Silicates.
(e) Zeolites and.
(f) Silicones.


15.4 Group -15

15.4.1- Properties and uses of nitrogen and.

15.4.2- Properties and uses of Phosphorus.

15.4.3- Allotrophic forms of phosphorus.
15.4.4- Preparation, Properties, Structure and uses of
(a) Ammonia.
(b) Nitric acid.
(c) Phosphine.
(d) Phosphorus halides,(PCl3.PCl5)
15.4.5- Structures of Oxides and Oxoacids of
(a) Nitrogen.
(b) Phosphoru.


15.5 Group -16

15.5.1-Preparation,properties,structures and uses of ozone and oxygen

15.5.2- Allotropic forms of sulphur;s;

15.5.3- Preparation, properties, structures and uses of sulphuric acid (including its industrial preparation);
15.5.4- Structures of oxoacids of sulphur.

15.6.1- Preparation, properties and uses of hydrochloric acid.

15.6.2- Trends in the acidic nature of hydrogen halides.

15.6.3- Structures of Interhalogen compounds.
15.6.4- Structures of oxides and oxoacids of halogens.


15.6 Group -17

15.7.1- Occurrence and uses of noble gases;

15.7.2- Structures of fluorides and oxides of xenon.

UNIT 16: d - and f- BLOCK ELEMENTS


16.1 Transition Elements General introduction.

16.2 Electronic configuration.

16.3 Occurrence and characteristics.

16.4 General trends in properties of the first-row transition elements -
(a) Physical properties.
(b) Ionization enthalpy.
(c) Oxidation states.
(d) Atomic radii.
(e) Colour.
(f) Catalytic behaviour.
(g) Magnetic properties.
(h) Complex formation.
(i) Interstitial compounds.

16.5 Alloy formation.

16.6 Preparation, properties and uses of (a). K2Cr2O7, (b). KMnO4.

16.7 Inner Transition Elements- General introduction.

16.8 Lanthanoids –
(a) Introduction.
(b) Electronic configuration.
(c) Oxidation states and.
(d) Lanthanoid contraction.

16.9 Actinoids –
(a) Introduction.
(b) Electronic configuration.
(c) Oxidation states.


UNIT 17: CO-ORDINATION COMPOUNDS


Group -1 and 2 Elements
17.1 Introduction to co-ordination compounds.

17.2 Werner's theory.

17.3 Important terms in Co-ordination compounds
(a) ligands,
(b) Co-ordination number,
(c) Denticity.
(d) Chelation.

17.4 IUPAC nomenclature of mononuclear co--ordination compounds.

17.5 Isomerism in coordination compounds.

17.6 Bonding-Valence bond approach

17.7 Basic ideas of Crystal field theory.

17.8 Colour of coordination compounds.

17.9 Magnetic properties of coordination compounds

17.10 Importance of coordination compounds
(a) In qualitative analysis.
(b) Extraction of metals.
(c) Biological systems.


UNIT 18: ENVIRONMENTAL CHEMISTRY


18.1 Environmental pollution –
(a) Atmospheric.
(b) water and.
(c) soil.

18.2 Atmospheric pollution –
(a) Tropospheric.
(b) And Stratospheric.

18.3 Tropospheric pollutants – Gaseous pollutants
(a) Oxides of carbon, nitrogen andsulphur, hydrocarbons;
(b) Their sources,harmful effects and prevention;
(c) Greenhouse effect and Global warming:
(d) Acid rain.

18.4 Particulate pollutants:
(a) Smoke, dust,smog, fumes, mist;
(b) Their sources, Harmful effects and prevention.

18.5 Stratospheric pollution-
(a) Formation and breakdown of ozone,
(b) Depletion of the ozone layer - its mechanism and effects.

18.6 Water Pollution – Major pollutants such as.
(a) Pathogens,
(b) Organic wastes and
(c) Chemical pollutants;
(d) Their harmful effects and prevention.

18.7 Soil pollution - Major pollutants such as.
(a) Pesticides (insecticides. herbicides and
(b) Fungicides),
(c) Their harmful effects and prevention.

18.8 Strategies to control environmental pollution


Section C - Organic Chemistry

UNIT 19: PURIFICATION AND CHARACTERISATION OF ORGANIC COMPOUNDS

19.1 Purification – principles and applications of -
(a) Crystallization,
(b) Sublimation,
(a) Distillation,
(c) Differential
(d) Extraction and
(e) Chromatography

19.2 Qualitative analysis – Detection of
(a) Nitrogen,
(b) Nulphur,
(c) Phosphoru,
(d) Halogens.

19.3 Quantitative analysis (Basic principles only) - Estimation of
(a) Carbon,
(b) Hydrogen,
(c) Nitrogen,
(d) Halogens,
(e) Sulphur,
(f) Phosphorus.

19.4 Calculations of empirical formulae and molecular formulae .

19.5 Numerical problems in organic quantitative analysis,



UNIT 20:SOME BASIC PRINCIPLES OF ORGANIC CHEMISTRY


20.1 Tetravalency of carbon.

20.2 Shapes of simple molecules - hybridization (s and p):

20.3 Classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen and sulphur;

20.4 Homologous series.

20.5 Isomerism – structural and stereoisomerism.

20.6 Nomenclature (Trivial and IUPAC)

20.7 Covalent bond fission –
(a) Homolytic.
(b) Heterolytic.

20.8 Intermediates
(a) Free radicals.
(b) Carbocations and.
(c) Carbanions.

20.9 Stability of carbocations and free radicals.

20.10 Electrophiles and nucleophiles.

20.11 Electronic displacement in a covalent bond
(a) Inductive effect.
(b) Electromeric effect.
(c) Resonance and.
(d) Hyperconjugation.

20.12 Common types of organic reactions-
(a) Substitution,
(b) Addition,
(c) Elimination and
(d) Rearrangement.



UNIT 21: HYDROCARBONS


21.1 Classification of hydrocarbons.

21.2 Isomerism in hydrocarbons.

21.3 IUPAC nomenclature of hydrocarbons.

21.4 General methods of preparation.

21.5 General properties and reactions of HYDROCARBONS.

21.6 Alkanes –
(a) Conformations.
(i) Sawhorse and.
(ii) Newman projections (of ethane).
(b) Mechanism of halogenation of alkanes.

21.7 Alkenes –
(a) Geometrical isomerism.
(b) Mechanism of electrophilic addition.
(c) Addition of hydrogen.
(d) Halogens.
(e) Water.
(f) Hydrogen halides -Markownikoffs rule.
(g) Peroxide effect.
(h) Ozonolysis and.
(i) Polymerization.

21.8 Alkynes –
(a) Acidic character.
(i) Chemical reactios :Addition of.
(ii) Hydrogen.
(iii) Halogens.
(iv) Water and.
(v) Hydrogen halide.
(b) Polymerization.

21.9 Aromatic hydrocarbons –
(a) Nomenclature,
(b) Benzene - structure and aromaticity:
(c) Mechanism of electrophilic substitution:
(i) Halogenation,
(ii) Nitration.
(iii) Friedel - Craft's alkylation and acylation,
(d) Directive influence of the functional group in mono-substituted benzene.


UNIT 22: ORGANIC COMPOUNDS CONTAINING HALOGENS


22.1 General methods of preparation halogens.

22.2 Nature of C-X bond.

22.3 Physical Properties of halogen.

22.4 Chemical reactions of halogens.

22.5 Mechanisms of substitution reactions.

22.6 Uses of halogens.

22.7 Environmental effects of
(a) Chloroform.
(b) Iodoform.
(c) Freons and.
(d) DDT.


UNIT 23: ORGANIC COMPOUNDS CONTAINING OXYGEN


23.1 Introduction
(a) General methods of preparation.
(b) Physical and Chemical Properties.
(c) Chemical reactions.
(d) Uses of ORGANIC COMPOUNDS CONTAINING OXYGEN.

23.2 (a) Alcohols
i Identification of primary,secondary and tertiary alcohols:
ii Mechanism of dehydration.
(b) Phenols:
i Acidic nature,
ii Electrophilic substitution reactions:
iii halogenation.
iv nitration
v Sulphonation.
vi Reimer -Tiemann reaction.
(c) Ethers
i. Structure.
ii Physical and chemical Properties
(d) Aldehyde and Ketones
i Nature of carbonyl group;
ii Nucleophilic addition to >C=O group,
iii relative reactivities of aldehydes and ketones;
iv Important reactions such as –
1 Nucleophilic addition reactions
(a) (addition of HCN.
(b) NH3, its derivatives),
2 Grignard reagent;
3 Oxidation:
4 Reduction
(a) Wolf Kishner and
(b) Clemmensen);
v. The acidity of α-hydrogen.
(a) Aldol condensation,
(b) Cannizzaro reaction.
(c) Haloform reaction,
vi Chemical tests to distinguish between aldehydes and Ketones.
(e) Carboxylic Acids-
i Acidic strength and factors affecting it,


UNIT 24: ORGANIC COMPOUNDS CONTAINING NITROGEN


24.1 General methods of preparation.

24.2 Properties, reactions and uses.

24.3 Amines.
(a) Nomenclature.
(b) Classification- identification of primary, secondary and tertiary amines.
(c) Structure.
(d) Basic character and strength of basic character.

24.4 Diazonium Salts:
(a) Importance in synthetic organic chemistry.


UNIT 25: POLYMERS


25.1 General introduction and.

25.2 Classification of polymers.

25.3 General methods of polymerization, -
(a) Addition.
(b) Condensation.
(c) Copolymerization.

25.4 Natural and synthetic rubber.

25.5 Vulcanization of Rubber.

25.5 Some important polymers with emphasis on their monomers and uses
(a) Polythene.
(b) Nylon.
(c) Polyester.
(d) Bakelite.


UNIT 26: BIOMOLECULES


26.1 General introduction and importance of biomolecules.

26.2 CARBOHYDRATES – Classification.
(a) Aldoses and ketoses.
(b) Monosaccharides (glucose and fructose).
(c) Oligosaccharides.
(d) Sucrose.
(e) Lactose and.
(f) Maltose.
(g) Polysaccharides.

26.3 PROTEINS –
(a) Elementary Idea of α-amino acids.
(b) Peptide bond.
(c) Polypeptides.
(d) Proteins structures (qualitative idea only).
i Primary.
ii Secondary.
iii Tertiary and.
iv Quaternary structure.
v Denaturation of proteins.

26.4 Enzymes.

26.5 VITAMINS –
(a) Classification
(b) Functions.

26.6 NUCLEIC ACIDS –
(a) Chemical constitution of DNA and RNA.
(b) Biological functions of nucleic acids.


UNIT 27: CHEMISTRY IN EVERYDAY LIFE


27.1 Chemicals in Medicines – Meaning and common examples.
(a) Analgesics,
(b) Tranquillizers,
(c) Antiseptics,
(d) Disinfectants,
(e) Antimicrobials,
(f) Anti-fertility drugs,
(g) Antibiotics,
(h) Antacids.
(i) Anti-histamines.

27.2 Chemicals in food – Common examples.
(a) Preservatives.
(b) Artificial sweetening agents -

27.3 Cleansing Agents –
(a) Soaps.
(b) Detergents.
(c) Cleansing action.


UNIT 28: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY


28.1 Detection of extra elements.
(a) Nitrogen.
(b) Sulphur.
(c) halogens in organic compounds.

28.2 Detection of the following functional groups;
(a) hydroxyl (alcoholic and phenolic).
(b) carbonyl (aldehyde and ketones) carboxyl.
(c) and amino groups in organic compounds.

28.3 The chemistry involved in the preparation of the following:
(a) Inorganic compounds .
i Mohr’s salt.
ii Potash alum.
(b). Organic compounds:
i Acetanilide.
ii p-nitro acetanilide.
iii aniline.
iv yellow iodoform.

28.4 The chemistry involved in the titrimetric exercises –
(a) Acids, bases and the use of indicators.
(b) oxalic-acid vs KMnO4.
(c) Mohr’s salt vs KMnO4.

28.5 Chemical principles involved in the qualitative salt analysts: ( Insoluble salts excluded).
(a) Cations – Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4 +
(b) Anions- CO3 2−, S2-,SO4 2−, NO3-, NO2-, Cl-,Br-, I-

28.6 Chemical principles involved in the following experiments:
(a) Enthalpy of solution of CuSO4.
(b) Enthalpy of neutralization of strong acid and strong base.
(c) Preparation of lyophilic and lyophobic sols.
(d) Kinetic study of the reaction of iodide ion with hydrogen peroxide at room temperature.


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