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.

http://jee.iitd.ac.in/

NON-METALS - IIT JEE Syllabus and Material

Authors

• Anonymous
• Narayana Rao KVSS

Published

Creative Commons Attribution 3.0 License

Version 5

Last edited: Apr 7, 2012

Exported: Apr 30, 2012

Original URL: http://knol.google.com/k/-/-/1zb6eis38d7or/7

JEE Syllabus

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.

 
Boron(B)

Compounds relevant to study of Boron

Borax (Na two B four O seven) Calamnite (Ca two B six O eleven)
Boron Trioxide (B two O three) Boric Acid (H three B O three)
Boron Nitride (B N)

Sodium Carbonate (Na two C O three)



Boron (B) - Preparation and Properties

atomic number electronic configuration

Z = 5, 1s²2s²2px¹

Main Ores of Boron

Borax, Kernite, Colemanite and Orthoboric acid.

Methods of Obtaining Boron

1. By the reduction of boric oxide y an electropositive metal like magnesium.
2. By the reductin of volatile boron compounds by dihydrogen at high temperatures (1270K).
3. By the electrolytic reduction of fused borates or other boron compounds (e.g., KBF-4, potasium tetrafluoroborate) in molten KCL/KF at 1073K.
4. By the thermal decomposition of boron tri-iodided over red hot tungsten.
5. By thermal decomposition of boron hydrides and boron halides at about 1173K.

Physical Properties of Boron

1. Boron is an extremely hard solid next to diamond.
2. Its melting point is 2450K and boiling point is 3925K.
3. It is a poor conductor of heat electricity.
4. It has two isotopic forms - B-10 and B-11. Relative abundance 19% and 81% respectively.

Chemical Properties of Boron

1. Combination with nonmetals: At room temperature, it reacts with flourine. Superficial reaction with oxygen. At higher termperatures, it reacts directly with all nonmetals except H, Ge, Te and nobles gases.
2. With water: It does not react with water even in the form of steam.
3. Acids: HCL does not react with boron.
When heated with concentrated sulphuric acid or nitric acid, boron is oxidized to boric acid.
Boron does not react with nonoxidizing acids.
4. Boron react with fused caustic alkalies like NaOH and KOH forming borates.
It dissolves in fused Na-2CO-3 and NaNO-3 mixture at 1173K.
5. Boron comines directly with almost all metals (except heavy metals) at higher temperatures.
Heavy Metals not combining with boron include Ag, Au, Cd, Hg, Ga, In, Tl, Pb, Sn, Bi etc.




Boron belongs to 13th group.
It has a very high melting point(2453 K).

It is extracted from minerals Borax(Na-2 B-4 O-7) or Calamnite (Ca-2 B-6 O-11)

Process of extracting Boron from Borax:
i) Borax is treated with concentrated hydrochloric acid. Boric acid is precipitated.
ii) boric acid is strongly heated. Boron trioxide is obtained (B-2 O-3).
iii) Boron trioxide is heated with Na, K or Mg pieces. Amorphous form of boron is obtained.

Alternatively mixture of boron tribromide vapours and hydrogen are passed over electrically heated filament of tungsten at 1200 degree centigrade. Crystalline form of Boron is obtained.

In another way, Boron trioxide can react with Aluminium to give Boron.

 

Silicon (Si)

Compounds relevant to study of silicon

Silica (Si O two)
Silicon Halide (Si X four) X is for halogen

silicon (Si) - Preparation and Properties

Electronic configuration of Silicon

Atomic Number is 14. 1s²2s²2p⁶3s²3p²

Methods of obtaining Silicon

1. Heating finely divided silica with magnesium powder.
2. Heating potassium silicoflouride with potassium metal.
3. Heating potassium silicoflouride wtih Al or Zn in an iron crucible.
4. Passing a current of SiCl-4 over molten aluminium.

Physical Properties of Silicon

Silicon is available in two allotropic forms. the amorphous silicon and the crystalline or admantine silicon.

Amorphous silicon is a dark brown powder which is insoluble in water.
Crystalline silicon forms pale yellow crystals.

Chemical properties of silicon

1. Silicon burns in air or oxygen forming silicon dioxide.
2. With halogens, it forms halides, SiX-4.
3. With fused acqueous caustic alkalies, silicon forms alkali silicates with liberation of hydrogen.
4. Silicon decomposes on red heating liberating hydrogen.
5. Metals like Magnesium and nonmetal carbon form silicides with silicon.

 

 

Sulphur (S)

Compound relevant to study of Sulphur

Hydrogen Sulphide (H two S)
Sulphur Dioxide (S O two)
Sodium Thio-Sulphate (Na two S two O three)

Ions formed by Sulphur

Sulphide ion (S O three (two-))
Thiosulphate ion (S two O three (two-))

Sulphur occurs in the native as well as combined form.Large quantites of sulphur are obtained from underground deposits in USA.

Partial combustion of Hydrogen sulphide produces sulphur.
Reaction of Hydrogen Sulphide with Sulphur dioxide also gives sulphur.
Sulphur occurs as S eight. It is a puckered ring with crown conformation.

Several allotropic forms of sulphur are available.

Rhombic sulphur (or alpha sulphur) is the stablest form. It is obtained by evaporation of solution of sulphur in carbon disulphide.

At about 95 C - 96 C rhombic sulphur is changed into another allotropic form monoclinic sulphur (als known as prismatic or beta sulphur).
Monoclinic sulphure has needle shaped crystals.

Other allotropic forms are amorphous (or colloidal) and plastic sulphur (or Gamma sulphur).

Amorphous sulphur is obtained by (1) the action of dilute Hydrochloric acid on sodium thio sulphate solution, and
(2)by passing Hydrogen sulphide through dilute nitric acid.

Plastic sulphur is obtained by pouring boiling sulphur in cold water. This results in rapid cooling. Plastic sulphur consists of a completely random arrangement of chains of sulphur atoms. On standing it passes over to the crystalline rhombic sulphur.

Sulphur is also active element like Oxygen. It combines with a large number of metals and nonmetals.

Sulphur is oxidized by concentrated nitric acid and sulphuric acid.
It also reacts with hot concentrated solution of alkalies.

 

Allotropes

 

Allotropes of Carbon

Carbon has two allotropic forms - diamond and graphite. Other amorphous carbons are actually micro crystals of graphite.

Diamond, an allotrope of Carbon is face centered crystal. It is the hardest natural substance. It is a nonconductor of electricity. It has high refractive inded (2.45) and much of the light that falls on it is internally reflected.

Diamond burns in air at 900 C and in oxygen at 700 C and forms carbon dioxide.

Graphite has a layer like structure in the three dimensional space and this gives it the lubricating property.

The carbon content of various amorphous forms of graphite; Peat (60%), Lignite (70%), Bituminous coal (78%) Semibituminous coal (83%) and Anthracite Coal (90%). The residue that remains after destructive distilation of coal in the absence of air is coke.

Graphite
• Graphite is a slippery black powder.
• Graphite is the only nonmetallic substance that conducts electricity.
• Each C atom is bonded to 3 other C atoms, forming one double bond and 2 single bonds.
• Every C atom in the graphite structure is bonded in the same way, with each carbon atom having one double bond and 2 single bonds.
• Graphite consists of a two dimensional layer in which C atoms are arranged in a series of regular hexagons.
• There are weak attractions between layers and the layers can readily slide past one another.
• By experiment, it has been determined that the 3 bonds associated with the C atoms are identical. Thus, the fourth pair of electrons is really delocalized. This accounts for the electrical conductivity of graphite.

• Diamond is a colorless crystal.
• Diamond is the hardest naturally occurring substance.
• Each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement.
• The tetrahedral arrangement of carbon atoms gives diamond its characteristic
physical properties such as:

o diamond is very hard
o diamond has a high melting point
o diamond is not easily compressed
o when given a good cut, diamond reflects light off of its facets.
• Diamond is actually a giant interlocking group of tetrahedrally arranged atoms. The bond angle between any two bonds in the crystal is 109.5o.

Allotropes of Phosphorus

Phosphorus has three main allotropes: white, red and black.

White phosphorus is poisonous and can spontaneously ignite when it comes in contact with air. For this reason, white phosphorus must be stored under water and is usually used to produce phosphorus compounds.

Red phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight. Red phosphorus is not poisonous and is not as dangerous as white phosphorus, although frictional heating is enough to change it back to white phosphorus. Red phosphorus is used in safety matches, fireworks, smoke bombs and pesticides.

Black phosphorus is also formed by heating white phosphorus, but a mercury catalyst and a seed crystal of black phosphorus are required. Black phosphorus is the least reactive form of phosphorus and has no significant commercial uses.



Allotropes of sulphur

Sulfur exists as a number of different allotropes. Below 95.6°C, the stable crystal form is rhombic, while above this temperature the element changes to a triclinic form. Both these forms contain cyclic S8 molecules. At temperatures just above its melting point, sulfur is a yellow liquid also containing S8 molecules. At about 160°C, the sulfur atoms link together in chains and the liquid becomes dark brown and more viscuous. If the molten sulfur is quickly cooled, for example, by pouring it into cold water, the result is a reddish-brown solid called plastic sulfur. Above 200°C the viscosity decreases.

Sulfur vapor contains a mixture of S2, S4, S6, and S8 molecules. So-called "flowers of sulfur" is a yellow powder obtained by subliming the vapor.


Rhombic sulphur
Yellow transparent crystals
Melt pt. 113 oC
Obtained when sulphur crystallises
from solution.




Monoclinic sulphur
Amber coloured needles
Melt pt. 119 oC
Obtained when sulphur
solidifies above 95.6 oC.


At atmospheric pressure the rhombic form is stable below 95.6 oC and the monoclinic form above this temperature. Only at the transition temperature can the two allotropes exist in equilibrium with each other.


When sulphur is heated it melts and undergoes a series of changes as the temperature rises.

 

Ozone

Ozone (O three) is an allotropic form of Oxygen.
It is naturally formed above 20 Km from the earth from oxygen by absorbing sunlight. Ozone layer protects earth from concentration of ultraviolet rays. chlorofluorcarbons (C Cl two F two) used as refrigerant releases active chlorine after absorbing sunlight and this active chlorine decomposes ozone leading to destruction of ozone layer.