Syllabus for JEE Main Paper 1 BE/B.Tech Chemistry

PHYSICAL CHEMISTRY
UNIT I: SOME BASIC CONCEPTS IN CHEMISTRY
Matter and its nature, Dalton's atomic theory, Concept of atom, molecule, element and compound, Laws of chemical combination, Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae, Chemical equations and stoichiometry.
UNIT 2: ATOMIC STRUCTURE
Nature of electromagnetic radiation, photoelectric effect, spectrum of the hydrogen atom, Bohr model of a hydrogen atom - its postulates, derivation of the relations for the 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, the quantum mechanical model of the atom and its important features, concept of atomic orbitals as one-electron wave functions, variation of 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 and extra stability of half-filled and completely filled orbitals.
UNIT 3: CHEMICAL BONDING AND MOLECULAR STRUCTURE
Kossel-Lewis approach to chemical bond formation, the 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, the
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, the concept of bond order, bond length and bond energy.
Elementary idea of metallic bonding, hydrogen bonding and its applications.
UNIT 4: CHEMICAL THERMODYNAMICS
Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state
functions, entropy, types of processes.
The 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.
The second law of thermodynamics - Spontaneity of processes, Δ S of the universe and Δ G of the
system as criteria for spontaneity. ΔG°(Standard Gibbs energy change) and equilibrium constant.
UNIT 5: SOLUTIONS
Different methods for expressing the concentration of solution - molality, molarity, mole fraction,
percentage (by volume and mass both), the vapour pressure of solutions and Raoult's Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non- ideal solutions, Colligative
properties of dilute solutions - a relative lowering of vapour pressure, depression of freezing point, the
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.

UNIT 6: EQUILIBRIUM
Meaning of equilibrium is the concept of dynamic equilibrium.
Equilibria involving physical processes: Solid-liquid, liquid-gas, gas-gas and solid-gas equilibria,
Henry's law. General characteristics of equilibrium involving physical processes.
Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and
Kc) and their significance, the significance of Δ G and Δ G ° in chemical equilibrium, factors affecting
equilibrium concentration, pressure, temperature, the effect of catalyst, Le Chatelier’s principle.
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted - 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, the solubility of sparingly soluble salts, solubility products
and buffer solutions.
UNIT 7: REDOX REACTIONS AND ELECTROCHEMISTRY
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning
oxidation number and balancing of redox reactions.
Electrolytic and metallic conduction, conductance in electrolytic solutions, 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.
UNIT 8: 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, the effect of temperature on the rate of reactions, Arrhenius theory,
activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation).

INORGANIC CHEMISTRY

UNIT 9: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Modern 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.
UNIT 10: 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.
UNIT 11: 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, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation, preparation, properties and uses of K2Cr2O7 and KMnO4. Inner Transition Elements
LanthanoidsActinoids - Electronic configuration and oxidation states.
UNIT 12: COORDINATION COMPOUNDS
Introduction to coordination compounds. Werner's theory, ligands, coordination number, denticity,
chelation, IUPAC nomenclature of mononuclear co-ordination 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).

ORGANIC CHEMISTRY

UNIT 13: 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 and phosphorus.
Calculations of empirical formulae and molecular formulae, numerical problems in organic quantitative
analysis,
UNIT 14: 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 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.
Common types of organic reactions- Substitution, addition, elimination and rearrangement.
UNITS 15: 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 (Markownikoffs 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 the functional group in mono- substituted
benzene.
UNIT 16: ORGANIC COMPOUNDS CONTAINING HALOGENS
General methods of preparation, properties and reactions, nature of C-X bond, mechanisms of
substitution reactions.
Uses, environmental
UNIT 17: 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 (Wolf Kishner and
Clemmensen), the acidity of 𝐀 -hydrogen. Aldol condensation, Cannizzaro reaction, Haloform reaction,
chemical tests to distinguish between aldehydes and ketones.
Carboxylic Acids: Acidic strength and factors affecting it.
UNIT 18: 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.
UNIT 19: BIOMOLECULES
General introduction and importance of biomolecules.
CARBOHYDRATES – Classification, aldoses and ketoses, monosaccharides (glucose and fructose) and constituent monosaccharides of oligosaccharides (sucrose, lactose and maltose).
PROTEINS - Elementary idea of 𝐀 -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.
Hormones (General introduction)
UNIT 20: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY
Detection of extra elements (Nitrogen, sulphur, halogens) in organic compounds, detection of the
following functional groups, hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones) carboxyl and amino groups in organic compounds.

The chemistry involved in the preparation of the following:
Inorganic compounds, Mohr’s salt, potash alum.
Organic compounds: Acetanilide, p-nitro acetanilide, aniline yellow, iodoform.
The chemistry involved in the titrimetric exercises – 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+, Al3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+
Anions- CO32−, S2-, SO42−, NO3-, NO2-, Cl-, 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. Kinetic study of the reaction of iodide ions with hydrogen peroxide at room temperature.

GRE Subject Test: Chemistry

What is the test pattern for GRE Chemistry

• No. of Questions: 130
• Type: Multiple Choice

Syllabus and Question Paper Pattern
 
I. ANALYTICAL CHEMISTRY — 15%

    Data Acquisition and Use of Statistics — Errors, statistical considerations
    Solutions and Standardization — Concentration terms, primary standards
    Homogeneous Equilibria — Acid-base, oxidation-reduction, complexometry
    Heterogeneous Equilibria — Gravimetric analysis, solubility, precipitation titrations, chemical separations
    Instrumental Methods — Electrochemical methods, spectroscopic methods, chromatographic methods, thermal methods, calibration of instruments
    Environmental Applications
    Radiochemical Methods — Detectors, applications

II. INORGANIC CHEMISTRY — 25%

    General Chemistry — Periodic trends, oxidation states, nuclear chemistry
    Ionic Substances — Lattice geometries, lattice energies, ionic radii and radius/ratio effects
    Covalent Molecular Substances — Lewis diagrams, molecular point groups, VSEPR concept, valence bond description and hybridization, molecular orbital description, bond energies, covalent and van der Waals radii of the elements, intermolecular forces
    Metals and Semiconductors — Structure, band theory, physical and chemical consequences of band theory
    Concepts of Acids and Bases — Brønsted-Lowry approaches, Lewis theory, solvent system approaches
    Chemistry of the Main Group Elements — Electronic structures, occurrences and recovery, physical and chemical properties of the elements and their compounds
    Chemistry of the Transition Elements — Electronic structures, occurrences and recovery, physical and chemical properties of the elements and their compounds, coordination chemistry
    Special Topics — Organometallic chemistry, catalysis, bioinorganic chemistry, applied solid-state chemistry, environmental chemistry

III. ORGANIC CHEMISTRY — 30%

    Structure, Bonding and Nomenclature — Lewis structures, orbital hybridization, configuration and stereochemical notation, conformational analysis, systematic IUPAC nomenclature, spectroscopy (IR and 1H and 13C NMR)
    Functional Groups — Preparation, reactions, and interconversions of alkanes, alkenes, alkynes, dienes, alkyl halides, alcohols, ethers, epoxides, sulfides, thiols, aromatic compounds, aldehydes, ketones, carboxylic acids and their derivatives, amines
    Reaction Mechanisms — Nucleophilic displacements and addition, nucleophilic aromatic substitution, electrophilic additions, electrophilic aromatic substitutions, eliminations, Diels-Alder and other cycloadditions
    Reactive Intermediates — Chemistry and nature of carbocations, carbanions, free radicals, carbenes, benzynes, enols
    Organometallics — Preparation and reactions of Grignard and organolithium reagents, lithium organocuprates, and other modern main group and transition metal reagents and catalysts
    Special Topics — Resonance, molecular orbital theory, catalysis, acid-base theory, carbon acidity, aromaticity, antiaromaticity, macromolecules, lipids, amino acids, peptides, carbohydrates, nucleic acids, terpenes, asymmetric synthesis, orbital symmetry, polymers

IV. PHYSICAL CHEMISTRY — 30%

    Thermodynamics — First, second, and third laws, thermochemistry, ideal and real gases and solutions, Gibbs and Helmholtz energy, chemical potential, chemical equilibria, phase equilibria, colligative properties, statistical thermodynamics
    Quantum Chemistry and Applications to Spectroscopy — Classical experiments, principles of quantum mechanics, atomic and molecular structure, molecular spectroscopy
    Dynamics — Experimental and theoretical chemical kinetics, solution and liquid dynamics, photochemistry

General Knowledge for Competitive Examinations

General Knowledge (GK) makes Integral Part of many competitive examinations in India. The GK Test examine your awareness and abilities from in and around your surroundings. In this portion questions are asked from day to day life experiences. Generally, whether its and admission test or recruitment exam questions are asked from the areas those we discuss often among friends, family, or listen over radio, television and social media etc.

General Knowledge: CHEMISTRY

Knowledge in Chemistry is essential for day to day living. Of course its essential to make scientific discoveries, and make things work. In competitive examinations Questions in General Knowledge are asked from Chemistry. Here are lessons useful for tests like UPSC Exam, SSC Exam, Bank PO Exam, Defence Exam, Teachers' Training Exam, Admission Test, Scholarship Tests etc.

Introduction to Chemistry

Atomic Structure

Periodic Classification of Elements

Chemical Bonding

Oxidation and Reduction

Chemistry Fun and Facts

• The only elements that are liquid at room temperature are bromine and mercury.
• Water expands as it freezes. An ice cube takes up about 9% more volume than the water used to make it.
• If you pour a handful of salt into a full glass of water, the water level will actually go down rather than overflowing the glass.

Non Metal

In modern periodic table there are 24 non metal elements. These are electronegative elements and bad conductor of heat and electricity. Here are some of the commonly occurring non metals and their properties-

Metallurgy

What is Metallurgy?

The process of extracting metals from ores is called metallurgy.

Ores - An ore is a type of rock that contains minerals with important elements including metals. The ores are extracted through mining; these are then refined to extract the valuable elements.

Fuels

Fuel is a substance that can supply energy alone or upon reaction with some other substance. Fuel when provide energy also produced heat which is measured in Calories. An ideal fuel should posses the following properties –

Carbon and Its Compounds

Carbon is a non metal, its atomic number is 6 and mass number 12. It is placed in Group 14 or IV A of Periodic Table.

Allotropy- The substances which shows similar chemical characteristics but different physical characteristics are called allotropes and this property of material is called allotropy. Carbon has three allotropes – Charcoal, Graphite and Diamond

Electrolysis

Electrolytes- Electrolytes are the materials which allow electric current to pass through them when in molten state and goes for chemical decomposition. For example; acids, bases, and salts.

Behavior of Gases

Boyle’s Law: Boyle's lawstates that the absolute pressure and volume of a given mass of confined gas are inversely proportional, if the temperature remains unchanged within a closed system.

Mathematically, V ∝ 1/p; when temperature T is constant
Or V = K./p
Thus PV = K where K is constant
P1V1 = P1V1

Acids, Bases and Salts

Acid – An acid is a chemical material which exhibits following properties –

Sour in taste; when sprinkled on a blue litmus paper, turns it red; contains replaceable hydrogen; gives out hydrogen ion H+ in Aqueous Solution according to Arrhenius Theorem; can donate a proton According to Bronsted Lowry concept and can accept electrons according to Lewis Concept

Oxidation and Reduction

Oxidation and Reduction - The earliest view of oxidation and reduction is that of adding oxygen to form an oxide (oxidation) or removing oxygen (reduction). They always occur together. For example, in the burning of hydrogen the hydrogen is oxidized and the oxygen is reduced. The combination of nitrogen and oxygen which occurs at high temperatures follows the same pattern.

Chemical Bonding

What is a Chemical Bond?

A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges, either between electrons and nuclei, or as the result of a dipole attraction.

Periodic Classification of Elements

• In periodic table Elements are classified on the basis of similarities in their properties.
• Döbereiner grouped the elements into triads and Newlands gave the Law of Octaves.
• Mendeléev arranged the elements in increasing order of their atomic masses and according to their chemical properties.

Atomic Structure

Atom - The name atom originated from the Greek Word atomos, meaning "indivisible" or uncuttable, or indivisible, something that cannot be divided further. Atoms are the basic building blocks of matter that make up everyday objects. The atom is a basic unit of matter that consists of a dense central nucleus surrounded by negatively charged electrons. The atomic nucleus contains a mix of positively charged protons and electrically neutral neutrons.

Introduction to Chemistry

Chemistry is the systematic study of composition of matter and also the chemical and physical properties related to different material objects.

Lavoisier (1743-1793), a French Chemist is regarded as the Father of Modern Chemistry.

VIT University IGNITE 2014 Registration Open

The VIT University Presents IGNITE: Inter School Science & Math Challenge in association with the Times of India (TOI)

Let your students reach for the stars!

A dream trip to NASA could just be around the corner for one of your students.

The VIT University in association with the Times of India brings you IGNITE- an Inter-School Examination that will pit India’s smartest students against each other testing their knowledge in Science and Math.


The examination will comprise of objective type questions in Math, Physics and Chemistry. The examination will be held across the country. The winner for each region will go on to battle it out in a highly competitive National Quiz.

Times Now will telecast the Quiz.

The top 3 finalist from the quiz will win the grand prize- an all-expenses paid trip to NASA.

Challenge Details

• Registration Deadline: 25 January 2014
• Duration of Examination: 90 Minutes
• Eligibility: 10th and 11th Standard students from India
• Examination Date: 31 January 2014

For registration, venue and other details visit www.educationtimes.com/vitignite

AIEEE 2012 Question Paper, Answer Key, Solution & Analysis

Are you an aspiring engineer, planning to appear for entrance exams like AIEEE and looking for previous years question papers and solutions, if yes, you are in the right place now. Here we are providing happenings from AIEEE 2012 to help you in preparing better. This section also useful to AIEEE 2012 test takers who are taking exam now and awaiting results.

Please not that AIEEE 2012 Results shall be publishind on official website aieee.nic.in during 1st week of June 2012.

Download AIEEE 2012 Question Paper, Answer Key & Solution Set C This solution is property of FIITJEE Ltd New Delhi.

Download AIEEE 2012 Question Paper, Answer Key & Solution Set C, Hindi Medium This solution is property of Resonance Kota and its associates.

AIEEE 2012 Question Paper Analysis

• The All India Engineering Entrance Examination (AIEEE) 2012 Offline version conducted on 29.04.2012.
• There were 30 questions in each subject of which 5 were Assertion Reason Type in Mathematics and 3 in Physics.
• Each Section i.e. Physics, Chemistry and Mathematics carries 120 marks that means a total aggregate of 360 marks.
• The Mathematics was in little higher side. As an analogy mathematics always seems bit tougher being science of sciences.

Click Here to Download AIEEE 2012 Chapter Wise Analysis The pdf attached to this link is property of Career Point Kota

• Please take in note AIEEE 2012 Online exam is scheduled from 07.05.2012. The results shall be declared during 1st week of June.

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AIEEE 2012 Offline Exam on 29.04.2012

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IIT JEE 2012 Question Paper and Solution

IIT JEE 2012 conducted on April 8, 2012. Download Question Papers and Solutions in PDF eBooks format as supplied by Resonance. These question papers and solutions will help you in analyzing your performance as well as in preparation for upcoming entrance exams.

Resonance is one of the well known coaching center of North India for IIT JEE preparation.

IIT JEE 2012 Paper 1 Physics

IIT JEE 2012 Paper 1 Chemistry

IIT JEE 2012 Paper 1 Mathematics

IIT JEE 2012 Paper 2 Physics

IIT JEE 2012 Paper 2 Chemistry

IIT JEE 2012 Paper 2 Mathematics

IIT JEE 2012 Results shall be declared on May 18, 2012

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