SRMJEEE Chemistry Syllabus 2017 – SRMJEEE Computer Based Test Chemistry Syllabus 2017 – SRMJEEE Online Test Chemistry Syllabus 2017 – SRM Chemistry Entrance Test Syllabus 2017 – SRMJEEE 2017 Chemistry Admission Test Syllabus – SRM University Chemistry Online Test Syllabus
Sri Ramaswamy Memorial University Joint Engineering Entrance Examination Chemistry Syllabus 2017 has been Published. All Students who are aspiring for Admission to B.E. / B.Tech Engineering Programs offered in SRM University Kattankulathur Campus, SRM University Ramapuram Campus, SRM University Vadapalani Campus and SRM University NCR Campus through SRMJEEE Online Entrance Test which is an All India Engineering Entrance Exam and searching for SRM University Online Exam Chemistry Syllabus 2017 are hereby informed that the SRM University Admission Department has Finalized the SRMJEEE 2017 Online Test Syllabus for Chemistry Subject and Published SRMJEEE 2017 Chemistry Online Test Syllabus. Students who wishes to apply for Admissions in SRM University and Interested to View SRMJEEE 2017 Chemistry Syllabus can Check SRM Joint Entrance Examination Chemistry Syllabus 2017.
All Questions Asked in SRM University Chemistry Online Entrance Test 2017 will be based on the SRMJEEE 2017 Chemistry Syllabus Prescribed by the University Officials. Students must note that the SRMJEEE 2017 Chemistry Test Syllabus will be based on the 12th Class / Qualifying Exam Chemistry Syllabus. Students must note that the SRMJEEE 2017 Chemistry Syllabus is Common for Online Test and Offline Test. Students who wishes to Crack SRMJEEE 2017 Exam has to Concentrate on SRMJEEE 2017 Chemistry Syllabus Topic Wise and SRMJEEE 2017 Chemistry Syllabus Subtopic Wise.
SRM University Engineering Entrance Test Syllabus :-
SRM University 2017 Chemistry Entrance Examination Syllabus :-
UNIT 1: Atomic Structure
Matter and its nature, Daltons 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.
Discovery of sub-atomic particles (electron, proton and neutron); 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 Bohrs model;
Dual nature of matter, De-Broglies relationship, Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, quantum mechanical model of atom, its important features,
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, Paulis exclusion principle and Hunds rule, electronic configuration of elements, extra stability of halffilled and completely filled orbitals.
UNIT 2: States of Matter
Classification of matter into solid, liquid and gaseous states.
Solid State: Classification of solids: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids (elementary idea); Braggs 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.
Liquid State: Properties of liquids – vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only). Gaseous State: Measurable properties of gases; Gas laws-Boyles law, Charles law, Grahams law of diffusion, Avogadros law, Daltons 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, Vander Waals equation, liquefaction of gases, critical constants.
UNIT 3: Chemical Families–Periodic Properties
Modern periodic law and present form of the periodic table, s & p block elements, periodic trends in properties of elements, atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity. Transition elements –d -block elements, inner transition elements – f-block elements. Ionization energy, electron affinity, lanthanides and actinides – general characteristics. Coordination Chemistry: Coordination compounds, nomenclature: terminology – Werners coordination theory. Applications of coordination compounds.
UNIT 4: Chemical Bonding, Molecular Structure and s-& p- block elements
Covalent bonding: Concept of electronegativity, Fajans 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, anti-bonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, concept of bond order, bond length and bond energy.
s-, p- block elements: Elementary idea of metallic bonding. Hydrogen bonding and its applications. Extractive metallurgy of sodium, lithium, properties of alkali metals, basic nature of oxides and hydroxides, compounds of alkaline earth metals, compounds of boron. Oxides, carbides, halides and sulphides of carbon group. Oxides – classification – acidic, basic, neutral, peroxide and amphoteric oxides.
UNIT 5 : Chemical Thermodynamics & Energetics
First law of thermodynamics, Energy changes during a chemical reaction, Internal energy and Enthalpy, Hesss law of constant heat summation, numerical, based on these concepts. Enthalpies of reactions (enthalpy of neutralization, enthalpy of combustion, enthalpy of fusion and vaporization).
Second law of thermodynamics – Spontaneity of processes; S of the universe and G of the system as criteria for spontaneity, Go (Standard Gibbs energy change) and equilibrium constant.
UNIT 6: Solutions
Different methods for expressing concentration of solution – Molality, molarity, mole fraction, percentage (by volume and mass both), vapour pressure of solutions and Raoults law – ideal and non-ideal solutions, vapour pressure – composition plots for ideal and non-ideal 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, Vant Hoff factor and its significance.
UNIT 7: Chemical Equilibrium
Meaning of equilibrium, concept of dynamic equilibrium. Equilibria involving physical processes: Solid-liquid, liquid-gas and solid-gas equilibria, Henrys law, Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of G and Go in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, effect of catalyst; Le Chateliers 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, solubility of sparingly soluble salts and solubility products, buffer solutions.
UNIT 8: Electrochemistry
Electrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration: Kohlrauschs 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; dry cell and lead accumulator; fuel cells; corrosion and its prevention.
UNIT 9: Surface Chemistry, Chemical Kinetics, Catalysis and Nuclear Chemistry
Adsorption – Physisorption and chemisorption and their characteristics, factors affecting adsorption of gases on solids – Freundlich and Langmuir adsorption isotherms, adsorption from solutions.
Catalysis – Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis and its mechanism.
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.
Rate of reaction, instantaneous rate of reaction and order of reaction. Factors affecting rates of reactions – factors affecting rate of collisions encountered between the reactant molecules, effect of
temperature on the reaction rate, concept of activation energy, catalyst. Rate law expression. Order of a reaction (with suitable examples).
Units of rates and specific rate constants. Order of reaction and effect of concentration (study will be confined to first order only). Theories of catalysis adsorption theory-some of important industrial process using catalysts.
Nuclear Chemistry: Radioactivity: isotopes and isobars: Properties of α, β and γ rays; Kinetics of radioactive decay (decay series excluded), carbon datting; Stability of nuclei with respect to proton-neutron ratio; Brief discussion on fission and fusion reactions.
UNIT 10: 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.
UNIT 11: 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 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.
Common types of organic reactions – Substitution, addition, elimination and rearrangement.
UNIT 12: 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, oxidation, 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-Crafts alkylation and acylation, directive influence of functional group in mono Substituted benzene.
UNIT 13: Organic Compounds Containing Oxygen
General methods of preparation, properties, reactions and uses.
Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration. Reaction of hydroxy derivatives.
Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer–Tiemann reaction. Addition to >C=O group, relative reactivities of aldehydes and ketones.
Aldehyde and Ketones: Nature of carbonyl group; 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: Reactions, Acidic strength and factors affecting it; reactions of acid derivaties.
UNIT 14: 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 15: Polymers
General introduction and classification of polymers, general methods of polymerization–addition and condensation, copolymerization; natural and synthetic rubber and vulcanization; some important polymers with emphasis on their monomers and uses – polythene, nylon, polyester and bakelite.
UNIT 16: Bio Molecules
Carbohydrates–Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides of oligosacchorides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen). 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.
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