BEEE Chemistry Syllabus

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BEEE 2019 Chemistry Syllabus

BEEE Chemistry Questions : 30

Unit 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.

Unit 2 :  States of Matter

Classi_cation of matter into solid, liquid and gaseous states. Solid State: Classi_cation 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. 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-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, Van der 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, lanthanides and actinides-general characteristics. Coordination Chemistry: Coordination compounds, nomenclature: terminology – Werner’s coordination theory.

Applications of coordination compounds.

Unit 4 : Atomic Structure

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 Bohr’s model; dual nature of matter, De-Broglie’s relationship, ( Angular momentum and magnetic quantum numbers ) and their signi_cance; shapes of s, p and d-orbitals, electron spin and spin quantum number; rules for _lling electrons in orbitals–Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic con_guration of elements, extra stability of half-filled and completely filled orbitals.

Unit 5 : Chemical Bonding and Molecular Structure

Covalent bonding : Concept of electro negativity, Fajan’s rule, dipole moment; Valence Shell Electron Pair Repulsion ( VSEPR ) theory and shapes of simple molecules.

Valence bond theory – Its important features, concept of hybridization involving s, p and d orbitals; resonance. types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic con_gurations of homonuclear diatomic molecules, concept of bond order, bond length and bond energy.

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, car bides, halides and  sulphides of carbon group.

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 Raoult’s law-ideal and non-ideal solutions, vapour pressure-composition plots for ideal andnon-ideal solutions; colligative properties of dilute solutionsrelative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure; determination of molecular mass using colligative properties; abnormal value

Unit 7 : Chemical Equilibrium

Meaning of equilibrium, concept of dynamic equilibrium. Equilibria involving physical processes: Solid- liquid, liquid-gas and solid-gas equilibria, Henry’s law, Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants ( Kp and Kc ) and their signi_cance, Le Chatelier’s principle.

Ionic equilibrium : Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted- Lowry and Lewis) andtheir 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:

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; dry cell and lead accumulator; fuel cells; corrosion and its prevention.

Unit 9 : Surface Chemistry, Chemical Kinetics and Catalysis

Adsorption-Physisorption and chemisorption and their characteristics, factors affecting adsorption of gases on solids-Freundlich and Langmuir adsorption isotherms, adsorption from solutions. Catalysis. Tyndall effect,

Brownian movement, electrophoresis, dialysis, coagulation and _occulation; emulsions and their characteristics. 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 speci_c rate constants. Nuclear Chemistry: adioactivity: isotopes and isobars: Properties of  and _ rays; Kinetics of radioactive decay (decay series excluded), carbon datting.

Unit 10 : Some Basic Principles of Organic Chemistry

Tetravalency of carbon; shapes of simple moleculeshy bridization ( s and p ); classi_cation of organic compounds based on functional groups: -C=C-, -C_C- and those containing halogens, oxygen, nitrogen and sulphur; homologous series; isomerism-structural and stereoiso merism.

Nomenclature (Trivial and IUPAC) Covalent bond _ssion – Homolytic and heterolytic: free radicals, car bocations and car banions; stability of car bocations and free radicals, electro philes and nucleo philes. Electronic displacement in a coval ent bond inductive effect, electromeric effect, resonance and hyper conjugation.

Unit 11 : Hydrocarbons

Classi_cation, isomerism, IUPAC nomenclature, ge eral methods of preparation, properties and reactions. Alkenes- Geometrical isomerism; mechanism of electrophilic addition: addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect);

ozonolysis, oxidation, and polymerization. Mechanism of electrophilic substitution: halogenation, nitration, Friedel- Craft’s alkylation and acylation, directive in_uence of functional group in monosubstituted benzene

Unit 12 : Organic Compounds Containing Oxygen

General methods of preparation, properties, reactions and uses. Alcohols: Distinction of primary, secondary and tertiary alcohols; mechanism of dehydration. Reactions of hydroxyl 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. Ethers: Structure. 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 derivatives.

Unit 13 : Organic Compounds Containing Nitrogen

General methods of preparation, properties, reactions and uses. Amines: Nomenclature, classi_cation, structure, basic character and identi_cation of primary, secondary and tertiary amines and their basic character.

Unit 14 : Polymers

General introduction and classi_cation of polymers, general methods of polymerization–addition and condensation, copolymerization; natural and synthetic rubber and vulcanization; monomers and uses – polythene, nylon, polyester and bakelite.

Unit 15 : Chemistry in Everyday Life

Chemicals in medicines-Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids. Cleansing agents–Soaps and detergents, cleansing action.