A Common Entrance Test, designated as Telangana State Education Common Entrance Test through Computer Based Test -2020 (TS Ed.CET-2020 (CBT) will be conducted by the convener, TS Ed.CET-2020, Osmania University on behalf of the Telangana State Council of Higher Education for admission into B.Ed.(Two years)Regular Course in the Colleges of Education in Telangana for the academic year 2020-2021
TS Ed.CET-2020 is a CBT test will be conducted by the convener of Osmania University on behalf of the Telangana State Council of Higher Education.
TS Ed.CET 2020 Exam will be held on 23th May 2020 (Saturday)
Students should satisfy the following requirements shall be eligible to appear for TS Ed.CET-2020 (CBT) for admission into 2-year B.Ed Course.
Part-A
| General English | 25 questions for 25 marks |
Part-B
| General English | 15 questions for 15 marks |
| Teaching Aptitude | 10 questions for 10 marks |
Part-C
Methodology: Candidate has to choose one of the following subjects. It consists of 100 Questions for 100 marks . Each carry one marks
| Mathematics | 100 questions for 100 mark |
| Physical Sciences 1. Physics 2. Chemistry | 100 questions for 100 marks 1. 50 questions for 50 marks 2. 50 questions for 50 marks |
| Biological Sciences 1. Botany 2. Zoology | 100 questions for 100 marks 1. 50 questions for 50 marks 2. 50 questions for 50 marks |
| Social Studies 1. Geography 2. History 3. Civics 4. Economics | 100 questions for 100 marks 1. 35 questions for 35 marks 2. 30 questions for 30 marks 3. 15 questions for 15 marks 2. 20 questions for 20 marks |
| English | 100 questions for 100 marks |
SYLLABUS : PHYSICAL SCIENCES
Physics Syllabus (Marks : 50)
- Vector Analysis : Scalar and vector fields, gradient of a scalar field and its physical significance. Divergence and curl of a vector field and related problems. Vector integration, line, surface and volume integrals. Stokes, Gauss and Greens theorems- simple applications.
- Mechanics of Particles : Laws of motion, motion of variable mass system, motion of a rocket, multi-stage rocket, conservation of energy and momentum. Collisions in two and three dimensions, concept of impact parameter, scattering cross-section,
- Mechanics of rigid bodies: Definition of Rigid body, rotational kinematic relations, equation of motion for a rotating body, angular momentum and inertial tensor. Euler‘s equation, precession of a top, Gyroscope,
- Central forces: Central forces – definition and examples, conservative nature of central forces, conservative force as a negative gradient of potential energy, equation of motion under a central force, gravitational potential and gravitational field, motion under inverse square law, derivation of Kepler‘s laws, Coriolis force and its expressions.
- Special theory of relativity: Galilean relativity, absolute frames, Michelson-Morley experiment, Postulates of special theory of relativity. Lorentz transformation, time dilation, length contraction, addition of velocities, mass-energy relation. Concept of four vector formalism.
- Fundamentals of vibrations: Simple harmonic oscillator, and solution of the differential equation– Physical characteristics of SHM, torsion pendulum, – measurements of rigidity modulus , compound pendulum, measurement of ‗g‘, combination of two mutually perpendicular simple harmonic vibrations of same frequency and different frequencies, Lissajous figures
- Damped and forced oscillations: Damped harmonic oscillator, solution of the differential equation of damped oscillator. Energy considerations, comparison with undamped harmonic oscillator, logarithmic decrement, relaxation time, quality factor, differential equation of forced oscillator and its solution, amplitude resonance, velocity resonance. Coupled Oscillators.
- Vibrating Strings: Transverse wave propagation along a stretched string, general solution of wave equation and its significance, modes of vibration of stretched string clamped at ends, overtones, energy transport, transverse impedance
- Vibrations of bars: Longitudinal vibrations in bars- wave equation and its general solution. Special cases
(i) bar fixed at both ends
(ii) bar fixed at the midpoint
(iii) bar free at both ends
(iv) bar fixed at one end. Transverse vibrations in a bar- wave equation and its general solution. Boundary conditions, clamped free bar, free-free bar, bar supported at both ends, Tuning fork. - Kinetic theory of gases: Introduction – Deduction of Maxwell‘s law of distribution of molecular speeds, Transport Phenomena – Viscosity of gases – thermal conductivity – diffusion of gases.
- Thermodynamics: Basics of thermodynamics-Kelvin‘s and Claussius statements – Thermodynamic scale of temperature – Entropy, physical significance – Change in entropy in reversible and irreversible processes – Entropy and disorder – Entropy of universe – Temperature- Entropy (T-S) diagram – Change of entropy of a perfect gas-change of entropy when ice changes into steam.
- Thermodynamic potentials and Maxwell’s equations: Thermodynamic potentials – Derivation of Maxwell‘s thermodynamic relations – Clausius-Clayperon‘s equation – Derivation for ratio of specific heats – Derivation for difference of two specific heats for perfect gas. Joule Kelvin effect – expression for Joule Kelvin coefficient for perfect and Vanderwaal‘s gas.
- Low temperature Physics: Joule Kelvin effect – liquefaction of gas using porous plug experiment. Joule expansion – Distinction between adiabatic and Joule Thomson expansion – Expression for Joule Thomson cooling – Liquefaction of helium, Kapitza‘s method – Adiabatic demagnetization – Production of low temperatures – Principle of refrigeration, vapour compression type.
- Quantum theory of radiation: Black body-Ferry‘s black body – distribution of energy in the spectrum of Black body – Wein‘s displacement law, Wein‘s law, Rayleigh-Jean‘s law – Quantum theory of radiation – Planck‘s law – deduction of Wein‘s distribution law, Rayleigh-Jeans law, Stefan‘s law from Planck‘s law. Measurement of radiation using pyrometers – Disappearing filament optical pyrometer – experimental determination – Angstrom pyroheliometer – determination of solar constant, effective temperature of sun.
- Statistical Mechanics: Introduction, postulates of statistical mechanics. Phase space, concept of ensembles and some known ensembles ,classical and quantum statistics and their differences, concept of probability, Maxwell-Boltzmann‘s distribution law -Molecular energies in an ideal gas- Maxwell Boltzmann‘s velocity distribution law, Bose-Einstein Distribution law, Fermi-Dirac Distribution law, comparison of three distribution laws, Application of B-E distribution to Photons-planks radiation formula, Application of Fermi-Dirac statistics to white dwarfs and Neutron stars.
- Interference: Principle of superposition – coherence – temporal coherence and spatial coherence – conditions for Interference of light Interference by division of wave front: Fresnel‘s biprism – determination of wave length of light. Determination of thickness of a transparent material using Biprism – change of phase on reflection – Lloyd‘s mirror experiment. Interference by division of amplitude: Oblique incidence of a plane wave on a thin film due to reflected and transmitted light (Cosine law) – Colours of thin films – Non reflecting films – interference by a plane parallel film illuminated by a point source – Interference by a film with two non-parallel reflecting surfaces (Wedge shaped film) – Determination of diameter of wire-Newton‘s rings in reflected light with and without contact between lens and glass plate, Newton‘s rings in transmitted light (Haidinger Fringes) – Determination of wave length of monochromatic light – Michelson Interferometer – types of fringes – Determination of wavelength of monochromatic light, Difference in wavelength of sodium D1,D2 lines and thickness of a thin transparent plate.
- Diffraction: Introduction – Distinction between Fresnel and Fraunhoffer diffraction Fraunhoffer diffraction:- Diffraction due to single slit and circular aperture – Limit of resolution – Fraunhoffer diffraction due to double slit – Fraunhoffer diffraction pattern with N slits (diffraction grating) Resolving Power of grating – Determination of wave length of light in normal and oblique incidence methods using diffraction grating. Fresnel diffraction-Fresnel‘s half period zones – area of the half period zones –zone plate – Comparison of zone plate with convex lens – Phase reversal zone plate – diffraction at a straight edge – difference between interference and diffraction.
- Polarization: Polarized light : Methods of Polarization, Polarization by reflection, refraction, Double refraction, selective absorption , scattering of light – Brewster‘s law – Malus law – Nicol prism polarizer and analyzer – Refraction of plane wave incident on negative and positive crystals (Huygen‘s explanation) – Quarter wave plate, Half wave plate – Babinet‘s compensator – Optical activity, analysis of light by Laurent‘s half shade polarimeter.
- Aberrations and Fiber Optics: Introduction – Monochromatic aberrations, spherical aberration, methods of minimizing spherical aberration, coma, astigmatism and curvature of field, distortion. Chromatic aberration – the achromatic doublet – Removal of chromatic aberration of a separated doublet. Fiber Optics : Introduction – Optical fibers –Principles of fiber communication – Step and graded index fibers – Rays and modes in an optical fiber – Fiber material – Types of optical fibers and advantages of fiber communication,
- Electrostatics: Electric Field:- Concept of electric field lines and electric flux, Gauss‘s law (Integral and differential forms), application to linear, plane and spherical charge distributions. Conservative nature of electric field E, irrotational field. Electric Potential:- Concept of electric potential, relation between electric potential and electric field, potential energy of a system of charges. Energy density in an electric field. Calculation of potential from electric field for a spherical charge distribution.
- Magnetostatics :Concept of magnetic field B and magnetic flux, Biot-Savart‘s law, B due to a straight current carrying conductor. Force on a point charge in a magnetic field. Properties of B, curl and divergence of B, solenoidal field. Integral form of Ampere‘s law, applications of Ampere‘s law: field due to straight, circular and solenoidal currents. Energy stored in magnetic field. Magnetic energy in terms of current and inductance. Magnetic force between two current carrying conductors. Magnetic field intensity. Ballistic Galvanometer:- Torque on a current loop in a uniform magnetic field, working principle of B.G., current and charge sensitivity, electromagnetic damping, critical damping resistance.
- Electromagnetic Induction: Faraday‘s laws of induction (differential and integral form), Lenz‘s law, self and mutual Induction. Continuity equation, modification of Ampere‘s law, displacement current, Maxwell equations
- Electromagnetic waves: Maxwell‘s equations in vacuum and dielectric medium, boundary conditions, plane wave equation: transverse nature of EM waves, velocity of light in vacuum and in medium, polarization, reflection and transmission. Polarization of EM waves, Brewster‘s angle, description of linear, circular and elliptical polarization.
- Atomic Spectra and Models Inadequacy of classical physics: Brief Review of Black body Radiation , Photoelectric effect, Compton effect, dual nature of radiation, wave nature of particles. Atomic spectra, Line spectra of hydrogen atom, Ritz Rydberg combination principle. Alpha Particle Scattering, Rutherford Scattering Formula, Rutherford Model of atom and its limitations, Bohr‘s model of H atom, explanation of atomic spectra, correction for finite mass of the nucleus, Bohr correspondence principle, limitations of Bohr model, discrete energy exchange by atom, Frank Hertz Expt. Sommerfeld’s Modification of Bohr‘s Theory. Wave Particle Duality de Broglie hypothesis, Experimental confirmation of matter wave, Davisson Germer Experiment, velocity of de Broglie wave, wave particle duality, Complementarity. Superposition of two waves, phase velocity and group velocity, wave packets ,Gaussian Wave Packet , spatial distribution of wave packet, Localization of wave packet in time. Time development of a wave Packet; Wave Particle Duality, Complementarity. Heisenberg Uncertainty Principle, Illustration of the Principle through thought Experiments of Gamma ray microscope and electron diffraction through a slit. Time independent and time dependent Schrodinger wave equation. Estimation of ground state energy of harmonic oscillator and hydrogen atom, non-existence of electron in the nucleus. Uncertainty and Complementarities. Nuclear Physics Size and structure of atomic nucleus and its relation with atomic weight; Impossibility of an electron being in the nucleus as a consequence of the uncertainty principle. Nature of nuclear force, NZ graph, Liquid Drop model: semi-empirical mass formula and binding energy, Nuclear Shell Model and magic numbers. Radioactivity: stability of the nucleus; Law of radioactive decay; Mean life and half-life; Alpha decay; Beta decay- energy released, spectrum and Pauli’s prediction of neutrino; Gamma ray emission, energy momentum conservation: electron-positron pair creation by gamma photons in the vicinity of a nucleus. Fission and fusion- mass deficit, relativity and generation of energy; Fission – nature of fragments and emission of neutrons. Nuclear reactor: slow neutrons interacting with Uranium 235; Fusion and thermonuclear reactions driving stellar energy (brief qualitative discussions), Classification of Elementary Particles
- Basic Electronics: Classification of solids in terms of forbidden energy gap. Intrinsic and extrinsic semiconductors, Fermi level, continuity equation – p-n junction diode, half wave and full wave rectifiers and filters, ripple factor, Characteristics of Zener diode and its application as voltage regulator. – p n p and n p n transistors, current components in transistors, CB,CE and CC configurations – concept of transistor biasing, operating point, fixed bias and self-bias transistor as an amplifier — concept of negative feedback and Positive feedback – Barkhausen criterion.
- Digital Principles: Binary number system, converting Binary to Decimal and vice versa. Binary addition and subtraction (1s‘ and 2’s complement methods). Hexadecimal number system. Conversion from Binary to Hexadecimal – vice versa and Decimal to Hexadecimal vice versa. Logic gates: OR,AND,NOT gates, truth tables, NAND, NOR as universal gates, Exclusive – OR gate, De Morgan’s Laws – statement and proof, Half and Full adders.
- Quantum Mechanics: de Broglie’s hypothesis — wavelength of matter waves, properties of matter waves, Properties of matter waves Phase and group velocities. Davisson and Germer experiment. Double slit experiment. Standing de Brogile waves of electron in Bohr orbits. Heisenberg’s uncertainty principle for position and momentum (x and px), Energy and time (E and t). Gamma ray microscope. Diffraction by a single slit. Position of electron in a Bohr orbit. Particle in a box. Complementary principle of Bohr. Schrodinger time independent and time dependent wave equations. Wave function properties — Significance. Basic postulates of quantum mechanics. Operators, Eigen functions and Eigen values, expectation values. Application of Schrodinger wave equation to particle in one and three dimensional boxes, potential step and potential barrier.
- Nuclear Physics: Basic properties of nucleus — size, charge, mass, spin, magnetic dipole moment and electric quadrupole moment. Binding energy of nucleus, deuteron binding energy, p-p and n-p scattering (concepts), nuclear forces. Nuclear models — liquid drop model, shell model. Range of alpha particles, Geiger — Nuttal law. Gammow’s theory of alpha decay. Geiger — Nuttal law from Gammow’s theory. Beta spectrum — neutrino hypothesis, Fermi’s theory of 13 —decay.
- Solid State Physics: Crystalline nature of matter. Crystal lattice, Unit Cell, Elements of symmetry. Crystal systems, Bravais lattices. Miller indices. Simple crystal structures (S.C., BCC, CsCI, FCC, NaCI diamond and Zinc Blends) Diffraction of X —rays by crystals, Bragg’s law, Experimental techniques – Laue’s method and powder method.
Chemistry Syllabus (Marks : 50)
- Atomic structure and elementary quantum mechanics
Black body radiation, Planck‘s radiation law, photoelectric effect, heat capacity of solids, Compton effect, De Broglie‘s hypothesis. Heisenberg‘s uncertainty principle, Sinusoidal wave equation, Hamiltonian operator, Schrodinger‘s wave equation, and its importance. Physical interpretation of the wave function, significance - Chemical Bonding Ionic solids
lattice and solvation energy, solubility of ionic solids rule, power and polarizability of ions, covalent nature of ionic bond, covalent bond – stereochemistry of inorganic molecules-Common hybridization and shapes of molecules. Molecular orbital theory: Shapes and sign convention of atomic orbital, modes of overlapping. concept of and bonds, criteria for forming molecular orbital from atomic orbital. LCAO concept. types of molecular orbital- bonding, antibonding and non bonding, electron density distribution diagram for H2 + , MOED of homonuclear – H2,He2+,B2, C2, N2, O2, F2(unhybridized diagrams only) and hetero nuclear diatomic molecules CO, CN- ,NO, NOand HF. Bond order and magnetic properties. - Periodic properties
Review of trends in atomic and ionic radii – covalent radii – single, double and triple bond covalent radii, vander Waal radii. radii of cations, anions isoelectronic ions, ionization energy Electropositivity, basic nature, reducing behavior, electron affinity and electro negativity. Methods of determination and evaluation – Pauling’s and Mulliken’s approach, application in predicting and explaining chemical behavior – nature of bond, bond length and bond angles, diagonal relationship. - s-block and p-block elements
Comparative study, salient feature of Hydrides ionic and covalent, polynuclear, complex hydrides, reducing properties, oxides- monoxides and super oxide basicity, oxidizing nature. Complexation tendencies,
Comparative study of group 13 -17. Hydrides – Classification – ionic, covalent, metallic and complex hydrides. Synthesis of each class of hydrides Structure of
(a) covalent hydrides, electron deficient hydrides, Diborane, decaborane.
(b) complex hydrides – borohydrides. Reactivity – stability, hydrolysis and reducing properties. Oxides – Classification – a) Normal – acidic, basic amphoteric and neutral, b) mixed, c) suboxide, d) peroxide, e) super oxide. Structure of oxides of C, N, P, S and Cl. Reactivity – thermal stability, hydrolysis. Halides classification ionic, covalent and complex halides. Structure of halides of B, C, Si, N, P, S. Reactivity – stability, hydrolysis. Lewis acid nature of boron trihalides. Oxy -acids – Oxy – acids of B, C, N, P, S and CI – structure and acidic nature. Carboranes – nomenculature, classification- closo, nido, and arachno, preparation and structure. Borazole – preparation properties and structure. Carbonyls –classification – mono and poly nuclear general preparation, structure and bonding in Ni(CO)4, Fe(CO)5 andCo2(CO)8. - d-block-elements
Chemistry of elements of First Transition series – electronic configuration, metallic nature, atomic and ionic radii, ionization potential-Oxidation state – relative stability of various oxidation states, ionic and covalent character, acidic and basic nature, oxidizing and reducing nature of various oxidation states, redox potential – Frost and Latimer diagrams – stability, disproportionation and comproportionation of different oxidation states. colour d-d transition, colour and spectral behaviour of transition metal ions with respect of d’-d 2 configuration. Magnetic behavior determination of magnetic moment, Gouy’s balance. paramagnetism, diamagnetism. Complexation behaviour, stability of complexes – oxidation states, pi complexes, class a, class-b and class-a/b acceptors. Catalytic properties – important examples. Chemistry of elements of Second and Third transition series – comparative treatment with their 3d analogues with respect to oxidation state, magnetic behavior, spectral properties. Study of Ti, Cr and Cu triads – Titanium triad – electronic configuration, reactivity of +III and +IV states – oxides, halides. Chromium triad – reactivity of +III and +VI states, Copper triad – reactivity of +I, +II, and +III states. - f-block elements Chemistry of Lanthanides
electronic structure, position in periodic table, oxidation state, Atomic and ionic radii, Lanthanide contraction – cause and consequences, anomalous behaviour of post lanthanides, basicity, Complexation-type of donor ligands preferred, magnetic properties- paramagnetism. Colour and spectra f-f transition. Occurrence and separation-ion exchange method, solvent extraction. Chemistry of Actinides-General features-electronic configuration, oxidation state, actinide contraction, colour and complex formation. Comparison with lanthanides. - Metals Theories of bonding in metals
Free electron theory – thermal and electrical conductivity of metals, drawbacks. Valence bond theory – explanation of metallic properties and its limitations. Band theory explanation of metallic properties, conductors, semi conductors and insulators. General methods involved in extraction of metals – minerals and ores, ore concentration – electromagnetic separation, gravity separation – wilfley table, hydraulic classifier, leaching, froth flotation. Calcination and roasting Acid and alkali digestion. Reduction of oxides, carbonates, halides, sulphides, sulphates – smelting, flux, auro reduction, alumino – thermic reduction, hydrometallurgy, electrolytic reduction. Purification of impure metals- liquation, frational distillation, zone refining oxidative processes- cupellation bassemerisation, pudding, poling, thermal decomposition, Amalgamation, Electrolysis. Alloys- Classification, substitutional solid solutions, interstitial solid solutions, intermetallic compounds, Hume – Rothery rules. Preparation of alloys fusion, electro deposition, reduction and compression. Uses ferrous and non-ferrous alloys. - Co-ordination chemistry
Nomenclature of inorganic molecules and complex compounds – A. Simple inorganic molecules – multiplying affixes, structural affixes
(i) cations – monotomic homopolyatomic,
(ii) anions – monoatomic, homopolyatomic, heteropolyatomic
(iii) radicals
(iv) isopolyanions
(v) heteropolyanions
(vi) salts and salt like compound
(vii) addition compounds. B. complex compounds -Werner’s theory – postulates, experimental evidences. Sidwick’s theory–calculation of EAN, limitations. Metal Ligand bondin in transition metal complexes – Valence bond theory – postulates, geometries of coordination number 4 – tetra hedral and square planer and 6 -octahedral. Limitations. Crystal field theory – features. Splitting of d – orbitals in octahedral, tetrahedral and square planar complexes, crystal field stabilization energy, (elementary treatment diagrams only). Magnetic properties of Transition metal complexes. Types of magnetic behavior spin only formula, calculation of magnetic moments. Electronic spectra of metal complexes d-d transitions, spectro chemical series. Determination of composition of complexes, Job’s method and mole ratio method. Stability constants, factors affecting stability of complexes. Isomerism in co-ordination compounds – Structural ionization, hydrate, linkage, coordination, coordination position and polymerization isomerism. Stereoisomerisms- geometrical and optical isomerism. Hard and soft acids and bases Classification, Pearson’s concept of hardness and softness, application of HSAB principles – stability of complexes, predicting the feasibility of a reaction.
ORGANIC CHEMISTRY - Stereochemistry of carbon compounds Molecular representations: Wedge, Fischer, Newman and saw-horse formulae. Isomerism: Definition of homomers and isomers. Classification of isomers: Constitutional and Stereoisomers – definition and examples. Constitutional isomers: chain, functional and positional isomers and metamerism. Stereoisomers: enantiomers and diastereomers – definitions and examples. Conformational and configurational isomerism- definition.
- Structural Theory in Organic Chemistry
Brief review of structural theory of organic chemistry, Hybridization, Bond length, bond angle, bond energy, curved arrow notation, drawing electron movements with half headed and double headed arrow. Types of bond fission and organic reagents (Electrophilic, Nucleophilic, and free radical reagents including neutral molecules like H2O2, BF3, NH3 & AICl3) Bond polarization: Factors influencing the polarization of covalent bonds, electronegativity – inductive effect. Application of inductive effect, (a) Basicity of amines (b) Acidity of carboxylic acids (c) Stability of carbonim ions. Resonance or Mesomeric effect, application to (a) acidity phenol, (b) acidity of carboxylic acides. Hyper conjugation and it application to stability to stability of carbonium ions. Free radicals and alkenes. Types of organic reactions: Addition electrophilic, nucleophilic and free radical Substitution – electrophilic, nuicleophilic and free radical. Elimination. Examples (mechanism not required). - Acyclic Hydrocarbons
Alkanes– IUPAC Nomenculature of hydrocarbons. Methods of preparation: hydrogenation of alkenes and alkynes Wurtz reaction, Kolbe‘s electrolysis, Corey-House reaction. Chemical reactivity – inert nature, free radical substitution mechanism, Halogenation examplesreactivity, selectivity and orientation. Conformational analysis of ethane and n-butane. Alkenes- Preparation of alkenes
(a) by dehydration of alcohols
(b) dehydrohalogenation of alkyl halides
(c) by dehalogenation of 1,2 dihalides(brief mechanism), Zaitsev‘s rule. Properties: Addition of Hydrogen – heat of hydrogenation and stability of alkenes. Addition of halogen and its mechanism. Addition of HX, Markonikov‘s rule, addition of H2O, HOX, H2SO4with mechanism and addition of HBr in the presence of peroxide (anti – Markonikov‘s addition). Oxidation – hydroxylation by KMnO4, OsO4, peracids (via epoxidation), hydroboration, ozonolysis –location of double bond. Dienes – Types of dienes, reactions of conjugated dienes – 1,2 and 1,4 addition of HBr to 1,3 – butadiene and Diels – Alder reaction. Alkynes– Preparation by dehydrohalogenation of dihalides, dehalogenation of tetrahalides acetylene from CaC2. Properties: Acidity of acetylenic hydrogen (formation of metal acetylides). preparation of higher acetylenes, Metal-ammonia reductions. physical properties. Chemical reactivity – electrophilic addition of X2, HX, H2O (tautomerism), Oxidation (formation of enediol, 1,2 diones and carboxylic acids), reduction and polymerization reaction of acetylene. - Benzene and its reactivity
Molecular formula of Benzene, structure of Benzene – open chain structure not possible, proposition of cyclic structure by kekule dynamic equilibrium, evidence based on ozonolysis experiment, concept of resonance, resonance energy. Heat of hydrogenation, heat of combustion of Benzene, mention of C-C bond lengths and orbital picture of Benzene. Concept of aromaticity – aromaticity (definition) Huckl’s rule – application to Benzenoid (Benzene, Napthalene, anthracene and Phenanthrace) and NonBenzenoid compounds (cyclopropenyl cation, cyclopentadienyl anion and tropylium cation). Reactions General mechanism of electrophilic substitution mechanism of nitration and sulfonation. Mechanism of halogenations, Friedel craft’s alkylation and acylation. Orientation of aromatic substitution – Definition ortho, para and meta directing groups. Ring activating and deactivating group with examples (Electronic Interpretation of various groups like NO2 and Phenolic). Orientation: (i) Amino methoxy and methyl groups, (ii) Carboxy, nitro, nitrile, carbonyl and sulfonic acid groups, (iii) Halogens (Explanation by taking minimum of one example from each type) - Arenes and Polynuclear Aromatic Hydrocarbons
Polynuclear hydrocarbons – Structure of naphthalene and anthracene (Molecular Orbital diagram and resonance energy) Reactivity towards electrophilic substitution. Nitration and sulphonation as examples.
Hydroxy compounds
Nomenclature and classification of hydroxyl compounds. Preparation: from carbonyl compounds. Aryl carbinols by hydroxyl methylation. Phenols –
(a) by diazotization
(b) from sulfonic acid
(c) from cumene
(d) by hydrolysis of halobenzene. Physical properties Hydrogen bonding (inter molecular and intramolecular) effect of hydrogen bonding on boiling point and water solubility Chemical properties (a) acidic nature of Phenols (b) Formation of aldoxade /phenoxides and their reaction with RX (c) replacement of OH by X using PCl5,PBr3, SOCI2 and with HX/ZnCl2. Esterifification by (a) acid halides, anhydrides and acids (mechanism) (b) Esters of inorganic acids (c) dehydration of alcohols.Oxidation of alcohols by CrO3 KMnO4. Spectral reactions of phenols – (a) Bromination,(b)Kolbe – Schmidt reaction (c) Riemer Tiemann (d) Azo coupling. Identification of alcohols by oxidation – KmnO4, Ceric ammonium nitrate – Lucas reagent; Phenols by reaction with FeCl3, and by the solubility in NaOH. Polyhydroxyl compounds Pinacol-pinacolone rearrangement Oxidative cleavage (Pb(OAc)4&HIO4).
Carbonyl compounds
Nomenclature of aliphatic and aromatic carbonyl compounds and isomerism. Synthesis of aldehydes & ketones from acid chloride by using 1,3-dithianes, nitriles and from carboxylic acids. Base catalysed reactions with particular emphasis on Aldol, Cannizaro reaction, Perkin reaction, Benzoin condensation, haloform reaction, Knoevengeal condensation. Oxidation reactions –KMnO4 oxidation and auto oxidation, reduction –catalytic hydrogenation, Clemmenson‘s reduction, Wolf-kishner reduction, MPV reduction, reduction with LAH, NaBH4. Analysis – 2,4 –DNP test, Tollen‘s test, Fehlings test, Scihff‘s test, haloform test (with equations). Introduction to carbonyl compounds.
Nitrogen compounds
Nitro hydro carbons: Nomenclature and classification – nitro hydrocarbons – structure. Tautomerism of nitroalkanes leading to acid and keto form. Preparation on Nitroalkanes. Reacivity – halogenation, reaction with HONO (“Nitrous acid), Nef reaction and Mannich reaction leading to Michael addition and reduction. Aromatic Nitro hydrocarbons: Nomenclature, Preparation of Nitrobenzene by Nitration (mechanism), from diazonium salts. Physical properties, chemical reactivity – orientation of electrophilic substitution on nitrobenzene. Reduction reaction of Nitrobenzenes in different media. Amines (AIiphatic and Aromatic): Nomenculature, classification into 1°, 2°, 3° Amines and Quaternary ammonium compounds. preparative methods –
1. Ammonolysis of alkyl halides
2. Gabriel synthesis
3. Hoffman’s bromamide reaction (mechamism). Reduction of Amides and Schmidt reraction. Chemical Properties: (a) Alkylation (b) Acylation (c) Carbylamine reaction (d) Hinsberg separation. Reaction with Nitrous acid of 1°, 2°, 3° (Aliphatic’and aromatic amines). Electophilic substitutions of Aromatic amines – Bromination and Nitration, oxidation of aryl and 3° Amines, diazotization. 6. Diazonium salts Preparation with mechanism. Synthetic importance – (a) Replacement of diazonium group by- OH, X (Cl) Sandmeyer and Gatterman reaction, by fluorine Schiemann’s reaction), by iodine, CN, NO2, H and aryl groups. Coupling Reraction of diazonium (i) with phenols (ii) with anilines. Reduction to phenyl hydrazines. - Heterocyclic Compounds
Introduction and definition: Simple 5 membered ring compounds with one hetero atom Ex. Furan. Thiophene and pyrrole. Importance of ring systems –presence in important natural products like hemoglobin and chlorophyll. Numbering the ring systems as per Greek letter and Numbers. Aromatic character –6-electron system (four-electrons from two double bonds and a pair of non-bonded electrons from the hetero atom). Tendency to undergo substitution reactions. - Carbohydrates Introduction
Classification and nomenclature –classification into mono, oligo and polysaccharides, into pentoses, hexoses etc., into aldoses and ketoses. Monosaccharides: All discussion to be confined to (+) glucose as an example of aldo hexoses and (-) fructose as example of ketohexoses. Chemical properties and structural elucidation: Evidences for straight chain pentahydroxy aldehyde structure (Acetylation, reduction to nhexane, cyanohydrin formation, reduction of Tollen‘s and Fehling‘s reagents and oxidation to gluconic and saccharic acids). Number of optically active, isomers possible for the structure, configuration of glucose based on D-glyceraldehyde as primary standard (No proof for configuration is required). Evidence for cyclic structure of glucose (some negative aldehyde tests and mutarotation).
Cyclic structure of glucose
Proposition of cyclic structure (Pyranose structure, anomeric Carbon and anomers). Proof for the ring size (methylation, hydrolysis and oxidation reactions). Different ways of writing pyranose structure (Haworth formula and chair conformational formula). Structure of fructose: Evidence of 2 –ketohexose structure (formation of penta acetate, formation of cyanohydrin its hydrolysis and reduction by HI to give 2-Carboxy-nhexane Same osazone formation from glucose and fructose, Hydrogen bonding in osazones, cyclic structure for fructose (Furanose structure,Haworth formula). Inter Conversion of Monosaccharides: Aldopentose to aldo hexose –eg: Arabinose to Dglucose, D-mannose (kiliani –Fischer method). Epimers, Epimerisation-Lobry debruyn van Ekenstein rearrangement. Aldohexose –Aldopentose eg: D-glucose to D-arabinose by Ruff‘s degradation. Aldohexose(+) (glucose) to ketohexose (–)(Fructose) and Ketohexose (Fructose) to aldohexose (Glucose). - Amino acids and proteins Introduction: definition of amino acids, classification of amino acids alpha, beta and gama amino acids. Natural and essential amino acids definition and examples, classification of alpha amino acids into acidic, basic and neutral amino acids with examples. Methods of synthesis: General methods of synthesis of alpha amino acids (specific examples –Glycine, Alanine, valine and Leucene) by following methods: a) From halogenated Carboxylic acid b)Malonic ester synthesis c) strecker‘s synthesis. Physical properties: Optical activity of naturally occurring amino acids: L –configuration, irrespective of sign of rotation. Zwitter ion structure –salt like character, solubility, melting points, amphoteric character, definition of isoelectric point. Chemical properties: General reactions due to amino and carboxyl groups –Lactams from gamma and delta amino acids by heating peptide bond (amide linkage). Structure and nomenclature of peptides and proteins, peptide synthesis.
PHYSICAL CHEMISTRY - Gaseous State
Deviation of real gases from ideal behavior. Vander Waals equation of state. Critical phenomenon. PV-isotherms of real gases, continuity of state. Andrew‘s isotherms of CO2. The vander Waal‘s equation and critical state. Derivation of relationship between critical constants and van der Waal‘s constants. Experimental determination criteria constants. The law of corresponding states, reduced equation of states. Joule Thomson effect and inversion temperature of a gas. Liquid action of gases: i) Linde‘s method based on Joule Thomson effect ii) Claude‘s method based on adiabatic expansion of a gas. - Liquid State
Intermolecular forces, structure of liquids (qualitative description). Structural differences between solids, liquids and gases. Liquid crystals, the mesomorphic state: Classification of liquid crystals into Semectic and Nematic, differences between liquid crystal and solid / liquid. Application of liquid crystals as LCD devices, lubricants and in digestion/ assimilation of food. - Solid state
Laws of Crystallography – (i) Law of Constancy of interfacial angles (ii) Law of Symmetry, Symmetry elements in crystals (iii) Law of rationality of indices. Definition of space lattice, unit cell. Bravais Lattices and Seven Crystal systems structure of NaCl (Bragg‘s method and Powder method). Defects in crystals. Stoichiometric and non stoichiometric defects. Band theory of semiconductors: Extrinsic and intrinsic semi conductors, n-type and p-type and their applications in photo electro chemical cells. - Dilute Solutions & Colligative Properties
Dilute Solutions, Colligative Properties, ideal and non ideal solution. Raoult‘s law, relative lowering of vapour pressure, molecular weight determination. Osmosis – laws of osmotic pressure, its measurement, determination of molecular weight from osmotic pressure. Elevation of boiling point and depression of freezing point. Derivation of relation between molecular weight and elevation in boiling point and depression in freezing point. Experimental methods for determining various colligative properties. Abnormal molar mass, Van‘thoff factor, degree of dissociation and assocoation of solutes. - Colloids& surface chemistry
Definition of colloids. Classification of colloids. Solids in liquids (sols): preparations and properties – Kinetic, Optical and Electrical: stability of colloids Protective action. Hardy– Schultz law, Gold number. Liquids in liquids (emulsions): Types of emulsions, preparation and emusifier. Liquids in solids(gels); Classification, preparations and properties, inhibition, General applications of colloids. - Solutions
Liquid – liquid mixtures, ideal liquid mixtures, Raoult‘s and Henry‘s laws. Non ideal systems. Axeotropes HCl-H2O and C2H5OH – H2O systems. Fractional distillation,. Partially miscible liquids- Phenol – Water, Trimethyl amine – Water and Nicotine –Water systems. Lower upper consolute temperatures. Effect of impurity on consolute temperature. Immiscible liquids and steam distillation. - Chemical Kinetics
Rate of reaction, Factors influencing the rate of a reaction -concentration, temperature, pressure, solvent, light and catalyst. Concentration dependence of rates, mathematical charecteristics of simple chemical reactions- Zero order, first order, second order, pseudo first order, half life and mean life. Determination of order of a reaction- differential method, method of integration, half life method and isolation method. Radio active decay as first order phenomenon. Arrhenius equation and concept of activation energy. Theories of chemical kinetics: effect of temperature on rate of reaction. Simple collision theory based on hard sphere model. - Thermodynamics
Definition of Thermodynamic terms: System, surroundings. types of systems, and intensive and extensive properties. State and path functions and their differentials. Thermodynamic process. Concept of heat and work. First law of Thermodynamics: Statement, definition of internal energy and enthalphy. Heat capacity, heat capacities at constant volume and pressure and their relationship. Joule’s law – Joule. Thomson coefficient and inversion temperature. Calculation of w,q, dU and dH for the expansion of ideal gases under isothermal and adiabatic conditions for reversible process. Temperature dependence of enthalpy – Kirchoffs equation. Second law of thermodynamic need for the law, different statements of the law. Carnot cycle and its efficiency, Carnot Theorem. Thermodynamic scale of temperature. Concept of entropy, entropy as a state function, entropy as a function of V and T, entropy is a function of P & T entropy change in physical processes. Gibbs and Helmholtz functions(G) and Helmholtz functions(A) as thermodynamic quantities. A&G as a criteria for thermodynamic equilibrium and spontaneity, their advantage over entropy change. Variation of G with P, V and T. - Electrochemistry & EMF
Electrical transport – conduction in metals and in electrolyte solutions, specific conductance and equivalent conductance, measurement of equivalent conductance, variation of specific and equivalent conductance with dilution. Migration of ions and Kholrausch‘s law, Arrhenius theory of electrolyte dissociation and its limitations, weak and strong electrolytes, Ostwald‘s dilution law, its uses and limitations. Debye-Huckel-Onsagar‘s equation for strong electrolytes (elementary treatment only). Transport number, definition and determination by Hittorf‘s method for attackable electrodes. Applications of conductivity measurements: Determination of degree of dissociation, determination of Ka of acids, determination of solubility product of a sparingly soluble salt, conductometric titrations. Electrolyte and Galvanic cells – reversible and irreversible cells, conventional representation of electrochemical cells. EMF of a cell and its measurement. Computation of EMF. Types of reversible electrodes- the gas electrode, metal-metal ion, metal-insoluble salt and redox electrodes. Electrode reactions, Nernst equation, cell EMF and single electrode potential, standard Hydrogen electrode – reference electrodes (calamel electrode) – standard electrode potential, sign conventions, electrochemical series and its significance. Applications of EMF measurements, Calculation of thermodynamic quantities of cell reactions (G, H and K). Determination of pH using hydrogen electrode, glass electrode and quinhydrone electrode, Solubility product of AgCl. Potentiometric titrations. - Photochemistry
Introduction to photochemical reactions, Difference between thermal and photochemical reactions, Laws of photo chemistry-Grotthus -Draper law, Stark –Einstein‘s Law of photo chemical equivalence. Quantum yield. Examples of photo chemical reactions with different quantum yields. Photo chemical combinations of H2–Cl2and H2–Br2reactions, reasons for the high and low quantum yield. Problems based on quantum efficiency, Consequences of light absorptions. Singlet and triplet states. Jablonski diagram Explanation of internal conversion, inter-system crossing, Phosphorescence, fluorescence.
GENERAL CHEMISTRY - Molecular spectroscopy Introduction to electromagnetic radiation, interaction of electromagnetic rations with molecules, various types of molecular spectra.
- Rotational spectroscopy (Microwave spectroscopy) Rotational axis, moment of inertia, classification of molecules (based on moment of inertia), rotational energies, selection rules, determination of bond length of rigid diatomic molecules eg. HCl.
- Infra red spectroscopy Energy levels of simple harmonic oscillator, molecular vibration spectrum, selection rules. Determination of force constant. Qualitative relation of force constant to bond energies. Anharmonic motion of real molecules and energy levels. Modes of vibrations in polyatomic molecules. Characteristic absorption bands of various functional groups. Finger print nature of infrared spectrum.
- Electronic spectroscopy
Bonding and antibonding molecular orbitals,electronic energy levels of molecules (σ, π, n),types of electronic transitions:σ-σ*, n-σ*, n-л*, л-л* with suitable examples. Selection rules, Terminology of chromophore, auxochrome, bathochromic and hypsochromic shifts. Absorption of characteristics of chromophones: diene, enone and aromatic chromophores. Representation of UV-visible spectra. - Photochemistry
Introduction to photochemical reactions, Differences between thermal and photochemical reactions, Laws of photo chemistry –Grotthus – Draper law, Start – Einstein‖s Law of photo chemical equivalence. Quantum yield. Examples of photo chemical reactions with different quantum yields. Photo chemical combinations of H2 – Cl2 and H2 – Br2 reactions, reasons for the high and low quantum yield. Problems based on quantum efficiency, Consequences of light absorptions. Singlet and triplet states. Japlonski diagram Explanation of internal conversion inter-system crossing, Phosphorescence, fluorescence.
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