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JSSC Download Admit Card PGTTCE 2016 Post Graduate Trained Teacher Competitive Examination : Jharkhand Staff Selection Commission

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Organisation : Jharkhand Staff Selection Commission(J.S.S.C.)
Announcement : Download Admit Card
Designation : PGTTCE-2016 Post Graduate Trained Teacher Competitive Examination

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Chemistry Syllabus :
1. Atomic structure, Periodic properties and chemical bonding — Idea of de Broglie matter waves, Heisenberg uncertainty principle, atomic orbitals, Schrodinger wave equation, significance, quantum numbers, radial and angular wave functions and probability distribution curves, shapes of S, p, and d orbitals, Aufbau and Pauli’s exclusion principles, Hund’s rule, electronic configuration classification of elements as s, p, d and f-blocks.

Periodic tables and periodic properties (atomic and ionic radii, ionization energy, electron affinity, electronegativity) and their trends in periodic table, Their applications in chemical bonding. Covalen bonding. V.B. Theory, VSEPR Theory, M O. Theory, homonuclear and heteronuclear diatomic molecules, bond order and magnetic properties.

Resonance, hydrogen bonds and vimder Waals forces. Ionic solids – Born-Haber cycle, Fajaris rule.

2. Gaseous states — Postulates of kinetic theory of gases, deviation from ideal behaviour van der Waal’s equation of state. Critical temperature, pressure and volume.

Liquification of gases, Critical constants and vander Waals constants, the law of corresponding states, reduced equation of state Molecular velocities — r:m.s. velocity, average velocity, most probable velocity. Maxwell’s distribution of molecular velocities.

3. Solid State — Space lattice, Unit cell. Laws of crystallography. X-ray diffraction by crystals. Bragg’s equation coordination number radius ratio rule, detects in crystals and their magnetic and electric behaviour semi-conductors and super conductors

4. Thermodynamics — Law of thermodynamics, work, heat, energy. State functions — E, H, S and G and their significance criteria for chemical equilibrium and sponteinity of reactions.

Variations of free energy with T, P and V Gibbs Helmhotts equation. Entropy changes in gases for reversible and irreversible processes. Hess law Bond energy.

5. Chemical kinetics and catalysis — Order and molecularity, chemical kinetics and its scope, rate of a reaction, factors influencing rate of reaction. Rate equations of zero, first and second order reactions. Pseudo order, half life and mean life. Determination of order of reactions.

Theories of chemical kinetics — collision theory, transition state theory, Arrhenius equation, concept of activation energy, effect of temperature on rate constant. Catalysis, characteristics of catalysed reactions, theories of catalysis, examples.

6. Electrochemistry — Electronic conduction in electrolytic solutions, specific, equivalents and molar conductances, effect of dilution on them, cell constant, experimental method of determining conductance.

Migration of ions and Kohlrausch, law. Arrhenius theory of electorlytic dissociation and its limitations, weak and strong electrolytes Ostwald’s dilution law, its uses and limitations Debye – HuckelOnsager’s equation (elementary treatment) Transport number – definition, determination by Hittor method.

Galvanic cells, electrodes and electrode reactions, Nernst equation, E.M.F. of cells, Hydrogen electrode, electrochemical series, concentration cell and their applications pH. Buffer solutions theory of buffer action,

7. Transition and inner transition metals and complexes — General characteristics of d-block elements, co-ordination components – nomenclature, isomerism and bonding in complexes V.B. theory and crystal field theory. Werners theory, eAN metal carbonyls, cyclopentadienys, olefin and acetylene complexes.

Compounds with metal-metal bonds and metal atom clusters. General chemistry of f-block elements Lanthanides and actinides – ionic radic, separation, oxidation states, magnetic and spectral properties.

8. Non-aqueous solvents — Physical properties of a solvent, types of solvents and their general characteristics, reactions in non-aqueous solvents with reference to liqued NH3 and liquid SO2.

9. Photochemistry — Interaction of radiation with matter, difference between thermal and photochemical processes. Lawa of photochemistry — Grothus-Drapper law, stark-Einstein law, Jablonski diagram. Fluerescence. phosphorescence, Quantum yield Photoelectric cells.

10. Hard and soft arids and bases — Classification of acids and bases as hard and soft, Pearson’s HSAB concept, acid-base strength and hardness and softness, symbiosis, theoretical basis of hardness and softness, symbiosis, theoretical basis of hardness and softness, electronegativity and hardness and softness.

11. Structure and Binding — Hybridization, bond lengths and bind angles bond energy, localized and delocalized chemical bond, van der Waals interactions, inclusion compounds, clatherates, charge transfer complexes, resonance, hyperunjugation, aromaticity, inductive and field effects, hydrogen bonding.

12. Mechanism of organic reactions — Homolytic and heterolytic bond breaking, types of reagents – carbocations. and nucleophiles, types of organic reactions, Reactive intermediates – Carbocations, carbanions, free radicals, carhbenes, arynes and nitrenes (with examples) Different types of addition, substitution and elimination reactions – SN1, SN2, SNi, E1, E2, E1cb etc.

13. Stereochemistry of Organic Compounds — Isomerism, Optical isomerism – elements of symmetry, molecular chirality, enantiomers, stereogenic centre, optical activity properties of enantiomers, chiral and achiral moleculers with tar stereogenic centres, diastereomers. threo and erythro diastereomers, meso compounds, resolution of enantiomers. inversion, retention and racemizarion.

Relative and absolute configuration requence rule, D & L and R & S nomenclature. Geometric isomerism: Determination of configuration of geometric isomers – E & Z nomenclature, geometric isomerism ot oximes and alecyclic compounds. Configuration and confurmation, conformations of ethane, butane and cyclohexane.

14. Organometallic Compounds — Organometallic compounds of Mg. Li & Zn their formation, preparation, structure and systhetic applications.

15. Organic Synthesis via enolates — Acidity of a-llydrogens, preparation, properties and synthetic applications of diethyl malonate and eithyl acctoacetate, keto-enol tautomeins.

16. Carbohydrates — Classification and nomenclature Monosaceharides, mechanism of asazone formation, interconversion of glucose and fructose, chain lengthening and chain shortening of aldoses and ketoses, Anomers and epimers Formation of glycosides, ethers and esters Ring structure of glucose and fructose mechanism of mutarotation.

17. Polymers — Addition or chain growth polymerization. Free radical vingt polymerization, ionic vingl polymerizations, Ziegler – Natta polymerization and vinigl polymers. Condensation or step-growth polymerization, Polyesters, polyamider, phenol-formaldelyde resins, urea-formaldelyde resins, epoxy.resins and polyurethanes.

Natural and synthetic rubbers. Inorganic polymeric systems – silicones and phosphazenes, nature of bonding in triphosphazenes

18. Study of following types of organic compounds :
a. Alkanes and cycloalkanes — Preparation of alkanes – wartz reactions Kolbe reaction, Corey – House reaction etc physical and chemical properties, free-radical halogenation of alkanes – reactivity and selectivity.
Cycloalkanes : Nomenclature, formation, properties – Baeger’s strain theory

b. Alkenes, cyclocalkenes, Dienes & Alkynes

c. Arenes and Aromaticity — Aromaticity : The Huckel rule, arematic ions, M.O. diagram, antiaromatic, Aromatic electrophilic substitution — Mechanism, role of s and p complexes.

Mechanism of nitration, halogenters sulphonation, mercuration and Friedel Crafts reaction. Energy profile diagram, activating and deactivating substituents, orientation, ortho-para ratio. Side-chain reactions of benzene derivatives. Birch reduction.

19. Study of some reactions — Pinacol – pinacotone rearrangement, aldol reaction, perkin reaction. Cannizzaro’s reaction, Mannich reaction, Clemmensen reduction, claisen rearrangement, Peimer Tiemann reaction, Friedel crafts reaction, Fries rearrangement. Reformatsky reaction.

20. Spectroscopy — Basic principles of the following type of spectroscopy and their applications in determining structures.
a. UV – Visible spectroscopy
b. IR – ”
c. NMR – ”
d. Mass – ”
e. ESR – “(cemplexes)

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