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UPPSC 2010 Syllabus for Chemistry (Subject Code 4):

1. Inorganic Chemistry:

1. 1. Atomic Structure: Elementary particles, Boh's and Sommerfeld models of the atom, Wave-particle duality De-Brogile equation, Heisenberg uncertainty principle, elementary ideas of Schrodigner wave equation, atomic number, electronic configuration of elements. Pauli's exclusion principle, Hund's rule of maximum spin multiplicity, aufbau principle, Long form of periodic classification of elements.
   2. Nuclear Chemistry: Natural and artificial radio-activity, half-life period, nuclear reactions, fission and fussion reactions, uses of radioactive isotopies.
2. Periodic Properties of the Elements: Atomic, covalent, Vander Wall and ionic, radii, ionization potential, electron affinity and electronegativity.
3. Salient features of s,p,d and f-block elements.
4. Chemical Bonding: Ionic, covalent (polar and non-polar), coordinate bonds, s-and p-Hydrogen bonding, concept of hybridization of atomic orbitals (sp, sp2, sp3, sp3d, sp3d and sp3d3). Prediction of shapes of simple inorganic molecules on the baiss of VSEPR theory Elementary ideas of molecular orbital theory.
5. General principles of extraction and purification of metals.
6. Structure and Bonding of: Diborane, boric acid, anhydrous aluminium chloride, nickle carbonyl and Xenon fluorides.
7. Redox Reactlons: Oxidation states, oxidation number, equivalent weights of oxidising and reducing agents, balancing of redox reactions.
8. Coordination Chemistry: Double salts and coordination compounds, Wemar's theory, Effective atomic number (EAN), Electronic configuration of complexes, IUPAC system of nomenclature.

1. Environment Pollution: Pollutants and their influence on environment.
2. Organic Chemistry:
1. Bonding in Carbon Compunds: sp, sp2 & sp3 hybridization, s-and p-bonds, inductive and electromeric effects, hyperconcjugation, reasonance.
2. Reaction Mechanism: Hemolytic and uerolytic the cleavage of bonds (free radicals carbonium ion and carbon ion) Addition and substitution reactions (E1, E2, SN1 and SN2, reactions).
3. Hydrocarbons: Studies of alkanes, alkenes, and alkynes.
4. Prespartion and Properties of the following Allphtaic Compounds: Halides, alcohols, ethers, aldehydes, ketones, acids, esters, amines, amides and hydroxyacids (lactric citric, maleic and fureirc acids).
5. Carbohydrates: Classification and general reactions, Structure of glucose, fructose and socurse.
6. Organometallic Compounds: Grignard reagents and their synthetic applicaticns.
7. Stereochemistry: Optical and geometrical isomerism, concept of conformation, Environmental pollution and control, plants as indicator of pollution.
8. Benzene and Its Simple Derivations: Benzene, toluene, xylene, phenols, halides, nitro and amino compounds, Benzoic, salicylic, cinnamic, mandelic and sulphonic acids, Aromatic aldehydes and ketones, Diazo and hydrazo compounds, Naphthalene, pyridine and quinoline.
9. Elementary idea of the chemistry of oils, tats, proteins, vitamins and their roles in nutrition and industry.
10. Basic principles involving spectral techniques (UV.visible i.n).

2. Physical Chemistry:

1. Gaseous State: Kinetic theory of gases and gas laws, Maxwell's law of distribution of velocities, vander Waals equation Critical behaviour of gases law of corresponding states, heat capacities of gases.
2. Physical Properties and Molecular Constitution: Molar volume, parachor, molar refraction, molar polarisation and dipolemoment.
3. Liquid state: Propertie of liquids, viscosity, surface tension and vapour pressure.
4. Solutions: Raoult's law, lowering of vapour pressure, depression of freezing point, elevation of boiling point, osmotic pressure, Determination of molecular weight of solutes, Association and dissociation of solutes.
5. Thermodynamics: The first law of thermodynamics, isothermal and adiabatic expansions. Joule-Thomson effect, enthalpy, heat capacities, Enthalpies of reaction formation, combustion and solution, Bond energies, Kirchoffs equation, second law of thermodynamics, entropy, free energy, Criteria of spontaneity and chemical equilibrium.
6. Chemical Equilbria: Law of mass action and its application to homogeneous and heterogeneous. Le-chatelier principle and its application to chemical equilibria.
7. Chemical Kinetics: Molecularity and order of reaction. First order and second order reactions. Determination of order of a reaction. Effect of temperature of reaction rate, energy of activation. Collision theory of reaction rates, theory of activated complex.
8. Electrochemistry: Faraday's laws of electrolysis, conductivity of an electrolyte, equivalent conductivity and its variation with dilution. Transport number, solubility of sparingly soluble salts.
9. Ionic Equilibria: Electrolytic dissociation, Ionic product of water, Ostwald dilution law, theory of strong electrolytes. Solubility product Acids & Bases (Bronsted concept and Lewis concept), acids and bases, hydroysis of salts, hydrogen ion concentration, pH, buffer solutions, theory of indicators.
10. Reversible Cells: Standards hydrogen and colomel electrodes, Electrodes and redox potentials, Concentration Cells.
11. Phase Rule: Explanation of terms involved. Application to one and two component systems, Distribution law.
12. Colloids: General nature of colloidal solutions and their classfication, General methods of preparation and properties of colloids. Coagulation, protective action and gold number. Adsorption, physiosorption and chemisorption, Freundlisch and langmuir isotherms.
13. Catalysis: Homogenous and heterogeneous catalysis. Catalytic promoters and poisoning.
14. Problems: Simple numerical and conceptual problems based on the full syllabus.

UPPSC Preliminary Exam 2010 Syllabus for Chemistry