Syllabus For AIPMT - 2009 chemistry

1. Some basic concepts in Chemistry

Importance of Chemistry, physical quantities and their measurement in Chemistry, SI Units, uncertainty in measurements and use of significant figures, Unit and dimensional analysis, Matter and its nature, laws of chemical combinations, atomic, and molecular, masses mole concept, molar masses, percentage composition and molecular formula, chemical stoichiometry.

2. States of matter

Three states of matter, gaseous state, gas laws (Boyle's Law and Charles Law), Avogadro's Law, Grahams'Law of diffusion, Dalton's law of partial pressure, ideal gas equation, Kinetic theory of gases, real gases and deviation from ideal behaviour, van der Waals’ equation, liquefaction of gases and critical points, Intermolecular forces; liquids and solids.

3. Atomic structure

Earlier atomic models (Thomson's and Rutherford) , emission spectrum of hydrogen atom, Bohr's model, of hydrogen atom, Limitations of Bohr’s model, dual nature of matter and radiation, Heisenberg uncertainty principle, quantum mechanical model of atom (quantum designation of atomic orbitals and electron energy in terms of principal, angular momentum and magnetic quantum numbers), electronic spin and spin quantum numbers, Pauli’s exclusion principle, general idea of screening (constants) of outer electrons by inner electrons in an atom, Aufbau principle, Hund's rule, atomic orbitals and their pictorial representation, electronic configurations of elements.

4. Classification of elements and periodicity in properties

Need and genesis of classification of elements (from Doebereiner to Mendeleev), Modern periodic law and present form of periodic table, Nomenclature of elements with atomic number > 100, electronic configurations of elements and periodic table, electronic configuration and types of elements and s, p, d and f blocks, periodic trends in properties of elements (atomic size, ionization enthalpy, electron gain enthalpy, valence/ oxidation states and chemical reactivity).

5. Chemical energetics

Some basic concepts in thermodynamics, first law of thermodynamics, heat capacity, measurement of Uand H, calorimetry, standard enthalpy changes, thermochemical equations, enthalpy changes during phase transformations, Hess's Law, standard enthalpies of formation, bond enthalpies and calculations based on them.

6. Chemical bonding

Kossel -Lewis approach to chemical bond formation, ionic bonds, covalent bonds, polarity of bonds and concept of electronegativity, valence shell electron pair repulsion (VSEPR) theory , shapes of simple molecules, valence bond theory, hybridization involving s, p and d orbitals and shapes of molecules  and  bonds; Molecular orbital theory involving homounclear diatomic molecules; Hydrogen-bonding.

7. Equilibrium

Equilibrium in physical and chemical processes
Equilibrium in physical and chemical processes, dynamic equilibrium, law of chemical equilibrium and equilibrium constant, homogeneous equilibrium, heterogenous equilibrium, application of equilibrium constants, Relationship between reaction quotient Q, equilibrium constant, K and Gibbs’ energy G; factors affecting equilibrium-Le Chateliar's principle.
Ionic equilibrium
Acids, Bases and Salts and their ionization, weak and strong electrolytes degree of ionization and ionization constants, concept of pH, ionic product of water, buffer solution, common ion effect, solubility of sparingly soluble salts and solubility products.

8. Redox reactions

Electronic concepts of reduction - oxidation, redox reactions, oxidation number, balancing of redox reactions.

9. Solid state Chemistry

Classification of solids based on different binding forces: molecular, ionic, covalent and metallic solids, amorphous and crystalline solids; unit cells in two dimensional and three dimensional lattices, calculation of density of a unit cell, packing in solids, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical and magnetic properties.

10. Chemical thermodynamics

Spontaneous processes, energy and spontaneity , entropy and second law of thermodynamics, concept of absolute entropy, Gibbs energy and spontaneity, Gibbs energy change and equilibrium constant.
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