KEAM Physical and Inorganic Chemistry Syllabus

Physical and Inorganic Chemistry syllabus — full chapter and topic list

Expand any chapter to see its topics and sub-topics. This is the whole examinable outline for Physical and Inorganic Chemistry in KEAM, not a summary of it.

1. 1

   Basic Concepts and Atomic Structure

   3 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and molar mass
     • Stoichiometry and limiting reagent
     • Empirical and molecular formulae
   • Structure of Atom
     • Bohr model and atomic spectra
     • Quantum numbers and orbitals
     • Electronic configuration and Hund's rule
   • Classification of Elements and Periodicity
     • Modern periodic law and trends
     • Ionization enthalpy, electronegativity, atomic radius
2. 2

   Chemical Bonding and States of Matter

   3 topics

   • Chemical Bonding and Molecular Structure
     • Ionic and covalent bonding
     • VSEPR theory and hybridisation
     • Molecular orbital theory and hydrogen bonding
   • States of Matter
     • Gas laws and ideal gas equation
     • Kinetic molecular theory
     • Real gases and van der Waals equation
   • The Solid State
     • Crystal lattices and unit cells
     • Packing efficiency and density
     • Defects and electrical/magnetic properties
3. 3

   Physical Chemistry: Energetics and Dynamics

   4 topics

   • Thermodynamics
     • First law, enthalpy and Hess's law
     • Entropy and Gibbs free energy
     • Spontaneity criteria
   • Equilibrium
     • Law of mass action and Kc, Kp
     • Le Chatelier's principle
     • Ionic equilibrium, pH and buffers
   • Chemical Kinetics
     • Rate law and order of reaction
     • Integrated rate equations
     • Arrhenius equation and collision theory
   • Solutions
     • Concentration terms and Raoult's law
     • Colligative properties
     • Van't Hoff factor and abnormal molar mass
4. 4

   Electrochemistry and Redox

   3 topics

   • Redox Reactions
     • Oxidation number and balancing
     • Redox titrations
   • Electrochemistry
     • Galvanic cells and electrode potential
     • Nernst equation and EMF
     • Conductance and electrolysis
   • Surface Chemistry
     • Adsorption and catalysis
     • Colloids and emulsions
5. 5

   Inorganic Chemistry of Elements

   5 topics

   • Hydrogen and s-Block Elements
     • Hydrogen, water and hydrides
     • Alkali metals and their compounds
     • Alkaline earth metals
   • The p-Block Elements
     • Group 13 to 18 trends
     • Compounds of boron, carbon and nitrogen
     • Oxygen, halogen and noble gas chemistry
   • The d- and f-Block Elements
     • Transition metal properties and oxidation states
     • Lanthanoids and actinoids
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in coordination compounds
     • Valence bond and crystal field theory
   • Metallurgy and Environmental Chemistry
     • Principles of isolation of metals
     • Thermodynamic and electrochemical principles
     • Environmental pollution

Physical and Inorganic Chemistry flashcards for KEAM

20 of 51 cards from the Physical and Inorganic Chemistry deck — real questions with worked answers.

1. State the law of conservation of mass.

   Matter can neither be created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products.

2. What is the difference between molarity (M) and molality (m)?

   Molarity = moles of solute per litre of solution (temperature-dependent). Molality = moles of solute per kilogram of solvent (temperature-independent).

3. What is the value of Avogadro's number, and what does it represent?

   6.022 x 10^23; the number of particles (atoms, molecules, ions) in one mole of a substance.

4. Define limiting reagent.

   The reactant that is completely consumed first in a reaction, thereby determining the maximum amount of product formed.

5. Give the de Broglie equation relating wavelength to momentum.

   lambda = h / (mv) = h / p, where h is Planck's constant, m is mass, and v is velocity.

6. State Heisenberg's uncertainty principle as an equation.

   Delta-x . Delta-p >= h / (4*pi); position and momentum cannot both be measured exactly at the same time.

7. What do the four quantum numbers n, l, m, and s represent?

   n = principal (shell/energy), l = azimuthal (subshell/shape), m = magnetic (orbital orientation), s = spin (+1/2 or -1/2).

8. State the Aufbau principle.

   Electrons fill orbitals in order of increasing energy, lowest energy orbital first (following the n+l rule).

9. State Hund's rule of maximum multiplicity.

   Electrons occupy degenerate orbitals singly with parallel spins before any orbital is doubly occupied.

10. What is Pauli's exclusion principle?

    No two electrons in an atom can have the same set of all four quantum numbers; an orbital holds a maximum of two electrons with opposite spins.

11. How does atomic radius vary across a period and down a group?

    It decreases across a period (left to right) due to increasing nuclear charge, and increases down a group due to added shells.

12. Define ionization enthalpy and state its trend in the periodic table.

    Energy required to remove the most loosely bound electron from a gaseous atom. It increases across a period and decreases down a group.

13. Which element has the highest electronegativity, and on what scale?

    Fluorine, with a value of 4.0 on the Pauling scale.

14. State the basis of the modern periodic law.

    Physical and chemical properties of elements are a periodic function of their atomic numbers.

15. What is the shape and hybridization of methane (CH4)?

    Tetrahedral shape with sp3 hybridization and a bond angle of 109.5 degrees.

16. According to VSEPR theory, what shape does a molecule with 3 bond pairs and 1 lone pair (e.g. NH3) adopt?

    Trigonal pyramidal (bond angle ~107 degrees).

17. What is the difference between a sigma bond and a pi bond?

    A sigma bond forms by head-on (axial) overlap of orbitals and is stronger; a pi bond forms by sideways (lateral) overlap and is weaker.

18. State the bond order formula in molecular orbital theory.

    Bond order = (number of bonding electrons - number of antibonding electrons) / 2.

19. Why is O2 paramagnetic according to MO theory?

    It has two unpaired electrons in its pi-antibonding (pi*) molecular orbitals.

20. State the ideal gas equation and define each term.

    PV = nRT, where P = pressure, V = volume, n = moles, R = gas constant, T = temperature in Kelvin.

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