IPU CET Chemistry Syllabus

Chemistry syllabus — full chapter and topic list

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

1. 1

   Physical Chemistry I

   4 topics

   • Some Basic Concepts of Chemistry
     • Mole concept and Avogadro number
     • Stoichiometry and limiting reagent
     • Concentration terms
   • States of Matter
     • Gas laws and ideal gas equation
     • Kinetic molecular theory
     • Real gases and van der Waals equation
   • Atomic Structure
     • Bohr model and hydrogen spectrum
     • Quantum numbers and orbitals
     • Electronic configuration and Aufbau principle
   • Chemical Bonding and Molecular Structure
     • Ionic and covalent bonding
     • VSEPR theory and hybridisation
     • Molecular orbital theory
2. 2

   Physical Chemistry II

   6 topics

   • Chemical Thermodynamics
     • First law and enthalpy changes
     • Hess's law
     • Entropy, Gibbs energy and spontaneity
   • Chemical and Ionic Equilibrium
     • Law of mass action and Kc, Kp
     • Le Chatelier's principle
     • pH, buffers and solubility product
   • Chemical Kinetics
     • Rate law and order of reaction
     • Integrated rate equations
     • Arrhenius equation and catalysis
   • Electrochemistry
     • Conductance and Kohlrausch law
     • Nernst equation and EMF
     • Electrolysis and Faraday's laws
   • Solutions and Colligative Properties
     • Raoult's law
     • Elevation and depression of boiling/freezing point
     • Osmotic pressure and van't Hoff factor
   • Surface Chemistry
     • Adsorption isotherms
     • Colloids and emulsions
3. 3

   Inorganic Chemistry

   6 topics

   • Periodic Classification
     • Modern periodic law
     • Periodic trends in properties
   • s-Block Elements
     • Alkali and alkaline earth metals
     • Important compounds and anomalous behaviour
   • p-Block Elements
     • Groups 13 to 18 trends
     • Important compounds of B, C, N, O and halogens
   • d- and f-Block Elements
     • Transition metal characteristics
     • Lanthanoids and actinoids
   • Coordination Compounds
     • Werner's theory and nomenclature
     • Isomerism in complexes
     • Valence bond and crystal field theory
   • Metallurgy and Hydrogen
     • Principles of metal extraction
     • Hydrogen and its compounds
4. 4

   Organic Chemistry

   6 topics

   • Basic Principles and Techniques
     • IUPAC nomenclature
     • Inductive, resonance and hyperconjugation effects
     • Reaction intermediates and mechanisms
   • Hydrocarbons
     • Alkanes, alkenes and alkynes
     • Aromatic hydrocarbons and benzene
   • Haloalkanes and Haloarenes
     • SN1 and SN2 mechanisms
     • Elimination reactions
   • Oxygen-Containing Functional Groups
     • Alcohols, phenols and ethers
     • Aldehydes, ketones and carboxylic acids
   • Nitrogen-Containing Compounds
     • Amines and diazonium salts
     • Cyanides and nitro compounds
   • Stereochemistry and Isomerism
     • Structural isomerism
     • Optical and geometrical isomerism
5. 5

   Applied and Environmental Chemistry

   4 topics

   • Biomolecules
     • Carbohydrates and proteins
     • Vitamins and nucleic acids
   • Polymers
     • Classification and types of polymerisation
     • Important natural and synthetic polymers
   • Chemistry in Everyday Life
     • Drugs and their classification
     • Soaps, detergents and food chemistry
   • Environmental Chemistry
     • Air and water pollution
     • Green chemistry

Chemistry flashcards for IPU CET

21 of 51 cards from the Chemistry deck — real questions with worked answers.

1. What is the mole concept, and how many entities does one mole contain?

   A mole is the amount of substance containing as many elementary entities as there are atoms in 12 g of carbon-12, equal to Avogadro's number = 6.022 x 10^23 entities.

2. State the formula relating molarity (M), moles of solute, and volume of solution.

   Molarity (M) = moles of solute / volume of solution in litres. Unlike molality, it is temperature-dependent.

3. What is the difference between empirical formula and molecular formula?

   Empirical formula gives the simplest whole-number ratio of atoms; molecular formula gives the actual number of atoms. Molecular formula = n x empirical formula, where n = molar mass / empirical formula mass.

4. State the ideal gas equation and the value of the gas constant R in SI units.

   PV = nRT, where R = 8.314 J K^-1 mol^-1 (or 0.0821 L atm K^-1 mol^-1).

5. State Dalton's law of partial pressures.

   The total pressure of a non-reacting gas mixture equals the sum of the partial pressures of the individual gases: P_total = P1 + P2 + P3 + ...

6. What are the values of critical temperature and the van der Waals equation for a real gas?

   Van der Waals equation: (P + an^2/V^2)(V - nb) = nRT, where 'a' corrects for intermolecular attraction and 'b' for molecular volume.

7. What are the four quantum numbers and what does each describe?

   Principal (n) = energy/shell; Azimuthal (l) = subshell/shape; Magnetic (m_l) = orbital orientation; Spin (m_s) = electron spin (+1/2 or -1/2).

8. State the Heisenberg uncertainty principle.

   It is impossible to determine simultaneously the exact position and momentum of an electron: Δx · Δp ≥ h/4π.

9. State Aufbau principle, Pauli exclusion principle, and Hund's rule.

   Aufbau: orbitals fill in increasing energy order. Pauli: no two electrons have identical four quantum numbers. Hund: orbitals of a subshell are singly filled before pairing.

10. Give the de Broglie equation for the wavelength of a moving particle.

    λ = h/mv = h/p, where h is Planck's constant, m is mass, v is velocity, and p is momentum.

11. What is the difference between sigma (σ) and pi (π) bonds?

    Sigma bonds form by head-on (axial) overlap of orbitals and are stronger; pi bonds form by sidewise (lateral) overlap of p-orbitals and are weaker. Single bond = 1 σ; double = 1 σ + 1 π; triple = 1 σ + 2 π.

12. State VSEPR theory and the shape of a molecule with 4 bond pairs (e.g., CH4).

    VSEPR: electron pairs around a central atom arrange to minimize repulsion. Four bond pairs give a tetrahedral shape with bond angle 109.5° (e.g., CH4).

13. What hybridization and geometry correspond to sp, sp2, and sp3?

    sp = linear, 180° (e.g., BeCl2); sp2 = trigonal planar, 120° (e.g., BF3); sp3 = tetrahedral, 109.5° (e.g., CH4).

14. Define bond order and how it is calculated in molecular orbital theory.

    Bond order = (number of bonding electrons - number of antibonding electrons) / 2. Higher bond order means greater bond strength and shorter bond length.

15. Why is hydrogen bonding important, and which atoms enable it?

    Hydrogen bonding occurs when H is bonded to highly electronegative F, O, or N. It raises boiling points, explains water's anomalous properties, and DNA base pairing.

16. State the first law of thermodynamics.

    Energy can neither be created nor destroyed: ΔU = q + w, where ΔU is change in internal energy, q is heat absorbed, and w is work done on the system.

17. What is enthalpy (H), and what does a negative ΔH indicate?

    Enthalpy H = U + PV is heat content at constant pressure. ΔH < 0 indicates an exothermic reaction (heat released); ΔH > 0 is endothermic.

18. State Hess's law of constant heat summation.

    The total enthalpy change of a reaction is the same whether it occurs in one step or several, depending only on initial and final states.

19. State the Gibbs free energy equation and the spontaneity condition.

    ΔG = ΔH - TΔS. A reaction is spontaneous when ΔG < 0, at equilibrium when ΔG = 0, and non-spontaneous when ΔG > 0.

20. How is entropy (S) described, and what is the second law of thermodynamics?

    Entropy is a measure of disorder/randomness. Second law: the entropy of the universe always increases for a spontaneous process (ΔS_universe > 0).

21. State Le Chatelier's principle.

    If a system at equilibrium is disturbed by a change in concentration, temperature, or pressure, it shifts to counteract the disturbance and re-establish equilibrium.

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