CBSE Class 12 Board Exam 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 CBSE Class 12 Board Exam, not a summary of it.

1. 1

   Physical Chemistry

   3 topics

   • Solutions
     • Concentration terms and Raoult's law
     • Colligative properties
     • Abnormal molar mass and van't Hoff factor
   • Electrochemistry
     • Galvanic cells and electrode potential
     • Nernst equation and EMF
     • Conductance and Kohlrausch's law
     • Electrolysis and Faraday's laws
   • Chemical Kinetics
     • Rate of reaction and rate law
     • Order and molecularity
     • Integrated rate equations
     • Arrhenius equation and activation energy
2. 2

   Inorganic Chemistry

   3 topics

   • The d- and f-Block Elements
     • Electronic configuration and oxidation states
     • Properties of transition elements
     • Lanthanoids and actinoids
     • Preparation of K2Cr2O7 and KMnO4
   • Coordination Compounds
     • Werner's theory and ligands
     • Nomenclature and isomerism
     • Valence bond and crystal field theory
     • Importance and applications
   • Qualitative Inorganic Analysis
     • Detection of cations (basic radicals)
     • Detection of anions (acidic radicals)
     • Group separation and confirmatory tests
3. 3

   Organic Chemistry I

   3 topics

   • Haloalkanes and Haloarenes
     • Nomenclature and nature of C-X bond
     • SN1 and SN2 mechanisms
     • Optical isomerism
   • Alcohols, Phenols and Ethers
     • Preparation and properties of alcohols
     • Acidity of phenols
     • Preparation and reactions of ethers
   • Aldehydes, Ketones and Carboxylic Acids
     • Nucleophilic addition reactions
     • Aldol and Cannizzaro reactions
     • Acidity and reactions of carboxylic acids
4. 4

   Organic Chemistry II and Biomolecules

   3 topics

   • Amines
     • Classification and preparation
     • Basicity of amines
     • Diazonium salts and their reactions
   • Biomolecules
     • Carbohydrates - mono, di and polysaccharides
     • Proteins, amino acids and enzymes
     • Vitamins and nucleic acids
   • Practical and Qualitative Organic Analysis
     • Detection of functional groups
     • Detection of elements (N, S, halogens)
     • Titrimetric estimation

Chemistry flashcards for CBSE Class 12 Board Exam

21 of 65 cards from the Chemistry deck — real questions with worked answers.

1. State Raoult's law for a solution of two volatile liquids.

   The partial vapour pressure of each volatile component in a solution is directly proportional to its mole fraction: p_A = p_A° x_A and p_B = p_B° x_B.

2. What is the van't Hoff factor (i), and what does i > 1 indicate?

   i = (observed colligative property) / (calculated/normal value) = number of particles actually present / number dissolved. i > 1 indicates dissociation of the solute (e.g., electrolytes).

3. Write the formula relating molal elevation of boiling point to molality.

   ΔT_b = K_b × m, where K_b is the molal elevation (ebullioscopic) constant and m is molality.

4. Define osmotic pressure and give its equation for a dilute solution.

   Osmotic pressure (π) is the excess pressure that must be applied to a solution to stop osmosis of solvent into it. π = CRT (or πV = nRT), where C is molar concentration.

5. What type of deviation from Raoult's law shows positive deviation, and what is the sign of ΔH_mix and ΔV_mix?

   Positive deviation occurs when A–B interactions are weaker than A–A and B–B. ΔH_mix > 0 (endothermic) and ΔV_mix > 0. Example: ethanol + acetone.

6. State Henry's law.

   The partial pressure of a gas over a solution is directly proportional to its mole fraction in the solution: p = K_H × x, where K_H is Henry's law constant.

7. Write the Nernst equation for an electrode at 298 K (using log).

   E = E° − (0.0591/n) log Q, where n is the number of electrons transferred and Q is the reaction quotient.

8. State the relationship between standard cell potential and Gibbs free energy change.

   ΔG° = −nFE°cell, where n is moles of electrons, F is the Faraday constant (96500 C/mol), and E°cell is the standard cell potential.

9. State Faraday's first law of electrolysis.

   The mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electricity (charge) passed: m ∝ Q, i.e., m = ZIt.

10. How does molar conductivity vary with dilution for a strong electrolyte versus a weak electrolyte?

    For strong electrolytes, molar conductivity increases slightly with dilution. For weak electrolytes, it increases sharply near infinite dilution due to increased degree of dissociation.

11. State Kohlrausch's law of independent migration of ions.

    The limiting molar conductivity of an electrolyte is the sum of the individual contributions of its cation and anion: Λ°m = ν₊ λ°₊ + ν₋ λ°₋.

12. Write the relationship between standard cell EMF and the equilibrium constant.

    E°cell = (0.0591/n) log Kc (at 298 K), or ΔG° = −RT ln Kc = −nFE°cell.

13. Define the order and molecularity of a reaction.

    Order is the sum of the powers of concentration terms in the experimentally determined rate law (can be zero/fractional). Molecularity is the number of reacting species in an elementary step (always a whole number, ≥1).

14. Write the integrated rate equation for a first-order reaction.

    k = (2.303/t) log([R]₀/[R]), or ln[R] = ln[R]₀ − kt.

15. What is the half-life expression for a first-order reaction, and what does it depend on?

    t₁/₂ = 0.693/k. It is independent of the initial concentration of the reactant.

16. State the Arrhenius equation and define each symbol.

    k = A e^(−Ea/RT), where k is rate constant, A is the frequency/pre-exponential factor, Ea is activation energy, R is gas constant, T is temperature.

17. What is activation energy, and how does a catalyst affect it?

    Activation energy is the minimum extra energy reactants must have to form products. A catalyst lowers Ea by providing an alternative reaction pathway, increasing the rate.

18. For a zero-order reaction, write the integrated rate law and the units of k.

    [R] = [R]₀ − kt. The units of k are mol L⁻¹ s⁻¹ (same as rate).

19. Why do transition (d-block) elements show variable oxidation states?

    Because the energies of the (n−1)d and ns electrons are very close, so electrons from both subshells can participate in bonding, giving multiple oxidation states.

20. Why are most transition metal compounds coloured?

    Due to d–d transitions: absorption of visible light promotes electrons between split d-orbitals; the colour seen is complementary to the light absorbed. (Requires partially filled d-orbitals.)

21. What are lanthanoid contraction and one of its consequences?

    Lanthanoid contraction is the steady decrease in atomic/ionic radii across the lanthanoid series due to poor shielding by 4f electrons. Consequence: Zr and Hf (and other 4d/5d pairs) have nearly identical sizes and similar properties.

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