NEET / State Class 12 Board (e.g. ISC) 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 NEET / State Class 12 Board (e.g. ISC), not a summary of it.

1. 1

   Physical Chemistry

   4 topics

   • Solutions
     • Concentration terms and Raoult's law
     • Colligative properties and molar mass determination
     • Abnormal molar mass and van't Hoff factor
   • Electrochemistry
     • Electrolytic and galvanic cells; electrode potential
     • Nernst equation and EMF of cells
     • Conductance, Kohlrausch's law and electrolysis
   • Chemical Kinetics
     • Rate of reaction and order of reaction
     • Integrated rate equations for zero and first order
     • Arrhenius equation and collision theory
   • Electrochemistry and Energetics Numericals
     • Faraday's laws of electrolysis
     • Relation between Gibbs energy, EMF and equilibrium constant
2. 2

   Inorganic Chemistry

   3 topics

   • The p-Block Elements (Groups 15-18)
     • Group 15: dinitrogen, ammonia, oxides of nitrogen, phosphorus allotropes
     • Group 16: dioxygen, ozone, sulphuric acid and oxoacids of sulphur
     • Group 17 and 18: halogens, interhalogens and noble gases
   • d- and f-Block Elements
     • Transition elements: variable oxidation states, colour, magnetism
     • Preparation and properties of KMnO4 and K2Cr2O7
     • Lanthanoid contraction and actinoids
   • Coordination Compounds
     • Werner's theory, ligands and nomenclature
     • Valence bond and crystal field theory
     • Isomerism and applications of coordination compounds
3. 3

   Organic Chemistry I

   3 topics

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

   Organic Chemistry II and Biomolecules

   3 topics

   • Amines and Diazonium Salts
     • Classification, preparation and basicity of amines
     • Reactions of diazonium salts and their synthetic uses
   • Biomolecules
     • Carbohydrates: monosaccharides, glycosidic linkage
     • Proteins: amino acids, peptide bond, structure
     • Nucleic acids, vitamins and hormones
   • Polymers and Chemistry in Everyday Life
     • Classification and types of polymerisation
     • Drugs, drug-target interaction; antibiotics and antiseptics

Chemistry flashcards for NEET / State Class 12 Board (e.g. ISC)

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

1. In an ideal solution, what is the value of ΔH(mixing) and ΔV(mixing)?

   Both are zero. Ideal solutions obey Raoult's law over the entire concentration range, and A–B interactions equal A–A and B–B interactions.

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

   The partial vapour pressure of each component is proportional to its mole fraction: p₁ = p₁°x₁ and p₂ = p₂°x₂. Total pressure = p₁°x₁ + p₂°x₂.

3. What is Henry's law and its mathematical form?

   The partial pressure of a gas over a solution is proportional to its mole fraction in solution: p = K_H · x. A higher K_H means lower solubility of the gas.

4. List the four colligative properties of solutions.

   Relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.

5. Give the formula for osmotic pressure of a dilute solution.

   π = CRT = (n/V)RT, where C is molar concentration, R the gas constant, and T the absolute temperature.

6. Define the van't Hoff factor (i) and its values for dissociation vs association.

   i = (observed colligative property)/(calculated). i > 1 for solutes that dissociate (e.g. NaCl, i≈2), i < 1 for solutes that associate (e.g. benzoic acid in benzene).

7. What distinguishes a positive deviation from Raoult's law?

   Vapour pressure is higher than predicted; ΔH(mix) > 0 (endothermic) and ΔV(mix) > 0. A–B forces are weaker than A–A/B–B (e.g. ethanol + acetone).

8. Write the formula for elevation of boiling point.

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

9. Write the Nernst equation for an electrode at 298 K (using log base 10).

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

10. Define molar conductivity and how it relates to conductivity.

    Λ_m = κ × 1000 / C, where κ is conductivity (S cm⁻¹) and C is molar concentration (mol L⁻¹). Units: S cm² mol⁻¹.

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. How does molar conductivity change with dilution for strong vs weak electrolytes?

    For both, Λ_m increases on dilution. Strong electrolytes increase slightly (more ion mobility); weak electrolytes increase sharply (greater degree of dissociation).

13. State Faraday's first law of electrolysis.

    The mass of a substance deposited/liberated at an electrode is proportional to the quantity of charge passed: m ∝ Q, where Q = I×t. (1 mole electrons = 1 F = 96500 C.)

14. Give the relationship between ΔG°, E°(cell), and the equilibrium constant.

    ΔG° = −nFE°(cell) and ΔG° = −RT ln K, so log K = nE°(cell)/0.0591 at 298 K.

15. What is the integrated rate equation for a first-order reaction?

    k = (2.303/t) log([A₀]/[A]), or ln[A] = ln[A₀] − kt. Units of k: s⁻¹ (time⁻¹).

16. How is half-life related to rate constant for first- and zero-order reactions?

    First order: t½ = 0.693/k (independent of concentration). Zero order: t½ = [A₀]/2k (proportional to initial concentration).

17. State the Arrhenius equation and the meaning of its terms.

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

18. What is the difference between order and molecularity of a reaction?

    Order is the experimentally determined sum of exponents in the rate law and can be zero/fractional. Molecularity is the number of reacting species in an elementary step; it is always a whole number ≥1.

19. How does a catalyst increase reaction rate?

    It provides an alternative pathway with lower activation energy, increasing the fraction of molecules that can cross the energy barrier. It does not change ΔG or equilibrium position.

20. A first-order reaction has k = 2.303×10⁻³ s⁻¹. How long for 90% completion?

    For 90% completion, t = (2.303/k) log(100/10) = (2.303/2.303×10⁻³)×1 = 1000 s.

21. Calculate E°(cell) for Zn|Zn²⁺||Cu²⁺|Cu given E°(Zn²⁺/Zn)=−0.76 V, E°(Cu²⁺/Cu)=+0.34 V.

    E°(cell) = E°(cathode) − E°(anode) = 0.34 − (−0.76) = +1.10 V.

See more Chemistry flashcards →

Planning Chemistry for NEET / State Class 12 Board (e.g. ISC)

Chemistry (NEET / State Class 12 Board (e.g. ISC)) FAQ