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🇮🇳 ISC Class 12 · subject
ISC Class 12 Chemistry Syllabus
Every chapter and topic of Chemistry examined in ISC Class 12 — 16 chapters, 45 topics, plus 51 flashcards written against it.
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 ISC Class 12, not a summary of it.
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Solid State
3 topics- Classification of Solids
- Crystal Lattices and Unit Cells
- Imperfections in Solids
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Solutions
2 topics- Types of Solutions
- Colligative Properties
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Electrochemistry
2 topics- Redox Reactions
- Electrochemical Cells
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Chemical Kinetics
2 topics- Rate of a Reaction
- Factors Affecting Rate of Reactions
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Surface Chemistry
3 topics- Adsorption
- Catalysis
- Colloids
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General Principles and Processes of Isolation of Elements
2 topics- Principles and Methods of Extraction
- Thermodynamic and Kinetic Aspects
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p-Block Elements
4 topics- Group 15 Elements
- Group 16 Elements
- Group 17 Elements
- Group 18 Elements
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d and f Block Elements
2 topics- Transition Elements
- Inner Transition Elements
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Coordination Compounds
3 topics- Ligands
- Coordination Number
- Bonding
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Haloalkanes and Haloarenes
3 topics- Nomenclature
- Nature of C-X Bond
- Physical and Chemical Properties
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Alcohols, Phenols and Ethers
3 topics- Nomenclature
- Properties
- Uses
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Aldehydes, Ketones and Carboxylic Acids
3 topics- Nomenclature
- Structure of Carbonyl Group
- Preparation and Properties
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Organic Compounds Containing Nitrogen
3 topics- Amines
- Cyanides and Isocyanides
- Diazonium Salts
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Biomolecules
4 topics- Carbohydrates
- Proteins
- Vitamins
- Nucleic Acids
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Polymers
3 topics- Classification of Polymers
- Polymerization
- Biodegradable Polymers
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Chemistry in Everyday Life
3 topics- Chemicals in Medicines
- Chemicals in Food
- Cleansing Agents
Chemistry flashcards for ISC Class 12
21 of 51 cards from the Chemistry deck — real questions with worked answers.
How are solids classified based on the arrangement of their constituent particles?
Into crystalline solids (regular, long-range ordered arrangement, definite geometry, sharp melting point, anisotropic) and amorphous solids (irregular, short-range order, no definite shape, melt over a range, isotropic).
What is a unit cell, and what are the three types of cubic unit cells?
A unit cell is the smallest repeating structural unit of a crystal lattice. The three cubic types are: simple/primitive cubic, body-centred cubic (bcc), and face-centred cubic (fcc).
How many atoms per unit cell are present in simple cubic, bcc, and fcc lattices?
Simple cubic = 1 atom, bcc = 2 atoms, fcc = 4 atoms per unit cell.
What is the packing efficiency of simple cubic, bcc, and fcc/ccp structures?
Simple cubic = 52.4%, bcc = 68%, fcc/ccp (and hcp) = 74%.
What is the difference between Schottky and Frenkel defects?
Schottky is a vacancy defect where equal numbers of cations and anions are missing (lowers density); Frenkel is a dislocation defect where a smaller ion (usually cation) leaves its site and occupies an interstitial site (density unchanged).
What are the different types of solutions based on the physical state of solute and solvent? Give examples.
Gas in liquid (CO2 in water), liquid in liquid (alcohol in water), solid in liquid (salt in water), gas in solid (H2 in palladium), solid in solid (alloys), and liquid in solid (amalgams), among nine total combinations.
State Henry's law and its mathematical expression.
The partial pressure of a gas over a solution is proportional to its mole fraction in the solution: p = KH·x, where KH is Henry's law constant.
What are colligative properties? Name the four.
Properties that depend only on the number of solute particles, not their nature: relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, and osmotic pressure.
State Raoult's law for a solution of a non-volatile solute.
The relative lowering of vapour pressure equals the mole fraction of the solute: (p°−p)/p° = x_solute.
Give the formula for elevation of boiling point and depression of freezing point.
ΔTb = Kb·m and ΔTf = Kf·m, where Kb is the molal elevation (ebullioscopic) constant, Kf is the molal depression (cryoscopic) constant, and m is molality.
What is the van't Hoff factor (i) and what does it indicate?
i = (observed colligative property)/(calculated value). i > 1 indicates dissociation; i < 1 indicates association of the solute.
Give the formula for osmotic pressure of a solution.
π = CRT = (n/V)RT, where C is molar concentration, R is the gas constant, and T is absolute temperature.
Define oxidation and reduction in terms of electrons and oxidation number.
Oxidation is loss of electrons (increase in oxidation number); reduction is gain of electrons (decrease in oxidation number).
What is the difference between a galvanic (voltaic) cell and an electrolytic cell?
A galvanic cell converts chemical energy into electrical energy via a spontaneous redox reaction; an electrolytic cell uses electrical energy to drive a non-spontaneous reaction.
State the Nernst equation for an electrode at 298 K.
E = E° − (0.0591/n)·log Q (or for a cell E_cell = E°_cell − (0.0591/n)·log Q), where n is the number of electrons transferred and Q is the reaction quotient.
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°−.
What is the relationship between standard cell potential and Gibbs free energy?
ΔG° = −nFE°_cell, where n is moles of electrons and F is the Faraday constant (96500 C/mol).
How is the rate of a reaction defined for aA + bB → cC + dD?
Rate = −(1/a)d[A]/dt = −(1/b)d[B]/dt = +(1/c)d[C]/dt = +(1/d)d[D]/dt.
What are the integrated rate law and half-life for a first-order reaction?
k = (2.303/t)·log([A]₀/[A]); half-life t½ = 0.693/k, which is independent of initial concentration.
List the main factors that affect the rate of a chemical reaction.
Concentration of reactants, temperature, presence of a catalyst, surface area of reactants, and (for gases) pressure; also nature of reactants and radiation/light.
State the Arrhenius equation and what it relates.
k = A·e^(−Ea/RT), relating the rate constant k to activation energy Ea, temperature T, and the pre-exponential (frequency) factor A.
Planning Chemistry for ISC Class 12
Chemistry is about 51% of the ISC Class 12 syllabus by topic count — 45 of 88 topics, spread over 16 chapters. At roughly 45 minutes per topic plus 12 minutes per sub-topic, a first pass runs to about 35 hours.
The heaviest chapters are p-Block Elements (4 topics), Biomolecules (4 topics), Solid State (3 topics) . Front-load those while your energy is high; the short chapters are better revision filler later.
Work top-down: read the chapter, then tick topics off individually rather than marking the whole chapter done. Sub-topics are where silent gaps hide.
Chemistry (ISC Class 12) FAQ
What is in the ISC Class 12 Chemistry syllabus?
Chemistry is split into 16 chapters — Solid State, Solutions, Electrochemistry, Chemical Kinetics, Surface Chemistry and General Principles and Processes of Isolation of Elements, and 10 more, containing 45 topics and 0 sub-topics in total.
How many chapters are there in Chemistry for ISC Class 12?
16 chapters. Chemistry accounts for about 51% of the topics in the whole ISC Class 12 syllabus (45 of 88).
How long should I spend on Chemistry for ISC Class 12?
Budget around 35 hours for a first pass through Chemistry — about 45 minutes per topic plus 12 minutes per sub-topic across its 45 topics. Add revision cycles on top.
Are there flashcards for ISC Class 12 Chemistry?
Yes — a 51-card Chemistry deck. Sample cards are printed on this page, and the full deck is free in the Examius app with spaced repetition scheduling.