ISC Class 11 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 ISC Class 11, not a summary of it.

1. 1

   Some Basic Concepts of Chemistry

   5 topics

   • General Introduction
   • Laws of Chemical Combination
   • Atomic and Molecular Masses
   • Mole Concept and Molar Masses
   • Stoichiometry and Stoichiometric Calculations
2. 2

   Structure of Atom

   3 topics

   • Discovery of Electron, Proton and Neutron
   • Atomic Number
   • Isotopes and Isobars
3. 3

   Classification of Elements and Periodicity in Properties

   3 topics

   • Significance of Classification, Brief History
   • Modern Periodic Law and the Present Form of the Periodic Table
   • Periodic Trends in Properties of Elements
4. 4

   Chemical Bonding and Molecular Structure

   8 topics

   • Valence Electrons
   • Ionic Bond
   • Covalent Bond
   • Bond Parameters
   • Lewis Structure
   • Polar Character of Covalent Bond
   • VSEPR Theory
   • Concept of Hybridization
5. 5

   States of Matter: Gases and Liquids

   3 topics

   • Three States of Matter
   • Types of Bonding
   • Liquid State

Chemistry flashcards for ISC Class 11

21 of 56 cards from the Chemistry deck — real questions with worked answers.

1. What is 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. Proposed by Antoine Lavoisier.

2. State the Law of Definite (Constant) Proportions.

   A given chemical compound always contains its constituent elements in a fixed ratio by mass, regardless of its source or method of preparation. Given by Proust.

3. State the Law of Multiple Proportions.

   When two elements combine to form more than one compound, the masses of one element that combine with a fixed mass of the other are in a simple whole-number ratio. Given by Dalton.

4. State Gay-Lussac's Law of Gaseous Volumes.

   When gases react, they do so in volumes that bear a simple whole-number ratio to one another and to the volumes of gaseous products, measured at the same temperature and pressure.

5. State Avogadro's Law.

   Equal volumes of all gases at the same temperature and pressure contain an equal number of molecules.

6. What is the value of Avogadro's number (NA)?

   6.022 x 10^23 particles (atoms, molecules, or ions) per mole.

7. Define one mole.

   The amount of a substance that contains as many elementary entities (atoms, molecules, ions) as there are atoms in exactly 12 g of carbon-12, i.e. 6.022 x 10^23 entities.

8. How is molar mass related to the mole and mass?

   Number of moles = given mass / molar mass (n = m / M). Molar mass is the mass of one mole of a substance in g/mol.

9. Define atomic mass unit (amu / u).

   One atomic mass unit is exactly 1/12th of the mass of one carbon-12 atom; 1 u = 1.66 x 10^-24 g.

10. What is the difference between average atomic mass and molecular mass?

    Average atomic mass is the weighted average mass of an element's isotopes; molecular mass is the sum of the atomic masses of all atoms in a molecule.

11. Define empirical formula and molecular formula.

    Empirical formula gives the simplest whole-number ratio of atoms in a compound; molecular formula gives the actual number of atoms. Molecular formula = n x empirical formula.

12. What is the molar volume of an ideal gas at STP?

    22.4 litres per mole at STP (273.15 K and 1 bar/1 atm).

13. Define limiting reagent.

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

14. Define molarity (M).

    The number of moles of solute dissolved per litre of solution (mol/L). Molarity = moles of solute / volume of solution in litres.

15. Define molality (m).

    The number of moles of solute dissolved per kilogram of solvent (mol/kg). Molality is independent of temperature.

16. How do you calculate mass percent of a solution?

    Mass percent = (mass of solute / mass of solution) x 100.

17. Who discovered the electron and by what experiment?

    J.J. Thomson discovered the electron using cathode ray (discharge) tube experiments. He determined its charge-to-mass ratio (e/m).

18. What are the charge and mass of an electron?

    Charge = -1.602 x 10^-19 C; mass = 9.11 x 10^-31 kg (about 1/1837 of a proton).

19. Who discovered the proton and how?

    The proton was discovered by Goldstein (canal/anode rays) and characterized by Ernest Rutherford. Charge = +1.602 x 10^-19 C, mass = 1.672 x 10^-27 kg.

20. Who discovered the neutron and what are its properties?

    James Chadwick discovered the neutron in 1932. It is electrically neutral with mass 1.675 x 10^-27 kg (slightly greater than a proton).

21. Define atomic number (Z) and mass number (A).

    Atomic number Z = number of protons in the nucleus (= electrons in a neutral atom). Mass number A = number of protons + number of neutrons.

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