CBSE 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 CBSE Class 11, not a summary of it.

1. 1

   Some Basic Concepts of Chemistry

   1 topic

   • General Introduction
2. 2

   Structure of Atom

   2 topics

   • Constituents of Atom
   • Quantum Mechanical Model of Atom
3. 3

   Classification of Elements and Periodicity in Properties

   1 topic

   • Modern Periodic Law and the Present Form of the Periodic Table
4. 4

   Chemical Bonding and Molecular Structure

   5 topics

   • Valence Electrons
   • Ionic Bond
   • Covalent Bond
   • Bond Parameters
   • Molecular Structure
5. 5

   States of Matter: Gases and Liquids

   5 topics

   • Three States of Matter
   • Gas Laws
   • Ideal Gas Equation
   • Kinetic Energy and Molecular Speeds
   • Liquefaction of Gases
6. 6

   Thermodynamics

   7 topics

   • Concepts of System
   • Types of Systems
   • Surroundings
   • Types of Processes
   • First Law of Thermodynamics
   • Enthalpy
   • Heat Capacity
7. 7

   Equilibrium

   4 topics

   • Equilibrium in Physical and Chemical Processes
   • Dynamic Nature of Equilibrium
   • Law of Chemical Equilibrium and Equilibrium Constant
   • Factors Affecting Equilibria
8. 8

   Redox Reactions

   1 topic

   • Concept of Oxidation and Reduction
9. 9

   Hydrogen

   3 topics

   • Position of Hydrogen in Periodic Table
   • Dihydrogen, H2
   • Hydrides
10. 10

    s-Block Elements (Alkali and Alkaline Earth Metals)

    2 topics

    • Group 1 Elements: Alkali Metals
    • Group 2 Elements: Alkaline Earth Metals
11. 11

    Some p-Block Elements

    1 topic

    • General Introduction to p-Block Elements
12. 12

    Organic Chemistry - Some Basic Principles and Techniques

    5 topics

    • General Introduction
    • Methods of Purification
    • Qualitative and Quantitative Analysis
    • Classification and IUPAC Nomenclature of Organic Compounds
    • Electronic Displacements in a Covalent Bond
13. 13

    Hydrocarbons

    1 topic

    • Classification of Hydrocarbons
14. 14

    Environmental Chemistry

    1 topic

    • Environmental Pollution

Chemistry flashcards for CBSE Class 11

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

1. What is the difference between an element, a compound, and a mixture?

   An element is a pure substance made of only one type of atom (e.g., O2). A compound is a pure substance formed by chemically combining two or more elements in a fixed ratio (e.g., H2O). A mixture is a physical combination of two or more substances in any ratio, retaining their properties (e.g., air).

2. State 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.

3. What are the mass and charge of the three fundamental subatomic particles (electron, proton, neutron)?

   Electron: mass 9.11x10^-31 kg, charge -1.6x10^-19 C (-1). Proton: mass 1.672x10^-27 kg, charge +1.6x10^-19 C (+1). Neutron: mass 1.674x10^-27 kg, charge 0 (neutral).

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

   Atomic number (Z) is the number of protons in an atom's nucleus (equal to electrons in a neutral atom). Mass number (A) is the total number of protons and neutrons (nucleons) in the nucleus.

5. State the Heisenberg Uncertainty Principle and its mathematical expression.

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

6. What do the four quantum numbers (n, l, m, s) represent?

   Principal (n): main energy level/shell size. Azimuthal (l): subshell/shape of orbital. Magnetic (m): orientation of orbital in space. Spin (s): direction of electron spin (+1/2 or -1/2).

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

   Aufbau: orbitals fill in order of increasing energy. Pauli: no two electrons in an atom can have all four quantum numbers identical (max 2 per orbital, opposite spins). Hund's rule: electrons occupy degenerate orbitals singly with parallel spins before pairing.

8. State the modern periodic law.

   The physical and chemical properties of elements are a periodic function of their atomic numbers.

9. How many periods and groups are in the modern periodic table, and how are blocks defined?

   There are 7 periods (horizontal rows) and 18 groups (vertical columns). Blocks (s, p, d, f) are defined by the subshell into which the last electron enters.

10. How do atomic radius and ionization enthalpy vary across a period and down a group?

    Across a period (left to right): atomic radius decreases, ionization enthalpy increases. Down a group: atomic radius increases, ionization enthalpy decreases.

11. Define electronegativity and state how it varies in the periodic table.

    Electronegativity is the tendency of an atom to attract the shared pair of electrons in a bond toward itself. It increases across a period and decreases down a group; fluorine is the most electronegative element.

12. What are valence electrons and why are they important?

    Valence electrons are the electrons in the outermost shell of an atom. They determine an element's chemical bonding behavior, valency, and chemical properties.

13. Define an ionic (electrovalent) bond and give an example.

    An ionic bond is the electrostatic force of attraction between oppositely charged ions formed by the complete transfer of electrons from a metal to a non-metal. Example: NaCl (Na+ and Cl-).

14. Define a covalent bond and distinguish single, double, and triple bonds.

    A covalent bond is formed by the mutual sharing of electron pairs between atoms. Single bond = 1 shared pair (e.g., H2), double bond = 2 shared pairs (e.g., O2), triple bond = 3 shared pairs (e.g., N2).

15. State the octet rule.

    Atoms tend to gain, lose, or share electrons so as to achieve a stable configuration of eight electrons in their valence shell (like the nearest noble gas).

16. Define bond length, bond angle, and bond enthalpy.

    Bond length: the equilibrium distance between nuclei of two bonded atoms. Bond angle: the angle between two bonds at an atom. Bond enthalpy: the energy required to break one mole of a particular bond in the gaseous state.

17. State the postulates of VSEPR theory used to predict molecular shapes.

    Electron pairs around a central atom arrange themselves to minimize repulsion. Repulsion order: lone pair-lone pair > lone pair-bond pair > bond pair-bond pair. The geometry depends on the number of bonding and lone pairs.

18. What hybridization and shape 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).

19. Why is the shape of a water molecule bent rather than linear?

    Oxygen in water is sp3 hybridized with two bond pairs and two lone pairs. The lone pair-bond pair repulsions push the O-H bonds closer, giving a bent shape with an angle of about 104.5°.

20. State Boyle's Law and Charles's Law.

    Boyle's Law: at constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure (PV = constant). Charles's Law: at constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature (V/T = constant).

21. State Gay-Lussac's Law and Avogadro's Law.

    Gay-Lussac's (pressure-temperature) Law: at constant volume, pressure of a fixed mass of gas is directly proportional to its absolute temperature (P/T = constant). Avogadro's Law: equal volumes of all gases at the same temperature and pressure contain equal numbers of molecules (V ∝ n).

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