Other Chapters For 11th

  • 11th-class English Chapter 10

    Just when Mr. Durrell was entertaining the idea of exploring animal conservation, he got a...
  • 11th-class English Chapter 9

    The story begins in Sotheby’s auction house, where a Chinese statue, belonging to an...
  • 11th-class English Chapter 8

    The Spider and the Fly' by Mary Howitt describes the entrapment of a silly fly who gives into...
  • 11th-class English Chapter 7

    “Desiderata” is an inspirational poem by Max Ehrmann in which he attempts to offer a positive...
  • 11th-class English Chapter 6

    John brown is an anti-war song composed and performed by the American singer-songwriter and...
  • 11th-class English Chapter 5

    The story begins with the description of a down-to-earth boot shop, belonging to the Gessler...
  • 11th-class English Chapter 4

    The narrator, Shankar and his friend Jayanto get away from their busy schedules to spend a...
  • 11th-class English Chapter 3

    A young and carefree Salvatore, who spent his days swimming in the sea, climbing rocks, and...
  • 11th-class English Chapter 2

    The Gift of India is a poem written in 1915 by the Indian poet, freedom fighter and politician...
  • 11th-class English Chapter 1

    The Dolphins’ by Carol Ann Duffy is a dramatic monologue written from the perspective of...

11th Class Chapter No 2 - Atomic Structure in Chemistry for ISC

Structure of Atom
Discovery of fundamental particles electron, proton and neutron), atomic number, isotopes and isobars. Thomson's model and its limitations. Rutherford's experimental model and its limitations. Dual nature of matter and light. Bohr's atomic model and its limitations (de Broglie's equation, Heisenberg’s uncertainty principle), concept of shells, subshells, orbitals. Quantum numbers, shapes of s, p and d orbitals. Rules for filling electrons in orbitals - aufbau principle, Pauli's exclusion principle and Hund's rule of maximum multiplicity. Electronic configuration of atoms, stability of half-filled and completely filled orbitals.

  1. Subatomic particles (electrons, protons and neutrons) their charges and masses: Concept of indivisibility of atom as proposed by Dalton does not exist. The atom consists of subatomic fundamental particles. Production of cathode rays and their properties. Production of anode rays and their properties.
    Chadwick’s experiment for the discovery of neutron and properties of neutron.
  2. Rutherford’s nuclear model based on the scattering experiment: Rutherford’s scattering experiment. Discovery of nucleus. Rutherford’s nuclear model of atom. Defects of Rutherford’s model. Electromagnetic wave theory and its limitations (Black body radiation and photoelectric effect)
    Planck’s quantum theory.
    Numericals based on the above.
  3. Types of spectra: emission and absorption spectra. Band and line spectra to be discussed.
  4. Bohr’s atomic model.
    Postulates of Bohr’s theory – based on Planck’s quantum theory.
    Merits of Bohr’s atomic model and explanation of hydrogen spectra.
    Calculations based on Rydberg’s formula.
    Numericals on Bohr’s atomic radii, velocity and energy of orbits (derivation not required).
    Defects in Bohr’s Model.
  5. Quantum mechanical model of an atom - a simple mathematical treatment. Quantum numbers; shape, size and orientation of s, p and d orbitals only (no derivation). aufbau principle, Pauli’s exclusion principle, Hund’s rule of maximum multiplicity. Electronic configuration of elements in terms of s, p, d, f subshells.
    • de Broglie’s equation. Numericals.
    • Heisenberg’s Uncertainty Principle. Numericals.
    • Schrodinger Wave Equation – physical significance of ψψ and |ψ|2|ψ|2.
    • Quantum numbers – types of quantum numbers, shape, size and orientation of the s, p and d subshells. Information obtained in terms of distance of electron from the nucleus, node, nodal planes and radial probability curve, energy of electron, number of electrons present in an orbit and an orbital.
    • aufbau principle, (n+l) rule.
    • Pauli’s exclusion principle.
    • Hund’s rule of maximum multiplicity.
    • Electronic configuration of elements and ions in terms of s, p, d, f subshells and stability of half-filled and completely filled orbitals.
Posted in 11th on February 13 2019 at 03:29 PM


  • 11th-class Chemistry Chapter 14

    Environmental chemistry is the scientific study of the chemical and biochemical phenomena that...
  • 11th-class Chemistry Chapter 13

    Hydrocarbons are the compounds of carbon and hydrogen only. Hydrocarbons are mainly obtained...
  • 11th-class Chemistry Chapter 12

    Organic chemistry is the chemistry of carbon, an element that forms strong chemical bonds to...
  • 11th-class Chemistry Chapter 8

    Redox is a chemical reaction in which the oxidation states of atoms are changed. Any such...
  • 11th-class Chemistry Chapter 11

    Elements in which the last electron enters in to any one of the three p-orbitals of their...
  • 11th-class Chemistry Chapter 10

    The s-Block of the periodic table constitutes Group1 (alkali metals) and Group 2 (alkaline earth...
  • 11th-class Chemistry Chapter 9

    Occurrence: It is the most abundant element in the universe. It is rarely found in the free...
  • 11th-class Chemistry Chapter 7

    When the number of molecules leaving the liquid to vapour equals the number of molecules...
  • 11th-class Chemistry Chapter 6

    Thermodynamical system : An assembly of externally large number of gas molecules is called a...
  • 11th-class Chemistry Chapter 5

    Intermolecular forces operate between the particles of matter. Intermolecular forces are the...

Comments (0)

No login