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Atomic Structure and Periodicity

Term 161

  • Q1(a) [4]: Describe the postulates of Bohr's theory of atom.
  • Q1(b) [4]: What is ionization energies and electronegativity.
  • Q1(c) [6]: Explain the periodicity of atomic volume and valency.

Term 171

  • Q1(a) [3+5]: Define orbit and orbital. Are 2P, 3f and 4S² orbital possible? Explain your answer.
  • Q1(b) [6]: What is the maximum number of electrons that can be present in the principal level for which n = 4?
  • Q5(c) [5]: Show the hydrogen bonding in acetic acid molecules and find Isotope, Isobar, Isotone from the following atoms: \({}^{12}_{6}C\), \({}^{14}_{6}C\), \({}^{28}_{14}Si\), \({}^{27}_{13}Al\) and \({}^{13}_{6}C\).
  • Q7(a) [8]: Write short notes on the followings: (i) Noble gasses; (ii) Hydrogen bonding; (iii) Normality and pH of solutions; (iv) Diamagnetism and paramagnetism.

Term 181

  • Q1(a) [3]: What is an orbital?
  • Q1(b) [3]: Write down the rules of ground state electron configuration of elements.
  • Q1(c) [3]: Write the name of the orbital for which the quantum numbers are \(n=2\) and \(l=1\).
  • Q1(d) [5]: Write the ground state electron configuration of element Na.
  • Q3(a) [2+4]: What is ionization energy? Explain "ionization energy increases across a period".
  • Q3(b) [2+2]: What are Nobel gases? What are their properties?
  • Q5(a) [2+3]: What are isotopes and isobars? Choose isotopes and isobars from the following list.
  • Q7(c) [4]: Why does the electron affinity decrease down a group except fluorine?

Term 201

  • Q1(a) [4]: Describe Rutherford's atomic model and mention its weakness.
  • Q1(b) [4]: Write down postulates of Bohr's theory.
  • Q1(c) [6]: Find out the number of orbitals for which the following sets of quantum numbers is possible \(n=3\), \(l=2\) and \(m=(+2)\).
  • Q2(a) [5]: Write down the ground state electron configuration of following elements: (i) C(6); (ii) S(16); (iii) Mo(42); (iv) Ni(28); (v) Na(11).
  • Q2(b) [6]: Explain "electron affinity of an element decreases down a group". Why is the value of electron affinity for fluorine out of line?
  • Q2(c) [3]: Why does the ionization energy of Na is lower than Li?

Term 211

  • Q1(a) [5]: Define isotope and isobar with example.
  • Q1(b) [2+2]: What is an orbital? Define Hund's rule.
  • Q1(c) [5]: Mention the significance of quantum numbers.
  • Q2(a) [5]: Write down the ground state electron configuration of the following elements: (i) C(6); (ii) S(16); (iii) Mo(42); (iv) Ni(28); (v) Na(11).
  • Q2(b) [2+4]: What is ionization energy? Why does the ionization energy decrease down a group in the periodic table?
  • Q2(c) [3]: Why is the electron affinity of Be negative?