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Chemical Bonding and Molecular Structure · I PU Chemistry

Name: ____________________
Date: ____________________
Mode: BalancedQuestions: 20Difficulty: MixedCheck code: 651062640

1. Why is O₂ paramagnetic according to molecular-orbital theory?

  1. It has a double bond in its Lewis structure
  2. All its electrons are paired
  3. It has zero bond order
  4. It has two unpaired electrons in degenerate π* orbitals

2. Intramolecular hydrogen bonding most directly means hydrogen bonding:

  1. within one molecule
  2. between different molecules
  3. inside an ionic lattice only
  4. between two hydrogen atoms

3. Which species is an odd-electron molecule?

  1. NO
  2. CO₂
  3. N₂
  4. CH₄

4. Why is the boiling point of H₂O much higher than that of H₂S?

  1. H₂S is an ionic substance
  2. Water forms an extensive intermolecular hydrogen-bond network
  3. The O–H covalent bond breaks during boiling
  4. H₂O has the greater molar mass

5. How many valence electrons are present in one CO₂ molecule?

  1. 16
  2. 12
  3. 20
  4. 22

6. Which compound is expected to have the larger lattice-enthalpy magnitude?

  1. KBr
  2. LiF
  3. MgO
  4. NaCl

7. How many sigma and pi bonds are present in one C₂H₂ molecule?

  1. 5 sigma and 0 pi
  2. 3 sigma and 1 pi
  3. 3 sigma and 2 pi
  4. 2 sigma and 3 pi

8. Why is CO₂ non-polar although each C=O bond is polar?

  1. Carbon and oxygen have equal electronegativity
  2. It contains no shared electron pairs
  3. Each C=O bond has zero dipole moment
  4. Its equal bond dipoles cancel in a linear molecule

9. A diatomic species has 8 bonding and 4 antibonding valence electrons. What is its bond order?

  1. 2
  2. 4
  3. 6
  4. 1

10. Which compound should show the greatest covalent character?

  1. LiI
  2. LiF
  3. NaF
  4. KF

11. Which species has equivalent bond lengths because of resonance?

  1. NO₃⁻
  2. H₂O
  3. NH₃
  4. CH₄

12. Which cation most strongly polarises the same anion?

  1. K⁺
  2. Al³⁺
  3. Mg²⁺
  4. Na⁺

13. Which molecule has an electron-deficient central atom in its usual Lewis structure?

  1. CH₄
  2. NH₃
  3. H₂O
  4. BF₃

14. Which carbon–carbon bond is shortest?

  1. C≡C
  2. C=C
  3. C–C
  4. All have equal length

15. What is the formal charge on nitrogen in NH₄⁺?

  1. −1
  2. +2
  3. +1
  4. 0

16. What is the hybridisation of each carbon atom in ethene, C₂H₄?

  1. sp³d
  2. sp²
  3. sp³
  4. sp

17. Which statement correctly describes resonance contributors of NO₃⁻?

  1. All N–O bonds have permanently different lengths
  2. Only electron placement changes; the atom arrangement stays fixed
  3. The nitrogen atom rapidly moves between three positions
  4. Three separate nitrate species exist in equilibrium

18. Which order of electron-pair repulsion is correct?

  1. LP–LP > LP–BP > BP–BP
  2. BP–BP > LP–BP > LP–LP
  3. LP–BP > LP–LP > BP–BP
  4. All repulsions are equal

19. Which Lewis contributor is generally preferred?

  1. The one with minimal formal-charge separation
  2. The one with the maximum number of formal charges
  3. The one placing negative charge on the less electronegative atom
  4. The one that changes the atomic skeleton

20. What is the molecular shape of XeF₄?

  1. Tetrahedral
  2. Square pyramidal
  3. Trigonal bipyramidal
  4. Square planar
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