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Chemical Bonding and Molecular Structure · I PU Chemistry

Name: ____________________
Date: ____________________
Mode: BalancedQuestions: 20Difficulty: MixedCheck code: 52755603

1. 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

2. 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

3. What are the electron geometry and molecular shape of NH₃, respectively?

  1. Tetrahedral; trigonal pyramidal
  2. Trigonal planar; trigonal planar
  3. Tetrahedral; bent
  4. Trigonal pyramidal; tetrahedral

4. 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

5. 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

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

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

7. Which change generally weakens and lengthens an O₂ bond?

  1. Adding an electron to an antibonding orbital
  2. Removing an electron from an antibonding orbital
  3. Increasing bond order
  4. Pairing core electrons

8. 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

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

  1. CH₄
  2. NH₃
  3. H₂O
  4. BF₃

10. Which compound should show the greatest covalent character?

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

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

  1. −1
  2. +2
  3. +1
  4. 0

12. 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

13. Which carbon–carbon bond is shortest?

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

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

  1. NO₃⁻
  2. H₂O
  3. NH₃
  4. CH₄

15. Which cation most strongly polarises the same anion?

  1. K⁺
  2. Al³⁺
  3. Mg²⁺
  4. Na⁺

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

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

17. 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

18. What is the molecular shape of XeF₄?

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

19. Which species is an odd-electron molecule?

  1. NO
  2. CO₂
  3. N₂
  4. CH₄

20. Which overlap forms a pi bond?

  1. Sidewise overlap of parallel p orbitals
  2. Head-on overlap along the internuclear axis
  3. Overlap of two spherical s orbitals only
  4. Overlap that produces cylindrical symmetry about the bond axis
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