Chemistry – Chemical Bonding Exam

Chemistry Examination

Assessment of Chemical Bonding Concepts

Class
1st Year
Subject
Chemistry (SNC)
Paper Type
Chapter Assessment

Chapter 3: Chemical Bonding

Q1. Multiple Choice Questions
10 Marks

Choose the correct option for each of the following questions. Each question carries 1 mark.

1. What is the shape of H2S molecule?
A Linear
B V-shaped
C Tetrahedral
D Trigonal planar
2. In Cl2 molecule, the overlap is of which type?
A s-s
B s-p
C p-p
D d-p
3. Which molecule exhibits asymmetrical electron density due to s-p overlap?
A HCl
B Cl2
C H2
D O2
4. Which statement is true for π bonds?
A They form from s-s
B They form by parallel p-orbital overlap
C They form by d-orbital overlap
D They are always stronger than σ bonds
5. Which of the following hybridizations leads to maximum bond strength and symmetry?
A sp
B sp3
C sp2
D p only
6. The shape of methane is explained by:
A VSEPR theory only
B sp3 hybridization
C Unhybrid orbitals
D Molecular orbital theory
7. What type of molecular orbital is formed when two atomic orbitals overlap with same sign wave functions?
A π*
B σ*
C Bonding orbital
D Anti-bonding orbital
8. Bond order is calculated using which formula?
A (b – a)/2
B a + b
C a – b
D (a – b)/2
9. Which molecular orbital is higher in energy than the atomic orbitals that form it?
A Bonding
B Non-bonding
C Hybrid
D Anti-bonding
10. Which of the following molecules has a triple bond according to MOT?
A H2
B O2
C He2
D N2
Q2. Short Answer Questions
15 Marks

Write down short answers to the following questions.

  1. Xenon is a noble gas (group 18); xenon trioxide has the following structure:
    i. By counting electron pairs around the central atom, explain why xenon trioxide has this shape.
    ii. Draw a structure of xenon trioxide showing partial charges on the atoms and the direction of the dipole in the molecule.
  2. Draw the orbital structures of the CO2 molecule in terms of VBT.
  3. HI is a strong acid and a robust reducing agent, whereas HF is a weaker acid. Explain. (Quick Check 3.5)
  4. Why is HCl molecule polar?
  5. How does the π bond form in O2?
  6. Draw the orbital overlap to show the formation of F2 and HF molecules. (Quick Check 3.6)
  7. Differentiate between sp and sp3 hybridization.
  8. How does hybridization help explain molecular shapes?
  9. Why is He2 molecule not formed?
  10. Difference between σ and π bonds.
  11. Give electronic configuration of nitrogen (N)
  12. Why does O2 molecule show paramagnetism?
  13. What happens to the energy of a molecule when bonding orbitals are formed?
  14. Describe the arrangement of molecular orbitals in N2.
  15. Name the geometry formed in sp3 hybridization.
Q3. Detailed Answer Questions
10 Marks

Write detailed answers to the following questions. (Answer any 2)

1. Explain the orbital hybridization for CH4, NH3, BF3, and BeCl3.
2. Differentiate between sp, sp2, and sp3 hybridization in terms of bond angles, geometry, and examples.
3. Explain sp3 hybridization in detail with reference to CH4. Include diagrams and electron configuration.

MCQ Section Score

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