FSc Part 1 Chemistry chapter 6: Chemical bonding MCQs with answers

By Team Megalecture · Updated 4 Nov 2026

29 exam-style questions on Chemical bonding, each with the answer and a short explanation. Ten of them are below to try. The chapter test draws ten fresh questions each time and is marked the moment you finish, with your score by topic.

29 questions · 3 topics · 10 per test

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What chapter 6 covers

Ten Chemical bonding questions with answers

Try each one, then open the answer. These ten stay the same; the test draws new ones every time.

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

  1. A
    sp
  2. B
    sp2
  3. C
    sp3
  4. D
    sp3d
Show answer

Answer: B. Each C forms three σ bonds (trigonal planar, 120°) using sp2 orbitals; the unhybridised p orbitals overlap sideways to form the π bond.

2. In the compound H3N→BF3, which statement is correct?

  1. A
    B donates a lone pair to N
  2. B
    F donates a lone pair to N
  3. C
    N and B are joined by an ionic bond
  4. D
    N donates its lone pair to the electron-deficient B atom
Show answer

Answer: D. B in BF3 has only six outer electrons and an empty orbital; the lone pair on N fills it, forming a coordinate covalent bond (arrow from donor N to acceptor B).

3. What is the H−O−H bond angle in a water molecule?

  1. A
    120°
  2. B
    109.5°
  3. C
    107.5°
  4. D
    104.5°
Show answer

Answer: D. O has two bond pairs and two lone pairs. Two lone pairs repel more strongly than one (as in NH3, 107.5°), squeezing the angle to 104.5°.

4. Why does the He2 molecule not exist?

  1. A
    He has no valence electrons
  2. B
    the numbers of bonding and antibonding electrons are equal, so the bond order is zero
  3. C
    He2 would be ionic
  4. D
    helium can form only π bonds
Show answer

Answer: B. He2 would have σ1s2 σ*1s2: bond order = (2 − 2) ÷ 2 = 0, so no stable bond.

5. What are the shape and bond angle of the BF3 molecule?

  1. A
    trigonal pyramidal, 107°
  2. B
    trigonal planar, 120°
  3. C
    T-shaped, 90°
  4. D
    tetrahedral, 109.5°
Show answer

Answer: B. B has three bond pairs and no lone pair, so the pairs spread out in a plane at 120°. NH3, with one lone pair, is the pyramidal one.

6. According to valence bond theory, the H−F bond is formed by overlap of

  1. A
    a 1s orbital of H with a half-filled 2p orbital of F
  2. B
    a 1s orbital of H with the 2s orbital of F
  3. C
    two p orbitals overlapping sideways
  4. D
    a 1s orbital of H with a completely filled 2p orbital of F
Show answer

Answer: A. A bond forms when two half-filled orbitals overlap and the electrons pair up. F (2s2 2p5) has one half-filled 2p orbital.

7. Which hydrogen halide has the highest bond energy?

  1. A
    HF
  2. B
    HCl
  3. C
    HBr
  4. D
    HI
Show answer

Answer: A. H−F is the shortest bond and the most polar, so it is the strongest. Bond energy falls to HI as the halogen gets larger.

8. Why is the first ionisation energy of nitrogen higher than that of oxygen?

  1. A
    oxygen atoms are larger
  2. B
    nitrogen has the greater nuclear charge
  3. C
    oxygen has fewer protons
  4. D
    nitrogen's half-filled 2p subshell is extra stable, while in oxygen a paired 2p electron is repelled and easily removed
Show answer

Answer: D. O has 8 protons, more than N, but its fourth 2p electron is paired and the repulsion makes it easier to remove. N has three unpaired 2p electrons (2p3).

9. Which carbon-carbon bond has the greatest bond energy?

  1. A
    C−C in ethane
  2. B
    C=C in ethene
  3. C
    C≡C in ethyne
  4. D
    C−C in benzene
Show answer

Answer: C. More shared pairs hold the atoms more strongly: C≡C (about 837 kJ mol−1) > C=C (about 614) > C−C (about 348).

10. Molecular orbital theory explains the paramagnetism of O2 because O2 has

  1. A
    two unpaired electrons in σ bonding orbitals
  2. B
    all electrons paired and a bond order of 2
  3. C
    one unpaired electron in the σ*2p orbital
  4. D
    two unpaired electrons in the π* antibonding orbitals
Show answer

Answer: D. The last two electrons go singly into the two degenerate π*2p orbitals (Hund's rule), giving two unpaired electrons. The Lewis structure O=O wrongly suggests all are paired.

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Chemical bonding: questions students ask

How many Chemical bonding MCQs are there?

29, each with the answer and a short explanation, across 3 topics: Periodic trends, ionic and covalent bonds, VSEPR theory, valence bond theory and hybridisation, Molecular orbital theory, bond energy and dipole moment. Every chapter test draws ten of them, so you can take it many times.

Is the FSc Part 1 Chemistry chapter 6 test free?

Yes. The test, the answers and the explanations are free and need no sign-up. Sign in only if you want your scores kept across devices.

How is the chapter test marked?

The moment you press Finish: your score, the right answer and an explanation for every question, and the ones you got wrong saved in My mistakes to retry.

Can I read the explanations in Urdu?

Yes. In practice mode and on your results you can switch the explanations to Urdu.

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