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MCQEasyJEE 2023VSEPR Theory & Shapes of Molecules

JEE Chemistry 2023 Question with Solution

Given below are two statements: Statement I: SO2\text{SO}_2 and H2O\text{H}_2\text{O} both possess V-shaped structure. Statement II: The bond angle of SO2\text{SO}_2 is less than that of H2O\text{H}_2\text{O}

  • A

    Both Statements I and Statement II are incorrect

  • B

    Both Statement I is correct but Statement II is incorrect

  • C

    Statement I is correct but Statement II is incorrect

  • D

    Statement I is incorrect but Statement II is correct

Answer

Correct answer:C

Step-by-step solution

Standard Method

Given: Two statements about the shapes and bond angles of SO2\text{SO}_2 and H2O\text{H}_2\text{O}.

Find: Which statement is correct.

  1. Statement I: Both SO2\text{SO}_2 and H2O\text{H}_2\text{O} have V-shaped (bent) structures because lone pairs are present on the central atom.
  • In SO2\text{SO}_2, sulfur forms two bonds with oxygen and has one lone pair.
  • In H2O\text{H}_2\text{O}, oxygen forms two bonds with hydrogen and has two lone pairs.

Therefore, Statement I is correct.

  1. Statement II: Compare their bond angles.
SO2:∠O-S-O≈119.5∘\text{SO}_2 : \angle \text{O-S-O} \approx 119.5^\circH2O:∠H-O-H≈104.5∘\text{H}_2\text{O} : \angle \text{H-O-H} \approx 104.5^\circ

Since the bond angle in SO2\text{SO}_2 is greater than that in H2O\text{H}_2\text{O}, the statement "The bond angle of SO2\text{SO}_2 is less than that of H2O\text{H}_2\text{O}" is incorrect.

Conclusion: Statement I is correct, but Statement II is incorrect. Therefore, the correct option is C.

Common mistakes

  • Assuming that all bent molecules have the same bond angle is incorrect. Molecular shape alone is not enough; lone pairs, bond pairs, and bond multiplicity must also be compared.

  • Thinking that H2O\text{H}_2\text{O} has a larger bond angle because oxygen is smaller is misleading. The correct comparison depends on electron pair repulsions and the bonding environment around the central atom.

  • Ignoring the effect of double bonds in SO2\text{SO}_2 leads to the wrong conclusion. Double bond regions exert greater repulsion, which increases the bond angle compared with H2O\text{H}_2\text{O}.

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