1. The H-C-H bond angle in CH₄ , the H-N-H bond angle in NH₃ , and the H-O-H bond angle in H₂O are all greater than 90° . 2. The H-O-H bond angle in H₂O is larger than the H-C-H bond angle in CH₄ . 3. The H-O-H bond angle in H₂O is smaller than the H-N-H bond angle in NH₃ . 4. The H-C-H bond angle in CH₄ is larger than the H-N-H bond angle in NH₃ .

Answer: 2. The H-O-H bond angle in H₂O is larger than the H-C-H bond angle in CH₄ . Key idea: lone pairs repel more than bond pairs, so bond angles shrink as lone pairs increase. CH₄ : 0 lone pairs, angle 109.5°. NH₃ : 1 lone pair, angle about 107°. H₂O : 2 lone pairs, angle about 104.5°. Statement 2 says the angle in water is larger than in methane. That is false, since 104.5° < 109.5°. Statements 1, 3 and 4 agree with the values above.

Topic: VSEPR theory and shapes of molecules· Chemical Bonding and Molecular Structure

Consider the molecules CH_4, NH_3 and H_2O. Which of the given statements is false ?

1. The \(H-C-H\) bond angle in \(CH_4\), the \(H-N-H\) bond angle in \(NH_3\), and the \(H-O-H\) bond angle in \(H_2O\) are all greater than \(90°\).

2. The \(H-O-H\) bond angle in \(H_2O\) is larger than the \(H-C-H\) bond angle in \(CH_4\).

3. The \(H-O-H\) bond angle in \(H_2O\) is smaller than the \(H-N-H\) bond angle in \(NH_3\).

4. The \(H-C-H\) bond angle in \(CH_4\) is larger than the \(H-N-H\) bond angle in \(NH_3\).

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Answer: 2. The \(H-O-H\) bond angle in \(H_2O\) is larger than the \(H-C-H\) bond angle in \(CH_4\).

Key idea: lone pairs repel more than bond pairs, so bond angles shrink as lone pairs increase.

\(\mathrm{CH_4}\): 0 lone pairs, angle 109.5°.
\(\mathrm{NH_3}\): 1 lone pair, angle about 107°.
\(\mathrm{H_2O}\): 2 lone pairs, angle about 104.5°.

Statement 2 says the angle in water is larger than in methane. That is false, since 104.5° < 109.5°. Statements 1, 3 and 4 agree with the values above.

Doubtly AI · 30 Oct 2026 AI-generated · not yet verified Report

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Consider the molecules CH_4, NH_3 and H_2O. Which of the given statements is false ?

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