The total number of nonbonding electron pairs present in the Lewis structure of CH4 is

Question

BlackTom AI · Accepted Answer

Carbon has four valence electrons and each hydrogen has one, so the total valence electrons available for CH4 are 4 + 4×1 = 8 electrons (which is 4 electron pairs).

Step-by-step reasoning and calculations:
1. Count valence electrons: C = 4, 4 H = 4×1 = 4, total = 4 + 4 = 8 electrons.
2. Convert to electron pairs: 8 electrons ÷ 2 = 4 electron pairs.
3. Build the Lewis structure: Carbon, being the central atom, forms four single C–H bonds. Each single bond contains one bonding pair (2 electrons).
4. Assign the bonding pairs: 4 bonds × 1 bonding pair per bond = 4 bonding pairs. These 4 bonding pairs use all 4 available electron pairs (4 × 2 electrons = 8 electrons).
5. Determine nonbonding (lone) pairs: total electron pairs (4) − bonding pairs (4) = 0 nonbonding pairs.

Why this is correct:
- A nonbonding electron pair (lone pair) is an electron pair localized on a single atom and not shared in a bond. In CH4 every valence electron is used to form the four C–H bonds, so there are no electrons left as lone pairs on carbon or on any hydrogen (hydrogen achieves its duet by sharing, not by keeping lone pairs).

Why the other options are incorrect:
- Any option claiming 1, 2, 3, or 4 nonbonding pairs would require more than 8 total valence electrons or fewer bonding pairs; neither is true for CH4. All available electrons are consumed in bonding, leaving zero lone pairs.

Conclusion: The total number of nonbonding electron pairs in the Lewis structure of CH4 is zero, which matches the provided answer.

The total number of nonbonding electron pairs present in the Lewis structure of CH4 is单项选择题

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