Which of the following molecules has the shortest carbon-carbon single bond length?

C H_{2}

C H - C - C H_{3}

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C H_{2}

C H - C = N

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C H_{2}

C H - C = O

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C H_{2}

C H - C H

C H_{2}

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Solution

The correct option is C $C H_{2}$ = $C H - C = O$
The bond between $C - O$ in $C = O$ will be minimum as oxygen have higher electronegativity than carbon. The $C = C$ bond is more likely to be added upon some reagent rather than the $C = O$ bond. The carbonyl group is more reactive than the alkene group. Hence carbon and oxygen in carbonyl compound will be more attracted towards each other. Hence they have small bond length.

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Similar questions

C H_{2} = C H - C \equiv C H

C H \equiv C - C \equiv C H

C H_{3} - C H = C H_{2}

C H_{2} = C H - C H = C H_{2}

C H_{3} - C H_{3}, C H_{2} = C H_{2}

C H \equiv C H

C H_{2} = C H - . . N H - C H_{3}

C H_{2} = C H - . . O . . - C H_{3}

C H_{2} = C H - . . O . . - C H = C H_{2}

C H_{2} = C H - N H_{2}

A g N O_{3}

C = C

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