Why do molecules with multiple bonds not considered to have more electron groups than molecules with single bonds?

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Why do molecules with multiple bonds not considered to have more electron groups than molecules with single bonds?

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Answer 1 · 2018-01-15T23:20:55

Because molecular shape has only to do with the number of bonding directions.

All that is accomplished by having a multiple-bond is more electron-repulsion of surrounding bonds. Consider comparing these three molecules:

The bond angles around the carbon are #180^@#, #180^@#, and (for the third molecule, calculated to be) #178.509^@#, respectively. So more or less, still approximately #180^@#.

Either way, the number of bonding groups around the carbon do NOT change for all three cases. The molecular shape is still basically linear around carbon.

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Why do molecules with multiple bonds not considered to have more electron groups than molecules with single bonds?

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