I read that $\ce{CCl2}$ is non-polar. When I read about the reason on the net it stated that $\ce{CCl2}$ has a linear structure, but according to VSEPR theory it should have bent V-shaped geometry. Please clarify.

  • $\begingroup$ Why bother about this compound ? It is not stable. It only exists as an intermediate in some reactions. You will never be able to store it in a flask with label CCl2. So why ? $\endgroup$
    – Maurice
    Dec 25, 2019 at 10:01
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    $\begingroup$ @Sameer My apologies, I misread the compound formula as dichloromethane, so I deleted my comment as irrelevant. Sorry for the confusion, this is a nice question. Have a look at What is the hybridization state of E (= Sn, C) in ECl₂? and the paper Martin refers to in his answer: doi.org/10.1039/b202865d, this should answer your question (yes, CCl₂ is bent). $\endgroup$
    – andselisk
    Dec 25, 2019 at 12:16
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    $\begingroup$ @Maurice "Science isn't about why; it's about why not". $\endgroup$
    – andselisk
    Dec 25, 2019 at 12:18
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    $\begingroup$ VSEPR theory is great, but only up to a certain point. You should probably not use it for "exotic" species like carbenes. Even though it happens to give the right result in this case, that's probably more of a coincidence than anything. $\endgroup$ Dec 25, 2019 at 14:18


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