# Can a Cl atom bond with a non-carbon atom?

I am currently doing the questions:

1. Write equations for the reaction of Chlorine with Propene and 2-butene using structural

So I know that Propene is $\ce{H3C-CH=CH2}$ and $\ce{Cl}$ is $\ce{Cl2}$ diatomic.

So:

$\ce{CH3-CH=CH2 + Cl2->}$ From this I observe that naturally, the double bond is removed in the presence of an addition reaction and that the Chlorine atom bonds to the $\ce{CH}$ pair and the other $\ce{Cl}$ atom does not bond to any of them but attaches itself at the end.

• Why did the second $\ce{Cl}$ pair not attach itself to $\ce{CH2}$? Does this mean that atoms can only bond to $\ce{CH}$ pair and nothing more than that, e.g. not $\ce{CH2}$ or $\ce{CH3}$, etc..

Second question for the reaction of 2-butene with Chlorine. I know that 2-butene is $\ce{H3C-CH=CH-CH3}$

So $\ce{H3C-CH=CH-CH3 + Cl2 ->}$ • I noticed, like what happened above, the chlorine atom bonds to only the $\ce{CH}$ pair. Here however there are two $\ce{CH}$ pairs so the Chlorine doesn't need to attach itself at the end of the chain, unlike the first picture.

Are my observations correct? My textbook has no mention of this.

• With respect to (1), I imagine that Cl bonding in those locations is energetically favorable given that there are no C-H bonds being broken. Of course this does NOT mean that atoms can only bond to the CH pair and nothing else but then we'd have to consider the C-H bond rupture which is an entirely separate process. – LordStryker Sep 29 '14 at 12:13 