- #1
AryaUnderfoot
- 17
- 0
For acyl chloride the very electronegative oxygen atom attracts electrons of the carbon atom, thus greatly polarised the C-Cl bond. But won't it attract electrons of the Cl atom too? Then with the electrons drifting towards the C atom, it's partial positive charge should be reduced, but why is that wrong?
Also, since the C-Cl bond is greatly polarised, the bonding should be stronger, isn't it? Like C-F bond is more polar than C-Cl bond, so the fluoroalkane is less reactive than chloroalkane, but why is that acyl chloride, with its very polarised C-Cl bond, so reactive?
And for chlorobenzene, the electrons on halogen atom are delocalised into the benzene ring, causing the polarity of C-X bond to decrease, but why is it that the bond is stronger than haloalkane?
I realize that this is a very long question, thank you for your patience
Also, since the C-Cl bond is greatly polarised, the bonding should be stronger, isn't it? Like C-F bond is more polar than C-Cl bond, so the fluoroalkane is less reactive than chloroalkane, but why is that acyl chloride, with its very polarised C-Cl bond, so reactive?
And for chlorobenzene, the electrons on halogen atom are delocalised into the benzene ring, causing the polarity of C-X bond to decrease, but why is it that the bond is stronger than haloalkane?
I realize that this is a very long question, thank you for your patience