BCl_3 does not exist as a dimer,whereas BH_3 | vedclass

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(B) In $BCl_3$,the boron atom has an incomplete octet. The lone pair of electrons on the chlorine atom is donated to the vacant $p$-orbital of the bor

Vedclass · Accepted Answer

$BCl_3$ has $p\pi - p\pi$ back bonding,but $BH_3$ does not have such multiple bonding.

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(B) In $BCl_3$,the boron atom has an incomplete octet. The lone pair of electrons on the chlorine atom is donated to the vacant $p$-orbital of the boron atom,resulting in $p\pi - p\pi$ back bonding. This stabilizes the molecule and satisfies the octet of boron,preventing dimerization. In $BH_3$,hydrogen does not have a lone pair to participate in back bonding,so $BH_3$ dimerizes to form $B_2H_6$ to complete the octet of boron.

$BCl_3$ does not exist as a dimer,whereas $BH_3$ exists as a dimer $(B_2H_6)$,because -

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