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 empty $p$-orbital and chlorine has lone pairs of electrons. This leads to $p\pi - p\pi$ back bonding,which reduce

Vedclass · Accepted Answer

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

Vedclass · Answer

(B) In $BCl_3$,the boron atom has an empty $p$-orbital and chlorine has lone pairs of electrons. This leads to $p\pi - p\pi$ back bonding,which reduces the electron deficiency of the boron atom and stabilizes the monomeric form.In $BH_3$,there is no such back bonding because hydrogen does not have lone pairs. To complete its octet and achieve stability,$BH_3$ undergoes dimerization to form $B_2H_6$ (diborane),which involves $3c-2e^-$ (three-center two-electron) bonds.

$Bond$	$E_{diss} (kJ \ mol^{-1})$
$C-A$	$240$
$C-B$	$328$
$C-C$	$276$
$C-D$	$485$

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

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