Consider the following halides: (1) ; BCl_3,( | vedclass

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(A) The Lewis acid strength of group $13$ trihalides depends on the ability of the central metal atom to accept an electron pair.In $BCl_3$,the boron

Vedclass · Accepted Answer

$1 > 2 > 3 > 4$

Vedclass · Answer

(A) The Lewis acid strength of group $13$ trihalides depends on the ability of the central metal atom to accept an electron pair.In $BCl_3$,the boron atom is small and undergoes $p\pi-p\pi$ back-bonding with chlorine,which reduces its electron deficiency.As we move down the group from $B$ to $In$,the size of the central atom increases,and the extent of back-bonding decreases significantly.Therefore,the electron deficiency increases as we move from $BCl_3$ to $InCl_3$.However,the Lewis acidity is also influenced by the electronegativity and the size of the central atom. For group $13$ trihalides,the order of Lewis acid strength is $BCl_3 > AlCl_3 > GaCl_3 > InCl_3$ due to the effective back-bonding in $BCl_3$ and the increasing metallic character down the group.Thus,the correct decreasing order is $(1) > (2) > (3) > (4)$.

Consider the following halides: $(1) \; BCl_3$,$(2) \; AlCl_3$,$(3) \; GaCl_3$,$(4) \; InCl_3$. What is the decreasing order of their Lewis acid strength?

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