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  • Which of the following statements about the Lewis acid strength of <img alt="\mathrm{BF}_3, \mathrm{BCl}_3" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7BBF%7D_3%2C%20%5Cmathrm%7

Which of the following statements about the Lewis acid strength of \mathrm{BF}_3, \mathrm{BCl}_3, and \mathrm{BBr}_3 is incorrect?

(i) The Lewis acid strength increases as the size of the halogen atom increases.
(ii) The Lewis acid strength increases as the electronegativity of the halogen atom increases.
(iii) The Lewis acid strength decreases as the size of the halogen atom increases.
(iv) The Lewis acid strength decreases as the electronegativity of the halogen atom increases.

Option: 1

i, ii
 


Option: 2

ii, iii
 


Option: 3

i, iv
 


Option: 4

ii, iv


Answers (1)

best_answer

A molecule is said to be a Lewis acid if it can accept a lone pair.

This anomaly is explained on the basis of the relative tendency of the halogen atom to back donate its unutilised electrons to vacant p-orbital of boron atom. In \mathrm{BF}_3, boron has a vacant 2 \mathrm{p}-orbital and each flourine has fully filled unutilised 2 p-orbitals. Fluorine transfers two electrons to vacant 2 p -orbital of boron, thus forming \mathrm{p} \pi-\mathrm{p} \pi bond.

The tendency to back donate decreases from \mathrm{F} to I as energy level difference between \mathrm{B} and halogen atom increases from \mathrm{F} to I.

So,the order of Lewis acidity is \mathrm{BBr}_3>\mathrm{BCl}_3>\mathrm{BF}_3

Posted by

Irshad Anwar

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