Boron halides can act as Lewis acids. Give reason.

Diborane is an important hydride of Boron a. During a class room discussion, a student argues that there is a covalent bond between boron atoms in diborane. What is your opinion. Give justification. b. Boron halides can act as Lewis acids. Give reason. c. Arrange the following Lewis acids in the increasing order of acidic strength. Substantiate your answer? 'BF_3 BCl_3, BBr_3'

SO_2 can act as

Why does BF_3' act as a lewis acid?

Borax, orthoboric acid and diborane are some useful compounds of boron Boric acid Is not a protonic acid but acts as a Lewis acid. Justify.

BCl_3 is a good Lewis acid. Why?

While sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions, ozone and nitric acid act only as oxidants, why?

The substance which can accept electrons is a Lewis acid. 'BCl_3, BF_3' and 'BBr_3' are Lewis acids. a. Arrange the above Lewis acids in the increasing,order of their acid strength. b. Give reason for this order of acidic strength, c. The chemistry of boron is different from that of other members of the same group. Mention any two differences and give reason.