To form a regular bond, an electron-deficient hydride does not have sufficient electrons in which 2 electrons are shared by 2 atoms.
e.g., B2 H6,
Al2 H6 etc.
Conventional Lewis structures cannot able to represent these hydrides. B2H6, for example, contains 4 regular bonds and 2 3 centered-2 electron bond.
They have a tendency to accept electrons because, these hydrides are electron-deficient. Hence, they act as Lewis acids.
\( B_{2}H_{6}+2NMe\rightarrow 2BH_{3}.NMe_{3}B_2H_6\)
\( +2CO→2BH_3.CO\)
Answered by Pragya Singh | 1 year agoWhat do you understand by the terms :
(i) Hydrogen economy
(ii) Hydrogenation
(iii) ‘syngas’
(iv) Water-gas shift reaction
(v) Fuel cell?
Do you expect different products in solution when aluminium (III) chloride and potassium chloride treated separately with
(i) alkaline water
(ii) acidified water, and
(iii) normal water. Write equations wherever necessary.
What do you expect the nature of hydrides is, if formed by elements of atomic numbers 15, 19, 23 and 44 with dihydrogen? Compare their behaviour with water.
How can saline hydrides remove traces of water from organic compounds?