Among NH3, H2O and HF, which would you expect to have highest magnitude of hydrogen bonding and why?

Asked by Abhisek | 1 year ago |  49

1 Answer

Solution :-

The extent of hydrogen bonding mainly depends on

(i) Electronegativity

(ii) Number of hydrogen atoms available for bonding.

Among oxygen, fluorine and nitrogen, the increasing order of their electro negativities are N < O < F.

Therefore, the expected order of the extent of hydrogen bonding is HF > H2O > NH3.

But, the actual order is H2O > HF > NH3.

Even though fluorine is more electronegative than oxygen, the extent of hydrogen bonding is high in water.

There is a shortage of hydrogens in HF, whereas there are exactly the right numbers of hydrogens in water. As a result, only straight chain bonding takes place.

On the other hand, oxygen forms a huge ring-like structure through its high ability of hydrogen bonding.

The extent of hydrogen bonding is limited In case of ammonia, because nitrogen has only 1 lone pair. Therefore, it cannot satisfy all hydrogens.

Answered by Pragya Singh | 1 year ago

Related Questions

What do you understand by the terms :

(i) Hydrogen economy 

(ii) Hydrogenation 

(iii) ‘syngas’ 

(iv) Water-gas shift reaction 

(v) Fuel cell?

Class 11 Chemistry Hydrogen View Answer

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.

Class 11 Chemistry Hydrogen View Answer

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.

Class 11 Chemistry Hydrogen View Answer

How can saline hydrides remove traces of water from organic compounds?

Class 11 Chemistry Hydrogen View Answer