The ionization enthalpy of H–H bond is higher (\( 1312 kJ mol^{–1}\)) which shows that hydrogen has a low tendency to form H+ ions. Its ionization enthalpy value is comparable to that of halogens. Hence, it forms
→ a large number of covalent bonds
→ diatomic molecules (H2)
→ hydrides with element
Hydrogen does not possess metallic characteristics (lustre, ductility, etc.) like metals because ionization enthalpy is very high.
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?