Question

How do the conductivities of various water-soluble molecular compounds compare with ionic compounds?

Answer 1

The ionic compounds are completely dissociated into ions in water hence they easily conduct electricity in aqueous solution

Ex

NaCl (S) + H₂O (l) $\rightarrow$ Na⁺ (aq) + Cl^- (aq)

As well as in molten form of ionic compounds their is also ions are present hence they also conduct electricity in molten of fused form

But in case of water soluble molecular compounds they have no ions neither in molten nor in aqueous form so they are not able to conduct electricity .

Ex:- NH₃ , PCl₃ etc

They forms either H-bond with water or Vanderwaal force of attractions .