(a) Hydrofluoric acid exists as dimeric molecule (H2 F2 ) due to hydrogen bonding. It, thus, exhibits dibasic nature and forms two series of salts, KHF2 as [K+ and F– --- H –– F] and KF[K+ and F– ]. HCl and HBr exists as monomeric molecules as hydrogen bonding is not present.
(b) I – ions is a strong reducing agent. Iodide thus reduces ferric into ferrous, Cl – ion is a weak reducing agent and does not reduce Fe3+ to Fe2+.
(c) No d-orbitals are present in fluorine while d-orbitals are present in other halogens. The formation of X3– ions involves sp3d-hybrizaion.
(d) HF attacks glass bottles. The sodium and potassium silicates are converted into flurosilicates
Na2 SiO3 + 6HF → Na2SiF6 + 3H2O
(e) The weakest acidic nature of HF is due to following three factors :
(i) Strong H–F bond as the dissociation energy is high.
(ii) Large heat of dehydration dues to hydrogen bonding.
(iii) Low value of electron affinity.