(1) Bond dissociation energy normally decreases while moving down a group because of the increase in the atomic size. However, F2 has a lower bond dissociation energy than Cl2 and Br2 because of the smaller atomic size of fluorine.
Hence, the increasing order for bond dissociation enthalpy is as follows:
I2< F2< Br2< Cl2
(2) Bond dissociation energy of a H-X molecule ( where X = F, Cl, Br, I ) decreases with an increase in the size of an atom. As H-I bond is the weakest, it will act as the strongest acid.
Therefore, the increasing order acidic strength is as follows:
HF <HCl<HBr< HI
(3) BiH3≤ SbH3<AsH3< PH3< NH3
On moving down a group from nitrogen to bismuth, the atomic size increases but the electron density of the atom decreases (rapid increase in the volume of atoms). Hence, the basic strength decreases.