`N_2` has greater bond energy than `N_(2)^(+)` but `O_2` has lower bond dissociation energy than `O_(2)^(+)`. Explain.

Explain why N_(2) has a greater bond dissociation energy than N_(2)^(+) while O_(2) has lesser bond dissociation energy than O_(2)^(+).

(a) H_(2)^(+)and H_(2)^(-) ions have same bond order but H_(2)^(-) ion is more stable. Explain. (b) N_(2) has a greater bond dissociation enthalpy than N_(2)^(+) ion hals more bond dissociation enthalpy than O_(2). Why ? (c ) Can we have ahomonuclear diatomic molecule with all its ground state molecular orbitals full of electrons ? (d) When a magnet is dipped in a jar of liquid oxygen, some oxygen clings to it. Assign reason :

The bonds present in N_(2)O_(5) are .

The bonds present in N_(2)O_(5) are .

The bonds present in N_(2)O_(5) are .

With the help of molecular oribital theory explain Why N_2 has greater dissociation energy than N_2^+ ?

Account for the following : (i) NH_(3) is a stronger base than PH_(3) (ii) Sulphur has a greater tendency for catenation than oxygen. (iii) Bond dissociation energy of F_(2) is less than that of Cl_(2) .

Bond dissociation energy of F_(2) is less that of Cl_(2) give reason.

Which of the halogens has highest value of bond dissociation energy?

How the bond energy varies from N_(2)^(Θ) and N_(2)^(o+) and why ?