`F_2` has lower bond dissociation enthalpy than `Cl_2.` Why?

(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 :

Assertion (A): F, has lower bond dissociation energy than Cl_(2) . Reason (R): Flourine is more electronegative than chlorine.

Give reasons : (i) PCl_(5) is more volatile than PCl_(3) . (ii) O-O bond has lower bond dissociation enthalpy than S-S bond. (iii) F_(2) is stronger oxidising than Cl_(2) .

N_(2)^(+) has greater bond dissociation enthalpy than N_(2) molecule.

What is meant by bond dissociation enthalpy?

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

i. Arrange the following in decreasing order of bond dissociation enthalpy F_(2) , Cl_(2) , Br_(2) , I_(2) ii. Bi does not form pπ-pπ bonds. Give reason for the observation. iii.Electron gain enthalpy of oxygen is less negative than sulphur. Justify