`H_(2)^(+) and H_(2)^(–)` have same bond order. Which is more stable?

Do N_(2)^(+) and O_(2)^(+) have same bond order?

Which two of H_(2)^(+), H_(2)^(-) and H_(2)^(2-) have the same bond order ?

(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 :

Expalin (a) H_(2)^(o+) and H_(2)^(Θ) ions have same bond order but H_(2)^(o+) ions are more stable than H_(2)^(Θ) (b) It is possible to have a diatomic molecule with its ground sate MO s full with electrons (c ) Why 2p_(x0 or 2p_(y) orbitals do not combine with 2s orbitals to form MO (Taking Z-axis as the internuclear axis) .

Do H_(2)^(+) and H_(2)^(-) ions have same or different bond orders ?

Calculate the bond order in (i) H_(2)^(+) (ii) H_(2)^(-) and H_(2)^(2-) have the same bond order?