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F2 has lower bond dissociation enthalpy ...

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

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Fluorine is expected to have the highest value of bond dissociation energy because it has the smallest size and highest eletronegativity value among halogens. Due to its extremely small size, the repulsions among shared electrons take place which reduces its bond dissociation enthalpy, which is less than that of `Cl_2`.
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(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

U-LIKE SERIES-THE P-BLOCK ELEMENTS -LONG ANSWER QUESTION-II
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