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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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Bond dissociation energy of F_(2) is less than that of CI_(2) . Explain. Or F_(2) has lower bond dissociation enthalpy than CI_(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 :

Knowledge Check

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

    A
    Both A and R are true and R is the correct explanation of A
    B
    Both A and R are true but R is NOT the correct explanation of A
    C
    A is true but R is false
    D
    A is false and R is True.

  • Bond dissociation enthalpy of the halogens shows the trend

    A
    `F-F lt Cl - Cl gt Br - Br gt I - I `
    B
    `F - F gt Cl - Cl gt Br - Br gt I-I`
    C
    `F - F gt Cl - Cl lt Br - Br gt I-I`
    D
    `F - F gt Br - Br gt Cl- Cl gt I -I`

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