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Introduction to d and f Block Elements

Which of the ...

Question

Which of the following is incorrect with respect to property indicated?

E . N . : F > C l > B r

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E . A . : C l > B r < F

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Oxidising power:

F_{2} > C l_{2} > B r_{2}

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Bond energy:

F_{2} > C l_{2} > B r_{2}

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Solution

The correct option is D Bond energy: $F_{2} > C l_{2} > B r_{2}$
A) $E . N . : F > C l > B r$ - Electonegativity decreases down the group and $F$ is the most electronegative element.
B) $E . A . : C l > B r < F$ - Electron affinity of fluorine is less than that of chlorine because of small size of $F$ atom. As a result, there is strong interelectronic repulsion in the relatively small $2 p$ orbitals of $F$ and thus, the incoming electron does not experience much attraction.
Oxidising power: $F_{2} > C l_{2} > B r_{2}$ - Flourine is stronger oxidising agent than chlorine because low bond dissociation energy of $F - F$ bond and high hydration enthalpy of $F^{-}$ .
Bond energy $F_{2} > C l_{2} > B r_{2}$ is wrong because low bond dissociation energy of $F - F$ bond than $C l - C l$ .

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Similar questions

F_{2} > C l_{2} > B r_{2} > I_{2}

F_{2} > C l_{2} > B r_{2} > I_{2}

C l > F > B r > I

F > C l > B r > I

F_{2} > C l_{2} > B r_{2} > I_{2}

F_{2} > C l_{2} > B r_{2} > I_{2}

C l > F > B r > I

F > C l > B r > I

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

F_{2} > C l_{2} > B r_{2} > I_{2} :

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

H O C l > H C l O_{2} > H C l O_{3} > H C l O_{4} :

(x^{2} + y^{2})

x

y

I_{2}, {B r}_{2}, {C l}_{2}, F_{2}

I_{2} < {B r}_{2} < {C l}_{2} < F_{2}

F_{2}, C l_{2}

B r_{2}

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