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Oxides and Oxoanions

Increasing ox...

Question

Increasing oxidising nature of $I_{2}, {B r}_{2}, {C l}_{2}, F_{2}$ is : $I_{2} < {B r}_{2} < {C l}_{2} < F_{2}$ .
if true enter 1, else enter 0.
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Solution

The correct option is A 1
Increasing oxidizing nature $I_{2} < {B r}_{2} < {C l}_{2} < F_{2}$ .

Fluorine has low heat of dissociation and high heat of hydration which more than compensates the lower value of electron affinity. Hence, fluorine is the strongest oxidizing agent.

Bromine and iodine have low dissociation energies than chlorine but they are poor oxidizing agents than chlorine. This is due to their small electron affinities and smaller hydration energies.

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Similar questions

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

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

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}

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