Increasing oxidising nature of $I_{2}, {B r}_{2}, {C l}_{2}, F_{2}$ is : $I_{2} < {B r}_{2} < {C l}_{2} < F_{2}$ .
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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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