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In spite of having less electron affinity than chlorine, fluorine is the strongest oxidizing agent among the halogens. The most important reason for this phenomenon is :
lower bond dissociation energy of $F_{2}$ than $C l_{2}$
much lower heat of hydration of $F^{-}$ than $C l^{-}$
much greater heat of hydration of $F^{-}$ than $C l^{-}$
greater electronegativity of $F$ than $C l$

A

lower bond dissociation energy of

F_{2}

than

C l_{2}

B

much greater heat of hydration of

F^{-}

than

C l^{-}

C

greater electronegativity of

F

than

C l

D

much lower heat of hydration of

F^{-}

than

C l^{-}

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Similar Questions

Q1

In spite of having less electron affinity than chlorine, fluorine is the strongest oxidizing agent among the halogens, The most important reason for this phenomenon is :

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Q2

Why the Bond dissociation energy of Cl-Cl is greater than F-F. And why the Bond Dissociation energy of H-F is greater than H-H.

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Q3

Fluorine has lesser electron affinity value than chlorine. However, fluorine shows the greater ease of formation of

F^{-}

ion. than chlorine for

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ion. How do you justify this?

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Q4

Reason
Due to inter-electronic repulsion between $$F$$ atom, $$F - F$$ bond length in $$F_{2}$$ molecule is higher than $$Cl - Cl$$ bond length in $$Cl_{2}$$ molecule.
Assertion
The bond dissociation energy of $$F_{2}$$ molecule is less than that of $$Cl_{2}$$ molecule.

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Q5

Assertion: F is more electronegative than

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.
Reason: F has high electron affinity than

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.

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