$F_{2}$ is better oxidising agent than $B r_{2}$ . It is due to:

small size of flourine atom

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more electron repulsions in flourine

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higher electronegativity of flourine

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non-metallic nature of fluorine

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Solution

The correct options are
A small size of flourine atom
B more electron repulsions in flourine
C higher electronegativity of flourine
F is more electronegative than Br. Therefore it can easily accept $e^{-}$ and oxidise others.
Therefore $F_{2}$ is better oxidising agent than $B r_{2}$

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F2 is better oxidising agent than Br2. It is due to:

The correct options are A small size of flourine atom B more electron repulsions in flourine C higher electronegativity of flourineF is more electronegative than Br. Therefore it can easily accept e− and oxidise others.Therefore F2 is better oxidising agent than Br2

$F_{2}$ is better oxidising agent than $B r_{2}$ . It is due to:

The correct options are
A small size of flourine atom
B more electron repulsions in flourine
C higher electronegativity of flourine
F is more electronegative than Br. Therefore it can easily accept $e^{-}$ and oxidise others.
Therefore $F_{2}$ is better oxidising agent than $B r_{2}$