Question

Fluorine (${{F}_{2}}$ ) is a better oxidising agent than bromine ($B{{r}_{2}}$ ). It is due to
(A) Small size of fluorine
(B) More electron repulsion in fluorine
(C) More electronegativity of fluorine
(D) Non-metallic nature of fluorine

Answer 1

Hint: Both bromine and fluorine are halogens and belong to group 17 of the periodic table. The halogens have seven electrons in their valence shell and thus require only one electron to complete their octet. This is the reason why halogens are very reactive.

Complete Step by Step Solution:
An oxidising agent is a substance that gains an electron from a reducing agent during a redox chemical reaction. It is also known as an oxidant. When there is a gain of electrons during a chemical reaction, then the reaction is known as reduction. When there is a loss of electrons during a chemical reaction, then the reaction is known as oxidation.

The elements that have higher electronegativity, have a higher tendency to gain an electron, that is, they are better oxidising agents. Fluorine is a highly electronegative element as compared to other elements in the group. Hence, fluorine is a better oxidising agent as compared to chlorine, bromine, and iodine.

Fluorine (${{F}_{2}}$) is a better oxidising agent than Bromine ($B{{r}_{2}}$). It is due to the high electronegativity of fluorine.
Correct Option: (C) More electronegativity of fluorine.

Note: Fluorine (${{F}_{2}}$) is very small in size as compared to bromine ($B{{r}_{2}}$), due to which the extra electron experiences significantly more electron repulsion in it. Also, fluorine is non-metallic in nature.