Question

among halogens f2 is strongest oxidising agent

Answer 1

Fluorine hydration energy is very high due to its small size.

Also, dissociation enthalpy of fluorine is less as compared to chlorine due to large electron-electron repulsion in fluorine.

Because of these factors, fluorine has high positive electrode potential than chlorine.

Hence, among halogens, F2 is strongest oxidising agent.

Answer 2

Among halogens, $\[{F_2}\]$ is the strongest oxidising agent due to high hydration enthalpy of $\[{F^ - }\]$ and low dissociation enthalpy of $\[F - F\]$ bond.

Explanation:

• Halogens have a high electronegativity value due to which they act as oxidising agents.
• They have a tendency to accept an electron to obtain the inert gas configuration. The element that accepts electrons undergoes reduction and oxidises other elements.
• The oxidising tendency of an element depends upon electronegativity, electron gain enthalpy, bond dissociation enthalpy and hydration energy.
• The oxidising power of an element increases with an increase in electronegativity.
• Among halogens, Fluorine has the highest electronegativity.
• The electron gain enthalpy of Fluorine is low due to its small size as electron gain enthalpy increases with an increase in size.
• However, the bond dissociation enthalpy of Fluorine is low and the hydration power is high.
• These two effects compensate for the low electron gain enthalpy of Fluorine and therefore, Fluorine is the strongest oxidising agent as compared to the other halogens.

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