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Fluorine is a stronger oxidising agent than chlorine because:
(a) F-F bond has a low enthalpy of dissociation.
(b) Fluoride ion ($F^-$) has high hydration enthalpy.
(c) Electron gain enthalpy of fluorine is less negative than chlorine.
(d) Fluorine has a very small size.
Choose the most appropriate answer from the options given:
Detailed Solution
$X_2(g)\xrightarrow{\Delta H_{diss}}2X(g)\xrightarrow{\Delta_{eg}H}X^-(g)\xrightarrow{\Delta_{hyd}H}X^-(aq)$. Adding these steps, more energy is released for fluorine due to its low bond dissociation enthalpy and high hydration enthalpy, making it the stronger oxidising agent.