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Explain why the electrons gain enthalpy ...

Explain why the electrons gain enthalpy of fluorine is less negative than that of chlorine?

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Atomic size of fluorine is less than chlorine. Hence , the interelectronic repulsion, i.e., the electrons already preset in `F` and the electron to be added is much more than the `Ci` atom. Hence, the incoming electron is accepted with diffculty in `F`. The energy released during formation of `F_((g))^(Theta)` from `F_((g))` is less than that of formation of `Cl^(Theta)` from `Cl_((g))`. Thus, negative gain enthalpy of `F` is lower than that of `Cl`.
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The negative electron gain enthalpy of fluorine is less than that of chlorine.

Electron Gain Enthalpy

Electron gain enthalpy of fluorine is less than that of chlorine - explain.

Assertion : The electron gain enthalpy of chlorine is less negative than that of fluorine. Reason : The fluorine atom is much smaller in size than that of chlorine.

(a) Halogens have maximum negative gain enthalpy in the respective periods of the periodic table. Why? (b) Although electron gain enthalpy of fluorine is less negative as compared to chlorine, fluorine is a stronger oxidising agent than chlorine . Why? Fluorine exhibits only-1 oxidation state, wherease other hlaogens exhibit +1,+3,+5, and +7 oxidation states also. explain.

(a) Halogens have maximum negative gain enthalpy in the respective periods of the periodic table. Why? (b) Although electron gain enthalpy of fluorine is less negative as compared to chlorine, fluorine is a stronger oxidising agent than chlorine . Why? Fluorine exhibits only-1 oxidation state, whereas other halogens exhibit +1,+3,+5, and +7 oxidation states also. Explain.

Why is the electron gain enthalpy of O or F less than that of S or Cl?

Electron gain enthalpies of noble gases are negative.

Electronegativity of fluorine is greater than that of chlorine.

Fluorine has the highest electronegativity among the ns^(2) np^(5) group on the Pauling scale, but the electron affinity opf fluorine is less than that of chlorine because: