When a chloride ion is formed from an isolate | vedclass

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Question

(D) The process of adding an electron to an isolated gaseous atom to form a gaseous anion is defined as electron gain enthalpy. $Cl(g) + e^- \rightarr

Vedclass · Accepted Answer

Ionization potential of $Cl^-$

Vedclass · Answer

(D) The process of adding an electron to an isolated gaseous atom to form a gaseous anion is defined as electron gain enthalpy. $Cl(g) + e^- \rightarrow Cl^-(g) + 3.8 \ eV$. Since energy is released,the electron gain enthalpy is $-3.8 \ eV$. The electron affinity is defined as the negative of the electron gain enthalpy,which is $+3.8 \ eV$. Conversely,the ionization potential of an ion is the energy required to remove an electron from it. For $Cl^-(g) \rightarrow Cl(g) + e^-$,the energy required is equal to the electron affinity of the neutral atom,which is the ionization potential of the $Cl^-$ ion. Therefore,the energy released during the formation of $Cl^-$ from $Cl$ is equal to the ionization potential of $Cl^-$.

When a chloride ion is formed from an isolated gaseous chlorine atom,$3.8 \ eV$ of energy is released. This value is equal to the:

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