When a chloride ion is formed from an isolate | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

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:

Similar Questions

Identify the set of elements in which they are arranged in the increasing order of electron gain enthalpies.

The $CORRECT$ order of $\Delta H_{eg}$ of the following elements is

The electron affinity of the following elements can be arranged as:

Which one of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) of the given atomic species?

For the process
$A_{(g)} + e^- \to A^{-}_{(g)};$ $\Delta H = x$
and $A^{-}_{(g)} \to A_{(g)} + e^-;$ $\Delta H = y$
Select the correct statement:

Vedclass Test Series

Exam Paper Generator

Online Exam Module