Electron Gain Enthalpy and its Applications

Which of the following represents the exothermic process?

The correct order of electron affinity of $16\mathrm{th}$ group elements is

Name the element with maximum electron affinity.

The electronic configuration of four elements I, II, III and IV are given:

I $: 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^5$

II $: 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^4$

III $: 1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^5$

IV $:$ $1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}^6 3{\mathrm{s}}^2 3{\mathrm{p}}^3$

Which element has highest value of $1^{\text{st }}$ Electron gain enthalpy (magnitude):

The formation of the oxide ion ${\mathrm{O}}^{2-}$(g) requires first an exothermic and then an endothermic step as shown below: $\mathrm{O}\left(\mathrm{g}\right)+{\mathrm{e}}^{-1}\to {\mathrm{O}}^{-}\left(\mathrm{g}\right);∆{\mathrm{H}}^0=-142 \mathrm{k}\mathrm{J} \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$
${\mathrm{O}}^{-}\left(\mathrm{g}\right)+{\mathrm{e}}^{-1}\to {\mathrm{O}}^{2-}\left(\mathrm{g}\right);∆{\mathrm{H}}^0=+844 \mathrm{k}\mathrm{J} \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$
This is because

Energy will be released in which of the following?

Among the following, Which will have lowest electron affinity ?

When 2 gm of chlorine is completely converted to Cl^- ion in a gaseous state, the amount of energy released in K Cal is:
Note: Chlorine has electron affinity 3.7 eV. $(1\mathrm{e}.\mathrm{V}=23.06\mathrm{K}. \mathrm{Cal}{\mathrm{mol}}^{-1})$

Arrange these elements in the increasing order of the magnitude (without sign) of their electron affinity or electron gain enthalpy based on their electronic configurations given below-

1. $2{\mathrm{s}}^{2}2{\mathrm{p}}^5$

2. $3{\mathrm{s}}^{2}3{\mathrm{p}}^5$

3. $2{\mathrm{s}}^{2}2{\mathrm{p}}^4$

4. $3{\mathrm{s}}^{2}3{\mathrm{p}}^4$

Find the correct order of electron gain enthalpy ($∆{}_{\mathrm{eg}}\mathrm{H}$) of the given elements.

Among the following, which is correctly represented the order of electron gain enthalpy?

$\mathrm{EA}$ values of $\mathrm{N}$ and $\mathrm{P}$ are exceptionally low, because:

In which of the following transformation the least energy is required?

The electron gain enthalpy (in $\mathrm{k}\mathrm{J}/\mathrm{m}\mathrm{o}\mathrm{l}$ ) of fluorine, chlorine, bromine and iodine, respectively, are

The formation of oxide ion $O^{2-}\left(g\right)$ require first an exothermic and then an endothermic step as shown below:

$O\left(g\right)+e^{-}\to O^{-}\left(g\right);∆H^o=-142 \mathrm{k}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

$O^{-}\left(g\right)+e^{-}\to O^{2-}\left(g\right);∆H^o=844 \mathrm{k}\mathrm{J}\mathrm{ }\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$

This is because

Fluorine has low electron affinity than chlorine because of

The atomic number of elements $\mathrm{A}, \mathrm{B}, \mathrm{C}$ and $\mathrm{D}$ are $\mathrm{Z}-1, \mathrm{Z}, \mathrm{Z}+1, \mathrm{Z}+2$ respectively. If $\mathrm{B}$ is a noble gas, choose the correct option
$\mathrm{i}) \mathrm{A}$ has higher electron affinity
$\mathrm{ii}) \mathrm{C}$ exists in $+2$ oxidation state
$\mathrm{iii}) \mathrm{D}$ is an alkaline earth metal

The correct order of electron affinity of the elements O, S and Se follows the order:

The equation used to represent the electron gain enthalpy is

Which of the following represents the correct order of increasing electron gain enthalpy with a negative sign for the elements $\mathrm{O}, \mathrm{S}, \mathrm{F} \mathrm{and} \mathrm{Cl}$?