Electron Gain Enthalpy and its Applications

Are electron affinity and electron gain enthalpy same?

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):

Correct statement is ?

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?

In which process maximum energy is released?

If $\mathrm{E}{\mathrm{A}}_1$ and $\mathrm{E}{\mathrm{A}}_2$ for oxygen atom is $-142\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ and $+844\mathrm{k}\mathrm{J}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ . The energy released from $2\mathrm{O}+2{\mathrm{e}}^{-}\to 2{\mathrm{O}}^{-}$ will be

Which one of the following arrangements represents the correct order of least negative to most negative electron gain enthalpy for C, Ca, Al, F and O?

In which of the following processes energy is absorbed?

Within each pair of element F & Cl, S & Se, and Li & Na, respectively, the elements that release more energy upon electron gain are

Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements O, S, F and Cl?

Electronic configurations of four elements E, F, G and H are given below:

$\left(\mathrm{E}\right)\mathrm{ }\mathrm{ }1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{\mathrm{6 \; \; \; }}$ $\left(\mathrm{F}\right)\mathrm{ }1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^4$

$\left(\mathrm{G}\right)\mathrm{ }1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^1$ $\left(\mathrm{H}\right)\mathrm{ }1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^5$

Which of the following is the correct order of increasing tendency to gain electron?

Which of the following has the highest electron affinity?