Electron Gain Enthalpy and its Applications

The electron affinity of bromine is $3.36 \mathrm{eV}$. How much energy in $\mathrm{kcal}$ is released when $8 \mathrm{g}$ of bromine is completely converted to ${\mathrm{Br}}^{-}$ ions in the gaseous state? ($1 \mathrm{eV}=23.06 \mathrm{kcal} {\mathrm{mol}}^{-1}$). (Give the value rounded-off to the nearest integer)

Name the element with maximum electron affinity.

The second-period element, for example, $\mathrm{F}$ has less electron gain enthalpy than the third-period element of the same group for example $\mathrm{Cl}$. Why?

The calculated electron gain enthalpy values for alkaline earth metals and noble gases are positive. How can you explain this?

How do Electron affinity change in a group and period?

Which of the following has the lowest electron affinity?

Consider the process:
$\mathrm{A}\left(\mathrm{g}\right)\stackrel{-{\mathrm{e}}^{-}}{⟶}{\mathrm{A}}^{+}\left(\mathrm{g}\right)$
If $△{\mathrm{H}}_{\mathrm{IE}}$ for the process is $21.4\mathrm{eV}/$ atom. What will be the value of $△{\mathrm{H}}_{\mathrm{eg}}$ electron gain enthalpy for ${\mathrm{A}}^{+}\left(\mathrm{g}\right)$ (in eV/atom)?

Which of the following set of elements will have no affinity for electron?

Which of them is an exothermic process

The formation of the oxide ion, ${\mathrm{O}}^{2-}\left(\mathrm{g}\right)$, from oxygen atom requires first an exothermic and then an endothermic step as shown below:

$\mathrm{O}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}⟶{\mathrm{O}}^{-}\left(\mathrm{g}\right); {\mathrm{\Delta H}}^{\circ }=-141 \mathrm{kJ} {\mathrm{mol}}^{-1}$

${\mathrm{O}}^{-}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}⟶{\mathrm{O}}^{2-}\left(\mathrm{g}\right); {\mathrm{\Delta H}}^{\circ }=+780 \mathrm{kJ} {\mathrm{mol}}^{-1}$

Thus process of formation of ${\mathrm{O}}^{2-}$ in gas phase is unfavourable even though ${\mathrm{O}}^{2-}$ is isoelectronic with Neon. It is due to the fact that,

Which of them has highest value of negative electron gain enthalpy ?

Which of the following processes will release minimum energy?

Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is :

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):

In periodic table, the basic character of oxides:

Which of the following option will release maximum energy on adding one electron?
(in there respective family) 
 

The electron affinity of the members of oxygen family of the periodic table, follows the sequence

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

Which of the following is not correct order?

Correct statement is ?