Electron Gain Enthalpy

The amount of energy released when $1\times {10}^{10}$ atoms of chlorine in vapour state are converted to ${\mathrm{Cl}}^{-}$ ions according to the equation,

$\mathrm{Cl}\left(\mathrm{g}\right) + {\mathrm{e}}^{-} \to {\mathrm{Cl}}^{-} \left(\mathrm{g}\right) \mathrm{is} 57.86 \mathrm{x} {10}^{-10} \mathrm{J}.$

Calculate the electron gain enthalpy of chlorine atom in terms of $\mathrm{eV}$ per atom.

Which of the following processes do not involve absorption of energy ?

In which of the following options the order of arrangement does not agree with the variation of property indicated against it ?

The highest electron affinity is shown by

Which of the following species has the highest electron affinity?

The element with positive electron gain enthalpy is

Which of the following atoms should have the highest first electron affinity?

The correct order of electron gain enthalpy with negative sign of $\mathrm{F}, \mathrm{Cl}, \mathrm{Br}$and $\mathrm{I}$, having atomic number $9,17,35$ and $53$ respectively, is

The order of decreasing negative electron gain enthalpy of $\mathrm{O}, \mathrm{S}, \mathrm{Se}$ is

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

The first ionisation potential of $\mathrm{Na}$ is $5.1 \mathrm{e} \mathrm{V}$. The value of electron gain enthalpy of ${\mathrm{Na}}^{+}$will be

How does the electron gain enthalpy vary across a period and down a group?

Electron affinity is positive, when

Which of the following processes involves absorption of energy?

Among the halogens, the element having the most negative electron gain enthalpy is _____.

Energy released when an electron is added to a neutral gaseous atom is called _____ enthalpy of the atom.

In the following pair, state which atom/ion has higher ionisation enthalpy and more negative electron gain enthalpy?

 $\mathrm{Br}, \mathrm{I}$

In the following pair, state which atom/ion has higher ionisation enthalpy and more negative electron gain enthalpy.

$\mathrm{Br}, {\mathrm{Br}}^{-}$.

The amount of energy released when one million atoms of iodine are completely converted into ${\mathrm{I}}^{-}$ ions in the vapour state according to the equation, $\mathrm{I}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}\stackrel{ }{\to }{\mathrm{I}}^{-}\left(\mathrm{g}\right)$ is $4.9\times {10}^{-13} \mathrm{J}$. Calculate the electron affinity of iodine in $\mathrm{e} \mathrm{V}$ per atom.

Define electron gain enthalpy. Describe the factors which determine the magnitude and sign of electron gain enthalpy. What are the general trends of variation of electron gain enthalpies in the periodic table?