Ionization Enthalpy and its Applications

The atomic number of Vanadium $\left(\mathrm{V}\right)$, Chromium $\left(\mathrm{Cr}\right)$, Manganese $\left(\mathrm{Mn}\right)$ and Iron $\left(\mathrm{Fe}\right)$ are, respectively, $23, 24, 25 \mathrm{and} 26$. Which one of these may be expected to have the highest second ionization enthalpy?

The correct order of $1^{\mathrm{st}}$ ionisation enthalpy among the following elements $\mathrm{Be}, \mathrm{B}, \mathrm{C}, \mathrm{N}, \mathrm{O}$ is

Which element has the highest first ionization potential?

The first ionization potential $\left(\mathrm{IP}\right)$ of the elements $\mathrm{Na},\mathrm{Mg},\mathrm{Si},\mathrm{P},\mathrm{Cl}$ and $\mathrm{Ar}$ are $5.14,7.65,8.15 10.49,12.97$ and $15.76 \mathrm{eV},$ respectively. The $\mathrm{IP}$ (in $\mathrm{eV}$) of $\mathrm{K}$ is closest to :

For an element $\left(\mathrm{M}\right),{\mathrm{IE}}_1$ and ${\mathrm{IE}}_2$ are $178$ and $348 \mathrm{kcal} {\mathrm{mol}}^{-1}$, respectively. What is the energy $\left(\mathrm{kcal} {\mathrm{mol}}^{-1}\right)$ required for the following reaction?

${\mathrm{M}}_{\left(\mathrm{g}\right)}\to {\mathrm{M}}_{\left(\mathrm{g}\right)}^{2+}+2{\mathrm{e}}^{-}$

The correct order for the first ionization enthalpy of $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}, \mathrm{Si}$ follows the order:

Which of the following do not show regular trend for ${\mathrm{IE}}_1$?

Which of the following relation is correct with respect to first (I) and second (II) ionisation potentials of sodium and magnesium ?

Which of the following relations are correct for $\mathrm{F} \& \mathrm{Cl}?$

The five successive I.P of element $\mathrm{x}$ are $7.1,14,29.3,113.7 \& 142.9\mathrm{eV}$ respectively then the formula of its chloride will be :-

The second ionization energy  $(\mathrm{in} \mathrm{kJ}/\mathrm{mol})$ of an element $\mathrm{X}$ is the energy required to

Which electronic configuration of an element has abnormally high difference between second and third ionization enthalpy?

The correct order of $1^{\mathrm{st}}$ ionisation enthalpy among the following elements $\mathrm{Be}, \mathrm{B}, \mathrm{C}, \mathrm{N}, \mathrm{O}$ is

Which of the following isoelectronic ions has the lowest first ionization enthalpy ?

Given elements are matched with their successive ionisation energies. What are these elements ?

What is the reason for ionisation enthalpy of nitrogen is more than oxygen ?

Among the following pairs, choose the pair in which $I{E}_2$ is more for $1^{st}$ element than $I{E}_2$ of $2^{nd}$ element.

Among the following statements, which statements are correct?

(i) Electron gain enthalpy values of elements may be exothermic (negative) or endothermic (positive).

(ii) Generally the radius trend and the ionization energy trend across a period are exact opposites.

(iii) The first ionization energy of sulphur is higher than that of phosphorus?

(iv) $\mathrm{T}{\mathrm{e}}^{2–}>{\mathrm{l}}^{–}>\mathrm{C}{\mathrm{s}}^{+}>\mathrm{B}{\mathrm{a}}^{2+}$ represents the correct decreasing order of ionic radii.