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?

For elements $\mathrm{B}, \mathrm{C}, \mathrm{N} \mathrm{Li}, \mathrm{Be}, \mathrm{O} \mathrm{and} \mathrm{F}$, the correct order of first ionisation enthalpy is

The correct order of metallic character is

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R.

Assertion A : The energy required to form ${\mathrm{Mg}}^{2+}$from $\mathrm{Mg}$ is much higher than that required to produce ${\mathrm{Mg}}^{+}$

Reason R:${\mathrm{Mg}}^{2+}$ is small ion and carry more charge than ${\mathrm{Mg}}^{+}$

In the light of the above statements, choose the correct answer from the options given below.

Correct order of first Ionisation energy for $\mathrm{Li},\mathrm{Be},\mathrm{C},\mathrm{B},\mathrm{N},\mathrm{O},\mathrm{F}$.

Triad-$\mathrm{I}$ $\left[{\mathrm{N}}^{3-},{\mathrm{O}}^{-,}{\mathrm{Na}}^{+}\right]$

Triad-$\mathrm{II}$$\left[{\mathrm{N}}^{+}, {\mathrm{C}}^{+}, {\mathrm{O}}^{+}\right]$

Choose the species with lowest IP form triad-I and highest IP form Triad-II.

Which of the following has higher ionisation enthalpy?
$\mathrm{Zn} \mathrm{or} {\mathrm{Zn}}^{+}$

For the process

$$\begin{gathered} {\mathrm{X}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-}\stackrel{}{\to }{\mathrm{X}}_{\left(\mathrm{g}\right)}^{-} ∆\mathrm{H}=-\mathrm{x} \\ {\mathrm{X}}_{\left(\mathrm{g}\right)}^{-}\stackrel{}{\to }{\mathrm{X}}_{\left(\mathrm{g}\right)}+{\mathrm{e}}^{-} ∆\mathrm{H}=\mathrm{y} \end{gathered}$$

First, second and third IP values are $100\mathrm{eV},150\mathrm{eV}$ $1500\mathrm{eV}$. Element can be -

For an element '$A$'.

$\mathrm{A}\stackrel{{\mathrm{IE}}_1}{\to }{\mathrm{A}}^{+}\stackrel{{\mathrm{IE}}_2}{\to }{\mathrm{A}}^{2+}\stackrel{{\mathrm{IE}}_3}{\to }{\mathrm{A}}^{3+}\stackrel{ }{\to }\dots \dots \dots \dots$

The ${\mathrm{IE}}_1$, and ${\mathrm{IE}}_3$ values are $27 \mathrm{kJ}/\mathrm{mol}$  and $51 \mathrm{kJ}/\mathrm{mol}$ respectively. Then the value of ${\mathrm{IE}}_2$ is _____ .

The incorrect statement among the following is

Incorrect order of ionisation potential

The incorrect statement is:

The correct order of ionization energy is

Arrange $\mathrm{B}\mathrm{e},\mathrm{}\mathrm{M}\mathrm{g},\mathrm{}\mathrm{C}\mathrm{a},\mathrm{}\mathrm{S}\mathrm{r}$ in the ascending order of ionisation 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 :