Ionization Enthalpy and its Applications

The first four ionisation energy values of metal are $191, 587, 872$ and $5962 \mathrm{kcal}/\mathrm{mol}$ respectively. The number of valence electrons in the element is:

The correct order of increasing first ionization energy is

Values of $1^{\mathrm{st}}$ four ionisation energies $\left(\mathrm{kJ}/\mathrm{mol}\right)$ ) of an element are, respectively $496, 4563, 6913, 9541;$ the electronic configuration of that element can be.

Total number of elements which have more ionization energy as compare to their next higher atomic number elements. $\mathrm{Li}, \mathrm{Be}, \mathrm{C}, \mathrm{N}, \mathrm{O}, \mathrm{F}, \mathrm{Ne}$.

For which of the following species $2^{\mathrm{nd}} \mathrm{IE}<1^{\mathrm{st}} \mathrm{IE}$

The increasing order of the first ionization enthalpies of the elements $\mathrm{B}, \mathrm{P}, \mathrm{S}$ and $\mathrm{F}$ (lowest first) is:

Which of the following relation is correct with respect to first (I) and second (II) ionization enthalpies of potassium and calcium?

Which represents Alkali metals (i.e. $1^{\mathrm{st}}$ group metals) based on $(\mathrm{IE}{)}_1 \mathrm{and} (\mathrm{IE}{)}_2$ values in (in $\mathrm{kJ}/\mathrm{mol}$)?

The first ionisation enthalpies (in $\mathrm{eV}$) of $\mathrm{N} \& \mathrm{O}$ are respectively given by:

Which of the following statements is/are correct?

Values of ${\mathrm{IE}}_1, {\mathrm{IE}}_2, {\mathrm{IE}}_3$ of an element are $9.3, 18.2$ and $553.8\mathrm{eV}.$ Predict group number in Modern Periodic Table.

How many of the following atoms have maximum ionisation energy than boron?

(i) $\mathrm{Be}$ (ii) $\mathrm{N}$ (iii) $\mathrm{Al}$ (iv) $\mathrm{Ga}$ (v) $\mathrm{Si}$ (vi) $\mathrm{Mg}$

Which of the following is the correct order of ionisation enthalpy?

(1) ${\mathrm{Be}}^{+}>\mathrm{Be}$

(2) $\mathrm{Be}>{\mathrm{Be}}^{+}$

(3) $\mathrm{C}>\mathrm{Be}$

(4) $\mathrm{B}>\mathrm{Be}$

The first ionization enthalpy of carbon is greater than that of boron, whereas the reverse is true for second ionization enthalpy. Explain.

Why second ionization enthalpy is always higher than the first ionisation enthalpy for every element?

A large difference between the third and fourth ionization energies indicates the presence of:

Which of the following represents the correct order of increasing first ionisation enthalpy for $\mathrm{Ca}, \mathrm{Ba}, \mathrm{S}, \mathrm{Se} \mathrm{and} \mathrm{Ar}$?

The set representing the correct order of first ionization potential is

lonisation energies of $\mathrm{Ni}$ and $\mathrm{Pt}$ in $\mathrm{kJ} {\mathrm{mol}}^{-1}$ are given below

So, select the correct statement

First $\mathrm{IE}$ of $5\mathrm{d}$ series elements are higher than those of $3\mathrm{d}$ and $4\mathrm{d}$ series elements. This is due to: