Ionization Enthalpy and its Applications

Select whether the following statement is True or False:

Boron has more ionisation energy than beryllium.

Explain why beryllium has more ionisation than boron.

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 maximum ionisation enthalpy in a period is shown by 

Name the element which has the highest ionisation enthalpy value. (Neon/ Helium)

Name the following:

The minimum amount of energy required to remove valence shell electron from a neutral isolated gaseous atom of an element.

The energy required to remove an electron from the outermost shell of an isolated gaseous atom is known as $I{E}_1$ of that atom.

Similarly, the energy required for the removal of the electron from the unipositive ion, diapositive ion and tripositive ion are known as  $I{E}_2,I{E}_3$ and $I{E}_4,$ respectively, and are called successive ionisation energies. The magnitude of the charge depends on the size of the orbital of electron. Electrons in smaller orbitals are on average close with each other and have more repulsion. Thus for $Be\left(2s^2\right),$ the $I{E}_1$ and $I{E}_2$ are $9.3$ and $18.2 eV$ $ato{m}^{-1},$ whereas for $Ca\left(4s^2\right),$ the values are $6.1 and 11.9 eV.$

Among the following ionisation reactions, which one will have the maximum value of ionisation energy?

Four elements have the following first ionization energies in ${\mathrm{kJmol}}^{-1}:762,709,579 \mathrm{and} 558.$ The elements are $\mathrm{Ga},\mathrm{Ge},\mathrm{In} \mathrm{and} \mathrm{Sn}$ (not in order). Which of these elements has the ionization energy of $762 \mathrm{kJ} {\mathrm{mol}}^{-1}?$  

The energy required to remove an electron from the outermost shell of an isolated gaseous atom is known as $I{E}_1$ of that atom.

Similarly, the energy required for the removal of the electron from the unipositive ion, diapositive ion and tripositive ion are known as  $I{E}_2,I{E}_3$ and $I{E}_4,$ respectively, and are called successive ionisation energies. The magnitude of the charge depends on the size of the orbital of electron. Electrons in smaller orbitals are on average close with each other and have more repulsion. Thus for $Be\left(2s^2\right),$ the $I{E}_1$ and $I{E}_2$ are $9.3$ and $18.2 eV$ $ato{m}^{-1},$ whereas for $Ca\left(4s^2\right),$ the values are $6.1 and 11.9 eV.$

The correct order of arrangement of the first ionisation energy of $\mathrm{C}, \mathrm{N}, \mathrm{O}$ and $\mathrm{F}$ (in decreasing values ) is: