Find the successive elements of the periodic table with ionisation energies, 2372, 520 and 890 kJ per mol respectively

The correct option is He, Li, Be.

To understand why this option is correct, let us analyze the periodic trends in ionization energy and look at the given ionization energy values:
First ionization energy: 2372 kJ/mol
Second ionization energy (for the next successive element): 520 kJ/mol
Third ionization energy (for the third successive element): 890 kJ/mol

First, we recall the definition of first ionization energy (${\mathrm{IE}}_1$), which is the energy required to remove the most loosely bound electron from an isolated gaseous atom.

Let us look at the general trends in the periodic table:
1. Ionization energy generally increases across a period (from left to right) due to increasing effective nuclear charge.
2. Ionization energy decreases down a group because the outermost electrons are farther from the nucleus and are more shielded by inner shell electrons.
3. Noble gases have exceptionally high ionization energies because of their stable, fully-filled valence shell configurations (ns²np⁶, or 1s² for Helium).

Now, let us evaluate the given values:
The first value of 2372 kJ/mol is extremely high. Such a high value is characteristic of a noble gas, specifically Helium (He), which has a stable 1s² configuration and is the smallest atom with no shielding electrons.
The second value drops dramatically to 520 kJ/mol. This sharp decrease indicates that the electron is removed from a new shell that is much farther from the nucleus and experiences shielding. This is characteristic of an alkali metal, Lithium (Li), which has the electron configuration [He] 2s¹.
The third value increases to 890 kJ/mol. This moderate increase is consistent with moving from left to right in the same period (from Lithium to Beryllium). Beryllium (Be) has the electron configuration [He] 2s². The ionization energy increases because Beryllium has a higher nuclear charge than Lithium, holding its 2s electrons more tightly.

Comparing the values for successive elements of the option He, Li, Be:
- Helium (He, atomic number 2): ${\mathrm{IE}}_1$ = 2372 kJ/mol
- Lithium (Li, atomic number 3): ${\mathrm{IE}}_1$ = 520 kJ/mol
- Beryllium (Be, atomic number 4): ${\mathrm{IE}}_1$ = 899 kJ/mol (which closely matches the given 890 kJ/mol)

Therefore, the successive elements corresponding to the ionization energies 2372, 520, and 890 kJ/mol are Helium, Lithium, and Beryllium.