The successive $5$ ionisation energies of an element are $800, 2427, 3658, 25024$ and $32824 \ kJ/mol$,respectively. By using the above values,predict the group in which the above element is present:

What is the correct order of the first ionization energy for $Li, Be, B,$ and $Na$?

Assertion $(A)$: Boron has a smaller first ionisation enthalpy than beryllium.
Reason $(R)$: The penetration of a $2s$-electron to the nucleus is more than the $2p$-electron; hence,the $2p$-electron is more shielded by the inner core of electrons than $2s$-electrons.

Which of the following elements has the highest first ionization enthalpy?

Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:

An atom with high electronegativity has