Match Column-I with Column-II.

Which of the following ionic species is isoelectronic with \(\mathrm{Be^{2+}}\)?

Amongst the elements with the following electronic configurations, which one of them may have the highest ionisation energy?

1. $\left[Ne\right]$ $3s^2$ $3p^2$

2. $\left[Ne\right]$ $3s^2$ $3p^3$

3. $\left[Ar\right]$ $3d^{10}$ $4s^2$ $4p^3$

4. $\left[Ne\right]$ $3s^2$ $3p^1$

Among the following, the most characteristic oxidation states for lead and tin are, respectively:

1. +4, +2

2. +2, +4

3. +4, +4

4. +2, +2

If an atom has electronic configuration 1s²2s²2p⁶3s²3p⁶3d³4s², we will place it in group number: