Question

Why is it not possible to form $N{a}^{+2}$ ion? Explain with respect to periodic properties.

Answer 1

1.Ionisation potential: The minimum amount of energy required to remove an electron from the outermost shell of a neutral isolated gaseous atom is called Ionisation energy or Ionisation potential.

Ex: $Na-e^{-}\to N{a}^{+}$($I.E_1$)

2.Na has electronic configuration- $1s^{2}2s^{2}2p^{6}3s^1$- it has 1 electron extra than the Ne(inert gas) configuration. By losing electron from $3s$ sub shell it attains Neon configuration - $1s^{2}2s^{2}2p^6$.

3. Na cannot turn to $N{a}^{+2}$ by losing the next electron from $2p$ sub shell because the species attains an unstable electronic configuration.To remove an electron from $N{a}^{+}$, a huge amount of energy is required as it moves from a stable state to unstable state.

$I.E_1$ < < < $I.E_2$

Hence, $N{a}^{+2}$ formation is not possible.