inert pair effect

Question

Inert pair effect increases down Group 14 leading to stabilization of which oxidation state?

RankGuru · Accepted Answer

1. **General Configuration**: Group 14 has the outer configuration $ns^2 np^2$.
2. **The Effect**: As we go down the group ($C 	o Si 	o Ge 	o Sn 	o Pb$), the $ns^2$ electrons become increasingly stable ('inert') and reluctant to take part in bonding.
3. **Reluctance Source**: This is due to poor shielding by $d$ and $f$ electrons, causing the $s$-electrons to be held more tightly by the nucleus.
4. **Result**: For heavy elements like Lead ($Pb$), the **$+2$** state (using only $p$ electrons) is much more stable than the $+4$ state.
5. **Consequence**: $Pb(IV)$ compounds act as strong oxidizing agents to return to the stable $Pb(II)$ state.

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