Question

Nearly every compound of silicon has the element in the ⁺4 oxidation state. In contrast, most compounds of lead have the element in the ⁺2 state.(b) Explain in terms of atomic and molecular properties.

Answer 1

This is due to the phenomenon known as the Inert pair effect.

Orbitals shield better with a lower azimuthal quantum number(l). Hence, s orbitals shield better than p which shields better than d which is better than f, etc.

The electronic configuration of Si is [Ne] 3s²3p². The 2s and 2p orbitals are shielding the electrons from the nucleus. So the s and p electrons are ready to be ionized. And hence shows a +4 oxidation state.

Similarly, as we move down the group, atomic size increases, and metallic character also increases. Also, lead is below Si and a lower oxidation state is more stable down the group. Hence lead shows a +2 oxidation state.

To learn more about the oxidation state, visit: brainly.com/question/11313964

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