In group IV A or 14 of the extended form of the periodic...

In group IV A or 14 of the extended form of the periodic table, with the increase in atomic number, the oxidizing power of tetravalent species increases in the order (a) $\mathrm{Ge}>\mathrm{Sn}>\mathrm{Pb}$ (b) $\mathrm{Pb}>\mathrm{Sn}>\mathrm{Ge}$ (c) $\mathrm{Pb}>\mathrm{Ge}>\mathrm{Sn}$ (d) $\mathrm{Ge}>\mathrm{Pb}>\mathrm{Sn}$

In group IV A or 14 of the extended form of the periodic table, with the increase in atomic number, the oxidizing power of tetravalent species increases in the order
(a) $\mathrm{Ge}>\mathrm{Sn}>\mathrm{Pb}$
(b) $\mathrm{Pb}>\mathrm{Sn}>\mathrm{Ge}$
(c) $\mathrm{Pb}>\mathrm{Ge}>\mathrm{Sn}$
(d) $\mathrm{Ge}>\mathrm{Pb}>\mathrm{Sn}$

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Key Concepts

Oxidizing Power in Redox Chemistry

Oxidizing power is a measure of a species’ ability to accept electrons and oxidize other substances. It is influenced by the stability of the oxidation state and the element's electron configuration. In the context of tetravalent species, changes in oxidizing power along the group can be attributed to these electronic and structural factors.

Inert Pair Effect

The inert pair effect is the phenomenon where the s-electrons in the valence shell of heavier elements are less inclined to participate in bonding, leading to a tendency for lower oxidation states. This effect becomes more pronounced as one moves down Group 14, thereby affecting the oxidizing behavior of tetravalent species and often resulting in heavier elements exhibiting a greater oxidizing power.

Periodic Trends in Group Elements

This concept pertains to the systematic changes in the properties of elements as one moves down a group in the periodic table. In Group IV A (or 14), factors such as atomic and ionic size, electronegativity, and effective nuclear charge evolve with increasing atomic number, which in turn impacts chemical behavior including reactivity and oxidation states.

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