The stability of +1 oxidation state increases in the sequence: (a) Tl<In<Ga<Al □(b) In<Tl<Ga<Al

step 1 The stability of the stability of plus one oxidation state, oxidation state increases in the seq

The stability of +1 oxidation state increases in the...

The stability of $+1$ oxidation state increases in the sequence: (a) $\mathrm{Tl}<\mathrm{In}<\mathrm{Ga}<\mathrm{Al}$ $\square$ (b) $\mathrm{In}<\mathrm{Tl}<\mathrm{Ga}<\mathrm{Al} \quad \square$ (c) $\mathrm{Ga}<\mathrm{In}<\mathrm{Al}<\mathrm{Tl}$ $\begin{array}{lll}\square & \text { (d) } \mathrm{Al}<\mathrm{Ga}<\text { In }<\mathrm{Tl} & \square\end{array}$

The stability of $+1$ oxidation state increases in the sequence:
(a) $\mathrm{Tl}<\mathrm{In}<\mathrm{Ga}<\mathrm{Al}$
$\square$ (b) $\mathrm{In}<\mathrm{Tl}<\mathrm{Ga}<\mathrm{Al} \quad \square$
(c) $\mathrm{Ga}<\mathrm{In}<\mathrm{Al}<\mathrm{Tl}$
$\begin{array}{lll}\square & \text { (d) } \mathrm{Al}<\mathrm{Ga}<\text { In }<\mathrm{Tl} & \square\end{array}$

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Key Concepts

Periodic Trends in Oxidation State Stability

Periodic trends explain changes in oxidation state stability across a group in the periodic table. In the context of Group 13 elements, as atomic number increases, the inert pair effect becomes more pronounced, thus stabilizing the lower oxidation state over the higher one. This trend is a fundamental concept in understanding the chemical behavior and reactivity of elements across a period or down a group.

Oxidation States in p-Block Elements

The oxidation states of p-block elements are determined by the energy dynamics of electron removal and the participation of valence electrons in bonding. For elements in Group 13, while lighter members typically form compounds in a higher oxidation state, the heavier members show a preference for a lower oxidation state as a direct consequence of the inert pair effect.

Inert Pair Effect

The inert pair effect describes the phenomenon where the outermost s electrons in heavier p-block elements are less inclined to participate in chemical bonding due to their lower reactivity, leading to the stabilization of lower oxidation states. This effect explains why heavier elements often exhibit oxidation states that are lower than what would be expected based on their group number.

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