Which of the following orders are correct? 1. stability of...

Which of the following orders are correct? 1. stability of $+3$ oxidation state decrease as $\mathrm{B}>\mathrm{Al}>$ $\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$ 2. stability of hydrides of group 13 element decreases as $\mathrm{B}>\mathrm{Al}>\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$ 3. reducing nature of group 13 elements decreases as $\mathrm{Al}>\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$ (a) $\mathrm{l}$ and 2 (b) 1 and 3 (c) 2 and 3 (d) 1,2 and 3

Which of the following orders are correct?
1. stability of $+3$ oxidation state decrease as $\mathrm{B}>\mathrm{Al}>$ $\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$
2. stability of hydrides of group 13 element decreases as $\mathrm{B}>\mathrm{Al}>\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$
3. reducing nature of group 13 elements decreases as $\mathrm{Al}>\mathrm{Ga}>\mathrm{In}>\mathrm{Tl}$
(a) $\mathrm{l}$ and 2
(b) 1 and 3
(c) 2 and 3
(d) 1,2 and 3

Key Concepts

Stability of Hydrides

This concept refers to the relative ease with which the hydrides (compounds in which hydrogen is bonded to another element) of main?group elements form and persist. The bonding and structural features, such as electron deficiency and cluster formation, as well as thermodynamic and kinetic factors, control the stability order of these hydrides. Trends in hydride stability are closely related to the electronic properties of the element and its tendency to form stable compounds with hydrogen.

Oxidation State Stability

This concept deals with how the tendency of an element to stabilize a particular oxidation state changes with atomic structure and periodic trends. In main?group elements, factors like effective nuclear charge, electron configuration, and the inert pair effect determine whether a high oxidation state (like +3) is favored. As one moves down a group, the inert pair effect becomes more pronounced, often lowering the stability of the higher oxidation state.

Reducing Nature of Elements

This concept addresses the propensity of an element to donate electrons, which is related to its reducing ability. It depends on factors like ionization energy, atomic size, and metallic character. In a group, as the capacity to lose electrons changes with these periodic properties, the reducing power can either increase or decrease. Recognizing such trends in reduction potentials is crucial for predicting reactivity in redox processes.

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