Stability of Highest Oxidation State

[ritwik06]

Homework Statement

Why does the stability of highest oxiation state decreases from group 13 to group 17?

Ans: My book says, that with the increase in atomic number, difference in energies between ns and np orbitals increases. Is it right? If so then can u please explain what relation exists between the statements.

 

[GCT]

It's better to consider this in terms of electron affinity. The energies between ns and np orbitals increases because of the increase in effective nuclear charge i.e. " it wants the electrons more " .

 

[Blueshift5]

The stability of the highest oxidation state decreases from group 13 to group 17 due to the increase in atomic number and the difference in energies between the ns and np orbitals. This is because as we move down the periodic table, the atomic radius increases and the effective nuclear charge decreases. This results in a decrease in ionization energy and an increase in the energy difference between the ns and np orbitals.

As a result, it becomes easier for the elements in group 13 to lose their outermost ns electron and achieve a stable +3 oxidation state. However, as we move towards group 17, the elements have a higher effective nuclear charge and smaller atomic radii, making it more difficult for them to lose their outermost np electrons and achieve a stable +7 oxidation state.

In addition, the stability of the highest oxidation state is also affected by the tendency of elements to gain or lose electrons. Group 13 elements have a greater tendency to lose electrons, while group 17 elements have a greater tendency to gain electrons. This also contributes to the decrease in stability of the highest oxidation state from group 13 to group 17.

Overall, the stability of the highest oxidation state is influenced by a combination of factors such as atomic radius, effective nuclear charge, ionization energy, and electron affinity.