Question

What is the PROBABLE electronic configuration of a species that underwent reduction? What is the PROBABLE electronic configuration of a species that underwent oxidation?

Answer 1

Upon redox reaction, a particular atom TENDS to assume a Noble Gas configuration.

Explanation:

And of course, this is a gross simplification, and it does not really apply to the transition metals.

For Group 1 and Group 2, these metals tend to be oxidized, and lose 1 or 2 electrons, to assume the electronic configuration of the last Noble Gas. And thus alkali metals and alkaline earth metals tend to assume oxidation numbers of `+I` and `+II` respectively. And thus these metals achieve the electronic configuration of the Noble Gas that immediately precedes it.

Non-metals, electron poor species, tend to be REDUCED, and assume the the electronic configuration of the NEXT Noble Gas. And thus `N^(3-), O^(2-), F^-` are isoelectronic with `Ne`, i.e. the next Noble Gas; i.e. Group 15 elements, chalcogens and halogens, `"Group 15"`, `"Group 16"`, and `"Group 17"` elements, generally assume oxidation numbers of `-III`, `-II`, and `-I` respectively.

Claro?