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

Mar 9, 2017

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 $+ I I$ 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 $N e$, i.e. the next Noble Gas; i.e. Group 15 elements, chalcogens and halogens, $\text{Group 15}$, $\text{Group 16}$, and $\text{Group 17}$ elements, generally assume oxidation numbers of $- I I I$, $- I I$, and $- I$ respectively.

Claro?