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

1 Answer
Mar 9, 2017

Answer:

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.

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