How do I know the likely oxidation states of metals, and non-metals?

Md Ariful Islam

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Md Ariful Islam

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........And non-metals typically form an ion isoelectronic with the next Noble Gas.

A Group 17 element typically forms an ion with a single negative charge:

$1/2X_2 + e^(-) rarr X^-$ $X=F, Cl, Br.......$

And a Group 16 element typically forms an ion with a double negative charge:

$1/2O_2(g) + 2e^(-) rarr O^(2-)$

In each case the element has formed an ion isoelectronic with the next (or last) Noble Gas. And we can go even farther than this, and consider Group 15.

$P(s) + 3e^(-) rarr P^(3-)$

And we can look at oxidation of the alkali metals (Group I):

$M(s) rarr M^(+) + e^-$ $M=Li, Na, K, etc.$

And of the alkaline earths (Group 2):

$M(s) rarr M^(2+) + 2e^-$ $M=Ca, Ba, Sr, etc.$

The point is that the Group number reflects electronic structure, i.e. the number of electrons present in the valence shell. Group I and Group II metals have 1 and 2 respectively. As increases across a Period, nuclear charge increases accordingly, and non-metals, to the RIGHT of the Period as we face it, tend to be oxidizing, and ADD electrons to their valence shell.

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