# Why do metals typically form positively-charged ions?

Aug 1, 2017

Why? Well metals are in general $\text{reducing agents.....}$

#### Explanation:

Why? Well metals are in general $\text{reducing agents.....}$ That is metals are electron-rich species, and undergo the following oxidation reaction....

$M \rightarrow {M}^{2 +} + 2 {e}^{-}$

On the other hand, non-metals, have high nuclear charge, and tend to accept electron-density, i.e. they are $\text{oxidizing agents....}$ The strongest oxidizing agents come from the right hand side of the Periodic Table, where the nuclear charge is HIGH, and the tendency to be reduced is marked.

$\frac{1}{2} {O}_{2} + 2 {H}^{+} + 2 {e}^{-} \rightarrow {H}_{2} O \left(l\right)$ ;E^@=1.229*V

$\frac{1}{2} {F}_{2} + {e}^{-} \rightarrow {F}^{-}$ ;E^@=2.87*V

Given the positions of oxygen and fluorine on the Periodic Table (to the right as we face it!), it is thus no coincidence that these elements are potent oxidizing agents.