Question

Two valence electrons occupy the outer energy level of the element strontium. If strontium forms an ion, what will be its likely charge?

Answer 1

+2

Explanation:

Strontium will lose the two outer valance electrons to form a stable noble gas electron structure. As electrons are negative losing two negative electrons will leave Strontium with a +2 charge.

Answer 2

Would it not be `Sr^(2+)`?

Explanation:

You gots a Group 2 metal, an alkaline earth, and these with TWO valence electrons, typically form `M^(2+)` ions upon oxidation...

`Sr rarr Sr^(2+) +2e^(-)`

We could write the entire electronic configuration of strontium metal as `Z=38`...

`underbrace(1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(10)4p^(6)5s^(2))_"electronic configuration of strontium metal"`

And upon oxidation....

`underbrace(1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)4s^(2)3d^(10)4p^(6))_"electronic configuration of strontium dication"`

The valence electrons are the `s` electrons...and these can be ionized...