Question #8b79c

Sulphur has a grown state electron configuration of `1s^22s^2 2p^6 3s^2 3p^4`

This is the same outer valance of Oxygen. This gives Sulphur two unpaired electrons in its outer shell. When joined to Oxygen or another element with a higher electron negativity than sulphur it can lose those two electrons resulting in a +2 charge.

When Sulphur is joined to an element with a lower electron negativity it can used the same two unpaired p electrons to bond resulting in a -2 charge. This would be sulphur's preferred state.

Since sulphur is in the third row it can hybridize its six valance electrons into the 3d orbitals resulting in an electron configuration
of `3s^1 3p^3 3d^2` This higher energy electron configuration will allow Sulphur to use all six of its valance electrons to form bonds. This results in a +6 charge or a +4 charge if only four bonds are formed.

S=O Sulphur monoxide shows sulphur with a + 2 charge losing two electrons to Oxygen.

O=S=O Sulphur dioxide shows sulphur with a +4 charge losing four electrons to Oxygen
O=
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O= S =O (Sulfate ion -2) shows sulphur with a +6 charge losing all
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O- six electrons to Oxygen.