Ion S2+
| Symbol | S2+ |
| Number | 16 |
| Atomic weight | 32.0590000 |
| Latin name | Sulfur, Sulphur |
| English name | Sulfur |
Electronic configuration of of Sulfur
S: 1s2 2s2 2p6 3s2 3p4 → S2+:1s22s22p63s23p2
Same electronic configuration has an ion of Sulfur +2 and Si, P+1, Cl+3
The order of filling the shells with electrons of Sulfur (S2+): 1s → 2s → 2p → 3s → 3p → 4s → 3d → 4p → 5s → 4d → 5p → 6s → 4f → 5d → 6p → 7s → 5f → 6d → 7p.
On the sub level ‘s’ there might be 2 electrons at most, on ‘p’ - up to 6, on ‘d’ - up to 10 and up to 14 on ‘f’
Sulfur has 16 electrons, let's fill electronic layers in described order:
2 electrons on 1s-sub level
2 electrons on 2s-sub level
6 electrons on 2p-sub level
2 electrons on 3s-sub level
2 electrons on 3p-sub level
Oxidation state of Sulfur
Atoms of Sulfur in compounds have an oxidation state of 6, 5, 4, 3, 2, 1, 0, -1, -2.
The oxidation state is the conditional charge of an atom in a compound: the bond in a molecule between atoms is based on the sharing of electrons, thus, if the atom’s charge virtually increases, then the oxidation state is negative (electrons carry a negative charge), if the charge decreases, then the oxidation state is positive.
Oxidation state of an ion S2+ = 2
Ions of Sulfur
Valence of S2+
Atoms of Sulfur in compounds have valence VI, V, IV, III, II, I.
Valence of Sulfur is an ability of an atom S to build chemical bounds. The valence is based on electronic configuration of atom: electrons participated in chemical bounds are known as valence electrons. In general the valence is:
The number of possible chemical bounds with other atoms
The valence has no sign.
Quantum numbers S 2+
Quantum numbers are defined by the last electron in configuration, for an ion S these numbers are N = 3, L = 1, Ml = 0, Ms = +½
Filling an electronic configuration (gif):
Result:
See all elements of the periodic table
Where is S in the periodic table?
