Sulfur (S) is in group 16 (also known as the chalcogens) of the periodic table. In its neutral state, sulfur has six valence electrons. Its electronic configuration is 1s22s22p63s23p4.
Fluorine (F) is in group 17 (also known as the halogens) of the periodic table. In its neutral state, fluorine has seven valence electrons. Its electronic configuration is 1s22s22p5.
In sulfur hexafluoride, there is one sulfur atom surrounded by six fluorine atoms. Each fluorine atom contributes one valence electron to form a covalent bond with the sulfur atom. This means that sulfur forms six single bonds with the six fluorine atoms.
However, since sulfur is in group 16, it needs eight valence electrons to satisfy the octet rule and achieve a stable electron configuration. Therefore, the sulfur atom in SF6 shares its six valence electrons with the six fluorine atoms and also gains two additional electrons from the fluorine atoms to complete its octet.
Counting all the valence electrons involved in the bonding, we have:
6 valence electrons from sulfur atom (S)
6 x 7 valence electrons from six fluorine atoms (6F)
+2 additional electrons gained by sulfur from fluorine atoms
Total valence electrons = 6 + 42 + 2 = 50 valence electrons
Therefore, sulfur hexafluoride (SF6) has a total of 50 valence electrons.
