How come Sulfur, the fluorides SF2, SF4, and SF6 are known to exist, whereas for oxyen only OF2 is known to exist?
2006-11-14 11:25:12 · 2 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
My guess would be that S is on the third period of the classification table, so it has one more layer of electrons. Maybe they have more ways of rearrangind themselves than oxygen. Even though S and O both have a valence of 6, S has more inner layers and more orbitals to play with.
2006-11-14 11:28:57 · answer #1 · answered by kihela 3 · 0⤊ 0⤋
Elements of the second period (i.e., oxygen) have only 2s and 2p valence orbitals available for bonding.
Elements in the third period and below (i.e., sulfur) are able to 'expand the octet.' One of the possible explanations of this is the presence of valence d orbitals. That is, the empty 3rd orbitals of sulfur can be used to accomodate some extra electrons for those covalent bonds.
2006-11-14 19:32:45 · answer #2 · answered by nazzyonenine 3 · 0⤊ 0⤋