CHEM 101 Lecture Notes - Lecture 16: Sulfur Hexafluoride, Lewis Structure, Formal Charge

• School: University of Victoria
• Department: Chemistry
• Course: CHEM 101
• Professor: Neil Burford

Document Summary

Elements which are in the third row or higher of the periodic table can expand their octet and form bonds with more than four other atoms. This is due to bonding of d-orbital electrons. Lewis structure is drawn in the same way, but with more orbitals included around the central atom. In compounds which have double or triple bonds, the placement of the double or triple bond can be uncertain. If multiple lewis structures have the same formal charges, then the extra bonds are shared between all bonds. This is drawn as a line (single bond) with a dotted line (fractional bond) If a double bond is shared, the resulting bonds are all equal. The resulting bonds are shorter than a single bond, but longer than a double bond. All three structures are equivalent, but the placement of the double bond is different. Each of the three placements is equally possible.