This preview shows page 1. Sign up to view the full content.
Unformatted text preview: Differneces between carbon and silicon stem form the smaller atomic radius of carbon, which explains the C=C and the C=O double bonds however, it is rare to see Si=Si and Si=O. Silicon atoms are too large for the side-by-side overlap of p-orbitals necessary for pi-bonds to form between them. ex. O=C=O IS A GAS AND -O-Si-O- is a mineral. Silicon compounds can also act as Lewis acids, whereas carbon compounds typically cannot. Because silicon atoms are bigger than C atoms and can expand its valence shell by using its d-orbitals, it can accommodate the lone pair f an attacking Lewis base. Exception is when C atoms have multiple bonds. See you all soon! Alissa...
View Full Document
- Fall '08