ChemistryWiki | RecentChanges | Preferences
|VSPER & Geometry Table
| #pairs of electron around central atom
||# lone pair on central atom
||Name of shape
- Two atoms bonding will always give linear geometry
- Hybridization is only on the central atom.
- All compounds with multiple bonds (i.e. double bonds) have a planar geometry
- C,N,O,F (sometime P,S,Cl) are the most common elements that form multiple bonds
- Compounds that have the potential to have d-orbitals (this excludes C,N,O,F) can exceed the Octet Rule/ Rule of 8.
- For compounds w/elements in 3rd energy (row) and higher, look for Lewis Dot Structure with single bonding first before more complex structure w/double bonds.
- The simple way of determining the Hybridization on the Central atom:
- Add up the number of outside atoms that central atom is bonding with.
- Add up the number of lone pairs on central atom
- Add together to get number.
- This number is number of Hybridized orbital
- Example CH4
- Central atom is bonded to 4 outside atoms and no lone pair so hybridization is sp3 where there are 4 of them.