Hybridization
and
Multiple Bonds
Draw dot structures for the
following elements:
•  Beryllium: 1s22s2
•  Boron: 1s22s22p1
•  Carbon: 1s22s22p2
•  Silicon: 1s22s22p63s23p2
Hybridization
It has been observed Beryllium, Boron, Carbon, and
Silicon can form the following compounds:
Hybridization: A combining of the s and p orbitals
for certain elements
Orbital diagram for Be:
Be will promote one 2s electron to the
2p level
The Theory of Hybridization
•  Beryllium: 1s22s2
sp hybrid orbital
•  Boron: 1s22s22p1
sp2 hybrid orbital
•  Carbon: 1s22s22p2
sp3 hybrid orbital
•  Silicon: 1s22s22p63s23p2
sp3 hybrid orbital
The Theory of Hybridization
•  An “s” electron is promoted up to the next
highest energy “p” orbital
•  The highest energy “s” and “p” orbitals
combine to form four equal energy “hybrid”
orbitals
The Hybrid Dot Structures:
•  Beryllium: 1s22s2
•  Boron: 1s22s22p1
•  Carbon: 1s22s22p2
•  Silicon: 1s22s22p63s23p2
Coordinate Covalent Bonding
Coordinate Covalent Bonding: The result of both shared electrons coming from one atom.
The bonds are the same as regular covalent bonds. The only
difference is the source of the electrons.
Working with Multiple Bonds
•  CCl4
•  O2
•  N2
Two shared pairs
Three shared pairs
Double bond
Triple bond
Structural
Formula
Multiples Bonds: The result of more than one shared pair of electrons. Working with Multiple Bonds
•  CO2
•  CO
Assignment
•  Dot Structures Handout
–  Mixes ionic and covalent compounds
–  Includes elements with hybrid orbitals
–  Includes molecules that form double and triple
bonds
Polyatomic Dot Structures
Example 1: Ammonium (NH4)+
N
H
H
H H
Total Number of Electrons = 9
Electrons after Ion Forms = 8
Ionic Dot Structure:
+
H
H N H
H
Polyatomic Ions
Example 2: Sulfate (SO4)2S
O
O
O
Total Number of Electrons = 30
Electrons after Ion Forms = 32
Ionic Dot Structure:
O
O S O
O
2-
O