2.2 Molecular Compounds
Molecular Compounds
•
•
•
•
2 or more non-metals
Made up of atoms held together by a covalent
bond
Electron sharing
Eg: Methane (CH4)
Diatomic molecules (O2, Br2)
Molecular Compounds
Properties
• Depend on their structure
• Can be gas, solid, or liquid at room temperature, but are
usually gases since they have low boiling points
• Have a variety of physical properties (waxy, flexible, or
rigid)
• Do not dissolve in water
• Poor electrical conductivity
Molecular Compounds
Properties
Ionic vs Molecular Compounds:
Copy summary chart on page 69
Molecular Compounds
Bonding Diagrams
• Bonding capacity – the number of covalent bonds
that an atom can form
H
# of
valence
electrons
Bonding
Capacity
C
N
O
F
Molecular Compounds
Bonding Diagrams
• Bonding capacity – the number of covalent bonds
that an atom can form
# of
valence
electrons
Bonding
Capacity
H
C
N
O
F
1
4
5
6
7
Molecular Compounds
Bonding Diagrams
• Bonding capacity – the number of covalent bonds
that an atom can form
H
C
N
O
F
# of
valence
electrons
1
4
5
6
7
Bonding
Capacity
1
4
3
2
1
•
Lone pair – a pair of electrons not involved in bonding
•
Draw Lewis Structures (see handout)
Examples
Draw the Lewis structure for:
phosphorus trichloride
carbon monoxide
ammonium ion
Pg 65 #1, pg 67 #2 & pg 69 #1-7