Covalent Bonding
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Covalent Bonding - Objectives
What we are going to learn today
Molecular Compounds
Polyatomic Compounds
Molecular Formulas
Structural Formula
Molecular Formulas
Definitions
• Covalent
• Co?
• Valent?
• Sharing
of electrons
between atoms
•
•
•
As opposed to ionic
bonding where electrons
are given or taken away.
Video Link
Video Link 2
Molecular Formulas
Definitions
Molecule – a neutral group
of atoms bonded by a
covalent bond.
• Diatomic – di=2 atomic =
atoms, molecule that
consists of only 2 atoms
•
• What
would you call a
molecule with 3 atoms or 1
atom?
Formula unit – formula for
an ionic compound (not a
molecule)
• Molecular formula –
formula for a compound
•
Molecular Formulas
Ionic compounds (generic)
• Give or take electrons
• Strong bonds
• High melting points
• High boiling points
• Solid at room temperature
• Formed by a metal and nonmetal
• Crystalline structure
Molecular Formulas
Covalent compounds (generic)
• Share electrons
• Weaker bonds
• Low melting points
• Low boiling points
• Liquid or gas at room
temperature
• Formed from two non-metals
• Non crystalline structure
Molecular Formulas
• What do they tell us?
Components (which
elements make up the
compound)
Ratio (how many of one
element compared to the
others)
•
•
•
This is not a lowest whole
number ratio – it is the actual
amount of each atom in the
molecule
Molecular Formulas
• What do they not tell us?
Structure (we have no idea, unless there
are only two atoms, how each atom is
connected)
•
H2O is it H-H-O or is it
H-O-H?
A structural Formula can give us these insights
•
•
Assessment
Of these compounds:
1.
2.
3.
Which does/do not exist?
Which is/are ionic
Which are covalent?
Assessment
Covalent Bonding - Objectives
What we are going to learn today
covalent bonding
octet rule
covalent bonds (single, double, triple)
coordinate covalent bonds
Polyatomic Ions
Covalent Bonding
Octet Rule
•
Still applies (most of the time) – atoms
still want a stable configuration
They will share electrons until they reach a noble gas
configuration
•
•
•
Example: CH4, CCl4
Structural Formulas
•
•
A lot like Lewis Dot Structures except covalent bonds
are shown by lines.
Every pair of shared electrons is a single line
Unshared
Pair
Shared
Pair
Hybridization
Even though we know the S orbital fills first before we start filling the P
orbitals, when we draw Lewis Dot structures, we put down four unpaired
electrons before we start filling in the second electrons in an orbital.
What happens in these cases is that the S orbital and the P orbitals can blend
together forming what is called hybrid orbitals.
sp3 hybrid orbital
Single, Double, and Triple Bonds
Single bonds involve
one set of orbitals
sharing one
electron a piece.
Weakest covalent
bond (longest)
Sigma bond (circle
overlap)
Single, Double, and Triple Bonds
Double bonds
involve two sets
of orbitals sharing
one electron from
each orbital
Middle strength,
middle length
Single, Double, and Triple Bonds
Triple bonds involve
three set of
orbitals sharing
one electron from
each orbital
Strongest covalent
bond (shortest)
Coordinate Covalent Bond
Coordinate covalent bond – a covalent bond
where 1 atom shares an electron pair
instead of both atoms sharing 1 a piece.
Polyatomic Ions
Polyatomic ions – tightly bound atomic
compounds that work as a single unit with a
charge.
Polyatomic Ions
Naming Molecules
Naming Molecules
Naming Molecules
Naming Molecules
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Geographic Region
Q1
Q2
Q3
Q4
United States
1254
1254
1254
1254
Europe and Asia
324
324
324
324
Australia
32
32
32
32
South America
2
2
2
2
Canada
1
1
1
1
Mexico
1
1
1
1
TOTALS
1614
1614
1614
1614
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Quarter
North America
Asia
Europe
Australia
Quarter
North America
Asia
Europe
Australia
Q1 2009
123
34
45
10
Q1 2009
123
34
45
10
Q2 2009
134
35
44
12
Q2 2009
134
35
44
12
Q3 2009
150
45
50
14
Q3 2009
150
45
50
14
Q4 2009
201
55
60
18
Q4 2009
201
55
60
18
Q1 2010
175
44
47
13
Q1 2010
175
44
47
13
Q2 2010
180
48
52
14
Q2 2010
180
48
52
10
Q3 2010
204
55
60
16
Q3 2010
204
55
60
4
Q4 2010
250
62
70
20
Q4 2010
250
62
70
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