Covalent Bonding
Download
Report
Transcript Covalent Bonding
Chemistry Matter and Change Chapter 8
COVALENT
BONDING
CHAPTER 8 MAIN IDEA
Covalent bonds form
when atoms share
electrons.
Chemistry Matter and Change Chapter 8
THE COVALENT
BOND
8.1 Main Idea
Atoms gain
stability when
they share
electrons and
form covalent
bonds.
8.1 OBJECTIVES
Apply the octet rule to atoms that
form covalent bonds.
Describe the formation of single,
double, and triple covalent bonds.
Contrast sigma and pi bonds.
List the diatomic elements
Relate the strength of a covalent
bond to its bond length and bond
dissociation energy.
REVIEW VOCABULARY &
CONCEPTS
Chemical bond
Valence electrons
Electronegativity
Lewis structure
NEW VOCABULARY &
CONCEPTS
Covalent bond
Molecule
Sigma (σ)bond
Pi (π)bond
Endothermic reaction
Exothermic reaction
Single bond
Double bond
Triple bond
WHY DO ATOMS BOND?
Sharing electrons takes less
energy than being “alone”
Octet is usually the most stable
electron configuration
WHAT IS A COVALENT BOND?
Shared pairs of electrons
http://www.glencoe.com/sites/co
mmon_assets/science/cmc/cim/an
imations/ch8_3_1.swf
SINGLE COVALENT BONDS
Two atoms share one pair of
electrons
Sigma bond (σ)
_
Either : or for a Lewis Structure
· · H H·· H
H
H+
or
H-
MULTIPLE COVALENT BONDS
Two atoms share more than one
pair of electrons
One pair is a sigma bond (σ)the
others are pi (π)bonds
Double bond shares 2 pair of
electrons
Triple bond shares 3 pair of
electrons
DOUBLE COVALENT BONDS
A π bond
A σ bond
TRIPLE COVALENT BONDS
COMPARING BONDS
Sigma (σ) Bonds
Pi (π) Bonds
Single
Paired
Centered
Parallel
s
p
orbital
electrons
One pair of
electrons is
shared
orbital
electrons
Multiple pairs of
electrons are
shared
DIATOMIC MOLECULES
Br I N Cl H O F
I couldn't
exist
without
you!
Oh, Ha Ha!
VIDEO
http://www.glencoe.com/sites/co
mmon_assets/science/cmc/cim/an
imations/ch8_1.swf
LEWIS STRUCTURES AND OCTET
Practice by drawing
H2
O2
+
N2
H2O
CO2
+
LEWIS STRUCTURES AND OCTET
Practice by drawing
H2
+
-
+
LEWIS STRUCTURES AND OCTET
Practice by drawing O2
σ
- -
+
- -
-
-
-
+
-
π
- -
- - -
+
-
+
-
STRENGTH OF COVALENT BONDS
Strength depends on distance of
the atoms from each other
With more bonds comes
stronger bonds
O2 is stronger than H2
BONDS AND ENERGY
Endothermic reactions require
additional energy for bonds to
break
Exothermic reactions release
energy when the bonds break
(spontaneous)
CAN YOU…
Apply the octet rule to atoms
that form covalent bonds.
Describe the formation of
single, double, and triple
covalent bonds.
Contrast sigma and pi bonds.
Relate the strength of a
covalent bond to its bond length
and bond dissociation energy.
Section 8.2 Chemistry Matter & Change
NAMING
MOLECULES
8.2 Main Idea
Specific rules are
used when naming
binary molecular
compounds, binary
acids and oxyacids
OBJECTIVES
Translate molecular formulas
into binary molecular names.
Name acidic solutions.
REVIEW VOCABULARY &
CONCEPTS
Ionic bond
Covalent bond
Formula unit
Oxyanion
Naming ionic substances
Molecule
NEW VOCABULARY &
CONCEPTS
Oxyacid
Binary acid
NAMING BINARY MOLECULAR
COMPOUNDS
1. Name the first element using
the entire name of the
element.
2. The second element in the
formula is named using the
root and suffix “-ide.”
3. Prefixes are used to indicate
the numbers of each element.
COMMON PREFIXES
Number of
atoms
1
2
3
4
5
Prefix
MonoDiTriTetraPenta-
Number of
atoms
6
7
8
9
10
Prefix
HexaHeptaOctaNonaDeca-
NAMING BINARY MOLECULAR
COMPOUNDS
Exceptions to the rules:
The first element never uses
“mono-”
There
is an understood 1 if
nothing is specified.
Awkward vowels can be
dropped
NAMING BINARY MOLECULAR
COMPOUNDS EXCEPTION
The first element never uses
“mono-”
There
is an understood 1 if
nothing is specified.
CO2 is carbon dioxide not
monocarbon dioxide
CO is carbon monoxide, not
monocarbon monoxide
PRACTICE NAMING BINARY
COMPOUNDS
FORMULA
SYSTEM NAME
N2O
dinitrogen monoxide
NO
nitrogen monoxide
N2O3
dinitrogen trioxide
NO2
nitrogen dioxide
N2O4
dinitrogen tetroxide
N2O5
dinitrogen pentoxide
NO3
nitrogen trioxide
NAMING BINARY ACIDS
The first word has the prefix
“hydro-” followed by the root of
the second element followed by
“-ic”
The second word is “acid”
HCl-
hydrochloric acid
PRACTICE NAMING BINARY
ACIDS
Hydrobromic acid
Hydrophosphic acid
Hydrosulfuric acid
HF
H2Se
HI
NAMING OXYACIDS
First word consists of the root of the
oxyanion (with prefixes if needed)
followed by a suffix as specified
If oxyanion ends in
Oxyanion ending
New suffix for acid
-ate
-ic
-ite
-ous
The second word is always “acid.”
NAMING OXYACIDS
Relationshi General
p
name
Oxyanion
name
Example
name
Example
formula
One more
oxygen than
(root)ic
Per(root)ic
acid
Perchlorate
Perchloric
acid
HClO4
Root(ic) acid
chlorate
Chloric acid
HClO3
Root(ous)
acid
Chlorite
Chlorous
acid
HClO2
One less
oxygen than
root(ic)
Two less
Hypo(root)ou
Hypochlorou
oxygens than
Hypochlorite
s acid
s acid
root(ic)
HClO
NAMING OXYACIDS
First word consists of the root of the
oxyanion (with prefixes if needed)
followed by a suffix as specified
The second word is always “acid.”
Compound
Oxyanion
Acid suffix
Acid name
HClO3
Chlorate
-ic
Chloric acid
HClO2
Chlorite
-ous
Chlorous acid
HNO3
Nitrate
-ic
Nitric Acid
HNO2
Nitrite
-ous
Nitrous Acid
Look at the
formula of the
molecule
Is it an acid?
Yes
Is there oxygen
present in the
compound?
No
Hydro(root) ic acid
Yes
No
Name the first element using a
prefix if necessary
Name the second element
indicating the number of atoms
and changing the suffix to –ide.
Root + -ic if the anion ends in –ate,
or
Root + -ous if the anion ends in –ite,
then
acid
PRACTICE NAMING OXYACIDS
Acid Formula
Acid Name
H2CO3
Carbonic Acid
HBrO3
Bromic Acid
H2C
Carbonic Acid
CH3COOH or CH3CO2H
Acetic acid
H3PO4
Phosphoric acid
H2SO4
Sulfuric acid
H2SO3
Sulfurous Acid
CAN YOU
Translate molecular formulas
into binary molecular names.
Name acidic solutions.
Section 8.3 Chemistry Matter & Change
MOLECULAR
STRUCTURE
8.3 Main Idea
Structural
formulas show
the relative
positions of
atoms within a
molecule.
OBJECTIVES
List the basic steps used to
draw Lewis structures.
Explain why resonance occurs
and identify resonance
structures.
Identify three exceptions to the
octet rule and name molecules in
which these exceptions occur.
REVIEW VOCABULARY &
CONCEPTS
Ionic bond
Covalent bond
Lewis-dot structure
Octet
NEW VOCABULARY &
CONCEPTS
Structural formula
Resonance
Coordinate covalent bond
Space filling model
Ball and stick model
MOLECULAR STRUCTURES
Many different ways to depict
the same thing
Molecular
formula
Structural formula
Lewis Structure
Space-filling model
Ball-and-stick model
MOLECULAR FORMULA
Indicates number of each
element in a molecule
H2O
C6H12O6
NH3
STRUCTURAL FORMULAS
Molecular model that shows the
relative positions of the atoms
O
H
H
LEWIS STRUCTURE
Shows shared electrons and
lone pairs
Shared
pairs are usually depicted
as lines
Lone pairs may be lines or dots
SPACE-FILLING MODEL
Atoms are shown in relative
size and position accounting for
lone pairs
BALL AND STICK MODELS
Show relative position of atoms
and bonds
Easier
to see double and triple
bonds and bond angles
HINTS FOR LEWIS STRUCTURES
1. Carbon is usually in the middle
2. Group 1 and 17 elements are
always at ends
3. Atoms that are less numerous
are usually in the middle
SIMPLE PRACTICE FOR LEWIS
STRUCTURES
H2O
HCl
CH3F
ORGANIC PRACTICE WITH
LEWIS STRUCTURES
Methane CH4
Ethane
C2H6
Propane C3H8
TRICKIER PRACTICE
CO2
HCN
BH3
NH4+
TRICKIER ORGANIC PRACTICE
C2H6
C2H4
C2H2
ethane
ethene
ethyne
RESONANCE STRUCTURES
More than one valid Lewis
structure is possible
Differ
in position of electrons, not
position of atoms
HINTS FOR FORMING LEWIS
STRUCTURES
Carbon is usually in the middle
Group 1 and 17 elements are always at ends
Atoms that are less numerous are usually in the
middle
Hydrogen always forms one single bond
Oxygen has two bonding electrons and two lone
pairs
Nitrogen has three bonding electron and one lone
pair
Group 13 elements have three bonding electrons
and zero lone pairs
Elements in groups 1, 2, 13 may break octet by
having fewer electrons
Phosphorus is a mess!
REALLY HARD
PCl5
SF6
C6H12O6
ORGANIC CHEATS
Common groups are often listed
differently in organic molecules
Ex: we write NH2CH2COOH
instead of C2NO2H5
CAN YOU
List the basic steps used to
draw Lewis structures.
Explain why resonance occurs
and identify resonance
structures.
Identify three exceptions to the
octet rule and name molecules in
which these exceptions occur.
Section 8.4 Chemistry Matter and Change
MOLECULAR
SHAPES
Main Idea
The VSEPR model
is used to
determine
molecular shape
OBJECTIVES
Summarize VSEPR bonding
theory
Predict the shape of, and bond
angles in, a molecule
Define hybridization
REVIEW VOCABULARY &
CONCEPTS
Atomic orbital
s orbital
p orbital
NEW VOCABULARY &
CONCEPTS
VSEPR theory
Hybridization
Trigonal planar
Trigonal pyramidal
Tetrahedral
Trigonal bipyramidal
Linear
Bent
Octahedral
VSEPR MODEL
Valence Shell Electron Pair
Repulsion
Electrons repel each other
Electrons
stay as far away from
each other as possible
Lone pairs occupy more space
than shared electrons
HYBRIDIZATION
Occurs because hybrid orbitals
are more stable in some cases,
notably carbon
Remodel the “hotel” to make the
“rooms” equal
CARBON HYBRIDIZATION
C: 1s22s22p2 1s22sp3
GETTING STARTED
Begin with Lewis Structure
Start with a tetrahedral and
modify as needed
Remember to use 3-D space not
2-D space
VIDEO
http://www.glencoe.com/sites/co
mmon_assets/science/cmc/cim/an
imations/ch8_2.swf
CH4: A TYPICAL TETRAHEDRAL
TETRAHEDRAL SHAPE
Four atoms are coming from the
center atom at equal angles
109.5° angle
TRIGONAL PYRAMIDAL
Three atoms coming from
central atom and one lone pair
Bond
Lone
angle 107°
pairs occupy more space than
shared pairs
BENT
Two atoms coming from central
atom and two lone pairs
104.5° bond angle
SUMMARY OF COMMON
MOLECULAR SHAPES
Molecul Tota Share
e
l
d
pair pairs
s
Lon
e
pair
s
Hybrid
orbital
Molecular shape
BeCl2
2
2
0
sp
Linear
AlCl3
3
3
0
sp2
Trigonal planar
CCl4
4
4
0
sp3
Tetrahedral
NH3
4
3
1
sp3
Trigonal
pyramidal
H2O
4
2
2
sp3
Bent
NbBr5
5
5
0
sp3d
Trigonal bipyramidal
SF
6
6
0
sp3d2
Octahedral
TETRAHEDRAL BASED SHAPES
Tetrahedral
Trigonal Pyramidal
Bent
NON-TETRAHEDRAL BASED SHAPES
Linear
Trigonal Planar
FEWER ELECTRONS THAN OCTET!
NON-TETRAHEDRAL BASED SHAPES
Trigonal Bipyramidal
Octahedral
MORE ELECTRONS THAN OCTET!
CAN YOU…
Summarize VSEPR bonding
theory
Predict the shape of, and bond
angles in, a molecule
Define hybridization
Chapter 8.5 Chemistry Matter and Change
ELECTRONEGATIVITY
AND POLARITY
Main Idea
A chemical bond’s
character is
related to each
atom’s attraction
for the electrons
in the bond.
OBJECTIVES
Describe how electronegativity
is used to determine bond type.
Compare and contrast polar
and nonpolar covalent bonds and
polar and nonpolar molecules
Generalize about the
characteristics of covalently
bonded compounds
REVIEW VOCABULARY &
CONCEPTS
Electronegativity
Electron affinity
Ionic bond
Covalent bond
NEW VOCABULARY &
CONCEPTS
Polar covalent bond
Electronegativity difference
Molecular polarity
Intermolecular forces
Solubility
Dipole
ELECTRON AFFINITY, ELECTRONEGATIVITY,
AND BOND CHARACTER
Electronegativity difference determines
the character of the bond between atoms
Most bonds are partly ionic and partly
covalent
Diatomics are 100% covalent
Electronegativity difference
Bond Character
> 1.7
Mostly ionic
0.4 - 1.7
Polar covalent
< 0.4
Mostly covalent
0
Nonpolar covalent
BOND CHARACTER
IONIC BONDS
Created when the
electronegativity difference is
greater than 1.7
Elements are far apart on
periodic table
Example:
Na and Cl
Na = 0.9
Cl = 3.0
Difference is 2.1 ionic bond
Electrons are transferred from Na to Cl
NON-POLAR COVALENT BONDS
Created when electronegativity
difference is 0
Usually
atoms of the same
element
Diatomics
COVALENT BONDS
Created when electronegativity
difference is < 0.4
Elements are usually close
together on the periodic table
IBr
POLAR-COVALENT BONDS
Created when electronegativity
difference is between 0.4 and 1.7
Most bonds fall into this
category
Electrons are shared unequally
H2O
POLAR COVALENT BONDS
Molecules have a partial
positive and a partial negative
side
DIPOLE INTERACTIONS
Reactions between oppositely
charged ends of a polar molecule
POLAR COVALENT BONDS
Polar bonds that are equal in
all directions in a molecule
create non-polar molecules
SOLUBILITY RULES
Like dissolves like
Polar
substances dissolve polar
substances
Non-polar substances dissolve
non-polar substances.
CAN YOU
Describe how electronegativity
is used to determine bond type.
Compare and contrast polar
and nonpolar covalent bonds and
polar and nonpolar molecules
Generalize about the
characteristics of covalently
bonded compounds