CHEMISTRY
STUDY GUIDE
COVALENT BONDING
I.
NAME: __________________________
DATE: ___________________________
PERIOD: _________________________
Chapter 8
THE COVALENT BOND - 8.1
A.
Why do atoms bond?
1.
Gaining stability
B.
What is a covalent bond?
1.
Shared electrons
a.
Please Define Covalent Bond:
b.
2.
C.
Please Define a Molecule:
Covalent bond formation
a.
Write the 7 diatomic molecule as formulas:
1.
hydrogen _____________________
2.
nitrogen ______________________
3.
oxygen _______________________
4.
fluorine _______________________
5.
chlorine _______________________
6.
bromine _______________________
7.
iodine _________________________
Single Covalent Bonds
1.
Please Define Lewis Structure:
2.
Group 17 and single bonds
a.
What is the family name of this Group 17? _____________________________
3.
Group 16 and single bonds
a.
What atom in Group 16 forms a molecule having two single covalent bonds
and two unshared pairs of electrons?
_________________________________________________________________
4.
Group 15 and single bonds
a.
What atom in Group 15 forms three single covalent bonds and has a pair of
unshared electrons? ________________________________________________
5.
6.
D.
E.
-2Group 14 and single bonds
a.
What atom in Group 14 forms four single covalent bonds and has no unshared
electrons? _________________________________________________________
The sigma bond
a.
Please Define the Sigma Bond:
Multiple Covalent Bonds
1.
Double bonds
a.
An example of this would be the ________________________ molecule.
2.
Triple bonds
a.
An example of this would be the ________________________ molecule.
3.
The pi bond
a.
Please Define the Pi Bond:
The Strength of Covalent Bonds
1.
Bond length
a.
Look at Table 8.1 on page 246.
1.)
As the number of covalent bonds increase the bond length ______________.
2.)
2.
As the bond length decreases in length its strength ____________________.
Bonds and energy
a.
Look at Table 8.2 on page 247.
1.)
The smaller bond length the __________________ the bond
dissociation energy.
b.
Please Define Endothermic Reaction:
c.
Please Define Exothermic Reaction:
-3II.
NAMING MOLECULES - 8.2
A.
Naming Binary Molecular Compounds
1.
The first element in the formula is always named first, using the entire element name.
B.
2.
The second element in the formula is named using its root and adding the suffix -ide.
3.
The first element in the compound name never uses the mono- prefix. The prefix
mono- is only used on the second atom if it is by itself.
4.
Common names for some molecular compounds
a.
What are the Scientific names for:
1.)
Ammonia (NH3): _____________________________________________
Hydrazine (N4H4): ____________________________________________
3.)
Nitric oxide (NO): _____________________________________________
Naming Acids
1.
Naming binary acids
a.
The first word has the prefix hydro- to name the hydrogen part of the compound.
The rest of the first word consists of a form of the root of the second element
plus the suffix -ic.
b.
2.
The second word is always acid.
Naming oxyacids
a.
First, identify the oxyanion present. The first word of an oxyacid’s name
consists of the root of the oxyanion and the prefix per- or hypo- if it is part
of the name, and suffix. It the oxyanion’s name ends with the suffix -ate,
replace it with suffix -ic. If the name of the oxyanion ends with the suffix
-ite, replace it with the suffix -ous.
b.
C.
2.)
The second word of the name is always acid.
Writing Formulas from Names
-4III.
MOLECULAR STRUCTURES - 8.3
A.
Structural Formulas
1.
Please Define Structural Formulas:
2.
Lewis structures
3.
Lewis structures for polyatomic ions
B.
Resonance Structures
1.
Please Define Resonance:
C.
Exceptions to the Octet Rule
1.
Odd number of valence electrons
a.
An example of this, is the molecule: _________________________________.
2.
Suboctets and coordinate covalent bonds
a.
An example of this, is the molecule: _________________________________.
b.
3.
IV.
Please Define Coordinate Covalent Bond:
Expanded octets
a.
An example of this, is the molecule: __________________________________.
MOLECULAR SHAPES - 8.4
A.
VSEPR Model
1.
Please VSEPR model:
2.
B.
Bond angle
Hybridization
1.
Please Define Hybridization:
-5V.
ELECTRONEGATIVITY AND POLARITY - 8.5
A.
Electron Affinity, Electronegativity, and Bond Character
1.
Electronegativity
a.
Please Define Electronegativity:
2.
B.
C.
Polar Covalent Bonds
1.
Molecular polarity
a.
Please Define Molecular Polarity:
2.
Polarity and molecular shape
3.
Solubility of polar molecules
Properties of Covalent Compounds
1.
Intermolecular forces
a.
Please Define Intermolecular forces:
2.
D.
Bond character
a.
Please Define Polar Covalent Bond:
Forces and properties
Covalent Network Solids
1.
Please Define Covalent Network Solid:
2.
Name some examples of Covalent Network Solids.
a. ______________________________________
b. ______________________________________
-63.
VI.
Name four characteristics of Covalent Network Solids
a.
Nonconductors of heat and electricity
b.
_______________________________
c.
_______________________________
d.
_______________________________
CHAPTER 8 ASSESSMENT pp. 274-277.
A.
Please do Problems 84, 86, 92, 93, 94, 95, 96, 108, 111, 112, 117, 118, 119, 120, 122,
124, 125, 127, and 128.