Arnoldi
Chemistry
Covalent Bonding
Chapter 8 Covalent Bonding
8.1 Molecular Compounds
1. Important Definitions
a. Covalent Bond
b. molecule
c. diatomic molecules
Our Special Diatomic Elements
H2, O2, N2, Cl2, Br2, I2, F2
d. molecular compound
(in other words, it is covalently bonded)
e. molecular formula
2. In a formula unit, the ionic formula is always the lowest ratio of atoms to each
other. In other words, you always have NaCl, never Na2Cl2. In a molecular formula,
it shows the actual ratio of atoms present, which may or may not be the lowest
ratio possible.
3. Look at the picture on page 206. What is the difference in atom arrangement
between several molecules of a covalent compound and several formula units of an
ionic compound?
4. Compared to ionic compounds, covalent compounds have _____________
melting and boiling points. This means that they are often in the ____________
or _______________ state of matter at room temperature.
5. Ionic compounds conduct when dissolved in water or melted. What do we know
about the conductivity of covalent compounds?
6. Answer Question # 4 on page 207 here.
8.2 The Nature of Covalent Bonding
7. Answer the question posed on the top of page 208.
8. Why do atoms want to share electrons covalently?
9. Important Definitions
a. Single Bond
b. Structural Formula
c. Unshared Pair
d. Double Bond
e. Triple Bond
SKIP the section on coordinate covalent bonds (pages 213 – 214).
SKIP the section on exceptions to the octet rule (page 216).
SKIP the section on bond dissociation energies (page 217).
SKIP the section on resonance (page 219).
SKIP all of section 8.3, Bonding Theories, (page 220 – 223).
8.4 Polar Bonds and Molecules
10. Important Definitions:
a. Polar Covalent Bond
b. Nonpolar Covalent Bond
c. Polar Molecule
SKIP the section on attractions between moleucles (Pages 228 – 229).
SKIP the section on Intermolecular Attractions and Molecular Properties (page 230).