CHAPTER 6A REVIEW SHEET
1. What are the two types of chemical bonds? What two periodic properties are used
to differentiate between the two?
2. What makes a covalent bond polar or nonpolar?
3. What type of charge exists on an atom in a molecule that has a higher electron
density?
4. Are there such things as molecules of sodium chloride? Why or why not?
5. CH4 is the _______________ formula for a __________ of methane, making the
formula a _______________ formula since methane is a _______________
_______________.
6. What’s the rule for determining which elements form diatomic molecules?
7. What’s the relationship between bond length and bond energy?
8. Use orbital notations to identify which electrons are shared in the compound HF.
9. What rule requires that most atoms try to attain eight valence electrons to become
stable?
10. Draw Lewis structures and resonance structures (if applicable) for each of the
following molecules.
a. CH3Cl
d. SeCl6 (expanded valence)
b. SiS2
e. NH2–
c. BO33– (expanded valence)
f. C2HCl
11. Using electron dots, determine the formula that will result from the combination
of the following atoms.
a. Cu (2 valence e–s) and O
b. Ba and F
c. Ga and S
12. Draw a simple crystal lattice of KF. How can one measure the strength of the
attractive forces within the crystal lattice?
13. What factors must be considered when determining whether an ionic or covalent
compound will conduct electricity?
14. How do the melting and boiling points of ionic compounds and molecular
compounds compare? What factors need to be considered when comparing these
two types of compounds?
15. What must be considered when comparing the aqueous solubility of ionic and
covalent compounds?