Academic Chemistry
Name ____________________
Chapter 6 Reading Guide
Period ____ Date __________
Section 6-1
1. Define chemical bond.
2. Nature favors arrangements in which potential energy is _______________________.
3. What is the main difference between ionic bonding and covalent bonding?
(what happens to the electrons?)
4. Are chemical bonds usually purely ionic, purely covalent, or other? Explain.
5. Define electronegativity. (from chapter 5 – or use glossary)
6. The degree to which a bond is ionic or covalent can be estimated by
_____________________________________________________________________.
7. If the difference in electronegativity values is greater than 1.7, the bond is classified as
_____________________.
If the difference in electronegativity values is between 0.3 and 1.7, the bond is classified as
_____________________.
If the difference in electronegativity values is less than 0.3, the bond is classified as
_____________________.
8. If a bond is polar covalent, the negatively charged electrons are pulled closer to one atom than
another. This results in a partial charge distribution. A partially negative charge is indicated by the
symbol ______. A partially positive charge is indicated by the symbol _____.
Section 6-2
1. Define molecule.
2. Define bond length.
Look at table 6-1 (pg. 168). Place the following bonds in order of increasing bond length.
H-H
C-H
N-H
C-N
N-N
C-C
3. Why do noble gas atoms exist independently in nature?
4. What is the “octet rule”?
5. List 2 main-group elements that are exceptions to the octet rule. Explain why they are exceptions.
6. Write the electron dot notation for the following elements:
Oxygen
Carbon
Magnesium
Neon
7. Draw the Lewis Structures for H2 and F2.
8. Define lone pair (unshared pair).
9. How many electrons are shared in a single bond? _______
double bond? ______
triple bond? _____
10. Draw the structural formulas for C2H4 and N2.
11. Look at table 6-2 (pg. 173). Place the following bonds in order of increasing bond length and bond
energy.
N═N
N≡N
N–N
Is there a relationship between the type of bond (single, double, triple) and the length of the bond?
Explain.
Which type of bond is the strongest?
Section 6-3
1. Define ionic compound.
2. How is an ionic crystal different from how a molecular compound is put together?
3. When sodium and chlorine bond, which element loses an electron? ____________ Which element
gains an electron? ________________
4. When calcium and fluorine bond, how many fluorine atoms are needed to accept calcium’s two valence
electrons?
5. An orderly arrangement of ions is called a _______________ ______________.
6. Compare/contrast the melting points of ionic and molecular solids.
7. Under what 2 circumstances can an ionic compound conduct an electrical current?
8. Define polyatomic ion.
9. How does a polyatomic ion gets its electrical charge?
10. What type of bond (ionic or covalent) holds the atoms of a polyatomic ion together?
Section 6-4
1. Why are metals such good conductors of electricity?
2. What does “delocalized” mean?
3. Define metallic bonding.
4. What causes the surface of a metal to look shiny?
5. Define malleability.
6. Define ductility.
7. How is the strength of a metallic bond determined?
8. Look at table 6-4 (pg. 182).
What is the general trend for metallic bond strength as you move across a period?
Section 6-5
1. For what does each letter in VSEPR stand?
2. What does the VSEPR theory state?
3. Look at Table 6-5 on pg. 186 to answer the following questions:
a) If a molecule has 4 atoms bonded to a central atom, what is the geometry (shape) of the
molecule?
_____________________
b) If a molecule has 3 atoms bonded to a central atom, and 0 lone pairs, what is the geometry
(shape) of the molecule? ____________________
c) If a molecule has 3 atoms bonded to a central atom, and 1 lone pair, what is the geometry
(shape) of the molecule? ____________________
d) If a molecule has 2 atoms bonded to a central atom, and 0 lone pairs, what is the geometry
(shape) of the molecule? ____________________
e) If a molecule has 2 atoms bonded to a central atom, and 1 lone pairs, what is the geometry
(shape) of the molecule? ____________________
f) If a molecule has 6 atoms bonded to a central atom, what is the geometry (shape) of the
molecule? ____________________
g) If a molecule has 2 atoms bonded to a central atom, and 2 lone pairs, what is the geometry
(shape) of the molecule? ____________________
h) If a molecule has 5 atoms bonded to a central atom, what is the geometry (shape) of the
molecule? ____________________
4. Define dipole.
5. How is a dipole represented?
6. Indicate the dipole in the molecule below.
H ― Cl
7. Explain why carbon dioxide, CO2, does NOT have a molecular dipole.