Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
1.
What is a chemical bond?
2.
Why do atoms form chemical bonds?
3.
What distinguishes an ionic bond from a covalent bond?
4.
What distinguishes a polar covalent bond from a nonpolar covalent bond?
5.
What is a dipole? What type of bond produces a dipole?
6.
How can you identify the negative and positive dipoles in a polar covalent bond?
7.
According to the general rules of electronegativities, what type of bond is formed by each of
the following pairs of elements? If the bond is polar covalent, identify the negative dipole (δ-)
and the positive dipole (δ+).
a.
potassium and chlorine
8.
b.
sulfur and sulfur
c.
carbon and bromine
d.
zinc and oxygen
Order the following covalent bonds from least to most polar.
a.
H – Cl
b.
H – Br
c.
H – Se
d.
H–C
e.
F–F
9.
What type of bond do nonmetals generally form with other nonmetals?
10.
What type of bond is generally formed between the alkali metals and the halogens?
11.
What type of bond is generally formed between the halogens and the oxygen group?
Cut along dotted line.
Assignment #1—Chemical Bonding (Predicting Bond Types)
Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
Assignment #2—Lewis Electron Dot Diagrams
12.
Draw the Lewis dot representations for each of the following neutral atoms:
a. sodium
e. magnesium
b. helium
f. fluorine
c. boron
g. nitrogen
d. krypton
h. oxygen
13.
Distinguish between single bonds, double bonds and triple bonds.
14.
Explain why the following Lewis structures for CHClO is incorrect.
H C
O
Cl
15.
Draw Lewis structures (or structural formulas) for the following molecules:
a.
Cl2
e.
carbon dioxide (CO2)
b.
hydrogen sulfide (H2S)
f.
methyl chloride (CH3Cl)
c.
nitrogen trichloride (NCl3)
g.
ethyne (C2H2)
h.
d.
silicon tetrahydride (SiH4)
Phosphorus trihydride (PH3)
16.
Which molecule(s) in question 15 include double bonds?
17.
Which molecule(s) in question 15 have triple bonds?
Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
Assignment #3—Binary Molecular Nomenclature
19.
Write the correct formula for each of the following compounds.
a.
carbon monoxide
b.
sulfur dioxide
c.
diphosphorus pentoxide
d.
nitrogen dioxide
e.
carbon dioxide
f.
phosphorus trichloride
g.
dinitrogen pentoxide
h.
phosphorus pentabromide
i.
silicon dioxide
j.
selenium tetrafluoride
Write the correct name for each of the following formulas.
a.
N2O
b.
P3N5
c.
NI3
d.
N2O4
e.
P4O10
f.
SO3
g.
SiI4
h.
N2O3
i.
CCl4
j.
As2O5
Cut along dotted line.
18.
Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
Assignment #4—Exceptions to the Octet Rule and Coordinate Covalent Bonding
20.
What is a coordinate covalent bond?
21.
Draw Lewis sructures (or structural diagrams) for the following polyatomic ions.
a.
OH-
b.
ClO3-
22.
State the Octet Rule. Name a compound in which the central atom does not follow this rule.
23.
Draw Lewis structures (or structural diagrams) for the following molecules.
a.
BeH2
c.
PCl5
b.
24.
SF6
d.
BH3
What are resonance structures? Write the possible resonance structures for NO3-.
Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
Assignment #5—Molecular Shapes and Polarity
25.
What do the letters VSEPR stand for? What is the basic assumption of this theory?
26.
How can you distinguish between a 3-atom linear molecule and a bent molecule? Give an
example of each.
27.
How can you distinguish between a trigonal pyramidal molecule and a trigonal planar
molecule? Give an example of each.
28.
Why is the bond angle in a trigonal pyramidal molecule different from that in a tetrahedral
molecule?
29.
What is the difference between a polar molecule and a nonpolar molecule?
30.
What makes a molecule polar?
31.
Give two examples of polar molecules that contain polar bonds. Give two examples of
nonpolar molecules that contain polar bonds.
32.
Complete the following table:
Formula
SbH3
Cl2O
BeH2
SiF4
PI5
SCl6
CO2
HCN
AsCl3
BH3
Lewis Structure
(or Structural Formula)
Name of Shape
Molecular
Polarity
Name
Chemistry Pre-AP: Covalent Bonding and Nomenclature Unit Homework
Class Period
Directions: Write your answers to the following questions in the space provided. For problem solving,
show all of your work and write your final answer on the blank line.
Assignment #6—Intermolecular Forces of Attraction
33.
What is a van der Waals force? Is it an example of a chemical bond? Why or why not?
34.
What is hydrogen bonding? Is it an example of a chemical bond? Give an example of a
substance that would exhibit hydrogen bonding.
35.
Arrange the following intermolecular attractions in order of increasing strength: dipole-dipole
interactions, London dispersion forces, hydrogen bonds.
36.
What is a temporary dipole? What types of molecules are capable of having temporary
dipoles? What is the name of the van der Waals force that involves temporary dipoles?
37.
For different substances of similar molar mass, which type of intermolecular force is the
weakest? Give an example of a molecule that would exhibit this force.
38.
What type of intermolecular forces of attraction would be exhibited by each of the following
substances?
a.
PF3
b.
HF
c.
N2
d.
BeH2
39.
The following substances have roughly the same molar mass. Which one is most likely to have
the highest boiling point: H2S, F2, or CO2? Explain your choice.