Chemistry 110 - 02
Fall 2016
Sixth Homework
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Finish studying Hill and McCreary Chapter 4 sections 7, 8, 3 – 5, and 9 - 12.
Begin studying Hill and McCreary Chapter 5 sections 1, 3, 4, and 5.
Finish learning the names and formulas of the polyatomic ions listed on the fifth homework.
The fifth quiz will include questions from the topics below. To be prepared for the quiz, you should
be able to answer these questions using only the periodic table you received in class and the
information given. Any quiz may include questions about lab safety and procedures.
Due 8:30 am Wednesday, October 26. 10 Points.
Late homework is not accepted after 8:30 am Thursday, October 27.
1. Predict which of these compounds has a stronger bond between the carbon atom
and the oxygen atom: CH4O or H2CO. Justify your answer.
2. Give the formula and the name of each of these binary compounds.
a. The compound formed from sodium and bromine.
b. The compound formed from calcium and fluorine.
c. The compound formed from magnesium and phosphorus.
d. The compound formed from aluminum and sulfur.
3. a. Using the idea of electrical attractions and repulsions, explain why the ions in calcium oxide
stay together. (Note: If your answer does not include attractions and/or repulsions between
charged particles then you have not answered the question.)
b. Draw a nanoscale picture of calcium oxide.
4. Draw an electron dot structure for each of these molecules. (There may be more than one
possible correct answer. Give just one.)
a. C4H11N
b. C2Cl2F2
c. C5H10O2
d. C6H10 with the six carbon atoms all in one ring.
5. For each of these compounds, indicate whether it is an ionic compound or a molecular
compound.
a. NaCl
b. NH3
c. Na2CO3
d. CH3CH3
e. NH4NO3
f. K3PO4
6. Give the formula of the cation in each of these compounds, and give the formula of the anion in
each of these compounds. Remember, each compound is composed of only one type of cation
and one type of anion.
a. NaCl
b. Ca(OH)2
c. Mg(NO3)2
d. (NH4)3PO4
e. K2SO4
f. Na2CO3
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7. Give the name of each of these compounds.
a. NaCl
b. Ca(OH)2
d. (NH4)3PO4
e. K2SO4
c. Mg(NO3)2
f. Na2CO3
8. Give the name of each of these compounds.
a. NaCN
b. KNO3
d. NaCH3CO2
e. LiOH
c. Ca(HCO3)2
f. BaCl2
9. Write the formula for each of these compounds.
a. sodium nitrate
b. potassium carbonate
d. magnesium phosphate
e. sodium hydroxide
g. water
h. calcium nitride
c. ammonium sulfate
f. lithium sulfide
10. Write the formula for each of these compounds.
a. ammonia
b. aluminum sulfate
d. magnesium cyanide
e. calcium oxide
g. barium sulfate
h. lithium chlorate
c. magnesium bicarbonate
f. potassium acetate
11. Predict what type of bonding (covalent bonding or ionic bonding) is expected between each of
these atoms. Briefly justify your answer.
a. C and S
b. Ca and Cl
c. N and O
12. For each molecule, use VSEPR to determine the shape of the molecule. For each molecule,
draw the molecule’s shape, give the name of the shape of the molecule, and indicate whether it
is a polar molecule or a nonpolar molecule. If it is a polar molecule, show which side of the
molecule has the bit of negative charge and which has a bit of positive charge. The
electronegativity of phosphorus is the same as that of hydrogen.
a. CO2
b. H2CO
c. CF4
d. H2O
e. PH3
13. For each molecule, use VSEPR to determine the shape of the molecule. For each molecule,
draw the molecule’s shape, give the name of the shape of the molecule, and indicate whether it
is a polar molecule or a nonpolar molecule. If it is a polar molecule, show which side of the
molecule has the bit of negative charge and which has a bit of positive charge.
a. OCl2
b. CH3Cl
c. HCN
d. NH3
14. a. Are these two molecules the same compound or isomers? (I strongly recommend you
borrow the model kit from the Building 15 office or the Tutoring Center and make these
compounds to check your answer.)
b. Are they polar molecules or nonpolar molecules?
Cl
H
C
Cl
H
H
H
C
Cl
Cl
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o15. a. What is the atomic mass of phosphorus?
b. What is the molecular mass of C6H12O6?
16. What is the molar mass of each of these?
a. C6H12O6
b. H2SO4
c. Na2HPO4
d. Ca(OH)2
17. Show your work. What is the mass of 3.48 moles of calcium chloride?
18. Answer Hill and McCreary Chapter 5 problem 30 a & b (on page 160).
19. Answer Hill and McCreary Chapter 5 problem 32 a & b (on page 160).
20. Show your work:
a. How many moles of butane is 6.98 g of butane (C4H10)?
b. How many grams of sodium sulfate is 0.538 moles of sodium sulfate?
21. The ions that transition metals form do not follow any obvious pattern. In fact, many transition
metals commonly form more than one type of ion. For example, iron commonly forms both
ferrous ion (Fe2+) and ferric ion (Fe3+). Fe2+ is also called “iron(II) ion”, which is read “iron two
ion”. Fe3+ is also called “iron(III) ion”, which is read “iron three ion”.
a. How many protons does a ferrous ion contain?
b. How many electrons does a ferrous ion contain?
c. How many protons does a ferric ion contain?
d. How many electrons does a ferric ion contain?
e. If you have a mineral supplement at home that contains iron, look at the label to answer this
question: Which of these two iron ions does it contain?
Myriads of motley molecules through space
Move round triumphant. By their whirlpool pace
Shall we be shaken? All in earth's vast span,
Our very bodies, veer to other shapes;
Mid the mad dance one stubborn power escapes,
Looks on and marvels, -'t is the soul of man.
from "Soul and Sense"
Hannah Kimball
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