Chemistry 110 - 02
Spring 2017
Sixth Homework
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Finish studying Hill and McCreary Chapter 4 sections 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.
Prepare for the next lab. Check the class calendar to see which lab we will perform.
The fourth 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, May 10. 10 Points.
Late homework is not accepted after the answer key is distributed on Wednesday, May 10.
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. 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.
3. Give the symbol for the monatomic ion made by each of these atoms.
a. potassium
b. iodine
c. calcium
d. phosphorus
4. Give the name for the monatomic ion made by each of these atoms.
a. potassium
b. iodine
c. calcium
d. phosphorus
5. How many valence electrons does each of the ions in the previous question have?
a. potassium
b. iodine
c. calcium
d. phosphorus
6. For each of these atoms, indicate whether it gains electrons or loses electrons when it becomes
an ion. Then tell how many electrons it gains or loses.
a. potassium
b. iodine
c. calcium
d. phosphorus
7. Give the symbol for the monatomic ion each of these elements forms. Then give the name of
each ion.
a. Cl
b. O
c. S
d. N
e. Ba
f. Li
8. How many electrons does each of these ions contain?
a. Fb. O2c. Sr2+
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9. Give the formula for each of these polyatomic ions.
a. nitrate ion
b. sulfate ion
c. hydroxide ion
d. acetate ion
e. ammonium ion
10. 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.
11. 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.
12. 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
13. 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
14. The formulas of each of these ionic compounds contains the digit “2”. For each compound,
what does the “2” indicate about the compound?
a. CaCl2
b. Mg(NO3)2
c. Na2CO3
15. What is the cation in each of these compounds? What is 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
16. 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
17. Give the name of each of these compounds.
a. NaCN
b. KNO3
d. NaCH3CO2
e. LiOH
c. Ca(HCO3)2
f. BaCl2
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18. 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
19. 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
20. 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
21. 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
22. 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
23. 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?
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24. Make a table of the atomic numbers and electronegativities of Cl, Br, and I. Use your table to
create a graph of the electronegativity versus the element’s atomic number. (Atomic number
goes on the horizontal axis.) Use this graph to predict an electronegativity for fluorine. Now
compare this predicted value to the actual electronegativity of fluorine. How good was your
prediction?
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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