Chemistry 110 - 02
Winter 2016
Fifth Homework
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Study Hill and McCreary Chapter 4 sections 7, 8, 3 – 5, and 9 - 12.
Work on the Oxygen Content of Air lab report which is due February 5.
Complete the prelab for the Molecular Models Lab and work on the report. It looks more like a
homework assignment than a lab report. Be sure to staple your pre-lab to the back of your
report. It is due February 5.
Learn the names and formulas for the polyatomic ions listed below.
The fourth quiz will include questions from the topics below and from the sixth homework. 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.
Using the periodic table, be able to give the symbol and name of the ion formed by each element in
Groups 1, 2, 16, and 17 (except Po) and by the elements aluminum, nitrogen, and phosphorus. (See
Figure 4.4)
Learn the names and formulas of these ten polyatomic ions. (I recommend making and using flash
cards.)
Name
ammonium ion
hydroxide ion
cyanide ion
carbonate ion
bicarbonate ion
nitrate ion
phosphate ion
sulfate ion
chlorate ion
acetate ion
Chemical formula
NH4+
OH−
CN−
CO32−
HCO3−
NO3−
PO43−
SO42−
ClO3−
CH3CO2−
Due 8:30 am Tuesday, February 2. 10 Points.
Late homework is not accepted after 8:30 am Wednesday, February 3.
1. Properly record the answers to these operations involving measurements.
a. 58.0 mL × 0.89 g/mL =
b.7.68 g – 6.942 g =
2. Properly record the results of these calculations.
a. 6.359 g / 2.4200 mL =
b. 23.34 g – 22.867 g =
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3. Perform these conversions. Show your work.
a. Convert 77.3 g to kg.
b. Convert 105.0 mL to L
c. Convert 0.8050 L to dL
d. Convert 8.43 m to cm.
e. Convert 364 mm to µm.
4. The density of zinc is 7.14 g/mL. What is the volume of 53.9 g of zinc? Show your
work.
5. Give the name of an element that is a nonmetal that is extremely corrosive to tissue and
metals, forms compounds with hydrogen in a 1 to 1 atom ratio, and is usually found as
diatomic molecules as an element.
6. Using the idea of electrical attractions and repulsions, explain why the atoms in a water molecule
stay together.
7. Draw the electron dot structure of each of these compounds.
a. CH4
b. C2H6
c. C3H8
8. Draw an electron dot structure for each of these molecules. Show all lone pairs.
a. HCl
b. H2CO
c. CF4
d. H2O
9. Draw an electron dot structure for each of these molecules. Show all lone pairs.
a. N2
b. CO2
c. C2H2
d. PH3
10. Draw an electron dot structure for each of these molecules. You may show bonding
pairs as dots or a line. Include all lone pairs. (There may be more than one possible
correct answer. Give just one.)
a. C3H8O
b. C2H4O
c. H2O2
d. C2H4Cl2
e. CH2Cl2
f. C2H7N
11. Predict which of these compounds has a stronger bond between the carbon atoms:
C2H6 or C2H2. Justify your answer.
12. For each of these bonds, indicate whether it is a polar bond or a nonpolar bond. If it is
a polar bond, show which atom has the little bit of positive charge and which atom has
a little bit of negative charge.
a. C-O
b. C-H
c. C-Cl
13. 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
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14. 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
15. How many electrons does each of these ions contain?
a. Fb. P3c. Sr2+
16. What is the name of each of these ions?
a. Fb. P317. Give the symbol for each of these ions.
a. potassium ion
b. iodide ion
c. Sr2+
c. calcium ion
d. sulfide ion
18. How many electrons does each of these ions contain?
a. potassium ion
b. iodide ion
c. calcium ion
d. sulfide ion
19. How many valence electrons does each of these ions contain?
a. potassium ion
b. iodide ion
c. calcium ion
d. sulfide ion
20. Give the formula for each of these polyatomic ions.
a. nitrate ion
b. sulfate ion
c. hydroxide ion
d. acetate ion
e. ammonium ion
21. Make a table of the atomic number and electronegativity 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?
When hydrogen played oxygen,
And the game had just begun,
Hydrogen racked up two fast points,
But oxygen had none.
Then oxygen scored a single goal,
And thus it did remain.
Hydrogen 2 and oxygen 1,
Called off because of rain.
"When Hydrogen Played Oxygen
anonymous
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