Name
Instructions – READ CAREFULLY!
This exam is schedule for 150 minutes I cannot give you extra time. You are free to leave if you finish.
In multiple part problems, points awarded will not be penalized for incorrect answer on previous parts, so simply move on if you get stuck on one part . If you need to, make up an answer for the previous part. Always neatly show work for partial credit.

The exam is worth 200 points.

You are only required to complete the first section of the exam.

On subsequent sections (2-4), you must clearly indicate whether you want the section to be evaluated.

All sections th at you mark “Yes, include this section in my grade” will be averaged with Section
1 to be included in the final 200 points.

Points earned in Sections 2-4 will be awarded as bonus points for Exams 1-3, respectively.
Bonus points will only be awarded if you mark “yes” for that particular section.
 A score of “A” on this exam automatically gives you a final course grade of “A”. This is only possible if you complete all four sections of the exam.

Section 2 Yes, I would like this section to be graded
1. What is the electron configuration of an element with 33 protons and 42 neutrons? (3 pts.)
2. Two of the following elements have exactly three unpaired electrons. Identify these two elements and justify your answer by showing the appropriate electron orbital diagrams. (8 pts)
3. Complete each of the following conversions: (8 pts.) a. 5.286 mg = _______ kg b. 1.0485 s 2 = _______ ns 2 c. 2.543
 m 3 = _______ m 3

4. Chlorine has two naturally occurring isotopes. Based on the information given in the following table, calculate the percent abundance and exact mass of the 35 Cl isotope. (7 pts.)
Cholrine-35
24.22
Chlorine-37 36.966
5. The density of liquid mercury is 13.534 g mL -1 . What mass of this liquid occupies exactly 1 L?
Report your answer in SI units. (8 pts.)

Section 3 Yes, I would like this section to be graded
1. Consider the following molecules. (10 pts.)
H
2
Se H
2
S H
2
O a. Order them by increasing boiling temperature.
_______
CH
3
OCH
3
< _______ < _______ < _______
H
<
2
Te
_______ b. Justify the trend you determined in part a.
2. Draw a Lewis structure for each of the following: (10 pts.)
CO
3
-2 CH
2
O CH
3
OH
2
+

3. For each of the compounds in problem 2, determine the shape and hybridization of all central atoms. (3 pts.)
2
3
-2
3
2
+
4. For the ionic compounds beolw, identify which atoms carry the charge(s). (2 pts.)
CO
3
-2 CH
3
OH
2
+
5. How much energy is necessary to heat 25 g of solid acetone at 94.8 ºC to 51.3 ºC? (10 pts.)
T b
(˚C)
56.05
T m
(˚C)
-94.8

H fusion
(J/g)
97.97

H vaporization
501.0
(J/g)
C (liquid)
J / (g ˚C)

2.175
C (gas)
J / (g ˚C)

1.291

Section 4 Yes, I would like this section to be graded
1. In each case, calculate the moles the indicated compound. (2 pts. each) a. 15.6 g of carbon dioxide. b. 43.2 L of carbon dioxide at STP. c. How many moles of CO
2
contain exactly 4.32 x 10 48 atoms of oxygen?
2. Write a balanced double replacement reaction between Iron (III) acetate and ammonium phosphate . (5 pts.)
3. 14 grams of a compound decomposes and produces 3.82 g of carbon and 10.18 g of oxygen.
Determine the empirical formula of this compound. (6 pts.)

4. Consider the combustion of nonane (C
9
H
20
). a. Write a balanced chemical equation for this reaction. (3 pts.)
_____ C
9
H
20
(l) + ____ O
2
(g)  _____ CO
2
(g) + _____ H
2
O (l) b. If 18 moles of nonane (C
9
H
20
) react, how many moles of oxygen are consumed? (3 pts.) c. Determine the % yield if 15 g of liquid water is collected after the combustion of 21.37 g of nonane. (7 pts.) d. Using the percent yield determined in part c, calculate the volume of CO
2
gas produced at
STP. Use 50% yield if you did not answer part c. (4 pts.)

Section 1 – You must complete all of this section.
1. Please assign oxidation states to Bromine in each of the following compounds: (2 pts. each)
Compound
Oxidation
State of Br
Br
2
NaBrO NaBrO
2
NaBrO
3
NaBrO
4
NaBr
2. Identify all water soluble compounds
– solubility rules are available at the back of the exam. (5 pts.)
C
8
H
18
CH
3
OH AgNO
3
AgCl (NH
4
)
3
PO
4
Ca(OH)
2
Lead iodide Manganese (II) sulfide
3. Determine a balanced net ionic equation for this reaction: (3 pts.)
AgNO
3
+ FeCl
3
 AgCl + Fe(NO
3
)
3
Silver acetate
4. Consider the following reaction: (10 pts.) a. Please identify what element is being oxidized and what element is being reduced. b. Please identify the oxidizing agent and the reducing agent.
Cr (s) + Cl
2
(g)  CrCl
2
(aq) + HCl (aq)
___________ is being oxidized.
___________ is being reduced.
___________ is the oxidizing agent.
___________ is the reducing agent.

5. Balance each half reaction and state whether it is an oxidation or reduction. (10 pts.)
Cr(s) + NO
3
-1  Cr(NO
3
)
2
HBrO
4
 Br
2
6. Please balance this using the half reaction method. (15 pts.)
MnO
4
+ HCl  Mn + Cl
2

7. How many grams of bromide are present in each of the following solutions? (10 pts.)
5 L of 5 M NaBr
5 mL of 500 mM MgBr
2
8. Calculate the volume of 3.6 M MgCl
2
that is needed to form 1.4 moles of AgCl. (10 pts.)
MgCl
2
+ 2 Ag  2 AgCl + Mg
9. Determine the concentration of sodium chloride (in molar units) is 35 mL of H
2
O is added to 59 mL of 3.8 M NaCl. (10 pts.)

10. CO
2
is bubbled through 3.8 L of 0.185 M Ni
2
(Cr
2
O
7
) according to the following chemical reaction.
Calculate: (15 pts.)
2 Ni
2
(Cr
2
O
7
) (aq) + CO
2
(g)  4 Ni(CrO
4
) (s) + C (s) ***this reaction is balanced*** a. The volume of CO
2
gas at STP that is required to completely react with the Ni
2
(Cr
2
O
7
). b. The mass of carbon that is produced.

Bonus:
Balance the following redox reaction. (up to 10 pts)
Ni(s) + CO
2
(g) + Cr(NO
3
)
2
(aq)  Ni(CO
3
)
2
(s) + Cr
3
N
2
(s) + NO
2
(g)

Equations of interest:
PV=nRT 𝑅 = 0.08206
𝐿 𝑎𝑡𝑚 𝑚𝑜𝑙 𝐾
Avagadro’s number = 6.022 x 10 -23 per mol

E = q = mc

T
+
2+
2
2+
2+
2+
2+
2+
Insoluble Compounds
Compounds Containing
Carbonate
Phosphate
Sulfide
Hydroxide
Notable Exceptions
Group IA and NH
4
+
Group IA and NH
4
+
Group IA, IIA, and NH
4
+
Group IA, NH
4
+
, Ca
2+
, Sr
2+
, Ba
2+