Final Review
Supplemental Instruction
Iowa State University
Leader:
Course:
Instructor:
Date:
Kia
CHEM 177
Kingston
December 8th, 2016
Final exams: 2 hours, 70 questions
Chapters 1-4; Basic concepts, stoichiometry, solution chemistry
Practice
1. What is the concentration of nitrate ion in a 425 mL solution containing 32.0 g of
Mg(NO3)2 (M=148.3g/mol).
2. What is the difference between an intensive and extensive property? Give an example of
each.
3. Two students count the grains of uncooked rice in a small cup. This measurement was
repeated four times by both students with the following results: Mark = 265, 263, 262,
266 and Luke = 250, 242, 270, 278. If the actual number of grains is 260, which student
is more accurate, which is more precise?
4. Naturally occurring rubidium consists of ONLY two isotopes. One of the isotopes
consists of atoms having a mass of 84.912 amu; the other of 86.901 amu. What is the
percent natural abundance of the heavier isotope? (MM of Rb = 85.47)
5. Name or give the appropriate formula for the following
a. Lithium Acetate
d. Vanadium (V) oxide
b. AlCl3
e. Silicon tetrafluoride
c. CoBr2
f. P2O5
6. Balance the following equations
a. __ Ba3N2 + __ HF  __ BaF2 + __ NH3
b. __CaCl2 + __ Na3PO4  __ Ca3(PO4)2 + __ NaCl
c. __ NH3 + __ O2  __ NO + __ H2O
7. Of the listed molecules, circle the strong electrolyte(s), underline the weak electrolyte(s),
and square the nonelectrolyte(s).
H2O NaOH CH3COOH HF HCl
8. What is the oxidation number of Re in Mg(ReO4)2
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Chapters 5-7; Thermodynamics, electronic structure of atoms, periodic trends
Practice
1. A small “coffee cup” calorimeter contains 110 g of H2O at 22.0 °C. A 100 g sample of
lead is heated to 90.0 °C and then placed in the water. The contents of the calorimeter
come to a temperature of 23.9 °C. What is the specific heat of lead? Specific heat of
water is 4.184 J/g*C
2. Write the balance equation that is associated with ΔH°f(NaOH(s))
3. What is the value of the quantum number l for a 5p orbital?
4. Write the electron configuration and determine how many unpaired electrons a groundstate gas phase Mn2+ ion has.
5. In a hydrogen atom, which transition requires the greatest input of energy?
a. n=7  n=3
c. n=3  n=7
b. n=2  n=1
d. n=1  n=2
6. In the Lewis structure for the selenite ion, SeO32-, how many lone pairs are around the
central atom?
7. Write the set of quantum numbers (n, l, ml, ms) that correspond to a valence electron in a
neutral atom of arsenic (As).
8. The ΔH°f of MgO is -602 kJ/mol. When 20.15 g MgO is decomposed at constant
pressure according to the equation below, how much heat will be transferred? Is it
released or absorbed?
2 MgO(s)  2 Mg(s) + O2(g)
9. A system consists of a gas contained in a thin balloon. If the balloon deflates as the
temperature of the gas changes from 90°C to 25°C, then
a. Heat is transferred out of the system and work is done on the system.
b. Heat is transferred out of the system and work is done by the system.
c. Heat is transferred into the system and work is done on the system.
d. Heat is transferred into the system and work is done by the system.
10. Which way do each of the following trends increase on the periodic table (up/down the
column, and left or right across the row)
a. Ionization energy
b. Effective nuclear charge
Chapters 8-9; Geometry and bonding
Practice
1. What is the geometry of the chlorate ion, ClO3-?
2. Determine the number of sigma and pi bonds in the following molecules
a. PF3
b. NH4+
c. C2H2
d. CO323. Draw the following Lewis structures, state the molecular geometry, and label the bond
angles of the following compounds
a. SiCl4
b. NH3
c. TeCl4
4. List the following in order of increasing lattice energy: LiCl, LiBr, CaO, SrO
5. Which of the following possess delocalized pi electrons (may be more than one)?
a. CH2Cl2
b. OCN-
c. N2O
6. Of the following, circle those that are polar, underline ionic, and square the nonpolar
H2O NaCH3COO CCl4 XeF4
Chapter 10; Ideal gas
Practice
1. A 3.0 L sample of helium gas is stored in a rigid, sealed container at 25 deg. C and 1.0
atm pressure. The temperature is increased to 125 deg. C. What is the new pressure of the
gas?
2. A mixture of 0.50 mol of H2 gas and 1.3 mol of Ar gas is in a sealed container with a
volume of 4.82 L. If the temperature of the mixture is 50.0 °C, what is the partial pressure
of H2 in the sample?
3. At constant temperature and pressure, 5.0 L of SO2 is combined with 3.0 L of O2
according to the equation listed below. After SO3 formation is complete, what is the
volume of the mixture?
4. If the density of a gas is 0.08987 g/L at STP conditions, what is its molar mass?
5. A gas behaves ideally at ______ temperatures and ______ pressures.
6. Which gas will diffuse faster; Ne or Kr? Why?
Chapter 11; Intermolecular forces
Practice
1. Which substance has the highest normal boiling point?
a. CH3Cl
b. CH3Br
c. CH3I
d. CH4
e. CH3OH
2. In liquid SO2, what intermolecular forces are at work? (ion-ion, ion-dipole, dipole-dipole,
dispersion)
3. Why does it take more energy to take a substance from a liquid to a gas than from a solid
to a liquid?
4. Would water boil at a lower or high temperature at the bottom of the Grand Canyon?
(elevation = 1850 ft above sea level) Why?
5. Describe the difference between adhesive forces and cohesive forces