Download Final review free response ch 1-4

Leader: Sara
Course: Chem 177
Instructor: Bonaccorsi
Date:
REVIEW FOR FINAL
Supplemental Instruction
Iowa State University
Chapter 1
 Difference between atom, element, compound, molecule, mixture, pure substance
 Identify Solids, Liquids, and Gases, also in context with periodic table
 Physical versus chemical properties and changes. Intensive versus extensive
 Unit Conversion
 Density
 Significant Figures
 Precision versus accuracy
1. Label the following as heterogeneous, homogeneous solution or pure substance.
If it is a pure substance is it an atom or a compound?
a. Koolaid
b. Snickers Blizzard
c. O3
d. Li
e. CH3
f. Ni
g. A nickel coin
2. Are the following physical or chemical properties? Also label the intensive ones.
a. Color
b. Reactivness
c. Boiling point
d. Density
e. Flammability
f. Molarity
3. If you have 37 x 10-5 Mg (Mega grams) and 104 mL of a solution, what I the
density?
4. How long is the pencil?
1 in
2in
3in
4in
5. Calculate the following calculations?
a. 5.52 + 4.1 + 3.238
b. 3.3 x 78.66
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Chapter 2
 Dalton’s Atomic Theory and Laws of Chemical Combinations (mass, composition,
proportions)
 Proton versus Neutrons versus Electrons
 Percent abundance, and mass spectrometry
 Periodic trends (diatomic, metals, nonmetals, metalloids, cations versus anions)
 Ionic (transferring of electrons) versus covalent (shared electrons)
 Naming: ionic, covalent, ions (oxy-ions), acids (binary and oxy-acids)
1. Fill in the following table
Symbol
Protons
Neutrons
Electrons
Net Charge
27Al3+
O2-
Kr
48
8
17
18
18
0
2. Name the following compounds or give the formula
a. Silver Bromide
b. Cobalt (III) Oxide
c. Lithium Iodinde
d. Lead (II) Nitride
e. Al(CN)3
f. SnSe2
g. Cu3P
h. NH4Cl
i. Diphosphorus Pentoxide
j. Carbon tetrabromide
k. Dinitrogen trioxide
l. N2O
m. NI3
n. CCl4
3. Fill in the tables:
\
4. How many lines on a mass spectroscopy would N2O give? Also find the molar
mass of Oxyen.
Isotope Atomic Mass
14N
14.0031
15N
15.0001
Abundance (%)
99.632
0.368
Isotope
16O
17O
18O
Abundance (%)
99.757
0.038
0.205
Atomic Mass
15.9949
16.9991
17.9992
Chap 3
 Balancing Equations: Conservation of mass and atoms
 What drives a chemical reaction (precipitating a solid, evolution of a gas, formation
of a nonelectrolyte (H2O)
 Combination, Decomposition, Combustion
 Moles versus mass versus moleculesmoving between units
 Stociometry, limiting reagents, and percent yield
1. Write the empirical and molecular formula for the following molecule: 9 Carbons,
6 Bromines, 3 Oxygens, and 9 Hydrogens
2. Complete and balance the following reactions:
a. Combination
___ H2 + ___ F2 
b. Decomposition
___ B2O3 
c. Combustion
___ C4H10

3. Balance the following equations:
a. __H2SO4 + ___ HI  ___H2S + ___ I2 + ___H2O
b. ___FeS2 + ___ O2  ___Fe2O3 +___ SO2
c. ___Al + ___FeO  ___Al2O3 +___Fe
d. ___K + ___Br2  KBr
e. ___P4 + ___O2  P2O5
f. ___C7H16 + ___O2  ___CO2 + ___H2O
g. ___C3H5OH + ___O2  ___CO2 + ___H2O
4. Write and balance the following reactions:
a. Zinc Carbonate can be heated to form Zinc Oxide and Carbon Dioxide
b. When Iron and water are left to sit, hydrogen gas is released and Iron (III)
Oxide forms.
5. If you have 4 g NaOH, and 10 g HBr, what is the limiting reagent and how much
salt is produced? In lab if you produce1 g salt, what is the percent yield?
6. How many moles of Al atoms are needed to combine with 1.58 mol of O atoms to
make aluminum oxide, Al2O3?
Chapter 4
 electrolytes versus nonelectrolytes, strond versus weak, strong acids and bases
 Molarity, dilution
 Precipitate
 Acid/Base (neutralizations) titrations, limiting reagents for aqueous solutions.
 REDOX oxidation numbers, LEO goes GER (OIL RIG)
1. Complete the molecular and write the complete ionic, and net ionic equations for
the following reactions, if a reaction will not occur say NO REACTION
a. ___Li2CO3 (aq) + ___Co(C2H3O2)2 (aq) 
b. ___Fe(NO3)3 (aq) + ___K2S (aq) 
c. ___Pb(NO3)2 (aq) + ___Li2SO4 (aq) 
2. What are the strong acids?
3. Assign Oxidation states to the following equations and tell what is being oxidized
and what is reduced?
a. Zn + 2HCl -> Zn2+ + H2 +2Cl-
b. 4 Fe + 3 O2 → 2 Fe2O3
c. C6H12O6 + 6 O2 → 6 CO2 + 6 H2O
4. You are performing a titration with HCl and Ba(OH)2
a. You start with 10 g HCl and mix it with 10 mL of water, what is the
concentration?
b. If you want to dilute it to .01 M, how much water must be added?
c. If you tritate that with 25 mL of unknown Ba(OH)2 what is the
concentration of that unknown?
d. How much H2O is produced?