CHEMISTRY 132S FINAL EXAM REVIEW
Name:____________________________
____ Section: _______
Part 1: Significant Figures, Unit Conversions, and Matter
1) Convert the following to scientific notation:
a) 73
f) 0.0000843
b) 0.023
g) 0.00568
c) 6590
h) 416500
d) 178
i) 2156000
e) 458212
j) 0.587
2) Convert the following from scientific notation:
a) 6.3 x 10-7
f) 7.558 x 10-3
b) 5 x 106
g) 2.001 x 109
-4
c) 5.6 x 10
h) 2.66 x 104
d) 4.55 x 10-7
i) 8.5 x 10-1
2
e) 7.568 x 10
j) 2.556 x 10-2
3) Carry out the following conversions giving your answers in scientific notation:
a) 8.79 x 10-4 L to cm3
f) 1.56 μg to g
b) 5.68 m to cm
g) 2.5 L to mL
c) 117 mg to g
h) 6.72 x 10-7 kg to mg
d) 7.8 g to kg
i) 5.36 mL to L
e) 101.3 cm3 to m3
j) 736.2 nm to m
4) How many sig figs are in the following numbers?
a) 236 m
f) 6532.000000 g
b) 2000 people
g) 8500 L
c) (1000 m)/(1 km)
h) 5.226 x 10-12 g
d) 5026 g
i) 400 m2
e) 600.0 mL
j) 0.000023 cm
5) Convert the following to the temperature indicated.
a)115oF to Celsius
b) -14oF to Celsius
c) 19oC to Fahrenheit
d) -33oC to Fahrenheit
f) 23oF to Kelvin
e) 598K to Celsius
6) If the density of gold is 19.3 g/cm 3 and the density of water is 1.00 g/cm3 what volume of water would be
needed to be the same mass as a gold bar with the measurements: 5 cm x 4cm x 15 cm?
7) Calculate the volume of a sheet of plywood with the following dimensions: Length: 2.78 cm; Width: 11.3 m;
Thickness: 7.53 mm
8) How many seconds are there in a leap year?
9) A clock gains 0.050 seconds in one hour. How many minutes does the clock gain in 365 days?
10) The density of a substance is 23.7 mg/mL. What is the density in g/L?
11) A car with a maximum speed of 115 km/hr can travel how many meters per second?
12) Complete the following:
A) _____mm2 = 1 m2
B) _____km2 = 1 m2
C) _____cm2 = 1 mm2
D) _____cm2 = 1 mm2
13) Vioxx is a drug used to treat arthritis. If a patient takes one 125 μg tablet per day, how many milligrams of
Vioxx are in their 1 month (30 day) supply?
14) A prescription pain reliever contains 30 mg of Codeine per tablet. The package directions recommend taking
no more than 8 tablets in a 24 hour period. How many grams of Codeine per day is the maximum recommended
dose?
15) What state of matter is represented by each of the following?
a) ice
b) clouds in the sky
c) hydrogen in the sun
d) rock
e) air
f) vegetable oil
16) Classify each of the following as either a chemical change (primarily) or a physical change.
a) electrolysis of water
b) separating an alcohol-water mixture
c) formation of fog
d) burning wood
e) rusting iron
f) converting sand to glass
17) Draw a graph of temperature vs. energy showing the phase changes. Be sure to label all the phases, phase
changes, melting points, boiling points etc.
18) For each of the following write whether it is a mixture (M), a solution (S), or a compound (C).
a) soda pop
b) sugar
c) milk
d) muddy water
e) baking soda (NaHCO3)
f) pizza
g) bronze
19) Define the following:
a) solid
e) evaporation
b) liquid
d) freezing
c) gas
f) melting
d) plasma
g) condensation
h) sublimation
i) deposition
j) heat of fusion
k) heat of vaporization
20) Complete the following table for the states of matter; with one being the lowest and 3 being the highest.
State of matter
Temperature
rank (1-3)
Kinetic energy
rank (1-3)
Distance between
molecules rank (1-3)
Solid
Liquid
Gas
Part 2: Periodic Table, Bonding, and Nomenclature
1) Which atom’s radius is bigger: Bi or P; Rb or Sb? Why?
Which is bigger: Mg or Mg2+?
Which is bigger: Se or Se2-?
Which is more electronegative: Se or Ga; Cl or At?
Which has the greatest electron affinity: Y or Tc; He or Rn?
Intermolecular
forces rank (1-3)
2) Complete the following table:
Atom/Ion/
Isotope
39K+1
Atomic #
Mass #
Protons
Neutrons
Electrons
41Ca
69Ga+3
37Cl-1
18O
235U+4
3) Naturally occurring silver consists of 51.8% Ag-107 and 48.2% Ag-109. What is the expected average molar
mass of a sample of natural silver, expressed to 3 decimal places?
4) What are the long and short electron configurations for the following. Pick 2 and write the orbital configurations
for them.
a) P
b) Cl
c) Ar
d) F-1
e) S-2
f) He
5) Name at least one trend among each of the following periodic families:
a. Alkali Metals
b. Alkaline Earth Metals
c. Halogens
d. Noble Gases
6) If a noble gas could form a +1 ion, which of the noble gases would form a +1 ion most easily?
7) With respect to electrons, how does an ionic bond differ from a covalent bond?
8) Indicate whether the following compounds are ionic, non-polar covalent, or polar covalent. Explain.
a) NaCl
b) H2O
c) NO2
d) CS2
e) Al2O3
f) BF3
9) Why does a certain covalent compound have a distinct odor while a certain ionic compound has no detectable
aroma?
10) How many valence electrons are there in:
a) Si
b) K+1
c) Ne
d) O-2
e) H-1
f) N
11) Why are some solvents polar and some non-polar? Which would you use to dissolve salt?
12) Draw electron dot structures (Lewis Structures) for:
a) C
b) He
c) P
d) N
e) Al
13) Write the chemical formula for the following compounds:
A. chlorine tetroxide
B. trisilicon tetranitride
D. radium carbonate
E. hydrobromic acid
G. sulfurous acid
H. chromium(II) oxalate
J. dinitrogen pentoxide
K. tungsten(V) bromide
C. iron(III) hydroxide
F. disilicon hexaiodide
I. phosphoric acid
L. tin(II) bicarbonate
f) S
M. mercury(I) nitrate
P. beryllium oxide
N. copper(I) phosphate
Q. molybdenum(VI) iodide
14) Write the name of the following compounds:
A. CoF3
B. PBr5
E. HNO3
F. Sn(CN)2
I. Cu(NO3)2•6H2O
J. NH4NO3
M. V2O5
N. Ni3(PO4)2•8H2O
Q. CS2
R. W(CN)6
C. KMnO4
G. LiOH
K. N2S5
O. H3PO4
S. TaCl3
O. sulfuric acid
R. ammonia
D. FeC2O4
H. Na2HPO4
L. CuSO4
P. S4N2
T. Li2Cr2O7
Part 3: VSEPR Theory (Molecular Geometry and Polarity)
a) In the following table draw the correct Lewis structure, indicate the molecule type (ABE format), the
bond angle, molecular and electron pair geometry, indicate whether they are polar or nonpolar and
which intermolecular forces they possess. Also, if it applies, draw the resonance structures.
Molecule
Lewis
Structure
Type
(ABE
format)
Electron
Pair
Geometry
Molecular
Geometry
Bond
Angle
Polarity
And
Intermolecular
Forces
Resonance
Structures
NO2+
SO3
PO43H3O+
SeO2
Li2S
CHCl3
b) Rank the intermolecular forces from weakest to strongest:
Part 4: Chemical Equations
1) Balance the following equations.
2) Classify each reaction as one of: synthesis(S), decomposition (D), single replacement (SR), double
replacement (DR), or combustion (C).
_______ a) __Sr + __O2 → __SrO
_______ b) __C6H12O6 + __O2 → __CO2 + __H2O
_______ c) __H3PO4 + __KOH → __K3PO4 + __H2O
_______ d) __H2O→__H2 + __O2
_______ e) __Fe(HCO3)3 + __MgSe → __Fe2Se3 + __Mg(HCO3)2
_______ f) __Br2 + __KCl → __KBr +__ Cl2
Part 5: Mole Conversions
Convert Moles to mass and to particles as indicated.
a) Convert 36.5 g of Sodium sulfate to moles
b) How many particles are there in 3.5 moles of NaCl?
c) How much do 2.8 moles of silver nitrate weigh?
d) 4.5 x 10^23 molecules of sugar (C6H12O6) represents this many moles?
e) 4.5 g of aluminum sulfide contain this many particles of aluminum sulfide.
f) 5.7 x 10^25 molecules of chlorine tetroxide weigh this many grams.
Part 6: Percent Composition:
Calculate the percent of H2O, Ni, P, and O in Ni3(PO4)2•8H2O.
Part 7: Acids and Bases:
1. Definitions: Give the definitions for the following terms:
a. Arrhenius acid
b. Arrhenius base
c. Bronsted-Lowry acid
d. Bronsted-Lowry base
e. Lewis acid
f. Lewis base
g. Conjugate pair
h. Weak acid
i. Strong acid
j. Weak base
k. Strong base
2. Identify the conjugate acid base pairs in the following:
a. HClO2(aq) + H2O(l) ↔ H3O+(aq) + ClO-(aq)
b. H2SO3(aq) + H2O(l) ↔ HSO3-(aq) + H3O+(aq)
c. HSeO3-(aq) + H2O(l) ↔ H3O (aq) + SeO32-(aq)
3. Calculate the pH, [H3O+], pOH, or [OH-] as indicated:
a. The hydrogen ion concentration of a soft drink is 7.3 x 10-4M. What is the pH, pOH, and [OH-] of the
solution?
b. The hydroxide ion concentration of a solution is 5.6 x 10-8M. What is the pH, pOH, and [H3O+] of the
solution?
c. The pOH of a given solution is 8.76, what is its pH, [OH-], and [H3O+]?
d. The pH of a solution is 13.19. What is its [H3O+], pOH and [OH-]?
4. Neutralization problems:
a. 53.7 mL of a 0.100M HCl acid is needed to neutralize 80.0 mL of KOH. What is he molarity of the
KOH solution?
b. What is the molarity of a CsOH solution if 29.61 mL of a 0.2500M HCl is needed to neutralize 60.00
mL of the CsOH solution?