Applied Chemistry
Name ____________________________________
Final Review
Test Date _________________ Time ___________
Proctor ____________________ Rm ___________
Metric
1) Complete the following metric conversions.
a. 2.6 kg = ________________g
c. 0.45 daL = __________________hL
b. 5.0 g = _________________mg
d. 0.009 km = _________________dm
c. 32 mL=_________________ L
e. 1.04 m = ___________________cm
2) Calculate the density of a substance with a mass of 2.5 g and a volume of 15 mL. Show all work and units.
Matter and Energy
3) Classify each of the following as a physical (P) or chemical (C) change.
a. Cutting Magnesium
__________
b. Lead nitrate plus potassium iodide forms a yellow solid
__________
c. Melting lauric acid
__________
d. Grinding CuSO4 ∙ 5H2O
__________
e. Magnesium plus hydrochloric acid produces heat plus many bubbles.
__________
4) Answer the following questions regarding 2Ca3(PO3)2
a. Element or Compound ________________
b. Formula or Symbol
e. Number of P atoms
________________
f. Number of O atom
________________
g. Total number of atoms
________________
________________
c. What is the coefficient? _______________
d. Number of Ca atoms
________________
5) Count the number of atoms in each of the following.
a. BaAsO4 _______
b. Sr(ClO2)2 _______
c. 3 (NH4)2C2O4 _______
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6) Directions: Complete the following tables.
State
Shape (Definite or Indefinite)
Volume
(Definite or Indefinite)
Solid
Liquid
Gas
7) Directions: Complete the following tables.
Separation
Definition
Technique
Type of Mixture
to Separate
Example
Distillation
Evaporation
Chromatography
Magnetic
Method
Filtration
Solutions
8) Complete the following concentration problems.
a. What is the concentration of a solution with 20 g of sugar dissolved in 80 g of solution?
b. What is the concentration of a solution with 20 g of sugar dissolved in 80 g of water?
c. Salt is dissolved in water. Salt would be called the ___________ and water is called the
_______________.
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9) Use the solubility curve to answer the following questions:
a. Which substance's solubility is affected MOST by temperature?
________________________
b. Name 3 substances that decrease in solubility as temperature increases?
_________________________________________________________________________________
c. Which two substances have the same solubility at 29 °C?
_________________________________________________________________________________
d. What mass of NH4Cl in 100 g water can be dissolved at 60 °C?
________________________
e. What type of solution exists when 100 g of NaNO3 at 50 °C?
(saturated/unsaturated/supersatured)
________________________
Water
10) Define the following terms related to water treatment and wastewater treatment.
a) Water Treatment Plant
b) Wastewater Treatment Plant
c) Aquifer
d) Aquitard
e) Point Source
f) Area Source
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11) Complete the following chart:
Material
Pore size (small, medium, large)
Aquifer or Aquitard
Sand
Gravel
Clay
12) A gas station has a leak in an underground tank. The soil around the tank becomes contaminated. Is this an
example of an area source or point source of pollution? Explain your answer.
Atomic Structure
13) The charge of an electron is _______________.
a. positive
b. negative
c. neutral
d. zero
14) What is the mass number of chlorine-35?
a. 12
b. 17
c. 18
d. 35
15) How many protons are in chlorine-35?
a. 12
b. 17
c. 18
d. 35
16) In a neutral atom, the number of ___________________ are equal.
a. protons and neutrons
c. neutrons and electrons
b. protons and electrons
d. protons and nuclei
17) An atom becomes an ion when it gains or loses __________________.
a. protons
c. electrons
b. neutrons
d. nuclei
18) When a chlorine atom gains one electron, its charge will become
a. positive.
b. negative.
c. neutral.
d. zero.
19) Carbon-12 and Carbon-14 are called _______________.
a. ions
b. cations
c. anions
d. isotopes
20) An atom's mass number includes the number of _____________________.
a. protons
c. protons and neutrons
b. neutrons
d. protons and electrons
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21) Complete the following chart:
Complete
Isotopic
Symbol
Atomic
Number
Mass
Number
13
27
+
# of p
11
34
12
6
41
20
79
C
# of e
10
-
# of n°
Charge
Cation
or
Anion
0
------
12
-2
0
-----
Ca 2
Nuclear
22) Define the following terms related to nuclear energy.
a. Radiation: _______________________________________________________________________
b. Fission: _________________________________________________________________________
c. Fusion: _________________________________________________________________________
d. Proper nuclear waste disposal: _______________________________________________________
e. Half-Life: _______________________________________________________________________
23) Show all work for the following half-life problems:
a. The half-life of cesium-137 is 30.2 years. If the initial mass of a sample of cesium-137 is 1.00 kg,
how much will remain after 151 years.
b. With a half-life of 28.8 years, how long will it take for 1g of strontium-90 to decay to 0.125g?
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Global Warming
24) Name all five greenhouse gases: 1) ___________________________ 2) ___________________________
3) ___________________________ 4) ___________________________ 5) ________________________
25) How does deforestation contribute to global warming? __________________________________________
Periodic Table
26) List the properties of metals: _______________________________________________________________
_______________________________________________________________________________________
27) List the properties of nonmetals: ____________________________________________________________
_______________________________________________________________________________________
28) As you move down a family, the atomic radius ________________________.
29) As you move across a period, the atomic radius ________________________.
30) Circle the larger atomic radius in each pair.
Ba or Mg
Sr or I
31) Circle the groups of elements (listed as atomic numbers) that have similar chemical properties.
3, 4, 5
81, 82, 83
16, 17, 18
8, 16, 34
32) Classifying elements - Identify the following elements as metal, nonmetal or metalloid.
a. phosphorus __________________
e. nickel
__________________
b.
lithium
__________________
f.
atomic number 52 ______________
c.
arsenic
__________________
g.
atomic number 64 ______________
d.
krypton
__________________
h.
atomic number 1 ______________
33) Complete the following chart:
Family/Group Name
Number of
Valence Electrons
Potassium
Calcium
Nickel
Fluorine
Xenon
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Bonding and Formula Writing
34) What is the difference between a covalent bond and an ionic bond? ________________________________
_______________________________________________________________________________________
35) Write the names or formulas for the following ionic compounds:
a. MgCl2
______________________________________
b. Al2O3
______________________________________
c. SrS
______________________________________
d. calcium oxide
______________________________________
e. potassium sulfide
______________________________________
36) Write the names or formulas for the following molecular compounds:
a. CO
______________________________________
b. SO3
______________________________________
c. N2O5
______________________________________
d. carbon dioxide
______________________________________
e. tetraphosphorus trisulfide
______________________________________
Chemical Reactions
37) List the signs of a chemical reaction: 1) __________________________ 2) __________________________
3) ___________________________ 4) ___________________________ 5) ________________________
38) Balance and Classify each equation.
a. _____________
____ Ca(OH)2 +
b. _____________
____ Al
c. _____________
____ Fe2O3
d. _____________
____ KClO3
e. _____________
____ CH4
+
____ H2O
____ O2
→
____ Al2O3
____ C
→
____ Fe
+
→
+
→
____ HCl
____ KCl
____ O2 →
+
+
+
____ CaCl2
____ CO
____ O2
____ CO2
+
____ H2O
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39) Which of the following is balanced correctly?
a.
O2 →
Na +
Na2O
8O2 →
b. C5H12 +
O2 →
c. 2H2 +
d. Na2SO4 +
5CO2 +
6H2O
H2O
2CaCl2 →
CaSO4 +
2NaCl
40) Which of the following is NOT balanced correctly?
a. Br2 +
2NaI →
2NaBr +
I2
b. Zn +
c.
2HCl →
ZnCl2 +
3O2 →
2H2S +
d. Ba(NO3)2 +
H2
2H2O +
Na2SO4 →
2SO2
BaSO4 +
NaNO3
41) Complete the following chart:
Characteristics
Litmus Test
pH range
Ions produced
Acid
Base
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