11U -- Unit 1--Matter—Practice Note: this sample test does not reflect length, weight and
necessarily every topic and type of question that will be on the unit test. It should not be your
only study tool, but rather used in conjunction with class notes, textbook and other resources.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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1. The particle that has the smallest mass is the
a. electron
d. nucleus
b. proton
e. ion
c. neutron
2. The element found in the periodic table in Group 6 and Period 4 is
a. hafnium, Hf
d. gadolinium, Gd
b. selenium, Se
e. chromium, Cr
c. lithium, Li
3. Which of the following matches of group number and common name is incorrect?
a. Group 7 - transition metals
d. Group 2 - actinides
b. Group 2 - alkali earth metals
e. Group 18 - noble gases
c. Group 17 - halogens
4. A nonmetal in Period 6 is
a. astatine
d. radon
b. iodine
e. rubidium
c. polonium
5. The properties of elements repeat periodically if they are arranged by
a. atomic mass
d. number of neutrons
b. atomic charge
e. number of electrons
c. atomic number
6. The mass listed for each element in the periodic table is
a. the mass of all of the isotopes of the element combined
b. the mass of the average number of neutrons in all of the isotopes of the element
c. the average of the atomic masses of all of the isotopes of the element
d. the exact mass of the protons and neutrons in the most common isotope of the element
e. the weighted average of the atomic masses of all of the isotopes of the element
7. Why does atomic radius decrease from left to right in a period?
a. Nuclear charge increases from left to right in a period.
b. Nuclear charge decreases from left to right in a period.
c. The number of energy levels increases from left to right in a period.
d. The number of energy levels decreases from left to right in a period.
e. The number of electrons decreases from left to right in a period.
8. Which of the following would have the highest electron affinity?
a. potassium
d. oxygen
b. helium
e. carbon
c. fluorine
9. Electronegativity is derived from
a. ionization energies
d. all of the above
b. electron affinity
e. none of the above
c. reactivity
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____ 10. Elements X and Y are in the same chemical family. Element X has a first ionization energy of 7.646 eV.
Element Y has a first ionization energy of 5.695 eV. Which is more reactive?
a. X
b. Y
c. They are equally reactive.
d. not enough information
e. X will be more reactive provided it reacts with another member of its family.
____ 11. Binary ionic compounds
a. contain two ions with charges of 2+ and 2–
b. are formed from the combination of two nonmetal ions
c. are composed of only two kinds of monatomic ions
d. contain a transition metal cation
e. contain double bonds
____ 12. The IUPAC name for P2I4(s) is
a. phosphorus iodide
d. phosphorus pentaiodide
b. diphosphorus tetraiodide
e. dipotassium tetraiodide
c. tetraphosphorus diiodide
____ 13. The chemical formula for iodine pentafluoride liquid is
a. IF5(l)
d. I2F5(l)
b. I5F(l)
e. I5F
c. I5F5(l)
____ 14. Hydroselenic acid is a very toxic substance. Its chemical formula is
a. HSe(aq)
d. H2SeO3(aq)
b. H2SeO2(aq)
e. H2SeO4(aq)
c. H2Se(aq)
____ 15. A student records the following evidence in a lab book.
Unknown Substance
Pure State
Solubility in Water
Solution Conductivity
I
solid
high
low
II
solid
low
low
III
solid
high
none
IV
solid
high
high
Which of the substances shown in the table above is most likely an ionic compound?
a. I
d. IV
b. II
e. none of the above
c. III
____ 16. The IUPAC name for AgNO3(s) is
a. silver(I) nitrite
d. silver nitrogen trioxide
b. silver nitrate
e. silver(II) nitrite
c. silver(I) nitrate
____ 17. What is the formula for zinc chloride?
a. ZnCl(s)
d. Zn1Cl2(s)
b. ZnCl2(s)
e. Zn2Cl1(s)
c. Zn1Cl1(s)
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____ 18. What is the formula for aqueous hydrogen fluoride?
a. HFl(aq)
d. HF
b. HFO3(aq)
e. H2F(aq)
c. HF(aq)
____ 19. Which one of the following formulas is incorrect?
a. Cu2O
d. Ba(HCO3)2
b. NaOH
e. ZnCl3
c. CO
____ 20. A compound composed of sodium, sulfur, and oxygen would be named
a. sodium peroxide
d. sodium sulfate
b. sulfuric acid
e. sodium hydroxide
c. sodium sulfide
____ 21. If the name of a chemical compound ends in "ide", the compound is
a. acidic
d. an oxide
b. binary
e. none of the above
c. basic
____ 22. In which of the following pairs of ions do both names end in "ate"?
a. ClO3–, ClO2–
d. CO32–, SO42–
–
–
b. NO3 , NO2
e. SO32–-, MnO4–
2–
–
c. CO3 , SO3
____ 23. If XF2 is the correct formula for a metallic fluoride, then the formula for the oxide of X is
a. X2O
d. XO2
b. XO
e. X2O2
c. XO4
____ 24. Galvanized steel is an effective method of corrosion prevention for all of the following reasons except
a. Zinc is a more active metal than iron.
b. Zinc is less electronegative than iron.
c. Zinc forms a protective layer on the iron.
d. Zinc is a relatively hard metal compared to iron.
e. A spontaneous cell is created when the zinc coating is broken.
____ 25. A sacrificial anode for the protection of iron is
a. a metal that oxidizes less easily than iron
b. a metal with a lower electronegativity than iron
c. a metal that oxidizes more easily than iron
d. any substance that is connected to an anode of a battery
e. an inert electrode
____ 26. The reaction of silver nitrate with zinc would be classified as a
a. combustion reaction
d. decomposition reaction
b. synthesis reaction
e. single displacement reaction
c. double displacement reaction
____ 27. Which of the following always indicates that a chemical reaction has taken place?
a. production of a gas
d. appearance of a new substance
b. absorption of heat
e. production of heat
c. change in colour
____ 28. Classify the following reaction: Mg(OH)2 + 2HNO3  Mg(NO3)2 + 2H2O
a. combustion
d. single displacement
b. synthesis
e. double displacement
c. decomposition
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____ 29. Engines are often constructed with aluminum alloys rather than pure aluminum because
a. alloys are lighter
b. pure aluminum is flammable
c. alloys are stronger
d. pure aluminum is easily worn away by corrosion
e. pure aluminum is too expensive
____ 30. Which gases cause acid rain?
a. nitrogen oxides
d. all of the above
b. sulfur oxides
e. none of the above
c. carbon dioxide
Short Answer
31. Complete the table below.
Element
name
fluorine
Element
symbol
Atomic
number
Group
number
Family
name
Period
number
noble gas
3
Metal or
nonmetal
Ba
32. State one characteristic physical property and one characteristic chemical property of the noble gas family.
33. What is electronegativity?
34. Elements A, B, and C are in the same chemical family. Element A bursts into pink flames when it dissolves in
water. Element B sizzles slightly when it dissolves in water. Element C sizzles and sometimes burns when it
dissolves in water. How would A, B, and C be arranged in the periodic table? Of the three, which would most
likely be highest in the group? Which would most likely be lowest?
35. Which element has the smallest atomic radius?
36. The electronegativity of magnesium, Mg, is 1.2. Would you expect aluminum's electronegativity to be higher
or lower?
37. For a science fair project, a student wants to design a simple device for removing certain gases from polluted
air. He knows that polar molecules dissolve well in water, so he bubbles polluted air through a jug of water to
remove unwanted gases. For his project, the student uses air containing the following gases:
1. N2(g)
5. CH4(g)
2. O2(g)
6. OCl2(g)
3. HF(g)
7. C3H8(g)
4. NH3(g)
8. CH3OCH3(g)
List the gases that will dissolve by writing down their corresponding numbers.
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38. For a science fair project, a student wants to design a simple device for removing certain gases from polluted
air. He knows that polar molecules dissolve well in water, so he bubbles polluted air through a jug of water to
remove unwanted gases. For his project, the student uses air containing the following gases:
1. N2(g)
5. CH4(g)
2. O2(g)
6. OCl2(g)
3. HF(g)
7. C3H8(g)
4. NH3(g)
8. CH3OCH3(g)
List the gases that will form hydrogen bonds with water by writing down their corresponding numbers.
39. Write a sentence to describe the theoretical structure of ionic compounds.
40. Briefly describe how polar covalent bonds occur.
41. Explain, in your own words, how and why ionic bonding occurs.
42. Draw the electron dot diagram for carbon monoxide and carbon dioxide.
43. Use electron dot diagrams to explain why hydrogen and nitrogen are diatomic elements.
44. Use an electron dot diagram to explain why ammonia is a polar molecule.
45. Predict the products and write a balanced chemical equation for the following chemical reaction:
Aqueous calcium chloride is added to a small amount of solution suspected to contain sodium phosphate.
46. Predict the products and write a balanced chemical equation for the following chemical reaction:
Potassium metal is added to water.
47. Predict the products and write a balanced chemical equation for the following chemical reaction:
Hydrochloric acid is neutralized by a magnesium hydroxide suspension.
48. What are the products of the reaction between zinc and hydrochloric acid?
49. Complete the following chemical reaction equation, including states of matter and balancing:
FeCl3(aq) + Zn(s) 
50. Complete the following chemical reaction equation, including states of matter and balancing:
C2H5OH(l) + O2(g) 
Essay
51. Producing electricity with nuclear power is still debatable. In a brief essay, give two reasons why we should
continue to use nuclear power and two reasons why we should not.
52. The names of pharmaceutical drugs are generally given trade names. Should pharmaceutical companies be
required to state the IUPAC name for the active ingredient? Why or why not?
53. Imagine you live in a poor community that has discovered gold deposits in its land. To recover gold from
rock, the ore is ground and mixed with lime. This mixture is then reacted with cyanide. The gold is then
absorbed by carbon. A gold mine can do wonders for the local community, but the risk of a cyanide spill has
some citizens up in arms. Decide if you think a gold mine and refinery should be constructed and support
your position.
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11U -- Unit 1--Matter--Practice
Answer Section
MULTIPLE CHOICE
1.
A
2.
E
3.
D
4.
A
5.
C
6.
E
7.
A
8.
C
9.
10.
11.
12.
13.
14.
15.
16.
D
B
C
B
A
C
D
B
17.
18.
19.
20.
21.
22.
23.
24.
B
C
E
D
B
D
B
D
25.
26.
27.
28.
29.
30.
C
E
D
E
C
D
SHORT ANSWER
31.
Element
name
Element
symbol
Atomic
number
Group
number
Family
name
Period
number
Metal or
nonmetal
fluorine
F
9
17
halogens
2
nonmetal
barium
Ba
56
2
alkali earth
metals
6
metal
argon
Ar
18
18
noble gas
3
nonmetal
32. Noble gases have extremely low boiling points. Thus, they are gases at SATP. They are also chemically
unreactive.
33. Electronegativity is a measure of an element's ability to attract electrons.
34. Element B would be highest and element A would be lowest. Element C would lie in between.
35. helium
36. higher
37. 3, 4, 6, and 8
38. 3 and 4
39. Theoretically, ionic compounds consist of very large numbers of positive and negative ions attracting one
another in a regular geometric three-dimensional arrangement called a crystal lattice.
40. When two nonmetals react with each other, they try to form stable octets. To do this, they share electrons. If
one atom is much more electronegative than the other, they will not share the electrons equally. Thus, one end
of the bond is more negative than the other and the bond is polar.
41. Atoms are more stable when they have eight valence electrons. Nonmetals will try to gain electrons to form a
stable octet and metals will try to give away electrons to form a stable octet. Thus, metals give electrons to
nonmetals. Subsequently, the two oppositely charged ions are attracted to one another.
42.
carbon dioxide
carbon monoxide
43. To obtain a full valence shell, hydrogen atoms will form covalent bonds with one another. Nitrogen will do
the same with itself, in order to give each atom a stable octet.
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44. The following diagram shows the electron dot diagram for ammonia. The high electronegativity of nitrogen
compared to hydrogen causes the electrons to spend more time with the nitrogen, thus causing a partial
negative charge at the nitrogen atom and a partial positive charge at the hydrogen atoms.
45.
46.
47.
48.
49.
50.
3CaCl2(aq) + 2Na3PO4(aq)
Ca3(PO4)2(s) + 6NaCl(aq)
2K(s) + 2HOH(l)
H2(g) + 2KOH(aq)
2HCl(aq) + Mg(OH)2(s)
2HOH(l) + MgCl2(aq)
hydrogen gas and zinc chloride
2FeCl3(aq) + 3Zn(s)  3ZnCl2(aq) + 2Fe(s)
C2H5OH(l) + 3O2(g)  2CO2(g) + 3H2O(g)
ESSAY
51. Pros
-Amounts of radioactive waste are small compared to waste produced by combustion reactions.
-No greenhouse gases are produced.
-Very little fuel is necessary to produce large amounts of electricity.
Cons
-There is a risk of leakage of radioactive tritium.
-Waste with extremely long half-lives are produced.
-There is a risk of a nuclear accident.
52. Pros
-It is easier for consumers to do their own research on the chemicals used in the drugs.
-It is easier for pharmacists to determine the contents of the drugs and advise the consumer or doctor.
Cons
-It might be very easy for other companies or organizations to copy the drugs.
53. Pros
-Apply modern methods to contain environmental damage.
-Community can force mining company to repair land when the project is complete.
-Community can force mining company to remove contaminants.
-Jobs will be generated.
-There will be more money going into the local economy.
Cons
-Cyanide is extremely toxic.
-Open-pit mines are an eyesore.
-Open-pit mines cause extreme damage to the local environment.
-Community may not have power to enforce environmental rules.