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TE S T S F O R
HI G H E R ST A N D A R D S
P ROVIDE F OCUS + FACILITATE ACHIEVEMENT
Tests for Higher Standards
Halifax County Public Schools
Chemistry
GENERAL & CP
3rd Nine Weeks Benchmark Test
2008 - 2009
Dr. S. Stuart Flanagan, Professor Emeritus
College of William and Mary
Copyright 2005, S. Stuart Flanagan and David E. W. Mott
Do not reproduce without permission.
CH.1f
1. A certain chemistry student was performing an experiment to see whether a balance
was precise and accurate, so she measured the mass of a 100 g metal weight. The data
she recorded is below:
Trial
1
2
3
4
5
mass in grams
101.0
101.1
100.9
100.9
101.1
When she looked at her data, she noticed that all the values were close together but all higher
than the expected value. What can she say about the balance?
A
B
C
D
It is accurate but not precise.
It is precise but not accurate.
It is neither precise nor accurate.
It is both precise and accurate.
CH.1f
2. If Agnes’s measure of the density of a substance is 1.81 g/cm3 and the
accepted value is 2.06 g/cm3, what is the percent error of her measurement?
F 12%
G 14%
H 88%
J 114%
CH.1g
3. The mass of 165.0 mL of ethyl alcohol, C2H6O, is 129.5 g. What is its density?
A
B
C
0.7848 g / cm3
1.274 mL / g
21.38 kg / mL
D
35.50 cc / kg3
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CH.2i
4. Rutherford’s alpha-particle experiment, pictured below, helped support what
idea?
beam of alpha particles
radioactive
substance
circular ZnS-coated
fluorescent screen
gold foil
F
G
H
J
Electrons have mass.
Electrons have a negative charge.
The charge of an electron is 1.
Atoms have a dense, positive nucleus.
CH.2d
5. Each of the elements in a group or family of the periodic table have what
characteristic in common?
A
B
C
D
the same atomic radius
very similar atomic masses
similar half-lives
the same number of valence electrons
CH.2b
6. Different isotopes of an element differ from each other because they have a
different number of which particles?
F
G
H
J
protons
electrons
photons
neutrons
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CH.2f
7. As you move from top to bottom and from left to right on the periodic table,
how does the atomic radius of the atoms change?
A
B
C
D
It decreases from top to bottom and increases from left to right.
It increases from top to bottom and increases from left to right.
It decreases from top to bottom and decreases from left to right.
It increases from top to bottom and decreases from left to right.
CH.2g
8. What is the most common oxidation state of the element described by the
following electron configuration: [Ne] 3s2 3p4?
F
G
H
J
–2
1
0
+2
CH.2h
9. Chlorine, Cl, is most like which of the following elements in its chemical and
physical properties?
A
B
C
D
Lithium, Li
Helium, He
Fluorine, F
Sulfur, S
CH.2i
10. Emission of light from an atom occurs when:
F
G
H
J
an electron jumps from a lower to a higher energy level.
an electron drops from a higher to a lower energy level.
an electron falls into the nucleus.
two electrons collide and are converted into pure energy.
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CH.3c
11. The molecular formula for the sugar glucose is C6H12O6. What would be its
empirical formula?
A
B
CHO
CH2O
C
D
6 CHO
C2H12O2
CH.1a
12. Study the following drawing. What is the liquid volume indicated on this
glass graduated cylinder?
mL
10
9
8
7
F
G
H
J
8.2 mL
8.0 mL
7 mL
8 mL
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CH.1b
13. Study the diagram of the Bunsen burner below. Which part of the flame is the
hottest?
A
B
C
A
B
C
D
A
B
C
None is hotter than any other.
CH.1b
14. A student needed to dilute some concentrated hydrochloric acid. How should
the student do this?
F
G
H
J
add distilled water directly to the acid
add acid to the distilled water
first heat the acid and then add acid to the distilled water
first heat the acid and then add distilled water to the acid
CH.3a
15. In the formula MgCl2 • 2H2O, the compound is referred to as:
A
B
C
D
a hydroxide.
a hydrate.
a dihydride.
anhydrous.
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CH.1d
16. What can be determined about a chemical reaction from the data and graph
below?
Volume of
Hydrogen
Produced
(liters)
Mass of
Zinc Used
(grams)
1
0.37
2
0.73
3
1.10
4
1.47
5
1.84
6
2.21
6
.
5
Mass of
zinc
4
3
2
1
0
.
.
.
.
.
1
2
3
Volume of
hydrogen (L)
F
G
H
J
The mass of zinc used and hydrogen production are directly proportional.
The mass of zinc used and hydrogen production are inversely proportional.
The mass of zinc used and hydrogen production are related, but not proportional.
The mass of zinc used and hydrogen production are unrelated.
_____________________________________________________________________________________________
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CH.1g
17. How many significant digits are in the measurement 0.030010 cm?
A
B
C
D
7
6
5
4
CH.2a
18. The atomic mass of each element is based on the relative mass of which
element?
F
G
H
J
oxygen - 16
hydrogen - 1
carbon - 12
nitrogen - 14
CH.2h
19. Which of the following is a chemical property?
A
B
C
D
boiling point
resists corrosion
dissolves in water
melting point
CH.2i
20. Of the following atomic models pictured below, which one is most accepted
today?
F
H
G
J
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CH.2f
21. Electronegativity involves the difference in attraction of atoms for electrons
in a bond. Which of the following bond pairs would have the greatest
electronegativity difference?
A
B
C
D
F-CI
Cl-Cl
Mg-Cl
H-Mg
CH.2g
22. What is the oxidation number for the polyatomic ion in the compound
potassium permanganate?
KMnO4
F
G
H
J
+1
–1
+4
–4
CH.2a
23. Consider the following entry for magnesium taken from the periodic table.
24.305
+2
Mg
Magnesium
12
[Ne]3s2
The number 12 represents —
A
B
C
D
the atomic mass number.
the atomic number.
the oxidation number.
the number of neutrons.
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CH.2e
24. Which of the following is considered a transition metal?
F
G
H
J
magnesium
silicon
sodium
gold
CH.2g
25. Which of the following electron configurations represents an element in an
excited state?
A
B
C
D
1s22s22p6
1s22s22p63s2
1s22s22p63s1
1s22s22p53s1
CH.2d
26. The following elements belong to which family (group) — Li, Na, K, Rb, Cs,
or Fr?
F
G
H
J
halogens
alkali metals
alkaline earth metals
metalloids
CH.2f
27. One of the periodic properties involves the amount of energy required to
remove the most loosely held electron from the outer energy level of the
atom (in the gas phase). This property is known as
A
B
C
D
electronegativity.
atomic radius.
ionization energy.
ionic radius.
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CH.2i
28. Originally, Mendeleev arranged the families (columns) in the periodic table
according to
F
G
H
J
alphabetic order.
atomic number.
atomic mass.
similar properties.
CH.2a
29. An atom with 3 neutrons, 2 protons, and 2 electrons would have the mass of
A
B
C
D
2 amu.
5 amu.
7 amu.
4 amu.
CH.2a, c
30. The number of neutrons in nickel-60 is
F
G
H
J
28.
30.
32.
60.
CH.2g
31. When electrons enter orbitals of equal energy, one electron enters each
orbital until all the orbitals contain one electron with parallel spins,
according to —
A
B
C
D
the Pauli Exclusion Principle
Hund’s Rule
The Heisenberg Uncertainty Principle.
the Electron Affinity Rule.
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CH.2g
32. How many orbitals are located in the p sublevel?
F
G
H
J
3
5
7
10
CH.2
33.
A
B
C
D
How many valence electrons does a carbon atom have?
2
3
4
6
CH.3a
34. Which is always named first, when naming an ionic compound?
F
G
H
J
anion
hydrogen atom
the element that has a greater mass
cation
CH.3e
35. Consider the experiment below in which two iron nails are placed in a copper
(II) chloride solution. Which of the following unbalanced reactions will
represent the single replacement reaction that would occur?
Copper (II)
chloride
solution
iron
nails
A
B
C
D
CuCl2 + Fe
Cu2Cl + Fe
CuCl2 + Fe
Fe + Cu →
→ Fe + Cl2 + Cu
→ Fe + CuCl2
→ FeCl2 + Cu
FeCl2 + Cu
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CH.3a
36. Name the following compound — CuO.
F
G
H
J
copper (I) oxide
copper (II) oxide
copper (III) oxide
copper (IV) oxide
CH.3b
37. In order to balance the following equation, which coefficient would need to
be placed in front of SO2?
__ SO2(g) + O2(g) + 2H2O(l) → 2H2SO4(l)
A
B
C
D
1
2
3
4
CH.3a
38. The chemical formula for sulfur difluoride would be
F
G
H
J
S2F.
S2F2.
SF2.
SF.
CH.3d
39. The type of bonding in sodium chloride is
A
B
C
D
nonpolar covalent.
polar covalent.
ionic.
metallic.
CH.3d
40. When electrons are shared unevenly between atoms, what type of bond
results?
F
G
H
J
ionic
nonpolar covalent
metallic
polar covalent
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