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Chemi1100pretest1
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1.
Accordingly to the periodic law the properties of elements repeat at regular intervals when the
elements are arranged in order of
a. their increasing atomic mass.
b. their increasing atomic size.
c. their increasing number of neutrons in the nucleus.
d. their increasing number of isotopes.
e. their increasing number of protons in the nucleus.
____
2.
a.
b.
c.
d.
e.
Which electrons have the greatest influence on the properties of elements?
those electrons in s orbitals
those electrons in d orbitals
core electrons
the outermost electrons
none of these
____
3.
a.
b.
c.
d.
e.
Cr
Ga
Sn
Sb
Li
____
____ is a d-transition metal.
4.
a.
b.
c.
d.
e.
Rb
Ho
Co
Ru
Bi
5.
a.
b.
c.
d.
e.
Cl
Sr
Co
K
N
____
6.
a.
b.
c.
d.
e.
What would be the outer electron configuration of group VIA (O, S, Se, . . .)?
ns2np6
ns2np2
ns2np4
np6
ns0np6
____
7.
What would be the outer electron configuration of alkaline earth metals?
a. ns2np2
b. np2
c. ns0np2
____
Which one of the following is an inner transition (f-transition) element?
Which of the following is not a representative element?
d. nd2
e. ns2
____
____
____
____
____
8.
Choose the term that best describes all members of this series of elements:
Xe, Rn, He, Ne, Kr
a.
b.
c.
d.
e.
metalloids
noble gases
alkaline earth metals
alkali metals
representative elements
9.
a.
b.
c.
d.
e.
Al
Si
P
S
Cl
Which element has the largest atomic radius?
10.
Arrange the following elements in order of increasing atomic radii.
K, Na, Mg, Cs, Cl
a.
b.
c.
d.
e.
Na < Mg < Cl < K < Cs
Cl < Mg < Na < K < Cs
Cs < K < Cl < Mg < Na
Cl < Mg < Cs < K < Na
Cl < Mg < Na < Cs < K
11.
a.
b.
c.
d.
e.
Cs
Rb
Ca
Ba
Na
Which element has the lowest first ionization energy?
12.
a.
b.
c.
d.
e.
Which of the following elements has the most negative electron affinity?
Si
P
S
Se
Te
____
13.
a.
b.
c.
d.
e.
Which one of the following species is not isoelectronic with neon?
Mg2+
Na+
O2
Si2+
Al3+
____
14.
Which ion has the largest radius?
+
a. Li
b. Na+
c. Be2+
d. Mg2+
e. Al3+
____
15.
a.
b.
c.
d.
e.
____
16.
Simple positively charged ions are always ____ than the neutral atoms from which they are formed.
smaller
larger
isoelectronic
the same size
more anionic
Arrange the following elements in order of decreasing electronegativities.
Al, Cs, Mg, Na, P
a.
b.
c.
d.
e.
P > Al > Mg > Na > Cs
Cs > Na > Mg > Al > P
Al > Mg > Na > Cs > P
P > Al > Mg > Cs > Na
P > Cs > Na > Mg > Al
____
17.
a.
b.
c.
d.
e.
Which of the following pairs of elements would be expected to form an ionic compound?
S / F
H / C
Rb / Cl
As / Br
C / I
____
18.
a.
b.
c.
d.
e.
Which of the following oxides does not give an acidic solution when dissolved in water?
SO2
CO2
N2O5
P4O10
Na2O
____
19.
a.
b.
c.
d.
e.
An amphoteric compound exhibits
acidic properties.
acidic and basic properties.
metallic properties.
basic properties.
ionic properties.
____
20.
a.
b.
c.
d.
e.
Atoms consist of three fundamental particles. What are these particles and their charges?
proton (+1), neutron (neutral) and electron (1)
proton (1), neutron (+1) and electron (neutral)
proton (+1), neutron (1) and electron (neutral)
proton (neutral), neutron (+1) and electron (1)
proton (1), neutron (neutral) and electron (+1)
____
21.
a.
b.
c.
d.
One of the following does not describe solids. Which one is it?
Particles in definite positions.
Definite shape.
Easily compressed.
Relatively high densities.
e. Particles compact.
____
22.
a.
b.
c.
d.
e.
All of the following are properties of antimony. Which one is not a physical property?
It is a solid at room temperature.
It has both yellow and gray forms (allotropes) in the solid state.
It burns in an atmosphere of chlorine.
It is one of the few substances that expands upon freezing.
The gray form melts at 631C.
____
23.
The following statements describe some physical and chemical properties of sucrose (table sugar).
Which response includes all that describe chemical properties, and none that describe physical properties?
I.
It is a colorless solid.
II.
It chars or blackens when heated gently.
III.
Its density is 1.6 g/mL.
IV.
It ignites and burns with a yellow flame when heated strongly.
V.
It is usually in the form of small crystals although it can occur as a powder.
a.
b.
c.
d.
e.
I, III, and IV
II and IV
II, IV, and V
I and V
another combination is the answer
____
24.
a.
b.
c.
d.
e.
Which of the following is not an intensive property of matter?
color
density
melting point
weight
boiling point
____
25.
Which response includes all of the following that involve chemical changes, and none that involve
physical changes?
I.
converting milk to cheese
II.
converting water to steam
III.
composting leaves
IV.
burning of gasoline
V.
melting wax
a.
b.
c.
d.
e.
II and V
I, III, and IV
I, II, and III
IV and V
III, IV, and V
____
26.
a.
b.
c.
d.
e.
Which mixture is incorrectly labeled?
homogeneous / sugar dissolved in water
homogeneous / sand stirred into water
heterogeneous / orange juice with pulp
heterogeneous / chocolate chip cookie
heterogeneous / concrete sidewalk
____
27.
What is the symbol for the element potassium?
a.
b.
c.
d.
e.
K
P
Pt
W
Po
____
28.
a.
b.
c.
d.
e.
Water is always 11.1% hydrogen and 88.9 % oxygen by mass. This is a statement of the
Law of Conservation of Matter.
Law of Definite Proportions.
Law of Multiple Proportions.
Law of Conservation of Matter and Energy.
none of these.
____
29.
Below is a list of physical properties and the fundamental unit used in the SI system to measure each.
Which unit is not the correct fundamental unit for the property?
a.
b.
c.
d.
e.
physical property / unit
length / meter
time / second
mass / gram
temperature / kelvin
electric current / ampere
____
30.
Below is a list of common prefixes used in the SI and metric systems. Included with each is an
abbreviation and meaning. Which set contains an error?
a. mega- M 106
b. decid
101
c. centi- c
102
d. micro- m
106
e. kilok
103
____
31.
a.
b.
c.
d.
e.
Which of the following is equivalent to 10 cm?
1m
0.1 dm
100 mm
1000 m
1 mm
____
32.
a.
b.
c.
d.
e.
Which of the following numbers has 4 significant figures?
0.04309
0.0430
0.0431
0.43980
0.043090
____
33.
The sum 2.834 + 5.71520 + 2.12 + 178.1 + 250.2619 expressed to the proper number of significant
figures is:
a. 439
b. 439.0
c. 439.03
d. 439.031
e. 439.0311
____
34.
Perform the indicated mathematical operations and express the answer in scientific notation rounded
off to the proper number of significant figures:
(8.001  102)  (2.88  103  2.4  103) =
a.
b.
c.
d.
e.
9.6  102
9.60  108
9.601  108
9.6  108
9.6  102
____
35.
If 5.76  1013 neon atoms (spherical) were laid in a line, each touching the next, the line would
measure 2.54 miles. What is the diameter of a neon atom in Å? (1 Å=1x10 10 m)
a. 0.92 Å
b. 0.71 Å
c. 1.86 Å
d. 1.44 Å
e. 1.74 Å
____
36.
a.
b.
c.
d.
e.
____
37.
At 25C, one milliliter of mercury has a mass of 13.6 grams. How many liters of mercury are required
to have a mass of 500 kg of mercury?
a. 500 L
b. 25.2 L
c. 42.1 L
d. 13.6 L
e. 36.8 L
____
38.
A metal cube having a mass of 112 grams is dropped into a graduated cylinder containing 30.00 mL
of water. This causes the water level to rise to 39.50 mL. What is the density of the cube?
a. 2.86 g/mL
b. 11.8 g/mL
c. 10.8 g/mL
d. 3.74 g/mL
e. 10.6 g/mL
____
39.
a.
b.
c.
d.
e.
____
40.
Gallium, a metal, has a freezing point near room temperature so it can be melted by holding it in your
hands. If gallium's melting point is 302.8 K, what is that temperature in C?
What is the area in square millimeters of a rectangle that is 8.632 cm long and 26.41 mm wide?
2280 mm2
3.060 mm2
22.80 mm2
0.3060 mm2
30.60 mm2
The density of mercury is 13.6 g/cm3. What is the mass of 6.50 cm3 of mercury?
0.478 g
88.4 g
18.9 g
2.38 g
1.10  102 g
a.
b.
c.
d.
e.
0.0C
575.8C
302.8C
39.8C
29.8C
____
41.
If a sample of butane, C4H10, contains a total of 8.0  103 atoms of carbon, how many molecules of
butane are in the sample?
a. 6.0  103
b. 3.0  103
c. 8.0  103
d. 1.1  104
e. 2.0  103
____
42.
Each response below lists an ion by name and by chemical symbol or formula. Also each ion is
classified as monatomic or polyatomic and as a cation or anion. Which response contains an error?
a. hydroxide / OH / monatomic / anion
b. carbonate / CO32 / polyatomic / anion
c. ammonium / NH4+ / polyatomic / cation
d. magnesium / Mg2+ / monatomic / cation
e. sulfite / SO32 / polyatomic / anion
____
43.
a.
b.
c.
d.
e.
What is the formula for ammonium fluoride?
AlF
Al2F3
NH3F
NH4F2
NH4F
____
44.
a.
b.
c.
d.
e.
What is the formula for aluminum oxide?
Al2O3
Ag2O3
AlO3
AlO
AlO2
____
45.
a.
b.
c.
d.
e.
Calculate the number of moles of oxygen atoms in 35.2 grams of oxygen.
2.20 moles
4.42 moles
0.54 moles
2.57 moles
1.13 moles
____
46.
a.
b.
c.
d.
e.
Determine the number of sulfur atoms in 27.1 g of molecular sulfur (S 8).
0.845
5.27  1023
5.09  1023
2.07  1023
0.106
____
47.
a.
b.
c.
d.
e.
Calculate the formula weight of NaHSO4.
193 amu
104 amu
120 amu
215 amu
185 amu
____
48.
a.
b.
c.
d.
e.
What is the mass in grams of 5.00  1012 water molecules?
1.50  1010 g
1.67  1035 g
2.17  1012 g
6.69  109 g
4.61  1013 g
____
49.
a.
b.
c.
d.
e.
Which of the following has no charge?
nucleus
neutron
proton
electron
alpha particle
____
50.
In interpreting the results of his "oil drop" experiment in 1909, Robert Millikan was able to determine
____.
a. the charge on a proton
b. that electrically neutral particles (neutrons) are present in the nuclei of atoms
c. that the masses of protons and neutrons are nearly identical
d. the charge on an electron
e. the extremely dense nature of the nuclei of atoms
____
51.
In the Rutherford gold foil experiment, the fact that most of the alpha particles were not deflected as
they passed through the gold foil indicates that
a. the nucleus is positively charged.
b. the atom is mostly empty space.
c. atoms are solid spheres touching each other in the solid state.
d. gold is very dense.
e. none of these is correct.
____
52.
a.
b.
c.
d.
e.
____
53.
The atomic number of an element gives the number of ____ and ____ in the atom while the mass
number gives the total number of ____ and ____.
a. neutrons; protons; neutrons; electrons
b. neutrons; electrons; protons; electrons
c. neutrons; electrons; neutrons; protons
d. protons; electrons; neutrons; electrons
e. protons; electrons; neutrons; protons
The number of electrons in a neutral atom of an element is always equal to the ____ of the element.
mass number
atomic number
atomic mass unit
isotope number
Avogadro's number
____
54.
a.
b.
c.
d.
e.
Isotopes are atoms of the same element that
have different numbers of electrons.
have different numbers of protons.
have different atomic numbers.
have different numbers of neutrons.
have different nuclear charges.
____
55.
a.
b.
c.
d.
e.
Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope.
38 p; 38 n; 38 e
38 p; 90 n; 38 e
52 p; 38 n; 52 e
38 p; 52 n; 38 e
90 p; 38 n; 90 e
Chapter 4 Values
The following values may be useful for solving some of the problem(s) below.
speed of light = 3.00  108 m/s
Planck's constant = 6.63  1034 Js
1 joule = 1 kgm2/s2
1 Ångstrom = 1  1010 m
____
56.
a.
b.
c.
d.
e.
What is the wavelength of yellow light having a frequency of 5.17  1014 Hz?
3.60  1010 m
1.55  1023 m
6.45  1028 m
5.80  107 m
2.72  106 m
____
57.
a.
b.
c.
d.
e.
What is the energy, in J/photon, of ultraviolet light with a frequency of 2.70  1016 Hz?
6.00  108 J/photon
8.00  106 J/photon
2.46  1018 J/photon
4.07  1019 J/photon
1.79  1017 J/photon
____
58.
a.
b.
c.
d.
e.
Calculate the energy (J/photon) of a photon of wavelength 3.65  106 m.
5.45  1020 J
1.82  1028 J
1.22  1014 J
6.05  1037 J
none of these
____
59.
a.
b.
c.
d.
e.
The Rydberg equation is an empirical equation that describes mathematically ____.
the lines in the emission spectrum of hydrogen
the results of the oil drop experiment
the results of the cathode ray experiments
the Bohr model of the atom
the possible paths of two isotopes of the same element in a mass spectrometer
____
60.
What is the velocity of a neutron of mass 1.67  1027 kg that has a de Broglie wavelength of 2.05 Å?
a.
b.
c.
d.
e.
19 m/s
1.94  103 m/s
8.13  107 m/s
1.93  104 m/s
5.16  104 m/s
____
61.
a.
b.
c.
d.
e.
What statement regarding quantum numbers is false?
The spin quantum number has values of either +1 or 1.
The principle quantum number has only integer values.
The angular momentum quantum number also has letter designations.
The magnetic quantum number has its values restricted by the l quantum number.
The magnetic quantum number is represented by ml.
____
62.
I.
II.
III.
Which response lists all the true statements about the four quantum numbers?
n = principal quantum number,
n = 1,2,3, . . .
l = angular momentum quantum number,
l = 0,1,2,3, . . ., (n1)
ml = magnetic quantum number,
ml = 0, 1, . . ., l
IV.
ms = spin quantum number,
____
____
____
a.
b.
c.
d.
e.
I, II, and IV
I, II, and III
I and III
II and III
II, III, and IV
63.
a.
b.
c.
d.
e.
8
2
16
18
25
64.
a.
b.
c.
d.
e.
1
2
0
2
3
The third energy level or shell of an atom can hold a maximum of ____ electrons.
Which of the following is not a valid magnetic quantum number for the 3d set of orbitals?
65.
What is the value of the angular momentum quantum number, l, for the following orbital?
a.
b.
c.
d.
e.
ms = ±
1
0
1
2
____
66.
All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a
statement of ____.
a. the Heisenberg Uncertainty Principle
b. the Bohr Theory
c. the Aufbau Principle
d. Planck's Theory
e. Hund's Rule
____
67.
Which element has the electron configuration below?
1s22s22p63s23p63d104s24p3
a.
b.
c.
d.
e.
V
Ca
P
As
Se
____
68.
a.
b.
c.
d.
e.
What is the electron configuration of tin, Sn?
[Kr]5s23d103f145p4
[Kr]5s23d104d145p4
[Kr]5s23d104f145p2
[Kr]5s24d105p2
[Xe]5s24d105p2
____
69.
a.
b.
c.
d.
e.
What is the electron configuration of the iron(III) ion?
Fe [Ar]4s23d3
Fe3+[Ar]3d5
Fe2+[Ar]4s23d3
Fe2+[Ar]3d5
Fe3+[Kr]3d5
____
3+
Which of the following sets of quantum numbers could represent the highest energy electron in V2+?
70.
n
l
ml
ms
4
0
0

4
1
1

3
2
1

3
1
0
+
4
2
1

a.
b.
c.
d.
e.
____
71.
a.
b.
c.
d.
Which of the following atoms has the greatest number of unpaired electrons in its ground state?
Fe
N
S
Ti
e. Cu
Chemi1100pretest1
Answer Section
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Elements
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Elements
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More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
More About the Periodic Table
Atomic Radii
Atomic Radii
Ionization Energy
Electron Affinity
Ionic Radii
Ionic Radii
Ionic Radii
Electronegativity
Electronegativity
Oxygen and the Oxides
Oxygen and the Oxides
Chemistry – A Molecular View of Matter
States of Matter
Chemical and Physical Properties
Chemical and Physical Properties
Chemical and Physical Properties
Chemical and Physical Changes
Mixtures, Substances, Compounds, and
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Mixtures, Substances, Compounds, and
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Mixtures, Substances, Compounds, and
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Measurements in Chemistry
Measurements in Chemistry
Measurements in Chemistry
Use of Numbers
Use of Numbers
Use of Numbers
The Unit Factor Method (Dimensional
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The Unit Factor Method (Dimensional
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Analysis)
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Compounds
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Compounds
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Atom
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Density and Specific Gravity
Density and Specific Gravity
Heat and Temperature
Chemical Formulas
Ions and Ionic Compounds
Names and Formulas of Some Ionic
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The Mole
The Mole
Formula Weights, Molecular Weights, and
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D
D
E
A
A
B
A
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
1
1
1
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Fundamental Particles
The Discovery of Electrons
Rutherford and the Nuclear Atom
Atomic Number
Mass Number and Isotopes
Mass Number and Isotopes
Mass Number and Isotopes
Electromagnetic Radiation
Electromagnetic Radiation
Electromagnetic Radiation
Atomic Spectra and the Bohr Atom
The Wave Nature of the Electron
The Quantum Mechanical Picture of the
A
D
E
D
E
D
D
B
C
A
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
PTS:
1
1
1
1
1
1
1
1
1
1
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Quantum Numbers
Atomic Orbitals
Atomic Orbitals
Atomic Orbitals
Electron Configurations
Electron Configurations
Electron Configurations
Electron Configurations
Electron Configurations
Paramagnetism and Diamagnetism