Test Bank General Chemistry, 10th edition 1
Chapter 2 – Atoms, Molecules, and Ions
1. Which of the following is/are postulates of Dalton’s atomic theory?
1.
Atoms combine in fixed ratios of whole numbers.
2.
Atoms of each element have different properties.
3.
Elements occur as solids, liquids, or gases.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
2. Which of the following statements best describes the particulate representation depicted by
the picture?
A)
The figure is a representation of a gas made up of a single element.
B)
The figure is a representation of a liquid mixture of two elements.
C)
The figure is a representation of a molecular solid.
D)
The figure is a representation of a liquid mixture of two compounds.
E)
The figure is a representation of a gas of a compound.
3. Which of the following is not a correct name–symbol combination?
A)
cobalt, Co
B)
vanadium, V
C)
neon, Ne
D)
scandium, Sc
E)
titanium, Mg
Test Bank General Chemistry, 10th edition 2
4. The symbol for tin is
A)
T.
B)
Tn.
C)
Si.
D)
Ti.
E)
Sn.
5. What is the symbol for the element phosphorus?
A)
Po
B)
P
C)
Pt
D)
K
E)
Pr
6. Which one of the following lists gives the correct symbols for the elements phosphorus,
potassium, silver, chlorine, and sulfur?
A)
P, Po, Ag, Cl, S
B)
K, Ag, Po, Cl, S
C)
P, K, Ag, Cl, S
D)
Ph, K, Ag, S, Cl
E)
Ph, Po, Ag, Cl, S
7. Which of the following lists gives the atomic symbols for potassium, magnesium, beryllium,
and sodium?
A)
Po, Mn, Br, Na
B)
P, Mn, Be, Se
C)
K, Mg, Be, Na
D)
Pt, Mg, Be, Sc
E)
K, Mn, Br, Na
8. The names of the elements whose symbols are Si, P, Mn, and S are, respectively,
A)
silicon, phosphorus, manganese, and sulfur.
B)
silicon, potassium, magnesium, and sulfur.
C)
silver, phosphorus, magnesium, and sodium.
D)
silver, potassium, manganese, and sodium.
E)
silicon, potassium, manganese, and sulfur.
9. Which of the following is the atomic symbol for the element cobalt?
A)
CO
B)
Co
C)
C
D)
co
E)
All of the above
10. A series of silicon–hydrogen compounds with the general formula SinH2n+2 can be
represented by the known compounds SiH4, Si2H6, and Si3H8. This best illustrates the law
of
A)
multiple proportions.
B)
conservation of charge.
C)
definite composition.
D)
conservation of mass.
E)
conservation of atoms.
11. According to the law of multiple proportions:
A)
the total mass is the same after a chemical change as before the change.
B)
it is not possible for the same two elements to form more than one compound.
C)
the ratio of the masses of the elements in a compound is always the same.
D)
if the same two elements form two different compounds, they do so in the same
ratio.
E)
none of these
12. Which of the following pairs of compounds can be used to illustrate the law of multiple
proportions?
A)
H2O and HCl
B)
NO and NO2
C)
NH4 and NH4Cl
D)
ZnO2 and ZnCl2
E)
CH4 and CO2
13. Cathode rays are
A)
anions.
B)
protons.
C)
cations.
D)
positrons.
E)
electrons.
14. A subatomic particle is
A)
a piece of an atom.
B)
only found in the nucleus of an atom.
C)
always positively charged.
D)
larger than the nucleus of an atom.
E)
always negatively charged.
Test Bank General Chemistry, 10th edition 5
15. Experiments were carried out in which a beam of cathode rays was first bent by a magnetic
field and then bent back by an electrostatic field until the beam hit the screen exactly where
it had been hitting before the fields were applied. This experiment permitted the direct
measurement of
A)
the ratio of mass to charge of an electron.
B)
the charge on the nucleus of an atom.
C)
the charge on the electron.
D)
the mass of the atom.
E)
the mass of the electron.
16. Who discovered the electron?
A)
Bohr
B)
de Broglie
C)
Rutherford
D)
Heisenberg
E)
Thomson
17. Which of the following conclusions regarding Rutherford’s gold foil experiment is not
consistent with the observations?
A)
The nucleus occupies only a small portion of the space of an atom.
B)
Most alpha particles travel straight through the gold foil.
C)
The nucleus occupies a large amount of the atom space.
D)
The nucleus, like the alpha particles used to bombard the gold foil, is positively
charged.
E)
Wide angle deflections result from a collision of an alpha particle and a gold atom
nucleus.
18. Who discovered the nucleus of an atom?
A)
Thomson
B)
de Broglie
C)
Rutherford
D)
Bohr
E)
Heisenberg
Test Bank General Chemistry, 10th edition 6
19. If the Thomson model of the atom had been correct, Rutherford would have observed
A)
alpha particles bouncing off the foil.
B)
alpha particles going through the foil with little or no deflection.
C)
alpha particles greatly deflected by the metal foil.
D)
positive particles formed in the foil.
E)
None of the above observations is consistent with the Thomson model of the atom.
20. The nucleus of a 208Pb nuclide contains
A)
208 neutrons and 290 electrons.
B)
82 protons and 208 neutrons.
C)
208 protons and 126 electrons.
D)
208 protons, 82 neutrons, and 208 electrons.
E)
82 protons and 126 neutrons.
21. If two different nuclides have the same atomic number, it must mean that
A)
they have the same atomic mass.
B)
they have the same mass number.
C)
they have the same number of protons.
D)
they have the same number of electrons.
E)
they have the same number of neutrons.
22. If two different nuclides have the same mass number, it must mean that
A)
the combined number of protons and neutrons are the same.
B)
both have the same number of neutrons.
C)
both have the same number of electrons.
D)
both have the same number of protons.
E)
they are isotopes.
23. The number of protons in a given nucleus determines the
A)
mass number.
B)
atomic number.
C)
number of electrons.
D)
number of protons.
E)
number of isotopes.
24. Which nuclide has the same number of protons as ?
A)
B)
C)
D)
E)
25. How many electrons does the ion have?
A)
18
B)
36
C)
16
D)
34
E)
19
26. How many protons are there in the chromium-52 nuclide?
A)
29
B)
76
C)
23
D)
24
E)
28
27. How many neutrons are there in the cobalt-59 nuclide?
A)
27
B)
2
C)
86
D)
59
E)
32
28. An atom that has the same number of neutrons as is
A)
.
B)
.
C)
.
D)
.
E)
.
29. Which combination of protons, neutrons, and electrons correctly represents a 56Fe nuclide?
A)
26 protons, 30 neutrons, 56 electrons
B)
26 protons, 30 neutrons, 30 electrons
C)
26 protons, 30 neutrons, 26 electrons
D)
56 protons, 26 neutrons, 56 electrons
E)
56 protons, 26 neutrons, 26 electrons
30. The species that has the same number of neutrons as is
A)
.
B)
.
C)
.
D)
.
E)
.
31. Which of the following nuclides contains more protons than neutrons?
A)
B)
C)
D)
E)
32. How many neutrons are there in 6 molecules of ?
A)
204
B)
102
C)
6
D)
396
E)
192
Test Bank General Chemistry, 10th edition 10
33. Suppose atom 1 has the same number of protons as atom 2, and atom 2 has the same number
of neutrons as atom 3. Atom 1 does not have the same number of neutrons as atom 3.
Which of the following statements is true?
A)
Atom 3 must have the same number of protons as atom 2.
B)
Atoms 1 and 2 must be isotopes.
C)
Atoms 1 and 3 must be isotopes.
D)
Atom 2 must have the same number of neutrons as atom 1.
E)
Atom 3 must have the same number of protons as atom 1.
34. Which of the following statements is true concerning the two nuclides and ?
A)
They have the same number of neutrons.
B)
They are isotopes.
C)
They have the same relative atomic mass.
D)
They have the same mass number.
E)
They have different chemical properties.
35. Which of the following atomic symbols represents an isotope of ?
A)
B)
C)
D)
E)
36. Which of the following represents a pair of isotopes?
Atomic Number
Mass Number
A)
I 17 36
II 18 36
B)
I 7 15
II 8 15
C)
I 17 35
II 17 37
D)
I 17 37
II 18 38
E)
I 7 16
II 8 17
37. There are three isotopes of carbon differing with respect to
A)
electron configuration.
B)
nuclear charge.
C)
number of neutrons.
D)
number of protons.
E)
atomic number.
38. Which of the following about the isotopes of a particular element is not true?
A)
Each unique isotope has a different atomic mass.
B)
Each unique isotope has a different atomic number.
C)
Each unique isotope has a different number of neutrons.
D)
Each unique isotope has the same number of protons.
E)
In neutral atoms of each unique isotope, the number of electrons equals the number
of protons.
39. The neutral atoms of all the isotopes of the same element have
A)
different numbers of protons.
B)
the same number of neutrons.
C)
the same number of electrons.
D)
the same mass.
E)
the same mass number.
Test Bank General Chemistry, 10th edition 12
40. What is the symbol of the nuclide having 15 protons and 16 neutrons?
A)
B)
C)
D)
E)
41. Which of the following has 62 neutrons, 46 protons, and 46 electrons?
A)
B)
C)
D)
E)
42. Which of the following elements has the largest atomic mass?
A)
rhenium
B)
manganese
C)
thallium
D)
argon
E)
fluorine
43. The mass spectrum of an element with two naturally occurring isotopes is shown below.
What is the best estimate of the element’s atomic mass?
Test Bank General Chemistry, 10th edition 13
A)
10 amu
B)
11 amu
C)
10.8 amu
D)
10.2 amu
E)
10.5 amu
44. The mass spectrum of an element with two naturally occurring isotopes is shown below. Its
average atomic mass would be best estimated as
A)
less than 26 amu but greater than 25 amu.
B)
less than 25 amu but greater than 24 amu.
C)
equal to 24 amu.
D)
equal to 25 amu.
E)
greater than 26 amu.
45. Lithium has two naturally occurring isotopes, 6Li and 7Li . The average atomic mass of
lithium is 6.941. Which of the following statements concerning the relative abundance of
each isotope is correct?
Test Bank General Chemistry, 10th edition 14
A)
The abundance of 7Li is greater than 6Li.
B)
The abundance of 7Li is less than 6Li.
C)
The abundance of 6Li is equal to the abundance of 7Li.
D)
Not enough data is provided to determine the correct answer.
E)
Based on the atomic mass, only 7Li occurs naturally.
46. A certain element is listed as having an atomic mass of 63.5 amu. It is probably true that this
element contains
A)
a mixture of isotopes.
B)
a mixture of neutrons.
C)
a mixture of isomers.
D)
a mixture of allotropes.
E)
a mixture of ions.
47. The average atomic mass of Eu is 151.96 amu. There are only two naturally occurring
isotopes of europium, 151Eu with a mass of 151.0 amu and 153Eu with a mass of 153.0 amu.
The natural abundance of the 131Eu isotope must be approximately
A)
60%.
B)
20%.
C)
50%.
D)
80%.
E)
40%.
48. Naturally occurring element X exists in three isotopic forms: X-28 (27.977 amu, 92.21%
abundance), X-29 (28.976 amu, 4.70% abundance), and X-30 (29.974 amu, 3.09%
abundance). Calculate the atomic weight of X.
A)
29.09 amu
B)
28.09 amu
Test Bank General Chemistry, 10th edition 15
C)
35.29 amu
D)
86.93 amu
E)
25.80 amu
49. Neon has three naturally occuring isotopes. The abundance of 20Ne is 90.48% and 22Ne is
9.25%. What is the percent abundance of 21Ne?
A)
9.25%
B)
0.27%
C)
49.9%
D)
33.2%
E)
81.2%
50. An element, X, has the following isotopic composition: X-200, 90%; X-199, 8.0%; and X-
202, 2.0%. Its average atomic mass is closest to
A)
200 amu.
B)
203 amu.
C)
199 amu.
D)
202 amu.
E)
201 amu.
51. Which of the following concerning atomic mass is/are correct?
1.
The atomic mass listed on a modern periodic table for each element is the
mass of the most abundant isotope.
2.
The atomic mass listed on a modern periodic table is a relative atomic mass,
based on the definition that 12C equals 12 amu.
3.
Relative atomic masses can only be determined with a mass spectrometer.
A)
1 only
B)
2 only
Test Bank General Chemistry, 10th edition 16
C)
1 and 2
D)
2 and 3
E)
1, 2, and 3
52. A periodic law based on atomic masses would necessitate Te and I changing places in the
periodic table. This was not done in the early periodic table because
A)
a periodic law based on atomic masses is not valid.
B)
it was thought that the atomic masses might be in error.
C)
iodine behaves chemically like chlorine and bromine.
D)
the tellurium samples could contain a heavy impurity.
E)
iodine contains one naturally occurring isotope, whereas tellurium consists of
several isotopes.
53. The elements in a row of the periodic table are known as
A)
metals.
B)
a period.
C)
metalloids.
D)
a family.
E)
a group.
54. Which of the following statements about different elements is incorrect?
A)
Potassium is an alkali metal.
B)
Fluorine is a halogen.
C)
Aluminum is a transition element.
D)
Barium is an alkaline earth metal.
E)
Helium is a noble gas.
55. Which of the following statements is not true about the element calcium?
A)
It is a metal.
B)
It is an alkaline earth metal.
C)
It is in period 4.
D)
It has chemical and physical properties most similar to silver.
Test Bank General Chemistry, 10th edition 17
E)
It is in group IIA (group 2).
56. The elements in groups 1A-8A or 1-2 and 15-18 are known as the
A)
main group.
B)
alkaline earth metals.
C)
metalloids or semimetals.
D)
halogens.
E)
transition metals.
57. Choose the group containing the most reactive nonmetals.
A)
Group 5A
B)
Group 3A
C)
Group 7A
D)
Group 8A
E)
Group 1A
58. Which element belongs to the transition metals?
A)
palladium
B)
sodium
C)
calcium
D)
iodine
E)
helium
59. Which of the following statements about different elements is/are true?
1.
As is a metalloid and Se is a nonmetal.
2.
Cu is a transition element and Ge is a metalloid.
3.
Both F and I are halogens.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
60. Which of the following is a metalloid?
A)
oxygen
B)
hydrogen
C)
silicon
D)
carbon
E)
copper
61. All of the following elements are best classified as metalloids except
A)
Si.
B)
Te.
C)
As.
D)
B.
E)
Ga.
62. Which formula is best described as a (condensed) structural formula?
A)
C2B10H12
B)
C6H11Cl
C)
CH3CH2CH2CH2Cl
D)
C12H22O11
E)
C2H6O
63. Which of the following is/are information that is unique to a space-filling molecular model?
1.
The model shows the relative sizes of each element.
2.
The model shows the charge distribution.
3.
The model shows the types of bonds (single or multiple) connecting the
atoms.
A)
1 only
B)
2 only
C)
3 only
D)
1 and 2
E)
1, 2, and 3
64. In a particular mass of KAu(CN)2, there are 8.87 1020 atoms of gold. What is the total
number of atoms in this sample?
A)
1.77 1021
B)
2.66 1021
C)
5.32 1021
D)
4.44 1021
E)
3.55 1021
65. A sample of TNT, C7H5N3O6 , has 7.68 1021 nitrogen atoms. How many hydrogen atoms
are there in this sample of TNT?
A)
1.54 1022
B)
10.24 1021
C)
1.28 1022
D)
7.68 1021
E)
1.79 1022
66. A 1.4-g sample of washing soda, Na2CO3 • 10H2O, has
2.9 1021
carbon atoms. How many
oxygen atoms are present in 1.4 g of washing soda?
A)
2.9 1022
B)
2.9 1021
C)
4.1 1021
D)
3.8 1022
E)
8.8 1021
67. A sample of the mineral troegerite, (UO2)3(AsO4)2 • 12H2O, has 1.33 1021 U atoms. How
many arsenic atoms are present in this sample of troegerite?
A)
2.00 1022
B)
1.60 1022
C)
2.66 1021
D)
6.65 1022
E)
8.87 1020
68. An ion is formed
A)
by either adding electrons to or subtracting electrons from the atom.
B)
by either adding protons to or subtracting protons from the atom.
C)
by either adding neutrons to or subtracting neutrons from the atom.
D)
All of the above are true.
E)
Two of the above are true.
69. The species Au+, Mg2+, and V3+ are all
A)
anions.
B)
isotopes.
C)
isoelectronic.
D)
allotropes.
E)
cations.
70. The species that is formed when a molecule gains or loses an electron is called
A)
an ion.
B)
a metalloid.
C)
an isotope.
D)
an atom.
E)
a metal.