Quarterly 1 Review
Trupia
____1. Which subatomic particles have a mass of
approximately 1 atomic mass unit each?
(1) proton and electron
(2) proton and neutron
(3) neutron and positron
(4) electron and positron
____6. All atoms of a given element must contain
the same number of
(1) protons
(2) neutrons
(3) electrons plus neutrons
(4) protons plus neutrons
____2. In Rutherford's gold foil experiments, some
alpha particles were deflected from their
original paths but most passed through the foil
with no deflection. Which statement about gold
atoms is supported by these experimental
observations?
(1) Gold atoms consist mostly of empty space.
(2) Gold atoms are similar to alpha particles.
(3) Alpha particles and gold nuclei have
opposite charges.
(4) Alpha particles are more dense than gold
atoms.
____7. What is the nuclear charge of an atom with a
mass of 23 and an atomic number of 11?
(1) 11+
(3) 23+
(2) 12+
(4) 34+
____8. What is the nuclear charge of an iron atom
(Fe)?
(1) +26
(3) +56
(2) +30
(4) +82
____9. What is the charge of the nucleus in an atom
of oxygen-17?
(1) 0
(3) +8
(2) –2
(4) +17
____3. Experiments performed to reveal the
structure of atoms led scientists to conclude that
____10. What is the atomic number of an element
an atom's
that has six protons and eight neutrons?
(1) positive charge is evenly distributed
(1) 6
(3) 8
throughout its volume
(2) 2
(4) 14
(2) negative charge is mainly concentrated in its
nucleus
____11. What is the atomic number of an element
(3) mass is evenly distributed throughout its
whose atoms each contain 47 protons, 60
volume
neutrons, and 47 electrons?
(4) volume is mainly unoccupied
(1) 13
(3) 60
(2) 47
(4) 107
____4. Which of the following particles has the
smallest mass?
____12. Compared to a proton, an electron has
(1) neutron
(3) proton
(1) a greater quantity of charge and the same
(2) electron
(4) hydrogen atom
sign
(2) a greater quantity of charge and the opposite
____5. Which subatomic particle has a negative
sign
charge?
(3)
the
same quantity of charge and the same
(1) proton
(3) neutron
sign
(2) electron
(4) positron
(4) the same quantity of charge and the opposite
sign
Quarterly 1 Review
Trupia
____13. The total mass of the protons in an atom of
gold-198 is approximately
(1) 79 atomic mass units
(2) 119 atomic mass units
(3) 198 atomic mass units
(4) 277 atomic mass units
____20. All the isotopes of a given atom have
(1) the same mass number and the same atomic
number
(2) the same mass number but different atomic
numbers
(3) different mass numbers but the same atomic
number
(4) different mass numbers and different atomic
____14. An atom of fluorine has a mass of 19 atomic
numbers
mass units. The total number of protons and
neutrons in its nucleus is
____21. The atomic mass of an element is the
(1) 9
(3) 19
weighted average of the
(2) 10
(4) 28
(1) number of protons in the isotopes of that
____15. The atomic mass of an atom is measured in
element
atomic mass units. This unit is based on
(2)
number
of neutrons in the isotopes of that
(3) 16O
(1) 1H
element
(4) 12C
(2) 14N
(3) atomic numbers of the naturally occurring
isotopes of that element
____16. An atomic mass unit is defined as exactly
(4) atomic masses of the naturally occurring
11
(1) 12
the mass of a 12C atom
isotopes of that element
11
the mass of a 14N atom
(2) 14
11
(3) 16
the mass of a 16O atom
____22. Which atom contains exactly 15 protons?
11
19
(1) phosphorus-32
(3) oxygen-15
(4) 19 the mass of a F atom
(2) sulfur-32
(4) nitrogen-15
____17. Which two particles make up most of the
____23. Isotopes of an element must have different
mass of a hydrogen-2 atom?
(1) electron and neutron (3) proton and neutron
(1) atomic numbers
(2) electron and proton (4) proton and positron
(2) mass numbers
(3) numbers of protons
____18. What is the total number of neutrons in the
(4) numbers of electrons
nucleus of a neutral atom that has 19 electrons
and a mass number of 39?
14
____24. The nuclides 14
6 C and 7 N are similar in that
(1) 19
(3) 39
they both have the same
(2) 20
(4) 58
(1) mass number
(3) number of neutrons
____19. Which isotopic notation represents an atom
of carbon-14?
(3) 614C
(1) 68C
8
(4) 14
(2) 6C
6 C
(2) atomic number
(4) nuclear charge
____25. Which electron configuration represents an
atom in an excited state?
(1) 2–7
(3) 2–8–1
(2) 2–6–2
(4) 2–8–8–2
____26. Which is the configuration of an atom in the
ground state?
(1) 2-8-2
(3) 2-7-2
(2) 2-8-3
(4) 2-7-3
Quarterly 1 Review
Trupia
____27. The principal quantum number of the
outermost electron of an atom in the ground
state is n = 3. What is the total number of
occupied principal energy levels contained in
this atom?
(1) 1
(3) 3
(2) 2
(4) 4
____28. What causes the emission of radiant energy
that
produces characteristic spectral lines?
(1) neutron absorption by the nucleus
(2) gamma ray emission from the nucleus
(3) movement of electrons to higher energy
levels
(4) return of electrons to lower energy levels
____29. Which electron configuration represents an
atom in an excited state?
(1) 2-2
(3) 2-8
(2) 2-2-1
(4) 2-8-1
____30. Which electron configuration represents an
atom of aluminum in an excited state?
(1) 2-7-4
(3) 2-8-3
(2) 2-7-7
(4) 2-8-6
____31. In an atom that has an electron configuration
of 1s22s22p3, what is the total number of
electrons in its sublevel of highest energy?
(1) 1
(3) 3
(2) 2
(4) 4
____32. An atom of phosphorus is in the ground
state. The total number of orbitals that contain
only one electron is
(1) 5
(3) 3
(2) 2
(4) 4
____33. What is the maximum number of electrons
in an orbital of any atom?
(1) 1
(3) 6
(2) 2
(4) 10
____34. Which of the following electron
configurations represents the element with the
smallest covalent radius?
(3) 1s22s22p4
(1) 1s22s22p2
2 2 3
(2) 1s 2s 2p
(4) 1s22s22p5
____35. What is the total number of occupied
sublevels in the third principal energy level of a
zinc atom in the ground state?
(1) 1
(3) 3
(2) 2
(4) 4
____36. Which electron configuration represents a
neutral atom of nitrogen in an excited state?
(3) 1s22s12p4
(1) 1s22s22p3
(2) 1s22s22p4
(4) 1s22s12p5
Quarterly 1 Review
Trupia
37. In the early 1900s, evidence was discovered that atoms were not “hard spheres.” It was shown that atoms
themselves had an internal structure. One experiment involved gold metal foil.
a Complete the simple model for an atom of gold-197 by placing the correct numbers in the two blanks.
b In the gold-foil experiment, alpha particles were directed toward the foil. Most of the alpha particles passed
directly through the foil with no effect. This result did not agree with the “hard spheres model” for the atom.
What conclusion about the internal structure of the atom did this evidence show?
c In the same experiment, some of the alpha particles returned toward the source. What does this evidence
indicate about the charge of the atom’s nucleus?
Quarterly 1 Review
Trupia
38. Base your answer to the following question on the following information.
In a laboratory, a glass tube is filled with hydrogen gas at a very low pressure. When a scientist
applies a high voltage between metal electrodes in the tube, light is emitted. The scientist analyzes the
light with a spectroscope and observes four distinct spectral lines. The table below gives the color,
frequency, and energy for each of the four spectral lines. The unit for frequency is hertz, Hz.
A spectral line in the infrared region of the spectrum of hydrogen has a frequency of 2.3 × 1014 hertz. Using your
graph, estimate the energy associated with this spectral line.
Quarterly 1 Review
Trupia
39. Base your answer to the following question on the data table below, which shows three isotopes of neon.
Based on natural abundances, the average atomic mass of neon is closest to which whole number?
____40. Which statement identifies the element
arsenic?
(1) Arsenic has an atomic number of 33.
(2) Arsenic has a melting point of 84 K.
(3) An atom of arsenic in the ground state has
eight valence electrons.
(4) An atom of arsenic in the ground state has a
radius of 146 pm.
____45. Which element is a member of the halogen
family?
(1) K
(3) I
(2) B
(4) S
____46. Which substance can not be decomposed by
a chemical change?
(1) Ne
(3) HF
(4) H2O
(2) N2O
____41. Which of the following elements in Period 3
____47. Which element has no known stable isotope?
has the greatest metallic character?
(1) Hg
(3) Se
(1) Ar
(3) Mg
(2) Po
(4) Zn
(2) Si
(4) S
____42. Which element is an alkali metal?
(1) hydrogen
(3) sodium
(2) calcium
(4) zinc
____48. Which element is a noble gas?
(1) krypton
(3) antimony
(2) chlorine
(4) manganese
____43. An atom of an element contains 20 protons, ____49. Which substance is the best conductor of
electricity?
20 neutrons, and 20 electrons. This element is in
(1) nitrogen
(3) sulfur
Group
(2)
neon
(4) silver
(1) 1
(3) 4
(2) 2
(4) 18
____50. Which substance can not be decomposed by
ordinary chemical means?
____44. Which element in Period 3 exists as
(1) methane
(3) ethanol
diatomic molecules at STP?
(2) mercury
(4) ammonia
(1) argon
(3) aluminum
(2) chlorine
(4) sodium
____51. At standard pressure, which element has a
melting point higher than standard temperature?
(3) Fe
(1) F2
(2) Br2
(4) Hg
Quarterly 1 Review
Trupia
____52. If the electron configuration of an atom of
____58. Which of the following ions has the smallest
radius?
element X is 2-6, the electron dot symbol for the
(3) K+
(1) F–
element is
–
(2) Cl
(4) Ca2+
(1)
(3)
____59. In the ground state, each atom of an element
has two valence electrons. This element has a
lower first ionization energy than calcium.
Where is this element located on the Periodic
(2)
(4)
Table?
(1) Group 1, Period 4 (3) Group 2, Period 3
(2) Group 2, Period 5 (4) Group 3, Period4
____53. Which element has a total of 5 valence
electrons present in the fifth energy level (shell)?
____60. Which element forms an ion that is larger
(1) Sb
(3) I
than its atom?
(2) Bi
(4) Br
(1) aluminum
(3) magnesium
(2) chlorine
(4) sodium
____54. Lithium and potassium have similar
chemical properties because the atoms of both
____61. As the elements in Period 2 of the Periodic
elements have the same
Table are considered in succession from left to
(1) mass number
right, there is a decrease in atomic radius with
(2) atomic number
increasing atomic number. This may best be
(3) number of electron shells
explained by the fact that the
(4) number of valence electrons
(1) number of protons increases, and the number
____55. What is the net charge of an ion that consists
of 10 electrons, 11 protons, and 12 neutrons?
(1) 1+
(3) 1–
(2) 2+
(4) 2–
of shells of electrons remains the same
(2) number of protons increases, and the number
of shells of electrons increases
(3) number of protons decreases, and the
number of shells of electrons remains the
same
(4) number of protons decreases, and the
number of shells of electrons increases
____56. Which chemical substances contain atoms in
which electrons from the two outermost
principal energy levels may be involved in a
chemical reaction?
____62. As the atoms in Period 3 of the Periodic
(1) halogens
(3) alkaline earths
Table are considered from left to right, the
(2) alkali metals
(4) transition elements
atoms generally show
(1) an increase in radius and an increase in
____57. Which elements form ions that are usually
ionization energy
colored in solid compounds and in solution?
(2) an increase in radius and a decrease
(1) alkali metals
ionization energy
(2) alkaline earth metals
(3) a decrease in radius and an increase in
(3) transition elements
ionization energy
(4) halogen elements
(4) a decrease in radius and a decrease in
ionization energy
Quarterly 1 Review
Trupia
____63. In Period 2 of the Periodic Table, which
Group contains the element with the highest first
ionization energy?
(1) alkali metals
(2) alkaline earth metals
(3) halogens
(4) noble gases
64. Base your answer to the following question on the information below
The table below lists physical and chemical properties of six elements at standard pressure that
correspond to known elements on the Periodic Table. The elements are identified by the code letters, D,
E, G, J, L, and Q.
Identify, by code letter, the element that is a noble gas in the “Properties of Six Elements at Standard Pressure”
table.
65. As a neutral sulfur atom gains two electrons,
what happens to the radius of the atom?
Quarterly 1 Review
Trupia
66. Base your answer to the following question on the information below.
A safe level of fluoride ions is added to many public drinking water supplies. Fluoride ions have been
found to help prevent tooth decay. Another common source of fluoride ions is toothpaste. One of the
fluoride compounds used in toothpaste is tin (II) fluoride.
A town located downstream from a chemical plant was concerned about fluoride ions from the plant
leaking into its drinking water. According to the Environmental Protection Agency, the fluoride ion
concentration in drinking water cannot exceed 4 ppm. The town hired a chemist to analyze its water.
The chemist determined that a 175-gram sample of the town’s water contains 0.000 250 grams of
fluoride ions.
How many parts per million of fluoride ions are present in the analyzed sample? Is the town’s drinking water
safe to drink? Support your decision using information in the passage and your calculated fluoride level.
67. Base your answer to the following question on the data table provided.
On the same grid, plot the data from the data table. Circle and connect the points.
68. Describe one chemical property of Group 1
metals that results from the atoms of each
metal having only one valence electron.
69. Base your answer to the following question on
the information below.
Potassium ions are essential to human health.
The movement of dissolved potassium ions, K
+
(aq), in and out of a nerve cell allows that cell
to transmit an electrical impulse.
What is the total number of electrons in a
potassium ion?
Quarterly 1 Review
Trupia
____70. The percent by mass of nitrogen in NH
4NO3
(formula mass = 80) is approximately
(1) 18%
(3) 32%
(2) 23%
(4) 35%
____71. A sample of a substance containing only
magnesium and chlorine was tested in the
laboratory and was found to be composed of
74.5% chlorine by mass. If the total mass of the
sample was 190.2 grams, what was the mass of
the magnesium?
(1) 24.3 g
(3) 70.9 g
(2) 48.5 g
(4) 142 g
____72. Base your answer to the following question
on the table below shows the data collected
during the heating of a 5.0 gram sample of a
hydrated salt.
____74. The percent by mass of water in BaCl2 • 2H
2O (formula mass = 243) is equal to
(1)
(3)
(2)
(4)
____75. What is the percent by mass of oxygen in
magnesium oxide, MgO?
(1) 20%
(3) 50%
(2) 40%
(4) 60%
____76. A 60. gram sample of LiCl • H2O is heated
in an open crucible until all of the water has
been driven off. What is the total mass of LiCl
remaining in the crucible?
(1) 18 g
(3) 42 g
(2) 24 g
(4) 60 g
____77. What is the total mass of 2.0 moles of H
2(g)?
(1) 1.0 g
(3) 3.0 g
(2) 2.0 g
(4) 4.0 g
After 60. minutes, how many grams of water
appear to remain in the salt?
(1) 0.00
(3) 1.9
(2) 2.0
(4) 0.90
____73. What is the percent by mass of hydrogen in
CH3COOH (formula mass = 60.)?
(1) 1.7%
(3) 6.7%
(2) 5.0%
(4) 7.1%
____78. What is the mass in grams of 2.0 moles of
NO2?
(1) 92
(3) 46
(2) 60.
(4) 30.
____79. The gram molecular mass of CO2 is the
same as the gram molecular mass of
(1) CO
(3) C2H6
(2) SO2
(4) C3H8
____80. What is the total mass of oxygen in 1.00
mole of
Al2(CrO4)3?
(1) 192 g
(3) 64.0 g
(2) 112 g
(4) 48.0 g
____81. Which quantity is equivalent to 39 grams of
LiF?
(1) 1.0 mole
(3) 0.50 mole
(2) 2.0 moles
(4) 1.5 moles
Quarterly 1 Review
Trupia
____82. The number of moles of molecules in a 12.0gram sample of Cl2 is
(1)
(2)
(3)
(4)
____83. What is the mass in grams of 1.00 mole of O
2 gas?
(1) 11.2
(3) 22.4
(2) 16.0
(4) 32.0
84. Fluorine is a Group 17 element. Fluorine is the most electronegative and reactive of all elements. It is a pale
yellow, corrosive gas, which reacts with practically all organic and inorganic substances.
a Draw the Lewis electron-dot structure for an atom of fluorine.
b What is the definition (or your interpretation} of the term "electronegativity".
c Explain why the electronegativity of elements in Group 17 decreases as you go down within that group.
85. A knowledge of the ionization energies of elements can be very useful in predicting the activity and type of
reaction an element will have.
a What does the ionization energy quantitatively measure about an atom?
b Why do ionization energies decrease from the top to the bottom of a group on the periodic table of elements?
c Why do ionization energies increase from left to right across any period?
86. Chorine is a member of the halogen (saltforming) group of elements. It is a greenishyellow gas, combining directly with nearly all
elements. In nature it is found in the combined
state only, chiefly with sodium as common salt
(NaCl), carnallite, and sylvite.
a Draw the electron-dot diagram of an atom of
chlorine.
b From the passage above give one physical
property and one chemical property of chlorine?
Quarterly 1 Review
Trupia
87. One electron is removed from both an Na atom and a K atom, producing two ions. Using principles of atomic
structure, explain why the Na ion is much smaller than the K ion. Discuss both ions in your answer.
88. The following procedures are carried out during a laboratory activity to determine the mass in grams of CuSO
4 in a hydrated sample of CuSO4 • 5H2O.
Step 1 Determine the mass in grams of the crucible and CuSO4•5 H2O.
Step 2 Determine the mass in grams of the crucible and CuSO4
Step 3 Determine the mass in grams of CuSO4 • 5 H2O.
Step 4 Determine the mass in grams of the empty crucible.
Step 5 Determine the mass in grams of CuSO4
Arrange the steps above in the order that the student should use to determine the mass of CuSO4 in the sample.
_______, _______, _______, _______, ________
89. A student heats a 243 gram sample of BaCl2 • 2H2O hydrated crystals?
a What was the percentage by mass of water in the hydrated crystals?[Show all work]
b If all the water was driven out of the crystal, what would be the expected weight of the BaCl2 sample
remaining?[Show all work]
90. The table below shows the data collected during the heating of a 10.0-gram sample of a hydrated salt.
a What is the percent by mass of water in the original sample?
b Why is it important in this experiment to heat the salt until the mass of salt remains constant?
Quarterly 1 Review
Trupia
91. In a laboratory experiment, a student determined the mass of the product, CaCl2(s), to be 45.5 grams.
a Calculate the gram formula mass of CaCl2(s). Round atomic masses from the Periodic Table to the nearest
tenth. [ Show all work. Indicate the correct answer in proper significant figures and include an appropriate unit.]
b Calculate the number of moles of CaCl2(s) produced. [Show all work. Indicate the correct answer in proper
significant figures.]
92. In a laboratory experiment, a student determined the mass of the product, KClO3(s), to be 45.7 grams.
a. Calculate the gram formula mass of KClO3(s). Round atomic masses from the Periodic Table to the nearest
tenth. [Show all work. Indicate the correct answer in proper significant figures and include an appropriate unit.]
b. Calculate the number of moles of KClO3(s) produced. [Show all work. Indicate the correct answer in proper
significant figures.]
93. Base your answers to the following questions on the information below.
Sodium is an essential ingredient in the human diet. The Federal Food and Drug Administration
recommends that the average adult daily requirement for sodum is 2.4 grams. Sodium is
ingested through consuming plant and animal tissues, but another good source is table salt,
sodium chloride.
a) Write the chemical formula of sodium chloride.
b) What is the gram-formula mass of a mole of sodium chloride?
c) How many moles of table salt, sodium chloride would need to be comsumed in order to ingest the 2.4 grams?
[Show all work]
Quarterly 1 Review
Answer Key
[New Exam]
1.
2
26.
1
41.
3
2.
1
27.
3
42.
3
3.
4
28.
4
43.
2
4.
2
29.
2
44.
2
5.
2
30.
1
45.
3
6.
1
31.
3
46.
1
7.
1
32.
3
47.
2
8.
1
33.
2
48.
1
9.
3
34.
4
49.
4
– increases; – The ion is
larger then the atom.
66. The water has a
fluoride level of 1.43
ppm, which is below the
maximum contaminant
level for fluoride, so it is
safe to drink; F– below 4
ppm, safe, below max
level; Safe: 1.43 ppm < 4
ppm
67.
10.
1
35.
3
50.
2
11.
2
36.
1
51.
3
12.
4
52.
4
13.
1
53.
1
14.
3
54.
4
15.
4
55.
1
16.
1
56.
4
17.
3
57.
3
18.
2
58.
1
68. Examples: -form 1+
ions -react vigorously
with water -easily lose
one electron -form ionic
bonds with nonmetals form halides with the
general formula MX
19.
4
59.
2
69. 18
20.
3
60.
2
70.
4
21.
4
37. a) 118 neutrons, 79
electrons. b) Acceptable
responses include, but are
not limited to, these
examples: – The atom’s
internal structure is
mostly empty space or –
mostly empty space
c) Acceptable responses
include, but are not
limited to, these
examples: – The nucleus
of the gold atoms have a
positive charge. or – Both
the nucleus of the gold
atoms and the alpha
particles have the same
charge. or – positive
charge
61.
1
71.
2
22.
1
72.
1
23.
2
73.
3
24.
1
74.
2
25.
2
75.
2
3
38. 1.5 ] 10–19 J ± 0.1 ] 10–19 62.
J
63.
4
39. 20
64. D or He
40.
1
65. Examples: – gets bigger;
Quarterly 1 Review
Answer Key
[New Exam]
76.
3
77.
4
78.
1
79.
4
80.
1
81.
4
b. Examples: Physical –
Chlorine is greenishyellow. – Chlorine is a
gas.
Chemical –
a Halogen; – very
reactive; combines with
sodium
87. Examples:
–K1+ has three energy
levels, while Na1+ has
83.
4
only two energy levels.
–Na+ has its valence
84.
electrons drawn closer to
the nucleus than K+
b) Electronegativity because the effect of the
is the relative measure of
nucleus is greater for Na+.
how strongly the nucleus
of an atom will attract 88. 4,1,3,2,5
electrons from another
atom. c) As you go
89. a) 36/ (137 + 71 + 36) ×
down the period the
100 = 15% b) 207 grams
nuclear charge gets
shielded by layers of more90. a) 20.% b) To insure
electrons and as the atom
that all of the water has
gets larger, the distance
been driven out of the salt.
to the nuclear charge gets
greater.
91. a) 40.1 + 2(35.5) = 101
82.
2
grams b) 45.5g x 1.00
85. a) The ionization energy
mole/101g = .450 mole
is the amount of energy
needed to remove the
92. a) 39.1 + 35.5 + 3(16.0)
most loosely bound
= 122.6 g
b) 45.7g x
electron from an atom.
1.00 mole/122.6g = .373
b) The electrons are
mole
farther away in the lower
periods so there is less 93. a) NaCl
b) 57.5 grams
pull from the nucleus.
c) 0.042
Also, there is shielding
from the electrons that are
closer to the nucleus. c)
Electrons are held tighter
to an atom because of the
increase in nuclear charge.
86.