Download Chemistry Benchmark 1 Review

Chemistry Benchmark 1 Review
Completion
Complete each statement.
1. Chemistry is the study of _____________________ and the changes that it undergoes.
2. A(n) ______________________ is a set of controlled observations that test the hypothesis.
3. 100.00 meters  50.000 centimeters  1.0000 kilometer = ____________________ meters.
4. A process that involves one or more substances changing into new substances is known as a
____________________ change.
5. Cutting a sheet of paper is an example of a ____________________ change.
6. A ____________________ property enables a substance to combine with or change into one or more
substances.
7. Sugar is a ____________________ form of matter with a definite shape and volume.
8. A ____________________ is a subatomic particle that has mass nearly equal to that of a proton, but it carries
no electrical charge.
9. Atoms with the same number of protons but different number of neutrons are called ____________________.
10. An alpha particle is _____________________ charged with two protons and neutrons.
11. Democritus believed that matter is made up of tiny individual particles known as a(n)
____________________.
12. The number of protons in an atom is called the ____________________ of the element.
13. The ____________________ principle states that a maximum of two electrons may occupy a single atomic
orbital, but only if the electrons have opposite spins.
14. The arrangement of electrons in an atom is called the ____________________ of an atom.
15. The group 2A elements are known as ____________________ metals.
16. Elements that have physical and chemical properties of both metals and nonmetals are known as
____________________.
Short Answer
17. Explain the difference between mass and weight.
18. Explain how hypothesis and theory are different.
Use the figure below to answer the question.
19. Infer a qualitative measurement that can be made from the scene shown.
20. Infer a quantitative measurement that can be made from the scene shown.
21. What must be immediately done if chemicals come in contact with the eyes or skin while performing an
experiment in the laboratory?
22. Evaluate this dimensional analysis setup. A paperclip is 3.2 cm long. How many paperclips would fit in a
football field (100 yards) if 1 inch = 2.54 cm?
23. What two things does a conversion factor do?
24. The data for two different measurements are shown below. Which experiment was more accurate? Explain
your answer.
Sample
Measured value
Accepted value
Distance
54,700 m
57,900 m
Mass
61.3 g
65.7 g
A student conducts an experiment to determine the effect of adding salt on the boiling temperature of water.
The results are shown below.
Sample
Amount of Salt
Boiling Temperature
Sample 1
0g
100.0° C
Sample 2
2g
102.3° C
Sample 3
5g
104.8° C
Sample 4
10 g
107.5° C
25. The student graphs this data using the axes shown. Is this graph correct? Explain your answer.
26. Define a base unit.
27. The distance between the earth and the sun is 90.0 million miles. Calculate this distance in meters up to three
significant digits.
28. Convert 600 mg to grams.
29. How many significant digits are there in 6.023  1023 molecules?
30. Identify both a physical change and a chemical change that could be done to a piece of paper.
31. Distinguish between element and compound.
32. Distinguish between homogeneous and heterogeneous mixtures. Give an example of each one.
33. Compare and contrast mass number and atomic mass.
34. What is the average atomic mass of this element?
Isotope
Mass (amu)
Percent Abundance
Phosphorus-29
29
5%
Phosphorus-31
31
71%
Phosphorus-32
32
24%
35. What is the average atomic mass of this element?
Isotope
Mass (amu)
Percent Abundance
Silver-105
105
48%
Silver-108
108
43%
Silver-109
109
9%
36. Write the chemical symbol for the isotope of cobalt with 37 neutrons.
37. Element X has an average atomic mass of 64.32 amu. If this element consists of only two isotopes, X-64 and
X-65, which isotope is present in the greater abundance? Explain how you can tell.
38. Define an atom.
39. What do you understand by the term atomic mass unit (amu)?
40. How are atomic number and mass number denoted in the chemical symbol of the isotope of an element?
Express the shortened notation for an isotope of element X with atomic number 92 and atomic mass 238.
41. Identify the element containing 34 protons.
42. What were the main flaws in Dalton’s atomic theory?
43. Summarize the relationship between wavelength, frequency, and energy of a wave.
44. A student records the following electron configuration for the element Arsenic (As). Evaluate this student’s
answer.
1s22s22p63s23p64s24d104p3
45. Explain why it is only possible for two electrons to exist in the same orbital.
46. Use the model of the atom shown to identify the correct element. Write the electron configuration and orbital
diagram for this element.
47. Which rule for filling of orbitals by electrons in the element Silicon is being violated in the orbital diagram
shown? Justify your answer.
48. Which rule for the filling of orbitals in the element Phosphorus is being violated in the orbital diagram
shown? Justify your answer.
49. Which rule for the filling of orbitals by electrons in the element Magnesium is being violated? Justify your
answer.
50. Define a photon. What is the formula used to calculate the energy of a photon?
51. Why does a piece of iron appear red when heated sufficiently and blue at a higher temperature?
52. What is the ground state electron configuration of chlorine and the number of valence electrons in it?
53. How many valence electrons are present in cesium? Write the electron configuration of cesium if the atomic
number is 55.
54. Write the noble gas form of the electron configuration and the electron dot structure of sodium and oxygen.
55. Write the noble gas form of the electron configuration and the electron dot structure of selenium and
phosphorus.
56. A student makes the following statement: “It’s easy to tell which energy level an element is in - you just count
down which row it is in, and that’s the energy level.” Is this student correct? Explain how you came to your
conclusion.
57. Explain what is meant by the “octet rule.” Does it hold true for the modern periodic table?
58. Label the blank periodic table with the following terms.
A: metalloids
B: element with the highest electronegativity
C: alkali metals
D: lanthanide series
E: element with the greatest atomic radius
F: noble gases
G: halogens
59. Explain the significance of the stair-step line located near the right-hand side of the periodic table
60. Do the figures in this partial periodic table demonstrate the trend in atomic radius, ionic radius, or neither of
these? Relate your answer to the structure of atoms across the periodic table.
61. Place these five elements in order of electronegativity, with the highest electronegativity first.
62. Identify the representative elements from the list given below.
Na, Ca, Sc, Co, Ni, Si, N, Se, Cl, Ge
63. Why is argon placed before potassium in the modern periodic table?
64. Why do elements in the same group have similar properties?
65. Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?
66. List the general electron configuration and location of the s, p, d, and f-block elements in the periodic table.
67. Use the periodic table to write the names of the third alkali metal and the first transition metal.
Problem
68. A vessel contains 30 mL of water. A sample of 5.0 g of copper metal is dropped into this vessel, raising the
level of water in it to 40 mL. What is the density of the copper sample?
69. When a 5.00-g metal piece, A, was immersed in 38.0 mL of water, the water level rose to 50.0 mL. Similarly,
when a 5.00-g metal piece, B, was immersed in 38.0 mL of water, the level of water rose to 60.0 mL.
Compare the density of the metal pieces, A and B.
70. Calculate the area of a rectangular piece of land with a length of 8.0  105 cm and a width of 4.0  103 cm.
Express your answer in meters.
71. Complete the following table:
Element
Number of
protons
Sodium
Phosphorus
15
Cobalt
27
Bromine
Silver
Number of
electrons
11
Number of
neutrons
12
Atomic
number
Mass number
31
32
35
80
61
47
72. An element X has two naturally occurring isotopes: X-79 (abundance = 50.69%, mass = 78.918 amu) and
X-81 (abundance = 49.31%, mass = 80.917 amu). Calculate the weighted atomic mass of X. Also, identify the
unknown element which exists as a reddish-brown gas and is a liquid at room temperature.
73. An element X has three naturally occurring isotopes: X-24, X-25, and X-26. The atomic mass of X-25 is
24.986 amu and the relative abundance is 10.00 %. The atomic mass of X-26 is 25.982 amu and the relative
abundance is 11.01 %.Given that the weighted atomic mass of the element X is 24.305, calculate the mass
contribution due to the isotope X-24 and identify the element.
74. Calculate the number of protons, electrons, and neutrons in an atom of the element Pb with mass number 207
and atomic number 82.
75. Fluorine (F) contains 9 proton and 10 neutrons. Calculate its mass in amu for 81 atoms. (Given: mass of a
proton = 1.007276 amu, mass of a neutron = 1.008665 amu).
76. Lead contains 82 protons and 125 neutrons. Write the shortened notation of the element with its symbol,
atomic number, and mass number.
77. How many sublevels and orbitals are possible in the third energy level?
78. Write the ground state electron configuration of sulfur and draw its electron-dot structure.
79. Two elements A and B have atomic numbers 8 and 17 respectively. Identify their groups in the periodic table.
80. An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than
krypton but less than iodine. Use the periodic table to identify the element.
81. Identify the element having the largest size and the element having the highest electronegativity from the list
of electron configurations given below:
a. [Ne] 3s23p3
b. [Ne] 3s23p4
c. [Ne] 3s23p5
d. [Ne] 3s23p34s23d3
82. Arrange the elements given below in the increasing order of their atomic size.
Element A 1s22s22p6
Element B 1s22s2
Element C 1s22s22p63s1
Element D 1s22s22p3
Chemistry Benchmark 1 Review
Answer Section
COMPLETION
1. ANS: matter
PTS:
NAT:
KEY:
2. ANS:
1
DIF: 1
B.2
STA: ABC 1.1
Chemistry | Matter
experiment
PTS:
OBJ:
STA:
KEY:
3. ANS:
1
DIF: 1
REF: Page 11
1.3.2 Compare and contrast types of data.
NAT: G.2
ABC 1.1
TOP: Compare and contrast types of data.
Theory | Scientific law
MSC: 1
1100.5
PTS:
OBJ:
STA:
KEY:
4. ANS:
1
DIF: 1
REF: Page 26
2.1.2 Explain how adding a prefix changes a unit.
NAT: UCP.1
ABC 1.1
TOP: Explain how adding a prefix changes a unit.
Meter | Kilometer | Centimeter
MSC: 2
chemical
PTS:
OBJ:
NAT:
TOP:
KEY:
5. ANS:
1
DIF: 1
REF: Page 62
3.2.2 Define chemical change and list several indications that a chemical change has taken place.
UCP.3 | B.3 STA: ABC 10.1
Define chemical change and list several indications that a chemical change has taken place.
Chemical change
MSC: 1
physical
PTS:
OBJ:
NAT:
TOP:
KEY:
6. ANS:
1
DIF: 1
REF: Page 61
3.2.1 Define physical change and list several common physical changes.
UCP.3 | B.2 STA: ABC 10.1
Define physical change and list several common physical changes.
Physical change
MSC: 2
chemical
PTS:
OBJ:
NAT:
KEY:
7. ANS:
1
DIF: 1
REF: Page 57
3.1.2 Distinguish between physical and chemical properties.
B.2
STA: ABC 10.1
TOP: Distinguish between physical and chemical properties.
Chemical property
MSC: 1
solid
PTS:
OBJ:
STA:
KEY:
REF: Page 7
OBJ: 1.2.1 Define chemistry and matter.
TOP: Define chemistry and matter.
MSC: 1
1
DIF: 1
REF: Page 58
3.1.3 Differentiate among the physical states of matter.
NAT: B.2
ABC 10.1
TOP: Differentiate among the physical states of matter.
Solids
MSC: 2
8. ANS: neutron
PTS:
OBJ:
NAT:
TOP:
KEY:
9. ANS:
PTS:
OBJ:
NAT:
TOP:
KEY:
10. ANS:
1
DIF: 1
REF: Page 96
4.2.2 Describe the structure of the nuclear atom, including the locations of the subatomic particles.
B.1 | G.3
STA: ABC 10.1 | ABC 10.2
Describe the structure of the nuclear atom, including the locations of the subatomic particles.
Neutron
MSC: 1
isotopes
1
DIF: 1
REF: Page 100
4.3.2 Define an isotope and explain why atomic masses are not whole numbers.
B.1
STA: ABC 10.1 | ABC 10.2
Define an isotope and explain why atomic masses are not whole numbers.
Isotopes
MSC: 1
positively
PTS: 1
DIF: 1
REF: Page 106
OBJ: 4.4.2 Characterize alpha, beta, and gamma radiation in terms of mass and charge.
NAT: B.1 | B.6
STA: ABC 10.1 | ABC 10.2
TOP: Characterize alpha, beta, and gamma radiation in terms of mass and charge.
KEY: Alpha radiations
MSC: 1
11. ANS:
atomos
atom
PTS:
OBJ:
NAT:
TOP:
KEY:
12. ANS:
1
DIF: 1
REF: Page 88
4.1.1 Compare and contrast the atomic models of Democritus and Dalton.
G.3 | UCP.2 | B.1 | B.2
STA: ABC 10.1
Compare and contrast the atomic models of Democritus and Dalton.
Atom
MSC: 1
atomic number
PTS:
OBJ:
NAT:
TOP:
KEY:
13. ANS:
1
DIF: 1
REF: Page 98
4.3.1 Explain the role of atomic number in determining the identity of an atom.
B.1
STA: ABC 10.1
Explain the role of atomic number in determining the identity of an atom.
Atomic number
MSC: 1
Pauli exclusion
PTS: 1
DIF: 1
REF: Page 136
OBJ: 5.3.1 Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron
configurations using orbital diagrams and electron configuration notation.
NAT: B.6
STA: ABC 10.1 | ABC 10.2
TOP: Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron
configurations using orbital diagrams and electron configuration notation.
KEY: Pauli exclusion principle
MSC: 1
14. ANS: electron configuration
PTS: 1
DIF: 1
REF: Page 135
OBJ: 5.3.1 Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron
configurations using orbital diagrams and electron configuration notation.
NAT: B.6
STA: ABC 10.2
TOP: Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron
configurations using orbital diagrams and electron configuration notation.
KEY: Electron configuration
MSC: 1
15. ANS: alkaline earth
PTS:
OBJ:
NAT:
TOP:
KEY:
16. ANS:
1
DIF: 1
REF: Page 155
6.1.1 Trace the development and identify key features of the periodic table.
G.3 | B.1 | UCP.1
STA: ABC 10.1
Trace the development and identify key features of the periodic table.
Alkaline earth metals
MSC: 1
metalloids
PTS:
OBJ:
NAT:
TOP:
KEY:
1
DIF: 1
REF: Page 158
6.1.1 Trace the development and identify key features of the periodic table.
G.3 | B.1 | UCP.1
STA: ABC 10.1
Trace the development and identify key features of the periodic table.
Metalloids
MSC: 1
SHORT ANSWER
17. ANS:
Mass is a measurement of the amount of matter in a substance, while weight is a measure of gravity’s effect
on that mass.
PTS: 1
DIF: Bloom's Level 2
NAT: UCP.2 | E.2
STA: ES 9.1
18. ANS:
A hypothesis is a prediction of the outcome of one experiment. A theory is a description of how a process is
believed to occur and is based on the results of many different experiments.
PTS: 1
DIF: Bloom's Level 4
NAT: UCP.2 | A.2
STA: ABC 1.1
19. ANS:
Answers should be descriptions of object without using numbers (counting or measuring).
PTS: 1
DIF: Bloom's Level 3
NAT: UCP.3 | A.1 | A.2
STA: ABC 10.1
20. ANS:
Answers should include a numerical value obtained from measurement or counting.
PTS: 1
DIF: Bloom's Level 3
NAT: UCP.3 | A.1 | A.2
STA: ABC 10.1
21. ANS:
Flush the area immediately with large quantities of water and inform the teacher of the spill and the chemical.
PTS: 1
DIF: 1
REF: Page 16
OBJ: 1.4.2 Apply knowledge of laboratory safety.
NAT: A.1 | A.2
STA: ABC 3.1
TOP: Apply knowledge of laboratory safety.
KEY: Laboratory safety
MSC: 1
22. ANS:
The second conversion factor, 1 inch = 2.54 cm, is reversed. It needs to be arranged so that the unit in the
denominator of one fraction can cancel out the unit in the numerator of the next fraction, and so on.
PTS: 1
DIF: Bloom's Level 6
STA: ABC 1.1
23. ANS:
1. cancels one unit
2. introduces a new unit
NAT: UCP.2
PTS: 1
DIF: Bloom's Level 2
NAT: UCP.2
STA: ABC 1.1
24. ANS:
The distance measurement has an error of 5.53%. The mass measurement has an error of 6.70%. Therefore,
distance was measured more accurately.
PTS: 1
DIF: Bloom's Level 6
NAT: UCP.2 | UCP.3
STA: ABC 1.1
25. ANS:
The independent variable should be placed on the X axis, and the dependent variable on the Y axis. This
graph is correct as shown.
PTS: 1
DIF: Bloom's Level 6
NAT: UCP.2
STA: ABC 1.1
26. ANS:
A base unit is a defined unit in a system of measurement that is based on an object or event in the physical
world. It is independent of other units.
PTS: 1
DIF: 1
REF: Page 26
OBJ: 2.1.1 Define SI base units for time, length, mass, and temperature.
NAT: UCP.1
STA: ABC 1.1
TOP: Define SI base units for time, length, mass, and temperature.
KEY: Base unit
MSC: 1
27. ANS:
1.44  1011m
PTS: 1
DIF: 1
REF: Page 34
OBJ: 2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1
STA: ABC 1.1
TOP: Use dimensional analysis to convert between units.
KEY: Miles | Meter
MSC: 3
28. ANS:
1mg = 1/ 1000 g
600 mg = 0.6 g
PTS:
OBJ:
STA:
KEY:
29. ANS:
1
DIF: 1
REF: Page 34
2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1
ABC 1.1
TOP: Use dimensional analysis to convert between units.
Gram | Milligram
MSC: 3
There are four significant digits in 6.023  1023 molecules.
PTS: 1
DIF: 1
REF: Page 39
OBJ: 2.3.2 Use significant figures and rounding to reflect the certainty of data.
NAT: E.2 | G.2
STA: ABC 1.1
TOP: Use significant figures and rounding to reflect the certainty of data.
KEY: Significant figures | Molecules
MSC: 2
30. ANS:
A physical change might be ripping it, crumpling it, or writing on it with pencils or pens. A chemical change
might be burning it or letting it rot.
PTS: 1
DIF: Bloom's Level 3
NAT: UCP.3 | B.2 | B.3
STA: ABC 10.1
31. ANS:
An element is the smallest piece of matter that retains its physical and chemical properties, and is made up of
only one type of atom. A compound is made of more than one different element chemically joined together. A
compound can be broken into smaller pieces by chemical means.
PTS: 1
DIF: Bloom's Level 2
NAT: UCP.2
STA: ABC 10.1
32. ANS:
A homogeneous mixture is a combination of substances in varying proportions where the individual
substances cannot be distinguished. Every part of the mixture has the same composition as any other part,
such as in a beverage made from powdered mix. In a heterogeneous mixture, the different substances can be
distinguished. Parts of the mixture have different compositions, as in a chocolate-chip cookie.
PTS: 1
DIF: Bloom's Level 3
NAT: UCP.2
STA: ABC 10.1
33. ANS:
Mass number is the total number of neutrons and protons in an individual atom. It is an integer number.
Atomic number, or average atomic number, is the weighted average mass of all of the different isotopes found
in a sample of an element. Because it is a weighted average, atomic mass is usually a decimal number.
PTS: 1
DIF: Bloom's Level 2
STA: ABC 10.1 | ABC 10.2
34. ANS:
(29*.05)+(31*.71)+(32*.24) = 31.14 amu
NAT: UCP.2 | B.1
PTS: 1
DIF: Bloom's Level 3
STA: ABC 10.1 | ABC 10.2
35. ANS:
(105*.48)+(108*.43)+(109*.09) = 106.65 amu
NAT: UCP.2 | B.1
PTS: 1
DIF: Bloom's Level 3
STA: ABC 10.1 | ABC 10.2
36. ANS:
NAT: UCP.2 | B.1
PTS: 1
DIF: Bloom's Level 3
STA: ABC 10.1 | ABC 10.2
NAT: B.1
37. ANS:
The more abundant isotope would be X-64. With only two isotopes, one can be certain that the weighted
average atomic mass will be closer to the isotope in greater abundance. Since the average mass is 64.32,
which rounds to 64, isotope X-64 must be more abundant than X-65.
PTS: 1
DIF: Bloom's Level 4
NAT: UCP.2
STA: ABC 10.1 | ABC 10.2
38. ANS:
An atom is the smallest particle of an element that retains the properties of the element.
PTS: 1
DIF: 1
REF: Page 90
OBJ: 4.1.2 Define an atom.
NAT: B.1
STA: ABC 10.1
TOP: Define an atom.
KEY: Atom
MSC: 1
39. ANS:
The atomic mass unit measures the mass of an atom relative to the mass of carbon-12 atom, which is taken as
a standard. One atomic mass unit is defined as 1/12 the mass of a carbon-12 atom.
PTS: 1
DIF: 1
REF: Page 102
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic
number.
KEY: Atomic mass unit
MSC: 2
40. ANS:
The atomic number is written as the subscript in the chemical symbol of an element and the mass number is
written as the superscript in the chemical symbol of an element. The notation for an isotope of element X is
denoted as
.
PTS: 1
DIF: 2
REF: Page 98 | Page 100
OBJ: 4.3.2 Define an isotope and explain why atomic masses are not whole numbers.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Define an isotope and explain why atomic masses are not whole numbers.
KEY: Atomic number | Mass number | Isotopes
MSC: 3
41. ANS:
The element containing 34 protons is Selenium (Se).
PTS: 1
DIF: 1
REF: Page 98
OBJ: 4.3.1 Explain the role of atomic number in determining the identity of an atom.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Explain the role of atomic number in determining the identity of an atom.
KEY: Atomic number
MSC: 1
42. ANS:
There were two main flaws in Dalton’s atomic theory.
a. Atoms are not indivisible. They are divisible into several subatomic particles.
b. All atoms of a given element may not have identical properties as their masses may vary slightly.
PTS:
OBJ:
NAT:
TOP:
KEY:
1
DIF: 2
REF: Page 90
4.1.1 Compare and contrast the atomic models of Democritus and Dalton.
G.3 | UCP.2 | B.1 | B.2
STA: ABC 10.1 | ABC 10.2
Compare and contrast the atomic models of Democritus and Dalton.
Dalton's atomic theory
MSC: 2
43. ANS:
As the amount of energy carried by a wave increases, the individual waves get closer together, increasing
their frequency but decreasing their wavelength.
PTS: 1
DIF: Bloom's Level 3
NAT: UCP.2 | B.6
STA: ABC 10.2 | ABC 10.3
44. ANS:
The “d10” should be preceded by a 3; although the first set of d-block elements are in the fourth period, these
electrons are actually contained in the third energy level due to the overlapping of energy levels and orbitals.
PTS: 1
DIF: Bloom's Level 6
NAT: UCP.2 | B.1
STA: ABC 10.2 | ABC 10.3
45. ANS:
Electrons have a spin. In any given orbital, only two electrons can exist because one will spin in an “upward”
direction while the other one spins in a “downward” direction. A pair of electrons can only exist in an orbital
if they are spinning in opposite directions.
PTS: 1
DIF: Bloom's Level 3
NAT: B.1
STA: ABC 10.2 | ABC 10.3
46. ANS:
The element is Silicon. The electron configuration is 1s2s222p63s23p6. The orbital diagram is shown below.
PTS: 1
DIF: Bloom's Level 5
NAT: UCP.2 | B.1
STA: ABC 10.2 | ABC 10.3
47. ANS:
This violates the Aufbau principle, which states that electrons must fill in the orbital with the lowest amount
of energy before filling any orbitals with a greater amount of energy. In the diagram shown, electrons are
placed in the 3p orbitals before the 3s is filled.
PTS: 1
DIF: Bloom's Level 4
NAT: UCP.2 | B.1
STA: ABC 10.2 | ABC 10.3
48. ANS:
This is violating Hund’s rule. According to Hund’s rule, single electrons must occupy the orbitals within the
same energy level and type of orbital before two electrons are allowed to occupy the same orbital. Here, two
electrons occupy the first 3p orbital before the other two orbitals have one electron.
PTS: 1
DIF: Bloom's Level 4
NAT: UCP.2 | B.1
STA: ABC 10.2 | ABC 10.3
49. ANS:
The Pauli exclusion principle is being violated. The Pauli exclusion principle requires that if two electrons
occupy the same orbital, they must have opposite spin directions. This is generally shown by having arrows
pointing either up or down in the orbital diagrams. Here, the two electrons in the 3s orbital are spinning the
same direction, as indicated by the arrows pointing the same direction.
PTS: 1
DIF: Bloom's Level 4
NAT: UCP.2 | B.1
STA: ABC 10.2 | ABC 10.3
50. ANS:
A photon is a particle of electromagnetic radiation that has no mass and carries a quantum of energy. The
energy of a photon can be calculated using the formula Equantum h , where E is energy of the photon, h is
Planck’s constant, and is frequency of the photon.
PTS: 1
DIF: 1
REF: Page 123
OBJ: 5.1.1 Compare the wave and particle models of light.
NAT: B.1
STA: ABC 10.2 | ABC 10.3
TOP: Compare the wave and particle models of light.
KEY: Photon | Energy levels
MSC: 1
51. ANS:
A piece of iron appears red when heated sufficiently and blue at a higher temperature, because the kinetic
energy of iron increases when it is heated. With an increase in the amount of energy, different colors of light
are emitted. These colors correspond to different frequencies and wavelengths.
PTS: 1
DIF: 1
REF: Page 122
OBJ: 5.1.2 Define a quantum of energy and explain how it is related to an energy change of matter.
NAT: B.6
STA: ABC 10.1
TOP: Define a quantum of energy and explain how it is related to an energy change of matter.
KEY: Quantum
MSC: 2
52. ANS:
The ground state electron configuration of chlorine is 1s22s22p63s23p5. It has 7 valence electrons.
PTS: 1
DIF: 1
REF: Page 138
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
STA: ABC 10.2 | ABC 10.3
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Valence electrons | Electron configuration
MSC: 2
53. ANS:
There is only one valence electron in cesium. The electron configuration of cesium with atomic number 55 is
[Xe]6s1.
PTS: 1
DIF: 1
REF: Page 140
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
STA: ABC 10.2 | ABC 10.3
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Valence electrons | Electron configuration
MSC: 1
54. ANS:
a. The noble gas form of the electron configuration of sodium is [Ne]3s1. Its electron dot structure is
b.
The noble gas form of electron configuration of oxygen is [He]2s22p4. Its electron dot structure is
PTS: 1
DIF: 2
REF: Page 138 | Page 140
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
STA: ABC 10.1 | ABC 10.2
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Electron configuration | Electron-dot structure
MSC: 2
55. ANS:
a.
The noble gas form of the electron configuration of selenium is [Ar]4s24p4. Its electron-dot structure is
b.
The noble gas form of the electron configuration of phosphorus is [Ne]3s23p5. Its electron-dot structure
is .
PTS: 1
DIF: 2
REF: Page 138
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
STA: ABC 10.1 | ABC 10.2
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Electron configuration | Electron-dot structure
MSC: 2
56. ANS:
No, the student is not correct. We know from writing electron configurations (Chapter 5) that elements in
each row of the d-block are actually contained in the energy level of the previous row; therefore one cannot
merely count down the rows. Periods and energy levels are not the same thing. One should also be careful
to not claim that the top row of the d-block is energy level 1 because it is the first row of that section.
PTS: 1
DIF: Bloom's Level 6
NAT: B.1 | B.6
STA: ABC 10.1
57. ANS:
The octet rule states that most elements would like to have eight electrons in their outer energy level to
become stable like the closest noble gas.
PTS: 1
STA: ABC 10.1
58. ANS:
DIF: Bloom's Level 4
NAT: B.2
PTS: 1
DIF: Bloom's Level 1
NAT: UCP.2 | B.2
STA: ABC 10.1
59. ANS:
The stairstep line separates the metals from the nonmetals on the periodic table. Elements that are adjacent
to this line are considered metalloids and have some properties of metals and some properties of nonmetals.
PTS: 1
STA: ABC 10.1
DIF: Bloom's Level 3
NAT: UCP.2 | B.2
60. ANS:
These show the atomic radius change. As electrons are added to the outer energy levels of an atom (as one
moves across the periodic table), the size of the atom decreases. This is because the additional positive
charge in the nucleus attracts the electrons more strongly and no additional shielding effect occurs across the
period.
PTS: 1
STA: ABC 10.1
61. ANS:
B, D, C, E, A
DIF: Bloom's Level 4
PTS: 1
DIF: Bloom's Level 4
STA: ABC 10.1
62. ANS:
Na, Ca, N, Si, Se, Cl, Ge
NAT: UCP.2 | B.1 | B.2
NAT: UCP.2 | B.2
PTS: 1
DIF: 1
REF: Page 154
OBJ: 6.1.1 Trace the development and identify key features of the periodic table.
NAT: G.3 | B.1 | UCP.1
STA: ABC 10.1
TOP: Trace the development and identify key features of the periodic table.
KEY: Metals
MSC: 2
63. ANS:
In the modern periodic table, the elements are placed in the order of their increasing atomic numbers. The
atomic number of argon is 18 while the atomic number of potassium is 19. Therefore, argon is placed before
potassium in the modern periodic table.
PTS: 1
DIF: 1
REF: Page 153
OBJ: 6.1.1 Trace the development and identify key features of the periodic table.
NAT: G.3 | B.1 | UCP.1
STA: ABC 10.1
TOP: Trace the development and identify key features of the periodic table.
KEY: Atomic number
MSC: 2
64. ANS:
Elements in the same group have the same electron configuration and number of valence electrons. Valence
electrons determine the properties of elements. Therefore, properties of elements in the same group are
similar.
PTS: 1
DIF: 1
REF: Page 159
OBJ: 6.2.1 Explain why elements in the same group have similar properties.
NAT: UCP.1 | B.1 | B.2
STA: ABC 10.1
TOP: Explain why elements in the same group have similar properties.
KEY: Groups | Electron configuration
MSC: 2
65. ANS:
The loss of an electron from a sodium atom results in a smaller radius. The electrostatic repulsion between the
remaining number of electrons decreases thus allowing them to be pulled closer to the nucleus. Therefore, the
size of a sodium ion (Na+) is less than that of a sodium atom (Na).
PTS:
OBJ:
NAT:
TOP:
1
DIF: 2
REF: Page 165
6.3.2 Relate period and group trends in atomic radii to electron configuration.
UCP.1 | B.1 | B.2
STA: ABC 10.1
Relate period and group trends in atomic radii to electron configuration.
KEY: Atomic size | Ionic radius
MSC: 2
66. ANS:
The general electron configuration and locations of the block elements are:
a. ns0-2 for s-block elements in groups 1 and 2.
b. ns0-2 and np0-6 for p-block elements in groups 13, 14, 15, 16, 17, and 18.
c. (n–1)d0-10 and ns0-2 for d-block elements in groups 3, 4, 5, 6, 7, 8, 9, 10, 11, and 12.
d. (n–2)f0-14, (n–1)d0-10, np0-6, and ns0-2 for f-block elements in lanthanide and actinide groups.
PTS: 1
DIF: 2
REF: Page 161
OBJ: 6.2.2 Identify the four blocks of the periodic table based on electron configuration.
NAT: UCP.1 | B.1 STA: ABC 10.1
TOP: Identify the four blocks of the periodic table based on electron configuration.
KEY: Electron configuration
MSC: 1
67. ANS:
Potassium is the third alkali metal and scandium is the first transition metal in the periodic table.
PTS:
OBJ:
NAT:
TOP:
KEY:
1
DIF: 1
REF: Page 156
6.1.1 Trace the development and identify key features of the periodic table.
G.3 | B.1 | UCP.1
STA: ABC 10.1
Trace the development and identify key features of the periodic table.
Alkali metals | Transition metals
MSC: 1
PROBLEM
68. ANS:
0.5 g/mL
PTS: 1
DIF: 1
REF: Page 28
OBJ: 2.1.3 Compare the derived units of volume and density.
STA: ABC 1.1
TOP: Compare the derived units of volume and density.
KEY: Mass | Density | Volume
MSC: 3
NOT: Density = mass / volume. The volume of the copper sample is = 40 mL - 30 mL = 10 mL.
69. ANS:
Metal A has a greater density than metal B.
The density of metal A = 0.417 g/mL.
The density of metal B = 0.227 g/mL.
PTS: 1
DIF: 2
REF: Page 29
OBJ: 2.1.3 Compare the derived units of volume and density.
TOP: Compare the derived units of volume and density.
MSC: 3
NOT: Density = mass / volume
70. ANS:
3.2  105 m2
PTS:
OBJ:
STA:
KEY:
NOT:
71. ANS:
STA: ABC 1.1
KEY: Mass | Density | Volume
1
DIF: 2
REF: Page 35
2.2.2 Use dimensional analysis to convert between units. NAT: UCP.1
ABC 1.1
TOP: Use dimensional analysis to convert between units.
Meter | Centimeter | Area
MSC: 3
Area = length * width. 1m = 100 cm.
Element
Sodium
Phosphorus
Cobalt
Bromine
Silver
Number of
protons
11
35
47
Number of
electrons
Number of
neutrons
15
27
16
45
47
Atomic
number
11
15
27
35
Mass number
23
59
108
PTS: 1
DIF: 3
REF: Page 98 | Page 99 | Page 100
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic
number.
KEY: Composition of elements
MSC: 3
NOT: Atomic number = number of protons = number of electrons. Mass number = number of protons +
number of neutrons.
72. ANS:
79.904 amu
Bromine
PTS: 1
DIF: 3
REF: Page 102 | Page 103
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic
number.
KEY: Atomic mass of isotopes
MSC: 3
NOT: Weighted atomic mass of element X = mass contribution of X-79 + mass contribution of X-81. Mass
contribution of each isotope = (mass in amu of the isotope) * (percent abundance).
73. ANS:
23.985 amu
Magnesium
PTS: 1
DIF: 3
REF: Page 102 | Page 103
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic
number.
KEY: Atomic mass of isotopes
MSC: 3
NOT: Weighted atomic mass of element X = mass contribution of X-24 + mass contribution of X-25 + mass
contribution of X-26. Mass contribution = (mass of the isotope in amu) * (percent abundance).
74. ANS:
Number of protons = atomic number = 82.
Number of electrons = number of protons = 82.
Number of neutrons = mass number – atomic number = 125.
PTS: 1
DIF: 2
REF: Page 98 | Page 101
OBJ: 4.3.1 Explain the role of atomic number in determining the identity of an atom.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Explain the role of atomic number in determining the identity of an atom.
KEY: Atomic number
MSC: 3
NOT: Atomic number = number of protons = number of electrons.
75. ANS:
1551.32 amu
PTS: 1
DIF: 2
REF: Page 102
OBJ: 4.3.3 Calculate the number of electrons, protons, and neutrons in an atom given its mass number and
atomic number.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic
number.
KEY: Mass of individual atoms
MSC: 3
NOT: The mass of an atom depends on the number of protons and neutrons. It is expressed in atomic mass
units (amu).
76. ANS:
PTS: 1
DIF: 1
REF: Page 100
OBJ: 4.3.2 Define an isotope and explain why atomic masses are not whole numbers.
NAT: B.1
STA: ABC 10.1 | ABC 10.2
TOP: Define an isotope and explain why atomic masses are not whole numbers.
KEY: Chemical symbol and notation
MSC: 3
NOT: Isotopes are written with a shortened type notation. The notation includes the chemical symbol, atomic
number and mass number. The atomic mass and the atomic number are written to the left of the chemical
symbol. The atomic mass is denoted as a superscript and the atomic number is denoted as a subscript.
77. ANS:
There are three sublevels and nine orbitals possible in the third energy level.
PTS: 1
DIF: 2
REF: Page 134
OBJ: 5.2.3 Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals.
NAT: B.6
STA: ABC 10.1 | ABC 10.2
TOP: Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals.
KEY: Energy levels | Sublevels | Atomic orbitals
MSC: 2
NOT: The number of sublevels is equal to the types of orbitals. The number of orbitals is equal to all the
integers ranging from positive to negative values.
78. ANS:
The ground state electron configuration of sulfur is [Ne]3s23p4. Its electron dot structure is
PTS: 1
DIF: 2
REF: Page 138
OBJ: 5.3.2 Define valence electrons and draw electron-dot structures representing an atom's valence
electrons.
NAT: B.1 | B.6
STA: ABC 10.1 | ABC 10.2
TOP: Define valence electrons and draw electron-dot structures representing an atom's valence electrons.
KEY: Electron-dot structure | Valence electrons
MSC: 3
79. ANS:
Element A belongs to group 6A and element B belongs to group 7A in the periodic table.
PTS: 1
DIF: 1
REF: Page 159
OBJ: 6.2.1 Explain why elements in the same group have similar properties.
NAT: UCP.1 | B.1 | B.2
STA: ABC 10.1
TOP: Explain why elements in the same group have similar properties.
KEY: Groups
MSC: 1
NOT: Groups indicate the number of valence electrons.
80. ANS:
Tellurium
PTS: 1
DIF: 1
REF: Page 157
OBJ: 6.1.1 Trace the development and identify key features of the periodic table.
NAT: G.3 | B.1 | UCP.1
STA: ABC 10.1
TOP: Trace the development and identify key features of the periodic table.
KEY: Periodic table
MSC: 2
NOT: Elements are arranged in the increasing order of their atomic numbers. Elements in groups have
similar properties.
81. ANS:
The element having the largest size has an electron configuration of [Ne] 3s23p34s23d3. The element having
the highest electronegativity has an electron configuration of [Ne] 3s23p5.
PTS: 1
DIF: 2
REF: Page 163 | Page 168
OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.
NAT: UCP.1 | B.1 | B.2
STA: ABC 10.1
TOP: Relate period and group trends in atomic radii to electron configuration.
KEY: Electron configuration | Atomic size | Electronegativity
MSC: 2
NOT: The size of the atom depends on the number of shells in an atom. Electronegativity increases across a
period.
82. ANS:
The arrangement of elements in the increasing order of their atomic size is B < A < D < C. Element B is the
smallest and Element C is the largest.
PTS: 1
DIF: 1
REF: Page 163
OBJ: 6.3.2 Relate period and group trends in atomic radii to electron configuration.
NAT: UCP.1 | B.1 | B.2
STA: ABC 10.1
TOP: Relate period and group trends in atomic radii to electron configuration.
KEY: Atomic size | Electron configuration
MSC: 2
NOT: The size of an atom depends upon the number of shells in an atom. In the same period, the atomic size
decreases from left to right.