Ch10 Atomic Theory & Periodic Table – Test Bank – 15e - Test Bank | Foundations of College Chemistry 15e by Hein Arena by Hein Arena, Willard. DOCX document preview.
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Package Title: Hein Test Bank
Course Title: Hein 15e
Chapter Number: 10
Question type: Multiple Choice
1) The distance between two consecutive wave peaks is known as
a) frequency.
b) wavelength.
c) amplitude.
Difficulty: easy
Learning Objective 1: List the three basic characteristics of electromagnetic radiation.
Section Reference 1: 10.1
2) The number of waves that pass a particular point per second is known as
a) frequency.
b) wavelength.
c) amplitude.
Difficulty: easy
Learning Objective 1: List the three basic characteristics of electromagnetic radiation.
Section Reference 1: 10.1
3) Which scientist developed the idea that electrons exist in specific regions at various distances from the nucleus?
a) Rutherford
b) Dalton
c) Thomson
d) Bohr
Difficulty: easy
Learning Objective 1: Explain the relationship between the line spectrum and the quantized energy levels of an electron in an atom.
Section Reference 1: 10.2
4) Small packets of light energy are known as
a) excited state energy.
b) ground state energy.
c) spectra of energy.
d) quanta of energy.
Difficulty: easy
Learning Objective 1: Explain the relationship between the line spectrum and the quantized energy levels of an electron in an atom.
Section Reference 1: 10.2
5) The lowest possible energy level for an electron is known as
a) ground state.
b) low state.
c) basement state.
d) excited state.
Difficulty: easy
Learning Objective 1: Explain the relationship between the line spectrum and the quantized energy levels of an electron in an atom.
Section Reference 1: 10.2
6) When an electron falls from one energy level to a lower energy level, the result is the emission of
a) a beta particle.
b) quantized energy.
c) a gamma particle.
d) gamma radiation.
Difficulty: easy
Learning Objective 1: Explain the relationship between the line spectrum and the quantized energy levels of an electron in an atom.
Section Reference 1: 10.2
7) The characteristic bright line spectrum of an element is produced when an electron
a) moves to higher energy levels.
b) falls back to lower energy levels.
c) is emitted as gamma radiation.
d) is absorbed into the nucleus.
Difficulty: easy
Learning Objective 1: Explain the relationship between the line spectrum and the quantized energy levels of an electron in an atom.
Section Reference 1: 10.2
8) Which of the following regions of the electromagnetic spectrum has the longest wavelength?
a) gamma ray
b) ultraviolet
c) infrared
d) microwave
Difficulty: medium
Learning Objective 1: List the three basic characteristics of electromagnetic radiation.
Section Reference 1: 10.1
9) Which of the following regions of the electromagnetic spectrum has the lowest energy?
a) ultraviolet
b) radio waves
c) infrared
d) microwave
Difficulty: medium
Learning Objective 1: List the three basic characteristics of electromagnetic radiation.
Section Reference 1: 10.1
10) In the third principal energy level, which sublevel contains electrons with the greatest energy?
a) 3d
b) 3f
c) 3p
d) 3s
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
11) Which sublevel will contain electrons with the lowest energy?
a) 3s
b) 3p
c) 3d
d) 4s
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
12) Which does not exist as an electron sublevel?
a) 2d
b) 4f
c) 5d
d) 7s
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
13) Which sublevel will contain electrons with the lowest energy?
a) 3p
b) 3d
c) 4s
d) 4p
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
14) How many orbitals are contained in the 2p sublevel?
a) 1
b) 2
c) 3
d) 4
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
15) A p-orbital can accommodate ____________.
a) 4 electrons
b) 6 electrons
c) 2 electrons with opposite spins
d) 2 electrons with parallel spins
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
16) How many orbitals are contained in the 3s sublevel?
a) 1
b) 2
c) 3
d) 4
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
17) What is the maximum number of electrons that can occupy a d-sublevel?
a) 2
b) 6
c) 10
d) 18
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
18) What is the maximum number of electrons that can occupy the second principal energy level?
a) 2
b) 4
c) 6
d) 8
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
19) What is the maximum number of electrons that can occupy the first principal energy level?
a) 2
b) 6
c) 8
d) 10
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
20) What is the maximum number of electrons that can occupy the third principal energy level?
a) 2
b) 6
c) 8
d) 18
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
21) What is the maximum number of electrons that can occupy the fourth principal energy level?
a) 2
b) 6
c) 18
d) 32
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
22) What is the maximum number of electrons that can occupy the 4f sublevel?
a) 2
b) 6
c) 10
d) 14
Difficulty: medium
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Reference: Section Reference 1: 10.3
23) How many orbitals are contained in the 3d sublevel?
a) 2
b) 5
c) 7
d) 10
Difficulty: easy
Learning Objective 1: Describe the principal energy levels, sublevels, and orbitals of an atom.
Section Reference 1: 10.3
24) Atoms of which element has the following electron configuration?
1s2 2s2 2p6 3s2 3p3
a) nitrogen
b) phosphorous
c) sulfur
d) argon
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
25) Atoms of which element has the following electron configuration?
1s2 2s2 2p6 3s1
a) sulfur
b) strontium
c) sodium
d) nitrogen
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
26) What is the total number of electrons in the second principal energy level of a sodium atom in the ground state?
a) 2
b) 6
c) 8
d) 11
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
27) What is the total number of electrons in the second principal energy level of a nitrogen atom in the ground state?
a) 2
b) 3
c) 5
d) 7
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
28) What is the total number of electrons in the third principal energy level of a chlorine atom in the ground state?
a) 2
b) 5
c) 7
d) 8
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
29) What is the total number of electrons in the second principal energy level of an oxygen atom in the ground state?
a) 2
b) 4
c) 6
d) 8
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
30) Which of the following corresponds to the excited state configuration for a boron atom?
a) 1s22s22p1
b) 1s32s2
c) 1s22s23s1
d) 1s22s32p2
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
31) How many sublevels are occupied in an atom of magnesium in the ground state?
a) 2
b) 3
c) 4
d) 5
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
32) How many unpaired electrons correspond to the ground state of oxygen?
a) 0
b) 1
c) 2
d) 3
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
33) How many orbitals in an oxygen atom in the ground state contain only one electron?
a) 1
b) 2
c) 3
d) 4
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
34) How many valence electrons are in an aluminum atom in the ground state?
a) 1
b) 2
c) 3
d) 13
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
35) How many valence electrons are in a lead atom in the ground state?
a) 2
b) 4
c) 6
d) 8
Difficulty: medium
Learning Objective 1: Use the guidelines to write electron configurations.
Learning Objective 2: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: Sections 10.4 and 10.5
36) How many valence electrons are present in the element with the following ground state electron configuration?
1s2 2s2 2p3
a) 2
b) 3
c) 5
d) 7
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
37) How many valence electrons are present in the element with the following ground state electron configuration?
1s2 2s2 2p1
a) 1
b) 2
c) 3
d) 4
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
38) Each horizontal row on the periodic table is called a
a) period.
b) family.
c) group.
d) cohort.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
39) Each vertical column on the periodic table is called a
a) series.
b) period.
c) principal quantum level.
d) group.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
40) On the periodic table, elements that behave in a similar manner are found in the same
a) series.
b) row.
c) group.
d) period.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
41) On the periodic table, elements in the same period contain the same number of
a) protons.
b) electrons.
c) principal energy levels in their ground state.
d) valence electrons in their ground state.
Difficulty: medium
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
42) On the periodic table, elements in the same group contain the same number of
a) protons.
b) electrons.
c) principal energy levels in their ground state.
d) valence electrons in their ground state.
Difficulty: medium
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
43) On the periodic table, the "transition elements" are found in the
a) A Groups.
b) B Groups.
c) C Groups.
d) D Groups.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
44) On the periodic table, the “transition elements” fill their last electrons in the ___ sublevel.
a) s
b) p
c) d
d) f
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
45) The element having electronic configuration [Ar] 4s2 3d8 is
a) s block element
b) p block element
c) d block element
d) f block element
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
46) The element having electronic configuration [Ne] 2s2 2p6 is
a) s block element
b) p block element
c) d block element
d) f block element
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
47) The “halogens” are in Group
a) 1A.
b) 2A.
c) 7A.
d) 8A.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
48) The “alkaline earth metals” have
a) one valence electron
b) two valence electrons
c) three valence electrons
d) four valence electrons
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
49) The number of valence electrons for most members of noble gases family is
a) 0
b) 7
c) 8
d) 6
Difficulty: medium
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
50) The “alkali” metals have
a) one unpaired electron.
b) two unpaired electrons.
c) zero unpaired electrons.
d) three unpaired electrons.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
51) The element with electronic configuration 1s2 2s2 2p2 belongs to
a) Group II A and second period.
b) Group IIIA and second period.
c) Group IVA and second period.
d) Group IVA and third period.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
52) The element with electronic configuration 1s2 2s2 2p2 3s2 belongs to
a) Group II A and second period.
b) Group IVA and second period.
c) Group IVA and third period.
d) Group II A and third period.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
53) Which pair of atomic numbers represents s block elements?
a) 7, 15
b) 6, 12
c) 3, 12
d) 9, 17
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
54) The electron configuration, [Ar] 4s1, is the ground state electron configuration of
a) potassium.
b) phosphorous.
c) fluorine.
d) sodium.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
55) The electron configuration, [Ne] 3s2 3p3, is the ground state electron configuration of
a) nitrogen.
b) phosphorus.
c) argon.
d) sulfur.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
56) Which element is in the p-block of the periodic table?
a) Eu
b) Li
c) V
d) B
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
57) Which element is in the s-block of the periodic table?
a) Na
b) S
c) Pm
d) Mn
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
58) Which element is in the d-block of the periodic table?
a) Cr
b) Am
c) Ca
d) As
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
59) Which of the following will have an outer electron configuration similar to that of oxygen?
a) N
b) F
c) Cl
d) Se
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
60) Similar chemical properties of Mg and Ca are due to
a) their similar electronic configurations
b) similar size
c) different period
d) their metallic nature
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
61) The ground state electron configuration for an atom of carbon is
a) 1s2 2s2.
b) 1s2 2s2 2p.2
c) 1s2 2s2 2p4.
d) 1s2 2s4.
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
62) The ground state electron configuration for an atom of sodium is
a) 1s2 2s2 2p6 3s1
b) 1s2 2s2
c) 1s2 2s2 2p6
d) 1s2 2s2 2p6 3s2 3p4
Difficulty: easy
Learning Objective 1: Use the guidelines to write electron configurations.
Section Reference 1: 10.4
63) What is the number of valence electrons in a halogen atom?
a) 2
b) 7
c) 8
d) 9
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
64) What is the number of valence electrons in an alkaline earth metal atom?
a) 1
b) 2
c) 7
d) 12
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
65) What is the number of valence electrons in an alkali metal atom?
a) 1
b) 2
c) 7
d) 8
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
66) Which of the following has no unpaired electrons in its ground state electron configuration?
a) Ra
b) Pb
c) O
d) C
Difficulty: easy
Learning Objective 1:
Section Reference 1:s 10.4 and 10.5
67) Which of the following elements has the greatest number of unpaired electrons in its ground state electron configuration?
a) C
b) O
c) N
d) F
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.4
68) All of the following are used to characterize electromagnetic radiation except
a) charge.
b) frequency.
c) speed.
d) wavelength.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.1
69) The maximum number of electrons that can fit into a single d orbital is
a) 2.
b) 6.
c) 10.
d) 14.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
70) Of the orbitals shown, the one with the lowest energy is
a) 2s.
b) 3s.
c) 3d.
d) 3p.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
71) The electron configuration of an atom is 1s2 2s2 2p3. The number of unpaired electrons in this atom is
a) 1.
b) 2.
c) 3.
d) 4.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
72) How many electrons are found in “s-type” orbitals in an atom of lithium?
a) 2
b) 1
c) 3
d) 0
Difficulty: hard
Learning Objective 1:
Section Reference 1: 10.4
73) The ground electron configuration of an atom is 1s2 2s2 2p2. This atom will have similar properties as
a) tin
b) antimony
c) boron
d) nitrogen
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.6
74) Which atom does not have an unpaired electron in its ground state electron configuration?
a) C
b) Ca
c) P
d) Cl
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.4
75) Which principal energy level is the first to contain f orbitals?
a) third
b) fourth
c) fifth
d) sixth
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
76) What is the number of orbitals in an f sublevel?
a) 2
b) 3
c) 5
d) 7
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
77) What is the maximum number of electrons that can occupy the second principal energy level?
a) 2
b) 6
c) 8
d) 18
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.3
78) What is the maximum number of electrons that can fit into the fourth principal energy level?
a) 18
b) 14
c) 24
d) 32
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.3
79) The element in period 5 with a full d sublevel and three unpaired electrons is:
a) In
b) Sb
c) Te
d) Y
Difficulty: hard
Learning Objective 1:
Section Reference 1: 10.5
80) Halogens belong to the
a) s block of the periodic table
b) p block of the periodic table
c) d block of the periodic table
d) f block of the periodic table
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
81) Alkali metals belong to the
a) s block of the periodic table
b) p block of the periodic table
c) d block of the periodic table
d) f block of the periodic table
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
82) Element with atomic number 24 belongs to the
a) s block of the periodic table
b) p block of the periodic table
c) d block of the periodic table
d) f block of the periodic table
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
83) Transition elements belong to the
a) s block of the periodic table
b) p block of the periodic table
c) d block of the periodic table
d) f block of the periodic table
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
84) As one descends Group 2A of the periodic table, the number of valence electrons found in each element
a) increases.
b) decreases.
c) remains the same.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
85) The line spectrum of different elements provides evidence for
a) electrons traveling in orbits around the nucleus.
b) the quantization of the energy of the electrons.
c) the ground-state of the atom.
d) the existence of a nucleus.
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.2
86) In an atom of chlorine, the total number of electrons in “p-type” orbitals is:
a) 3
b) 6
c) 5
d) 11
Difficulty: hard
Learning Objective 1:
Section Reference 1: 10.4
87) The abbreviated electron configuration for arsenic is:
a) [Ar]4s24p3
b) [Ar]4s24d104p3
c) [Ar]4s23d104p3
d) [Zn]4p3
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.5
88) Which element has a ground state electron configuration with two unpaired electrons in the 3p sublevel?
a) P
b) Mg
c) Cl
d) Si
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
89) The element with an abbreviated electron configuration [Kr]5s24d6 is:
a) ruthenium
b) manganese
c) bromine
d) iron
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
90) Atoms of which two elements in the ground state contain the same number of valence electrons?
a) Al and Si
b) Al and B
c) Al and Zn
d) Al and Ge
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
91) Atoms of which atomic number will have similar chemical properties to phosphorus?
a) Z = 15
b) Z = 8
c) Z = 35
d) Z = 32
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
92) Choose the correct orbital diagram for arsenic.
a) 
b) 
c) 
d) 
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4 and 10.5
93) The following figure shows a(an):
a) d orbital
b) p orbital
c) s orbital
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
94) The following figure shows a(an):
a) d orbital
b) p orbital
c) s orbital
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
95) The following figure shows a(an):
a) d orbital
b) p orbital
c) s orbital
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
Question type: True/False
96) In the ground state, electrons tend to occupy orbitals of the lowest energy.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
97) The orbital diagram shown below is that of manganese.
1s 2s 2p 3s 3p 4s 3d
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.4
98) The second principal energy level contains s and p orbitals.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
99) Elements of s and p block elements are also called representative elements.
Difficulty: easy
Learning Objective 1: Describe how the electron configurations of the atoms relate to their position on the periodic table and write electron configurations for elements based on their position on the periodic table.
Section Reference 1: 10.5
100) The 4s energy sublevel fills before the 3d energy sublevel.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
101) The third principal energy level can hold a maximum of 18 electrons.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
102) The element represented by 1s2 2s2 2p5 has one unpaired electron.
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.4
103) The maximum number of valence electrons an atom can have is two.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
104) The second principal energy level contains four orbitals.
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.3
105) All noble gases have eight electrons in their outer principal energy level.
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.5
106) An orbital represents a region around the nucleus in which the probability of finding an electron is 100%.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
107) In order for two electrons to occupy the same orbital they must have opposite spins.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
Question type: Essay
108) Explain how a bright line spectrum is produced.
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.2
Solution: To form a bright line spectrum, elements in the gaseous phase are heated to high temperatures or subjected to high voltages. The electrons absorb the energy and jump from their ground state to a higher energy level known as an excited state. The electrons then fall back down to the ground state and emit energy as a colored light. The light passes through a prism or diffraction grating which separates the various components of the light into the different colors of the bright line spectrum.
109) Fill the following table:
Element | Atomic Number | Group Number | Abbreviated Ground-state Electron Configuration | Number of Valence Electrons |
Li | ||||
Ca | ||||
Si |
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
Solution:
Element | Atomic Number | Group Number | Condensed Ground-state Electron Configuration | Number of Valence Electrons |
Li | 3 | 1A | [He]2s1 | 1 |
Ca | 20 | 2A | [Ar]4s2 | 2 |
Si | 14 | 4A | [Ne]3s23p2 | 4 |
110) Fill the following table:
Element | Atomic Number | Group Number | Abbreviated Ground-State Electron Configuration | Number of Valence Electrons |
N | ||||
S | ||||
Br |
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
Solution:
Element | Atomic Number | Group Number | Abbreviated Ground-State Electron Configuration | Number of Valence Electrons |
N | 7 | 5A | [He]2s22p3 | 5 |
S | 16 | 6A | [Ne]3s23p4 | 6 |
Br | 35 | 7A | [Ar]4s23d104p5 | 7 |
111) How many unpaired electrons are in the ground state electron configuration of each of the following elements?
a) Boron
b) Selenium
c) Chlorine
d) Krypton
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
Solution: a) Boron has one unpaired electron; b) Selenium has two unpaired electrons; c) Chlorine has one unpaired electron; d) Krypton has no unpaired electrons
112) Prepare a chart showing the first four principal energy levels, their sublevels, the maximum number of electrons per sublevel, and the maximum number of electrons per principal energy level.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
Solution:
Principal Sublevels Maximum Number of Maximum Number of Electrons
Energy Level Electrons per Sublevel per Principal Energy Level
1 1s 2 2
2 2s 2 8
2p 6
3 3s 2 18
3p 6
3d 10
4 4s 2 32
4p 6
4d 10
4f 14
113) A. Write complete electron configurations for aluminum, nickel, and rubidium.
B. Using the electron configurations written on part A, complete the following table.
Element | Total number of electrons in s sublevels | Total number of electrons in p sublevels | Total number of electrons in d sublevels |
aluminum | |||
nickel | |||
rubidium |
Difficulty: medium
Learning Objective 1:
Section Reference 1: 10.4 and 10.5
Solution:
A. aluminum 1s22s22p63s23p1
nickel 1s22s22p63s23p64s23d8
rubidium 1s22s22p63s23p64s23d104p65s1
Element | Total number of electrons in s sublevels | Total number of electrons in p sublevels | Total number of electrons in d sublevels |
aluminum | 6 | 7 | 0 |
nickel | 8 | 12 | 8 |
rubidium | 9 | 18 | 10 |
114) List the following orbitals in order of increasing energy:
4d, 3p, 1s, 2p, 4p, 5s, 3d, 2s, 6s, 5p, 4s, and 3s.
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
Solution:
Lowest Energy 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s Highest Energy
115) Write orbital diagrams for the following elements in their ground states.
a) Fluorine
b) Oxygen
c) Carbon
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
Solution:
a) Fluorine ↑↓ ↑↓ ↑↓ ↑↓ ↑
1s 2s 2p
b) Oxygen ↑↓ ↑↓ ↑↓ ↑ ↑
1s 2s 2p
c) Carbon ↑↓ ↑↓ ↑ ↑
1s 2s 2p
116) Write orbital diagrams for the following elements in their ground states.
a) Lithium
b) Sodium
c) Nitrogen
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.4
Solution:
a) Lithium ↑↓ ↑
1s 2s
b) Sodium ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑
1s 2s 2p 3s
c) Nitrogen ↑↓ ↑↓ ↑ ↑ ↑
1s 2s 2p
117) In the designation 4p3; what is the significance of 4, p, and 3?
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.3
Solution: In the designation 4p3 each number or letter signifies something about the electrons and their energy positions. The 4 indicates that the electrons are in the fourth principal energy level. The p indicates that the electrons are in a p type sublevel. The 3 indicates that there are three electrons in that sublevel.
118) Write abbreviated electron configurations for:
a) Scandium (Z = 21)
b) gallium (Z = 31)
c) Rubidium (Z = 37)
Difficulty: easy
Learning Objective 1:
Section Reference 1: 10.5
Solution: a) [Ar]4s23d1; b) [Ar]4s23d104p1; c) [Kr]5s1
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Test Bank | Foundations of College Chemistry 15e by Hein Arena
By Hein Arena, Willard
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