Chapter 5 Practice Test
Moore
1. In the electron cloud model of the atom, an orbital is
defined as the most probable
A)
B)
C)
D)
charge of an electron
conductivity of an electron
location of an electron
mass of an electron
A) 1
A) s
A) a positively charged electron cloud surrounding a
positively charged nucleus
B) a positively charged electron cloud surrounding a
negatively charged nucleus
C) a negatively charged electron cloud surrounding
a positively charged nucleus
D) a negatively charged electron cloud surrounding a
negatively charged nucleus
3. The wave-mechanical model of the atom is required to
explain the
mass number and atomic number of an atom
organization of atoms in a crystal
radioactive nature of some atoms
spectra of elements with multielectron atoms
4. What is the total number of sublevels that contain
electrons in the third principal energy level of a nickel
atom in the ground state?
A) 1
B) 2
C) 3
D) 4
5. What is the total number of orbitals in the d sublevel of
an atom?
A) 1
B) 7
C) 3
D) 5
6. In which group of elements do most atoms have
completely filled s and p valence sublevels?
A) halogens
C) alkali metals
B) noble gases
D) alkaline earth metals
7. What is the total number of sublevels in an atom's fourth
principal energy level?
A) 8
B) 16
C) 3
D) 4
8. Atoms of an element in the ground state found in Period
4 of the Periodic Table must have
A)
B)
C)
D)
B) 2
C) 6
D) 10
10. Which sublevel contains a total of 5 orbitals?
2. Which phrase describes an atom?
A)
B)
C)
D)
9. What is the maximum number of electrons in an orbital
of any atom?
a 3d sublevel
4 valence electrons
electrons in the fourth principal energy level
similar properties to the other elements in the
period
B) p
C) d
D) f
11. An electron will emit energy in quanta when its energy
state changes from 4p to
A) 5s
B) 5p
C) 3s
D) 6p
12. Energy is absorbed when an electron moves from a 3d
sublevel to a
A) 1s sublevel
C) 3p sublevel
B) 2s sublevel
D) 4p sublevel
13. An electron in an atom will emit energy when it moves
from energy level
A) 2s to 3p
C) 2p to 3s
B) 2s to 2p
D) 2p to 1s
14. What is the electron configuration of a fluoride ion (F –)
in the ground state?
A) 1s 22s 22p 4
C) 1s 22s 22p 6
B) 1s 22s 22p 5
D) 1s 22s 22p 7
15. An atom with the electron configuration of ls 22s 22p 63s
2 3p 6 4s 2 3d 5 has an incomplete
A)
B)
C)
D)
2p sublevel
second principal energy level
third principal energy level
4s sublevel
16. What is the electron configuration of a Mn atom in the
ground state?
A)
B)
C)
D)
1s 22s 22p 63s 2
1s 22s 22p 63s 23p 64s 23d 5
1s 22s 22p 63s 23p 64s 13d 54p 1
1s 22s 22p 63s 23p 63d 7
17. Which is the electron configuration of a
ground state?
A) 1s 1
C) 1s 22s 1
31H
atom in the
B) 1s 2
D) 1s 22s 2
18. What is the maximum number of electrons that can
occupy the 4d sublevel?
A) 6
B) 2
C) 10
D) 14
19. What is the total number of occupied sublevels in an
atom of chlorine in the ground state?
A) 1
B) 5
C) 3
D) 9
26. Which electron notation represents the valence
electrons of a phosphorus atom in the ground state?
A)
20. Which electron configuration represents a neutral atom
of nitrogen in an excited state?
A) 1s 22s 22p 3
C) 1s 22s 12p 4
B) 1s 22s 22p 4
D) 1s 22s 12p 5
21. A sulfur atom and a chlorine atom have the same
number of
A)
B)
C)
D)
valence electrons
unpaired valence electrons
3s electrons
3p electrons
1s 22s 1 and 1s 22s 2
1s 22s 2 and 1s 22s 22p l
1s 22s 22p 5 and [Ne]3s 23p 5
1s 22s 22p 6 and [Ne]3s 23p 5
C) B
D) Be
24. What is the total number of unpaired electrons in an
atom of oxygen in the ground state?
A) 6
B) 2
C) 8
D) 4
25. Which orbital notation represents a boron atom in the
ground state?
A)
A)
C)
Which atom is represented by this notation?
B) N
D)
B)
23. The orbital notation of an atom in the ground state is
A) C
C)
27. Which orbital notation correctly represents the
outermost principal energy level of oxygen in the
ground state?
22. Which electron configurations represent the first two
elements in Group 17 (VIIA) of the Periodic Table?
A)
B)
C)
D)
B)
D)
28. Which is the orbital notation for the electrons in the
third principal energy level of an argon atom in the
ground state?
A)
B)
C)
D)
29. What is the total number of partially occupied 2p
orbitals in a nitrogen atom in the ground state?
A) 1
B)
C)
D)
B) 2
C) 3
D) 5
30. The bright-line spectrum of sodium is produced when
energy is
A) absorbed as electrons move from higher to lower
electron shells
B) absorbed as electrons move from lower to higher
electron shells
C) released as electrons move from higher to lower
electron shells
D) released as electrons move from lower to higher
electron shells
31. The diagram below represents the bright-line spectra of
four elements and a bright-line spectrum
produced by a mixture of two of these elements.
35. How do the energy and the most probable location of an
electron in the third shell of an atom compare to the
energy and the most probable location of an electron in
the first shell of the same atom?
A) In the third shell, an electron has more energy and
is closer to the nucleus.
B) In the third shell, an electron has more energy
and is farther from the nucleus.
C) In the third shell, an electron has less energy and is
closer to the nucleus.
D) In the third shell, an electron has less energy and is
farther from the nucleus.
Which two elements are in this mixture?
A)
B)
C)
D)
barium and hydrogen
barium and lithium
helium and hydrogen
helium and lithium
A) n
from 2nd to 3rd shell
from 2nd to 1st shell
from 3rd to 2nd shell
from 3rd to 1st shell
33. During a flame test, ions of a specific metal are heated
in the flame of a gas burner. A characteristic color of
light is emitted by these ions in the flame when the
electrons
A) gain energy as they return to lower energy levels
B) gain energy as they move to higher energy levels
C) emit energy as they return to lower energy
levels
D) emit energy as they move to higher energy levels
34. Given the bright-line spectra of three elements and the
spectrum of a mixture formed from at least two of these
elements:
Which elements are present in this mixture?
A) E and D, only
C) D and G, only
B) 2n
C) n 2
D) 2n2
37. In order for electrons to occupy the same orbital, they
must have
32. Which electron transition represents a gain of energy?
A)
B)
C)
D)
36. The maximum number of electrons that can occupy a
principal energy level (n) of an atom is equal to
B) E and G, only
D) D, E, and G
A)
B)
C)
D)
E)
different magnetic quantum numbers
different azimuthal quantum numbers
the same spin
opposite spins
two electrons cannot occupy the same orbital
38. Given the nuclear equation:
Which particle is represented by
A)
B)
C)
?
D)
39. Which equation represents the radioactive decay of
?
A)
B)
C)
D)
40. The chart below shows the spontaneous nuclear decay
of U-238 to Th-234 to Pa-234 to U-234.
What is the correct order of nuclear decay modes for
the change from U-238 to U-234?
A)
B)
C)
D)
-
decay, decay, - decay
- decay, - decay,
decay
decay, decay, decay
decay, - decay, - decay
C)
A) a moderator
C) a fuel rod
D)
42. Which reaction is matched correctly with the particle
represented by letter X?
A)
B)
C)
D)
B) moderator
D) internal shield
44. In a fission reactor, the speed of the neutrons may be
decreased by
Which particle is represented by X?
B)
Which structure is indicated by letter A?
A) turbine
C) control rod
41. Given the fusion reaction:
A)
43. The diagram below represents a nuclear reactor. The
arrows indicate the direction of the flow of water.
B) an accelerator
D) shielding
45. The fission process in a reactor can be regulated by
adjusting the number of neutrons available. This is
done by the use of
A) moderators
C) coolants
B) control rods
D) shielding
Answer Key
Chapter 5 Practice
1.
C
37.
D
2.
C
38.
A
3.
D
39.
A
4.
C
40.
D
5.
D
41.
D
6.
B
42.
A
7.
D
43.
C
8.
C
44.
A
9.
B
45.
B
10.
C
11.
C
12.
D
13.
D
14.
C
15.
C
16.
B
17.
A
18.
C
19.
B
20.
C
21.
C
22.
C
23.
D
24.
B
25.
B
26.
B
27.
C
28.
B
29.
C
30.
C
31.
B
32.
A
33.
C
34.
A
35.
B
36.
D