Practice Test H.1 (pg 1 of 6)
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6.
(Ch 6, 7, and 21)
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This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing
conditions outlined below.
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DO NOT USE A CALCULATOR. You may use ONLY the blue periodic table.
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Try to work at a pace of 1.2 min per question. Time yourself. It is important that you practice working for speed.
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Then when time is up, continue working and finish as necessary.
Of the following transitions in the Bohr hydrogen atom,
the _________ transition results in the emission of the
shortest wavelength photon.
a. n = 1 to n =6
b. n = 6 to n = 1
c. n = 6 to n = 3
d. n = 2 to n = 1
e. n = 1 to n = 4
There are __________ possible values for the magnetic
quantum number (mL, 3rd quantum #) of an electron in
5f subshell.
a. 1
b. 5
c. 7
d. 10
e. 14
In a px orbital, the subscript x denotes the _______ of
the electron.
a. energy
b. spin of the electrons
c. probability of the shell
d. size of the orbital
e. axis along which the orbital is
aligned
Which sketch represents an orbital with the quantum
numbers n = 3, l = 0, and mL = 0 ?
a
5.
Electrons, Periodicity, and Nuclear
b
c
d
e
How many electrons in an atom can possess the a
principal quantum number of n = 3
a. 3
b. 6
c. 8
d. 10
e. 18
An electron can NOT have which set of the following
quantum numbers n = __, l = __, mL = ___ .
a. 6, 1, 0
b. 3, 2, 3
c. 3, 2, -2
d. 1, 0, 0
e. 3, 2, 1
7.
How many p-orbitals are filled in a Kr atom?
a. 3
b. 6
c. 9
d. 18
e. 27
8.
How many unpaired electrons are in the iron atom
a. 0
b. 2
c. 3
d. 4
e. 8
9.
Which of the following is not a valid set of four
quantum numbers? (n, l ,ml, ms)
a. 2, 0, 0, +½
b. 2, 1, 0, −½
c. 3, 1, −1, −½
d. 1, 0, 0, +½
e. 1, 1, 0, +½
10. [Ar]4s23d104p3 is the electron configuration of a(n)
______ atom.
a. As
b. V
c. P
d. Sb
e. Sn
11. How many unpaired electrons are in the Ni2+ ion?
a. 0
b. 2
c. 3
d. 4
e. 6
12. List the following species in order from smaller to
larger size (radii).
a. Se2− < Kr < Rb+
b. Kr < Se2− < Rb+
c. Rb+ < Kr < Se2−
d. Rb+ < Se-2 < Kr
e. They are all the same size.
13. All of the ________ have a valence shell electron
configuration of ns2
a. noble gases
b. halogens
c. chalcogens
d. alkali metals
e. alkaline earth metals
Unit H.1 Practice Test (pg 2 of 6)
Electrons, Periodicity, and Nuclear (Ch 6, 7, & 21)
14. The elements in the ______ period of the periodic table
have a core-electron configuration that is the same as
the electron configuration of neon.
a. first
b. second
c. third
d. fourth
e. fifth
15. Pick the graph below that best represents the
relationship between energy and wavelength of light.
E
E
E
λ
λ
a
b
E
λ
E
λ
c
λ
d
e
21. The ground state electron configuration of a highly
reactive metal is
a. a
b. b
c. c
d. d
e. e
22. The largest principal quantum number in the ground
state electron configuration of iodine is _______
a. 1
b. 4
c. 5
d. 6
e. 7
Use the choices below to answer the next 6 questions
a. 1s22s22p63s23p64s23d104p65s1
b. 1s22s22p63s23p5
c. 1s22s22p63s23p64s23d8
d. 1s22s22p63s23p64s23d104p6
e. 1s22s22p33s1
23. Identify the element whose 3+ ion has the following
electron configuration: [Xe] 4f14 5d3
a. W
b. Lu
c. Ta
d. Nb
e. Y
16. The ground state electron configuration of a transition
metal is
a. a
b. b
c. c
d. d
e. e
24. In a multi-electron atom, how many electrons can have
the quantum numbers: n = 4, l = 1, mL = −1
a. 1
b. 2
c. 6
d. 10
e. 0, this is not a valid set of 3 numbers
17. An electron configuration of an excited atom is
a. a
b. b
c. c
d. d
e. e
25. In copper, which of the following electrons,
characterized by the four quantum numbers, has the
lowest energy?
a. n = 4, l = 0, mL = 0, ms = −½
b. n = 3, l = 2, mL = 0, ms = +½
c. n = 3, l = 1, mL = −1, ms = +½
d. n = 3, l = 1, mL = 0, ms = −½
e. electrons c and d are degenerate and are of the
same energy.
18. The ground state electron configuration of an element
with the smallest number of valence electrons is
a. a
b. b
c. c
d. d
e. e
19. The ground state electron configuration of a chemically
un-reactive element is
a. a
b. b
c. c
d. d
e. e
20. The ground state electron configuration of an element
that forms a -1 ion is
a. a
b. b
c. c
d. d
e. e
26. To remove which electron from gallium would you
expect an extraordinarily high increase in successive
ionization energy?
a. 2nd
b. 3rd
c. 4th
d. 5th
e. none, all successive ionization energies increase
steadily
27. To remove the second electron from which would you
expect an extraordinarily high increase in the second
successive ionization energy?
a. Ca
b. K
c. Ga
d. Ge
e. Se
Unit H.1 Practice Test (pg 3 of 6)
Electrons, Periodicity, and Nuclear (Ch 6, 7, & 21)
28. Which of the following correctly represents the second
ionization of phosphorus?
a. P + e- → P−
b. P + P−1 → e−
c. P + P+ → e−
d. P+ → P+2 + e−
e. P+ + e− → P
35. Which of the following sets contains species that are
isoelectronic?
a. Br, Kr, Rb
b. O2−, S2−, Se2−
c. Al3−, S2−, Ar
d. Cl+, Ar, K−
e. F−, Ne, Na+
29. The electron configuration of the ground state for the
Ag atom is an exception to the electron-filling rules.
Which configuration below is most likely to represent
Ag.
a. [Ar] 4s24d9
b. [Kr] 5s14d10
c. [Kr] 5s23d9
d. [Ar] 4s14d10
e. [Kr] 5s24d10
36. In general, as you go across a period in the periodic
table from left to right: the atomic radius ______, the
electron affinity becomes ______ negative, and the first
ionization energy ______.
a. decreases, decreasingly, increases
b. increases, increasingly, decreases
c. increases, increasingly, increases
d. decreases, increasingly, increases
e. decreases, decreasingly, decreases
30. Which equation correctly represents the electron
affinity of sulfur?
a. S + e− → S− + EA
b. S + EA→ S+1 + e−
c. S → S− + e− + EA
d. S− + EA → S + e−
e. S+ + e− → S + EA
37.
Use the choices below to answer 4 questions
a. [Kr] 5s1
b. [Ne] 3s23p1
c. [Ar] 4s23d104p4
d. [Ne] 3s23p6
e. [Ar] 4s1
31. The atom with the largest atomic radius is ________
a. a
b. b
c. c
d. d
e. e
32. The electron configuration of the two atoms that will
form isoelectronic ions are
a. a + c
b. b + c
c. c + d
d. b + e
e. a + e
33. The electron configuration of the atom that is expected
to have the highest first ionization energy is _______
a. a
b. b
c. c
d. d
e. e
34. The electron configuration of the atom that is expected
to form a stable 2− ion is ______
a. a
b. b
c. c
d. d
e. e
131I
has a half-life of 3.5 days. Assuming you start with
an 8.0 g sample, what mass will remain after two
weeks?
a. 4.0 g
b. 2.4 g
c. 2.0 g
d. 1.0 g
e. 0.5 g
38. Which reaction below best represents the transmutation
that occurs inside the nucleus during beta decay?
a. 11p → 10n + 0−1e
b. 11p → 10n + 0+1e
c. 10n → 11p + 0+1e
d. 10n → 11p + 0−1e
e. 10n → 11n + 0−1e
39. A sample of radioactive cadmium has a half life of 15
days. If you have a sample that originally weighed 40 g
and later weighs 2.5 g. How much time elapsed
between the initial and final masses?
a. 600 days
b. 100 days
c. 60 days
d. 45 days
e. 37.5 days
40. Which one of the following processes results in an
increase in the atomic number?
a. gamma emission
b. positron emission
c. beta emission
d. alpha emission
e. electron capture
41. Fill in the blank in the following nuclear equation
252 Cf + 10 B → 259 Lr + _____
98
5
103
a. 5 0-1e
b. 3 10n
c. 3 11p
d. 3 0+1e
e. 5 10n
Unit H.1 Practice Test (pg 4 of 6)
Electrons, Periodicity, and Nuclear (Ch 6, 7, & 21)
42. An element that participates in electron capture could
accomplish the same transmutation by
a. positron emission
b. alpha emission
c. beta emission
d. alpha and beta occurring together
e. neutron emission
43. Make the selection that correctly fills in the three
blanks in the equation below.
27 ____Si
→ 27 13 _____ + _____
a. 14, Al, 0+1e
b. 28, P, 0+1e
c. 13, Al, 0-1e
d. 14, Al, 0-1e
e. there is not enough information to identify all of
the three blank
44. What is the mass number of a neutron?
a. 0
b. 1
c. 2
d. 3
e. 4
45. In balancing the nuclear reaction
238 U → X + 4 He
92
2
What is the identity of element X?.
a. Pu
b. Np
c. Th
d. U
e. Pa
49. Tritium decays by a first-order process that has half-life
of 12.5 years. How many years will it take to reduce the
radioactivity of a tritium sample to 15% of it original
value?
a. 64 yrs
b. 54 yrs
c. 34 yrs
d. 24 yrs
e. 14 yrs
50. For a first order reaction that has a half-life of 69 s at
80°C, the value of the rate constant, k, is closest to?
a. 0.01 s−1
b. 0.1 s−1
c. 1 s−1
d. 10 s−1
e. 100 s−1
51. If the half-life of a reaction is independent of
concentration, what is the order of the reaction?
a. zero
b. first
c. second
d. half-life is unrelated to the order of the reaction
e. unable to be determined without knowing starting
concentrations
52. Which species contains the most neutrons?
a. 5926Fe3+
b. 5626Fe
c. 6029Cu
d. 6130Zn
e. 6030Zn+2
46. Identify the type of decay that the radioactive nuclide,
88Rb is likely to participate in?
a. alpha
b. positron
c. beta
d. electron capture
e. either c or d
53. Which type of radiation changes both the atomic
number and mass number of the emitting atom?
a. alpha
b. beta
c. gamma
d. positron
e. electron capture
47. The reaction below is an example of
38 Ca
→ 3819K
+ _______
20
a. alpha decay
b. beta decay
c. electron capture
d. positron decay
e. nuclear transmutation
54. Which represents the 235U atom?
48. Radium undergoes alpha decay. The product of this
reaction also undergoes alpha decay. What is the
product of this second decay reaction ?
a. Rn
b. U
c. Th
d. Hg
e. Po
Protons
Electrons
Neutrons
(A)
46
46
143
(B)
46
46
92
(C)
92
92
143
(D)
92
92
146
(E)
92
92
235
55. A particular nuclear decay has a rate constant of
0.00346 min−1 What is the half-life?
a. 3.3 hours
b. 1.6 hours
c. 0.0012 min
d. 0.0024 min
e. 0.0050 min
Unit H.1 Practice Test (pg 5 of 6)
Electrons, Periodicity, and Nuclear (Ch 6, 7, & 21)
56. The half-life of 14C is 5570 years. How many years will
it take for 90% of a sample to decompose?
a. 5,013 years
b. 11,000 years
c. 18,600 years
d. 23,000 years
e. 50,130 years
57. The half-life of 99Tc is 6.00 hours. If it takes exactly
12.00 hours for the manufacturer to deliver a 99Tc
sample to a hospital, how much must be shipped in
order for the hospital to receive 10.0 mg?
a. 40.0 mg
b. 30.0 mg
c. 20.0 mg
d. 15.0 mg
e. 4.0 mg
58. An atom of phosphorus-28, 29P, contains
a. 15 electrons, 15 protons, 16 neutrons.
b. 15 electrons, 15 protons, 15 neutrons.
c. 15 electrons, 15 protons, 14 neutrons.
d. 15 electrons, 15 protons, 29 neutrons.
e. 15 electrons, 15 protons, 29 neutrons.
Practice Test H.1 (pg 6 of 6)
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Electrons, Periodicity, and Nuclear (Ch 6, 7, and 21)
ANSWERS