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Name:____________________Quantum Numbers Multiple Choice Practice Problems

Protons

1) __________ and __________ reside in the atomic nucleus. A) Protons, electrons B) Electrons, neutrons C) Protons, neutrons D) none of the above E) Neutrons, only neutrons

2) The atomic number indicates __________. A) the number of neutrons in a nucleus B) the total number of neutrons and protons in a nucleus C) the number of protons in a neutral atom D) the number of atoms in 1 g of an element E) the number of different isotopes of an element

3) All atoms of a given element have the same __________. A) mass B) number of protons C) number of neutrons D) densityE) number of electrons and neutrons

Neutrons & Isotopes

4) Which atom has the smallest number of neutrons? A) carbon-14 B) nitrogen-14 C) oxygen-16 D) fluorine-19 E) argon 18

5) Which atom has the largest number of neutrons? A) phosphorus-30 B) chlorine-37 C) potassium-39 D) argon-40 E) calcium-40

6) There are ________electrons, _________protons, and ________neutrons in an atom of 13355 Cs.

A) 132, 132, 54 B) 54, 54, 132 C) 78, 78, 54 D) 55, 55, 78 E) 78, 78, 132


7) An atom of the most common isotope of gold, 197Au, has ___ protons, ___ neutrons, and ___ electrons.

A) 197, 79, 118 B) 118, 79, 39C) 79, 197, 197 D) 79, 118, 118E) 79, 118, 79

8) Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 6530

Zn? A) 30 p+, 35 n, 30 e-

B) 29 p+, 29 n, 63 e-

C) 63 p+, 29 n, 63 e-

D) 34 p+, 29 n, 34 e-

E) 34 p+, 34 n, 29 e-

9) Which isotope has 45 neutrons?A) 80

36KrB) 80

35BrC) 78

34SeD) 34

17ClE) 103

45Rh

10) Which isotope has 36 electrons in an atom? A) 80

36KrB) 80

35BrC) 78

34SeD) 78

34SeE) 103

45Rh

11) Isotopes are atoms that have the same number of __________ but differing number of ________. A) protons, electrons B) neutrons, protons C) protons, neutrons D) electrons, protons E) neutrons, electrons

12) The nucleus of an atom does not contain __________. A) protons B) protons or neutrons C) neutrons D) subatomic particles E) electrons

13) The nucleus of an atom contains __________. A) ElectronsB) ProtonsC) neutrons D) protons and neutronsE) protons, neutrons, and electrons


14) Different isotopes of a particular element contain the same number of __________. A) protons B) neutrons C) protons and neutrons D) subatomic particles E) protons, neutrons, and electrons

15) In the symbol, 13xC, x = _________

A) 7 B) 13 C) 12 D) 6E) not enough information to determine

16) In the symbol, 137X, X = __________.

A) N B) C C) Al D) K E) not enough information to determine

17) In the symbol, x6C, x = __________.

A) 12 B) 13 C) 7 D) 7 E) A and B

18) In the symbol, x6C, x is __________.

A) the number of neutronsB) the atomic numberC) the mass number D) the isotope numberE) the elemental symbol

Average Atomic Mass

19) The atomic mass unit is presently based on standard reference nucleus of_______ isotope. A) HydrogenB) OxygenC) SodiumD) CarbonE) Helium


20) Silver has two naturally occurring isotopes with the following isotopic masses:107

47Ag 10947Ag

(106.90509 amu) (108.9047 amu)

The average atomic mass of silver is 107.8682 amu. The percent abundance of the lighter of the two isotopes is

A) 24.221% B) 48.168%C) 51.835%D) 75.783% E) 90.474%

21) The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope % Mass

209X 76.01 209.3

208X 13.01 208.0

206X 11.02 206.0

A) 219.7 B) 208.9C) 220.42 D) 218.5 E) 221.0

22) Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope % Mass

40X 13.01 40.10

41X 6.98 41.00

44X 79.99 43.98

A) 43.26 B) 39.68 C) 39.07 D) 38.64 E) 33.33


23) The element X has two naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope % Mass

266X 97.51 266.01

264X 2.50 264.21

A) 261.75B) 262.03C) 265.99 D) 263.15 E) 233.33

24) The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is __________ amu.

Isotope % mass

53X 19.61 52.62

56X 53.91 56.29

58X 26.48 58.31

A) 33.33B) 55.74C) 56.11 D) 57.23 E) 56.29

25) The average atomic weight of an element, which has two naturally occurring isotopes, is 63.5. One of the isotopes has an atomic weight of 62.9 amu and constitutes 69.1% of the isotopes. The other isotope has an abundance of 37.1%. The atomic weight (amu) of the second isotope is __________ amu.

A) 63.2 B) 63.8 C) 64.1 D) 64.6 E) 28.1


Electrons & Ions

26)How many electrons are in a neutral oxygen atom?A) 6B) 8C) 10D) 16E) None of the above answers

27)How many electrons are in an oxygen atom with charge of -2?A) 6B) 8C) 10D) 16E) None of the above answers

28)How many electrons are in the ion Li+?A) 6B) 8C) 10D) 16E) None of the above answers

29)How many electrons are in the ion N-3?A) 1B) 2C) 3D) 4E) None of the above answers

30)How many electrons are in the ion Br-?A) 34B) 35C) 36D) 80E) None of the above answers


31)How many electrons are in a Neon atom?A) 9B) 10C) 20D) 21E) None of the above answers

32)How many electrons are in an Iron atom?A) 23B) 26C) 27D) 28E) None of the above answers

33)How many electrons are in the ion Fe+3?A) 23B) 26C) 27D) 28E) None of the above answers

34)How many electrons are in the ion Fe+2?A) 23B) 26C) 27D) 28E) None of the above answers

35)How many electrons are in the ion V+4?A) 19B) 20C) 21D) 23E) None of the above answers


36)How many electrons are in a neutral Vanadium atom?A) 19B) 20C) 21D) 23E) None of the above answers

37)How many electrons are in a neutral Chlorine atom?A) 16B) 17C) 18D) 36E) None of the above answers

38)How many electrons are in the ion Cl-?A) 16B) 17C) 18D) 36E) None of the above answers

Quantum Theory

Principal

39) __________ orbitals are spherically symmetrical. A) sB) pC) d D) fE) g

40) All of the orbitals in a given electron shell have the same value of the __________ quantum number.

A) Principal B) AzimuthalC) Magnetic D) SpinE) Psi


Azimuthal

41) The __________ quantum number defines the shape of an orbital.A) SpinB) MagneticC) PrincipalD) AzimuthalE) Phi

42) The n = 1 shell contains __________ p sub-orbitals. All the other shells contain __________ p sub- orbitals.

A) 3, 6B) 0, 3C) 6, 2 D) 3, 3E) 0, 6

43) There are __________ orbitals in the second shell. A) 1B) 2C) 4 D) 8E) 9

44) The azimuthal quantum number is 3 refers to _____ orbitals.A) sB) pC) dD) fE) g

45) The lowest energy shell that contains d orbitals is the shell with n = __________. A) 3B) 2C) 4D) 1E) 5

46) The principal quantum number of the first d orbital is __________. A) 1B) 2C) 3D) 4E) 0


47) Which of the orbitals below do not exist due to the constraints upon the azimuthal quantum number?

A) 3f B) 2sC) 2pD) all of the aboveE) none of the above

48) Which of the orbitals below do not exist due to the constraints upon the azimuthal quantum number?

A) 4fB) 4dC) 4pD) 4sE) none of the above

49) Which one of the following is an incorrect orbital notation? A) 4fB) 2dC) 3sD) 2pE) 3d

50) If an electron has a principal quantum number (n) of 4 and an azimuthal quantum number (l) of 2, the orbital designation is _________.

A) 3p B) 4d C) 4s D) 4pE) 4d

Magnetic

51) There are __________ sub-orbitals in the 3rd shell. A) 25 B) 4C) 9 D) 16E) 1

52) All of the sub-orbitals in a given orbital have the same value of the __________ quantum number. A) PrincipalB) AzimuthalC) MagneticD) A and BE) B and C


53) Which one of the following is not a valid value for the magnetic quantum number of an electron in a 4f orbital?

A) 2B) 4C) 0D) 1E) -1

54) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.

A) 2, 0, 0B) 2, 1, -1C) 3, 1, -1D) 2, 3, 1E) 3, 2, 1

55) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.

A) 6, 1, 0B) 3, 2, 3C) 3, 2, -2D) 1, 0, 0E) 3, 2, 1

Spin

56) The p-orbital can accommodate a maximum of __________ electrons. A) 6B) 2C) 10D) 3E) 5

57) How many quantum numbers are necessary to designate a particular electron in an atom? A) 3B) 4C) 2D) 1E) 5

58) At maximum, an f-orbital can hold __________ electrons, a d-orbital can hold __________ electrons, and a p-orbital can hold __________ electrons.

A) 14, 10, 6B) 2, 8, 18C) 14, 8, 2 D) 2, 12, 21E) 2, 6, 10


59) Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, l, ml, and ms)

A) 2, 2, -1, -½B) 1, 0, 0, +½C) 3, 3, 3, +½ D) 5, 4,- 5, +½E) 3, 3, 3, -½

60) Which of the following is not a valid set of four quantum numbers? (n, l, ml, ms )A) 2, 0, 0, -½B) 2, 1, 0, -½C) 1, 0, 0, +½D) 3, 1, -1, -½E) 1, 1, 0, +½

61) Which of the following is a valid set of four quantum numbers?(n, l, ml, ms)A) 3, 2, 0, +½B) 2, 1, 2, +½C) 1, 0, 1, +½ D) 2, 2, 1, -½E) 1, 1, 0, -½

Energy Level Diagram

62) The lowest orbital energy is reached when the number of electrons with the same spin is maximized. This statement describes __________.

A) Pauli Exclusion Principle B) Planck's constant C) deBroglie hypothesis D) Heisenberg Uncertainty Principle E) Hund's rule

63) Which one of the following is the correct electron configuration for a ground-state nitrogen atom?

A)

B)

C)

D)

E) None of the above is correct.


64) Which electron configuration denotes an atom in its ground state?

A)

B)

C)

D)

E)

65) Which electron configuration represents a violation of the Aufbau Principle?

A)

B)

C)

D)

E)

66) Which electron configuration represents a violation of the Aufbau Principle?

A)

B)

C)

D)


E)

67) Which electron configuration represents a violation of the Pauli Exclusion Principle?

A)

B)

C)

D)

E)


A)

B)

C)

D)

E)


A)

B)

C)


D)

E)

70) Which electron configuration represents a violation of Hund's rule for an atom in its ground state?

A)

B)

C)

D)

E)


A)

B)

C)

D)

E)



A)

B)

C)

D)

E)

Auf Bau

73) Which two elements have the same ground-state electron configuration?A) I and SB) Cu and AgC) Li and Na D) Cl and ArE) No two elements have the same ground-state electron configuration.

74) How many different principal quantum numbers can be found in the ground state electron configuration of ruthenium?

A) 2B) 3C) 5D) 4E) 6

75) The ground state electron configuration of Fe is __________. A) 1s2 2s2 3s2 3p6 3d6

B) 1s2 2s2 2p6 3s2 3p6 4s2 3d6

C) 1s2 2s2 2p6 3s2 3p6 4s2 D) 1s2 2s2 2p6 3s2 3p6 4s2 4d6

E) 1s2 2s2 3s2 3p10


76) The ground state electron configuration of Ga is __________. A) 1s2 2s2 3s2 3p6 3d10 4s2 4p1

B) 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p1

C) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

D) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4d1

E) [Ar] 4s2 3d11

77) The 2p orbital in the ground state of atomic Neon contains __________ electrons. A) 2B) 6C) 8D) 10E) 36

78) The second shell in the ground state of atomic argon contains __________ electrons. A) 2B) 6C) 8D) 18E) 36

79) The ______ orbital is partially filled in Manganese atom. A) 3sB) 4sC) 4pD) 3dE) 4d

80) The azimuthal quantum number for the outermost electrons in a Phosphorus atom in the ground state is

A) 0B) 1C) 2D) 3E) -1

Noble Gas Shortcut

81) The ground state configuration of Ne is __________.A) [He] 2s2 2p2

B) [He] 2s2 2p3

C) [He] 2s2 2p4

D) [He] 2s2 2p6

E) [F] 2s2 2p6

82) The ground state configuration of iodine is __________.A) [Ar] 4s2 3d3


B) [Xe] 6s2 4f14 5d4

C) [Ne] 3s1

D) [Xe] 6s2 4f7

E) [Kr] 5s2 4d10 5p5 83) Which is the correct ground-state electron configuration for silver?

A) [Kr] 5s2 4d9

B) [Kr] 5s1 4d10

C) [Kr] 5s2 4d10

D) [Xe] 5s2 4d9

E) [Xe] 5s1 4d10

84) The ground-state electron configuration of the element __________ is [Kr] 5s1 4d5. A) NbB) MoC) CrD) MnE) Tc

85) The ground-state electron configuration of __________ is [Ar] 4s1 3d5. A) VB) MnC) FeD) CrE) K

86) The principal quantum number for the outermost electrons in a Iodine atom in the ground state is A) 2B) 3C) 5D) 4E) 1

Exceptions

87) Which of the following elements has a ground-state electron configuration different from the predicted one?

A) CuB) Ca C) XeD) ClE) Ti

Periodic Table

88) Horizontal rows of the periodic table are known as __________.A) PeriodsB) GroupsC) Metalloids D) Metals


E) Nonmetals

89) Vertical columns of the periodic table are known as __________. A) MetalsB) PeriodsC) Nonmetals D) GroupsE) Metalloids

90) Elements __________ exhibit similar physical and chemical properties. A) with similar chemical symbols B) with similar atomic masses C) in the same period of the periodic table D) on opposite sides of the periodic table E) in the same group of the periodic table

91) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?

A) H, LiB) Cs, SrC) C, Si D) Ga, GeE) C, O

92) Which pair of elements would you expect to exhibit the greatest similarity in their physical and chemical properties?

A) As, SbB) C, NC) K, Ca D) H, HeE) Si, P

93) Which pair of elements below should be the most similar in chemical properties? A) C and OB) B and AsC) I and Br D) K and KrE) Cs and He

94) In the periodic table, the elements are arranged in __________.A) alphabetical order B) order of increasing atomic number C) order of increasing metallic properties D) order of increasing neutron content E) reverse alphabetical order

Periodic Families


95) Elements in Group 1 are known as the __________. A) ChalcogensB) Alkaline Earth MetalsC) Alkali Metals D) HalogensE) Noble Gases

96) Elements in Group 2 are known as the __________. A) Alkaline Earth MetalsB) Alkali MetalsC) Chalcogens D) HalogensE) Noble Gases

97) Elements in Group 17 are known as the __________. A) Chalcogens B) Alkali MetalsC) Alkaline Earth Metals D) HalogensE) Noble Gases

98) Elements in Group 18 are known as the __________. A) HalogensB) Alkali MetalsC) Alkaline Earth Metals D) ChalcogensE) Noble Gases

99) The elements in groups 1, 16, and 17 are called, __________, respectively. A) Alkaline Earth Metals, Halogens, and Chalcogens B) Alkali Metals, Chalcogens, and Halogens C) Alkali Metals, Halogens, and Noble Gases D) Alkaline Earth Metals, Transition Metals, and Halogens E) Halogens, Transition Metals, and Alkali Metals

100) Which of the following elements is a metalloid? A) BB) CC) GaD) SeE) In

101) Copper is a __________ and helium is a __________. A) Metal, NonmetalB) Metal, MetalC) Metal, Metalloid


D) Metalloid, NonmetalE) Nonmetal, Metal

102) Sulfur is a __________ and nitrogen is a __________. A) Metal, Metalloid B) Nonmetal, Metal C) Metalloid, Metalloid D) Nonmetal, Nonmetal E) Nonmetal, Metalloid

103) Calcium is a __________ and silver is a __________. A) Nonmetal, Metal B) Metal, Metal C) Metalloid, Metal D) Metal, Metalloid E) Nonmetal, Metalloid

104) Elements in group __________ have an ns2 np6 electron configuration in the outer shell. A) 1B) 2C) 17D) 18E) 12

105) Which group in the periodic table contains elements with the valence electron configuration of ns2 np1?

A) 1B) 2C) 12D) 13E) 17


MC Answer Key

1) C2) C3) B4) B5) D6) D7) E8) A9) B10)A11)C12)E13)D14)A15)D16)A17)E18)C19)D20)C21)B22)A23)C24)C25)D26)B27)C28)E29)E

30)C31)B32)B33)A34)E35)A36)D37)B38)C39)A40)A41)D42)B43)B44)D45)A46)C47)A48)E49)B50)B51)C52)D53)B54)D55)B56)A57)B58)A

59)B60)E61)A62)E63)D64)D65)A66)C67)C68)B69)C70)C71)B72)D73)E74)C75)B76)C77)B78)C79)D80)B81)D82)E83)B84)B85)D86)C87)A


88)A89)D90)E91)A92)A93)C

94)B95)C96)A97)D98)E99)B

100) A101) A102) D103) B104) D105) D

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