Deck 2: Quantum Mechanics in Action: Atoms

Question 1

Which of the following statements is true?

A)The s orbital is spherical.
B)The s orbital has no nodal planes.
C)The s orbital is symmetrical.
D)The s orbital is associated with the l quantum number 0.
E)All of the above.

Answer 1

All of the above.

Question 2

How many nodal planes are present in an f-orbital?

A)2
B)3
C)7
D)4
E)5

Answer 2

3

Question 3

Which set of orbitals encompass two shapes?

A)The s orbitals.
B)The p orbitals.
C)The d orbitals.
D)Both B and C, above.
E)Both A and C, above.

Answer 3

The d orbitals.

Question 4

Which set of quantum numbers,n,l,m_l,could correspond to one of the highest energy electrons in Zr?

A)4, 2, -2
B)4, 2, +3
C)3, 2, -2
D)4, 3, -2

Question 5

What are the possibilities of the spin quantum number for Mg?

A)m_s = 1
B)m_s = 0
C)m_s = +1/2
D)m_s = - ½
E)Both C and D

Question 6

Which set of quantum numbers could correspond to a 4f-orbital?

A)n = 4, l = 4, m_l = +3
B)n = 4, l = 3, m_l = +4
C)n = 4, l = 3, m_l = -3
D)n = 3, l = 2, m_l = +1
E)n = 3, l = 2, m_l = 0

Question 7

Where is the nodal plane in a 1s orbital?

A)Along the x-axis.
B)Along the y-axis.
C)Along the z-axis.
D)Mid-way between the x and y-axes.
E)There is none.

Question 8

The three quantum numbers for an electron in a hydrogen atom in a certain state are n = 4,l = 1,m_l = 1.The electron is located in what type of orbital?

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

Question 9

Which set of quantum numbers corresponds to the electrons in He?

A)n = 1, l = 0, m_l = 1
B)n = 1, l = 0, m_l = 0
C)n = 1, l = 1, m_l =-0
D)n = 1, l = 0, m_l = -1
E)n = 1, l = 2, m_l = 0

Question 10

How many nodes are present in a 3s- and a 3p-orbital,respectively?

A)2;1
B)0; 1
C)0; 2
D)1; 1
E)2; 2

Question 11

Which of the following statements is true?

A)A 2s orbital has one nodal plane.
B)An electron in a p-orbital has zero probability of being found at the nucleus.
C)A p-orbital has a spherical boundary surface.
D)An s-orbital becomes more dense as the distance from the nucleus increases.
E)An electron in an s-orbital has a zero probability of being found at the nucleus.

Question 12

Where is the nodal plane for the p_x orbital?

A)On the x-z plane.
B)On the y-z plane.
C)On the x-y plane.
D)Midway between the x-y and the y-z plane.
E)The p_x orbital does not have a nodal plane.

Question 13

What is the only secondary quantum number associated with the 4s orbital?

A)l = 0
B)l = 1
C)l = 2
D)l = 3
E)l = 4

Question 14

What is the principle quantum number for gallium?

A)n = 1
B)n = 2
C)n = 3
D)n = 4
E)n = 5

Question 15

What is the l corresponding to the outermost p electrons in sulfur?

A)l = 0
B)l = 1
C)l = 2
D)l = 3
E)l = 4

Question 16

Nodal planes in orbitals can be accounted for by the wavelike behavior of electrons.

Question 17

How many total nodal planes are present in the 3d-orbitals?

A)15
B)0
C)5
D)20
E)10

Question 18

The total number of orbitals in a shell with principal quantum number 5 is

A)32.
B)50.
C)25.
D)40.
E)5.

Question 19

Which orbitals have the greatest number of nodes?

A)The s orbitals.
B)The p orbitals.
C)The d orbitals.
D)The f orbitals.
E)All orbitals have the same number of nodes.

Question 20

What shape do the p-orbitals have that each accommodates one nodal plane?

A)A spherical shape.
B)A dumbbell shape centered at the nucleus.
C)A clover leaf shape centered at the nucleus.
D)A clover leaf shape centered above and below the nucleus.
E)A toroidal shape around a dumbbell.

Question 21

Which of the following statements is true?

A)A p-electron penetrates more than an s-electron through the inner shells of an atom.
B)A p-electron penetrates less than a d-electron through the inner shells of an atom.
C)A p-electron has a nonzero probability density at the nucleus.
D)A d-electron has a nonzero probability density at the nucleus.
E)A p-electron experiences a smaller effective nuclear charge than an s-electron.

Question 22

Write the ground-state electron configuration of a tin(IV)ion.

A)[Kr]4d³5s¹5p⁶
B)[Kr]4d⁴5p⁶
C)[Kr]4d⁵5s²5p³
D)[Kr]4d⁵5p⁵
E)[Kr]4d¹⁰

Question 23

How many f electrons are in a gadolinium atom?

A)7
B)6
C)5
D)4
E)3

Question 24

How many unpaired electrons are in a chromium atom?

A)0
B)5
C)6
D)4
E)3

Question 25

Write the ground-state electron configuration of a samarium atom.

A)[Xe]4f⁷5d¹
B)[Xe]5d⁸
C)[Xe]4f⁷6s¹
D)[Xe]4f⁸
E)[Xe]4f⁶6s²

Question 26

Write the ground-state electron configuration of a lead atom.

A)[Xe]4f¹⁴5d⁵6s¹6p⁶7s²
B)[Xe]4f¹⁴5d¹⁰6s²6p²
C)[Xe]4f¹⁴5d¹⁰6s¹6p³
D)[Xe]4f¹⁴5d¹⁰6p⁴
E)[Xe]4f¹⁴5d⁹6s²6p³

Question 27

Write the ground-state electron configuration of Sb.

A)[Kr]4d⁸5s¹5p³
B)[Kr]4d⁵5s¹5p⁶
C)[Kr]4d¹⁰5p²
D)[Kr]4d¹⁰5s²5p³
E)[Kr]4d¹⁰5s²

Question 28

Write the ground-state electron configuration of a europium atom.

A)[Xe]5d⁷6s²
B)[Xe]4f²5d⁵6s²
C)[Xe]4f⁹
D)[Xe]4f⁷6s²
E)[Xe]4f⁵5d²6s²

Question 29

Write the ground-state electron configuration of In⁺.

A)[Kr]4d⁷5s²5p³
B)[Kr]4d⁸5s¹5p³
C)[Kr]4d⁵5s¹5p⁶
D)[Kr]4d¹⁰5s²
E)[Kr]4d¹⁰5s¹5p¹

Question 30

Write the ground-state electron configuration of Ru²⁺.

A)[Kr]4d⁵5s¹
B)[Kr]4d⁷
C)[Kr]4d⁵5p¹
D)[Kr]4d⁸
E)[Kr]4d⁶

Question 31

How many unpaired electrons are in a xenon atom?

A)0
B)1
C)2
D)3
E)4

Question 32

Write the ground-state electron configuration of Sb³⁺.

A)[Kr]4d⁸5s¹5p³
B)[Kr]4d⁵5s¹5p⁶
C)[Kr]4d¹⁰5p²
D)[Kr]4d¹⁰5s¹5p¹
E)[Kr]4d¹⁰5s²

Question 33

Write the ground-state electron configuration of Pb²⁺.

A)[Xe]4f¹⁴5d⁵6s¹6p⁶
B)[Xe]4f¹⁴5d¹⁰6s²
C)[Xe]4f¹⁴5d⁵6s²6p⁵
D)[Xe]4f¹⁴5d¹⁰6s¹6p¹
E)[Xe]4f¹⁴5d¹⁰6p²

Question 34

The three quantum numbers for an electron in a hydrogen atom in a certain state are n = 4,l = 2,m_l = 1.The electron is located in what type of orbital?

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

Question 35

How many unpaired electrons are in a calcium atom?

A)1
B)2
C)3
D)4
E)5

Question 36

How many unpaired electrons are in a chromium trivalent ion?

A)0
B)5
C)6
D)4
E)3

Question 37

Write the ground-state electron configuration of a terbium atom.

A)[Xe]4f¹¹
B)[Xe]4f¹⁰6s¹
C)[Xe]4f⁹6s²
D)[Xe]4f⁴5d⁵6s²
E)[Xe]4f⁶5d⁵

Question 38

Write the ground-state electron configuration of Tl⁺.

A)[Xe]4f¹⁴5d¹⁰6p²
B)[Xe]4f¹⁴5d¹⁰6s²
C)[Xe]4f¹⁴5d¹⁰6s¹6p¹
D)[Xe]4f¹⁴5d⁸6s¹6p³
E)[Xe]4f¹⁴5d⁵6s¹6p⁶

Question 39

A chloride ion contains how many unpaired electrons?

A)8
B)6
C)4
D)2
E)0

Question 40

An aluminum atom contains how many unpaired electrons?

A)7
B)6
C)5
D)4
E)3

Question 41

Which of the following species is isoelectronic with As^3-?

A)Na⁺
B)Cl ^-
C)Ar
D)Kr
E)Ba²⁺

Question 42

Which of the following has the largest atomic radius?

A)S^{2 -}
B)Cl
C)Cl ^-
D)K⁺
E)S

Question 43

Which of the following species is isoelectronic with Kr?

A)K⁺
B)Cl ^-
C)Ar
D)Xe
E)Sr²⁺

Question 44

Which of the following has the smallest atomic radius?

A)Cl
B)P
C)S
D)Si
E)Al

Question 45

Which of the following has the largest atomic radius?

A)F
B)O
C)N
D)C
E)B

Question 46

Which of the following is likely to form ions two units lower in charge than expected from the group number?

A)Tl
B)Hg
C)Zn
D)Se
E)Cd

Question 47

Which of the following species is isoelectronic with Ra²⁺?

A)I^-
B)Kr
C)Xe
D)Rn
E)Fr

Question 48

Which of the following atoms or ions is isoelectronic with Be²⁺?

A)Na⁺
B)Br ^-
C)He
D)Xe
E)He⁺

Question 49

Write the ground-state electron configuration of Fe³⁺.

A)[Ar]3d⁵4s²
B)[Ar]3d³4s²
C)[Ar]3d³4s⁰
D)[Ar]3d⁶4s¹
E)[Ar]3d³4s³

Question 50

Of the following,which has the largest atomic radius?

A)Ga
B)Ge
C)As
D)Se
E)Br

Question 51

Which of the following species is isoelectronic with S^{2 -} ?

A)Mg²⁺
B)Rb⁺
C)Ar
D)As^{3 -}
E)Br ^-

Question 52

What is the ground-state electron configuration of Rb⁺?

A)[Kr]
B)[Kr]5s¹
C)[Ar]
D)[Ar]4s¹
E)[Kr]4d¹⁰

Question 53

For F^-,write the ground-state electron configuration.

A)[Ne]2p⁵
B)[Ne]
C)[Ar]
D)[He]2p⁵
E)[He]1s²

Question 54

All the following can have the ground-state electron configuration [Xe]4f¹⁴5d¹⁰ except

A)Pb⁴⁺.
B)Hg²⁺.
C)Bi⁵⁺.
D)Tl⁺.
E)Au⁺.

Question 55

From the data below,which elements are likely to be nonmetals? Element
First ionization energy,kJ.mol ^{- 1
--------------------------}
1
1310
2
980
3
418
4
2080
5
947

A)3 and 5
B)3 only
C)1 and 4
D)1 and 2
E)2 and 5

Question 56

What is the ground-state electron configuration of Nb?

A)[Kr]4d⁴5s¹
B)[Kr]4d⁵5s²
C)[Kr]5d³4s²
D)[Kr]5d³5s²
E)[Kr]4d³5s²

Question 57

Write the ground-state electron configuration of Cl⁺.

A)[Ne]3s²3p⁴
B)[Ne]3s²3p⁵
C)[Ne]3s¹3p⁴
D)[Ne]3s²3p⁶
E)[Ar]3s²3p⁴

Question 58

From the data below,which element is likely to be a metal? Element
First ionization energy,kJ.mol ^{- 1
--------------------------}
1
1310
2
1011
3
418
4
2080
5
947

A)2
B)5
C)3
D)1
E)4

Question 59

All the following can have the ground-state electron configuration [Kr]4d¹⁰ except

A)Cd²⁺.
B)Ag⁺.
C)Pd.
D)In⁺.
E)Sn⁴⁺.

Question 60

Si⁴⁺ is isoelectronic with which of the following?

A)K⁺
B)Ne
C)Kr
D)Cl^-
E)Sr²⁺

Question 61

What are the subshell notation and the number of orbitals having the quantum numbers n = 4,l = 3?

A)4d and 5
B)4p and 3
C)3f and 7
D)3d and 5
E)4f and 7

Question 62

Which of the following is likely to form ions two units lower in charge than expected from the group number?

A)Hg
B)Cd
C)Sb
D)Ge
E)Zn

Question 63

In each pair,which ionization reaction is larger?
(a)I₃ of B; or I₃ of Be
(b)I₄ of C; or I₃ of B

Question 64

If the second ionization energy of copper is 1958 kJ·mol^-1,the first ionization energy is likely to be greater than 1958 kJ·mol^-1.True or false?

Question 65

All the following are non-metals except

A)C.
B)S.
C)Ga.
D)Se.
E)Cl.

Question 66

Consider the following ground-state electronic configurations.Which atom has the lowest first ionization energy?

A)[Ne] 3s²3p⁵
B)[Ne] 3s²3p³
C)[Ne] 3s²3p¹
D)[Ne] 3s²3p⁴

Question 67

Consider the following ground-state electronic configurations.Which atom has the highest electron affinity?

A)[He] 2s²2p⁵
B)[He] 2s²2p³
C)[He] 2s²2p¹
D)[He] 2s²2p⁴

Question 68

Which atom has the highest second ionization energy?

A)Cs
B)Na
C)Li
D)K

Question 69

Which atom has the lowest electron affinity?

A)Al
B)Si
C)P
D)S

Question 70

Consider the following ground-state electronic configurations.Which atom has both the highest first ionization energy and the highest electron affinity?

A)[Ne] 3s²3p⁵
B)[Ne] 3s²3p³
C)[Ne] 3s²3p¹
D)[Ne] 3s²3p⁴

Question 71

All the following are transition metals except:

A)Cd.
B)Cu.
C)Pd.
D)Pb.
E)Ag.

Question 72

All the following are metalloids except:

A)B.
B)As.
C)Ge.
D)Sb.
E)Si.

Question 73

What are the subshell notation and the number of orbitals having the quantum numbers n = 4,l = 2?

A)4d and 10
B)4f and 14
C)4d and 5
D)4p and 3
E)4f and 7

Question 74

Which atom has the highest first ionization energy?

A)Mg
B)Ca
C)Sr
D)Ba

Question 75

Which atom has the highest first ionization energy?

A)Pb
B)Sn
C)Ge
D)Si

Question 76

Which of the following elements has the least metal character?

A)In
B)Ge
C)Te
D)I
E)Tl

Question 77

Given the elements Cl,Ge,and K and three values of possible first ionization energies,418,1255,784 kJ.mol ^{- 1},match the atoms with their first ionization energies.

A)Cl (418), Ge (784), and K (1255 kJ.mol 1^{- 1})
B)Cl (1255), Ge (784), and K (418 kJ.mol ^{- 1})
C)Cl (784), Ge (1255), and K (418 kJ.mol ^{- 1})
D)Cl (1255), Ge (418), and K (784 kJ.mol ^{- 1})
E)Cl (418), Ge (1255), and K (784 kJ.mol ^{- 1})

Question 78

Which of the following has similar properties to Al?

A)Li
B)Be
C)Si
D)Ga
E)Mg

Question 79

Which of the following would be most reactive with air and water?

A)Ba
B)Mg
C)Ga
D)Br

Question 80

All the following are metals except:

A)Cd.
B)Zn.
C)Ge.
D)Al.
E)Ga.