Deck 8: Periodic Properties of the Elements

Question 1

An element that has the valence electron configuration 5s²4d⁵ belongs to which period and group?

A)period 4; group 8
B)period 5; group 9
C)period 5; group 7
D)period 5; group 3
E)period 5; group 13

Answer 1

period 5; group 7

Question 2

An element that has the valence electron configuration 5s²5p³ belongs to which period and group?

A)period 5; group 15
B)period 5; group 2
C)period 5; group 3
D)period 5; group 5
E)period 4; group 13

Answer 2

period 5; group 15

Question 3

An element that has the valence electron configuration 2s²2p² belongs to which period and group?

A)period 1; group 18
B)period 2; group 12
C)period 2; group 4
D)period 2; group 14
E)period 2; group 8

Answer 3

period 2; group 14

Question 4

Identify the number of valence electrons for Cd.

A)8
B)10
C)12
D)2
E)6

Question 5

An element that has the valence electron configuration 6s²5d⁴ belongs to which period and group?

A)period 6; group 16
B)period 6; group 12
C)period 6; group 4
D)period 6; group 6
E)period 6; group 2

Question 6

Identify the ground-state electron configuration for Cd.

A)[Kr]5s²5d¹⁰
B)[Kr]5s²4d¹⁰5p²
C)[Kr]4d¹⁰
D)[Kr]5s²4d⁸
E)[Kr]5s²4d¹⁰

Question 7

Identify the ground-state electron configuration for Se.

A)[Ar]4s²3d¹⁰4p⁴
B)[Ar]4s²4d¹⁰4p⁴
C)[Ar]4s²3d^104p6
D)[Ar]4s²3d¹⁰
E)[Ar]3d¹⁰4p⁴

Question 8

Identify the number of valence electrons for Pb.

A)4
B)2
C)28
D)12
E)26

Question 9

An element that has the valence electron configuration 6s²6p⁶ belongs to which period and group?

A)period 6; group 16
B)period 6; group 18
C)period 7; group 16
D)period 7; group 18
E)period 7; group 17

Question 10

An element that has the valence electron configuration 4s²4p⁴ belongs to which period and group?

A)period 4; group 16
B)period 4; group 6
C)period 4; group 8
D)period 5; group 6
E)period 5; group 18

Question 11

An element that has the valence electron configuration 4s² belongs to which period and group?

A)period 4; group 2
B)period 4; group 14
C)period 4; group 6
D)period 4; group 1
E)period 4; group 9

Question 12

Identify the ground-state electron configuration for I.

A)[Kr]5s²4d¹⁰5p⁶
B)[Kr]5s²4d¹⁰5p⁵
C)[Kr]4d¹⁰5p⁶
D)[Kr]5s²5p⁶
E)[Kr]5s²5d¹⁰5p⁶

Question 13

Identify the number of core electrons for O.

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

Question 14

An element that has the valence electron configuration 6s²5d⁷ belongs to which period and group?

A)period 7; group 9
B)period 6; group 7
C)period 6; group 2
D)period 6; group 9
E)period 7; group 7

Question 15

An element that has the valence electron configuration 3s¹ belongs to which period and group?

A)period 4; group 7
B)period 4; group 2
C)period 4; group 1
D)period 3; group 2
E)period 3; group 1

Question 16

Identify the number of core electrons for Cd.

A)44
B)48
C)46
D)45
E)47

Question 17

Identify the number of valence electrons for O.

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

Question 18

Identify the ground-state electron configuration for Pb.

A)[Xe]6s²6p²
B)[Xe]6s²5d¹⁰6p²
C)[Xe]6s²5f¹⁴6d¹⁰6p²
D)[Xe]6s²4f¹⁴5d¹⁰6p²
E)[Xe]6s²4f¹⁴5d^106s26p²

Question 19

Identify the ground-state electron configuration for Sr.

A)[Kr]5s²4d²
B)[Kr]5s²4d^105p2
C)[Kr]5s²
D)[Kr]5s²5d¹⁰5p²
E)[Kr]5s²4d¹⁰

Question 20

An element that has the valence electron configuration 3s²3p⁶ belongs to which period and group?

A)period 3; group 17
B)period 3; group 2
C)period 3; group 7
D)period 3; group 3
E)period 3; group 5

Question 21

Using the periodic table, identify the element with the following exception electron configuration: [Kr]5s¹4d⁸

A)Tc
B)Ru
C)Os
D)Rh
E)V

Question 22

Using the periodic table, identify the element with the following exception electron configuration: [Kr]5s¹4d¹⁰

A)Cd
B)Hg
C)Pd
D)Au
E)Ag

Question 23

Use the periodic table to determine the ground-state electron configuration for the following element: Sc

A)[Ar]4s²3d¹
B)[Ar]4s²3d²
C)[Ar]4s³
D)[Ar]3d³
E)[Ar]4s²3d³

Question 24

Use the periodic table to determine the ground-state electron configuration for the following element: Te

A)[Kr]5s²4d¹⁰5p⁶
B)[Kr]5s²4d¹⁰5p⁴
C)[Xe]5s²4d¹⁰5p⁴
D)[Xe]6s²5d¹⁰4f¹⁴6p⁴
E)[Kr]5s²4d⁶

Question 25

Using the periodic table, identify the element with the following exception electron configuration: [Kr]5s¹4d⁷

A)Mo
B)Tc
C)Rh
D)Ru
E)Pd

Question 26

Using the periodic table, identify the element with the following exception electron configuration: [Ar]4s¹3d¹⁰

A)Ga
B)Zn
C)Cu
D)Ni
E)Cd

Question 27

Using the periodic table, identify the element with the following exception electron configuration: [Xe]6s¹5d⁹

A)Au
B)Pt
C)Pd
D)Tl
E)Hf

Question 28

Using the periodic table, identify the element with the following exception electron configuration: [Kr]5s¹4d⁵

A)Zr
B)Ni
C)Re
D)Tc
E)Mo

Question 29

Using the periodic table, identify the element with the following exception electron configuration: [Ar]4s¹3d⁵

A)Ni
B)Co
C)Cr
D)Mn
E)Fe

Question 30

Using the periodic table, identify the element with the following exception electron configuration: [Kr]5s¹4d⁴

A)Ti
B)Zr
C)Nb
D)W
E)Mn

Question 31

Using the periodic table, identify the element with the following exception electron configuration: [Kr]4d¹⁰

A)Sn
B)Ru
C)Sr
D)Cd
E)Pd

Question 32

Use the periodic table to determine the ground-state electron configuration for the following element: F

A)[He]2s²2p⁵
B)[He]2s²3p⁵
C)[He]3s²2p⁵
D)[He]2s²1d¹⁰2p⁵
E)[He]3s²3p⁵

Question 33

Use the periodic table to determine the ground-state electron configuration for the following element: Si

A)[Ne]3s²3p¹
B)[Ne]3s²3p³
C)[Ne]3s²3p⁶
D)[Ne]3s²3p²
E)[Ne]3s²3p⁴

Question 34

Use the periodic table to determine the ground-state electron configuration for the following element: Fe

A)[Ar]4s²4d⁶
B)[Ar]4s²3d⁶
C)[Ar]4s²5d⁶
D)[Ar]4s²5d³
E)[Ar]4s²3d⁸

Question 35

Use the periodic table to determine the ground-state electron configuration for the following element: Co

A)[Ar]4s²3d⁷
B)[Ar]4s²3d⁹
C)[Ar]4s²3d⁵
D)[Ar]3d⁹
E)[Ar]4s²3d³

Question 36

Using the periodic table, identify the element with the following exception electron configuration: [Xe]6s¹5d¹⁰

A)Hg
B)Au
C)Cd
D)Ir
E)Rg

Question 37

Use the periodic table to determine the ground-state electron configuration for the following element: As

A)[Ar]4s²4d⁵4p⁵
B)[Ar]4s²3d¹⁰4p⁵
C)[Ar]4s²4d¹⁰4p⁵
D)[Ar]4s²4d¹⁰4p³
E)[Ar]4s²3d¹⁰4p³

Question 38

Use the periodic table to determine the ground-state electron configuration for the following element: Zr

A)[Kr]5s²4d¹⁰5p²
B)[Kr]5s²5p²
C)[Kr]5s²5d²
D)[Kr]5s²4d²
E)[Kr]5s²4d¹⁰5p⁴

Question 39

An element that has the valence electron configuration 6s²6p² belongs to which period and group?

A)period 6; group 16
B)period 6; group 6
C)period 6; group 4
D)period 6; group 14
E)period 6; group 9

Question 40

Use the periodic table to determine the ground-state electron configuration for the following element: Mn

A)[Ar]4s²3d⁵
B)[Ar]4s²3p⁵
C)[Ar]4s²3d¹⁰4p⁵
D)[Kr]5s²4d⁶
E)[Ne]3s²3p⁴

Question 41

Use the periodic table to predict the most stable oxidation state for the following element: Pb

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

Question 42

Use the periodic table to predict the most stable oxidation state for the following element: Ga

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

Question 43

Use the periodic table to predict the most stable oxidation state for the following element: B

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

Question 44

How many unpaired electrons are present in the ground-state Kr atom?

A)1
B)2
C)0
D)3
E)5

Question 45

Use the periodic table to predict the most stable oxidation state for the following element: Ca

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

Question 46

How many unpaired electrons are there in the ground-state of As?

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

Question 47

How many valence electrons does an atom of S have?

A)3
B)1
C)2
D)4
E)6

Question 48

Use the periodic table to determine the ground-state electron configuration for the following element: Ga

A)[Ar]4s²3d¹⁰4p²
B)[Ar]4s²3d⁹
C)[Ar]4s²3d¹⁰
D)[Ar]4s²4p²
E)[Ar]4s²3d¹⁰4p¹

Question 49

Use the periodic table to predict the most stable oxidation state for the following element: Al

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

Question 50

Use the periodic table to predict the most stable oxidation state for the following element: Br

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

Question 51

How many of the following elements have one unpaired electron in the ground state? B Al S Cl

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

Question 52

How many of the following elements have two unpaired electrons in the ground state? C O Ti Si

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

Question 53

How many unpaired electrons are present in the ground-state Ge atom?

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

Question 54

Use the periodic table to predict the most stable oxidation state for the following element: F

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

Question 55

Use the periodic table to predict the most stable oxidation state for the following element: K

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

Question 56

Use the periodic table to predict the most stable oxidation state for the following element: O

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

Question 57

How many unpaired electrons are present in the ground-state P atom?

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

Question 58

Identify the number of valence electrons for Mn.

A)8
B)7
C)5
D)2

Question 59

Use the periodic table to predict the most stable oxidation state for the following element: Na

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

Question 60

Identify the element that has a ground-state electronic configuration of [Ar]4s²3d¹⁰4p¹.

A)Al
B)In
C)Ga
D)B

Question 61

How many valence electrons does an atom of Al possess?

A)1
B)2
C)5
D)3
E)8

Question 62

Place the following in order of increasing atomic radius. As O B

A)As < Br < O
B)O < As < Br
C)Br < As < O
D)As < O < Br
E)O < Br < As

Question 63

Identify the species that has the smallest radius.

A)cation
B)anion
C)neutral
D)All of the above are the same size.

Question 64

Place the following in order of increasing radius. Ca²⁺ S²⁻ Cl⁻

A)Ca²⁺ < Cl⁻ < S²⁻
B)Cl⁻ < Ca²⁺ < S²⁻
C)S²⁻ < Cl⁻ < Ca²⁺
D)Ca²⁺ < S²⁻ < Cl⁻
E)Cl⁻ < S²⁻ < Ca²⁺

Question 65

Which reaction below represents the second ionization of Sr?

A)Sr(g)→ Sr⁺(g)+ e⁻
B)Sr²⁺(g)+ e⁻ → Sr⁺(g)
C)Sr⁺(g)+ e⁻ → Sr(g)
D)Sr^⁻(g)+ e⁻ → Sr²⁻(g)
E)Sr⁺(g)→ Sr²⁺(g)+ e⁻

Question 66

Identify the complete electronic configuration for Mn.

A)1s²2s²2p⁶3s²3p⁶4s²4d⁵
B)1s²2s²2p⁶3s²3p⁶4s¹3d⁶
C)1s²2s²2p⁶3s²3p⁶4s²3d⁵
D)1s²2s²2p⁶3s²3p⁶4s²4p⁵

Question 67

Place the following in order of increasing radius. Br⁻ Na⁺ Rb⁺

A)Br⁻ < Rb⁺ < Na⁺
B)Na⁺ < Rb⁺ < Br⁻
C)Rb⁺ < Br⁻ < Na⁺
D)Br⁻ < Na⁺ < Rb⁺
E)Rb⁺ < Na⁺ < Br⁻

Question 68

How many valence electrons do the noble gases possess?

A)1
B)2
C)7
D)6
E)8

Question 69

How many valence electrons does an atom of Cu possess?

A)2
B)9
C)11
D)3
E)1

Question 70

How many valence electrons do the alkali earth metals possess?

A)1
B)2
C)7
D)6
E)8

Question 71

Place the following elements in order of decreasing atomic radius. Xe Rb Ar

A)Ar > Xe > Rb
B)Xe > Rb > Ar
C)Ar > Rb > Xe
D)Rb > Xe > Ar
E)Rb > Ar > Xe

Question 72

How many valence electrons does an atom of Ba possess?

A)2
B)1
C)8
D)6
E)3

Question 73

What period 3 element has the following ionization energies (all in kJ mol^-1)? IE₁ = 1012 IE₂ = 1900 IE₃ = 2910 IE₄ = 4960 IE₅ = 6270 IE₆ = 22 200

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

Question 74

How many valence electrons does an atom of Ti possess?

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

Question 75

Identify the element that has a ground-state electronic configuration of [Kr]5s²4d⁵.

A)Tc
B)Mn
C)Nb
D)Ru

Question 76

Choose the statement that is TRUE.

A)Outer electrons efficiently shield one another from nuclear charge.
B)Core electrons effectively shield outer electrons from nuclear charge.
C)Valence electrons are the most difficult of all electrons to remove.
D)Core electrons are the easiest of all electrons to remove.
E)All of the above are true.

Question 77

How many valence electrons do the halogens possess?

A)5
B)6
C)2
D)1
E)7

Question 78

Place the following elements in order of increasing atomic radius. P Ba Cl

A)Ba < P < Cl
B)P < Cl < Ba
C)Cl < P < Ba
D)Cl < Ba < P
E)Ba < Cl < P

Question 79

Place the following in order of decreasing radius. Te²⁻ F⁻ O²⁻

A)F⁻ > O²⁻ > Te²⁻
B)F⁻ > Te²⁻ > O²⁻
C)Te²⁻ > O²⁻ > F⁻
D)Te²⁻ > F⁻ > O²⁻
E) O²⁻ > F⁻ > Te²⁻

Question 80

Which reaction below represents the first ionization of O?

A)O⁺(g)+ e⁻ → O(g)
B)O(g)+ e⁻ → O⁻(g)
C)O⁻(g)→ O(g)+ e⁻
D)O(g)→ O⁺(g)+ e⁻
E)O⁻(g)+ e⁻ → O²⁻(g)