Deck 8: Periodic Properties of the Elements

Question 1

Choose the orbital diagram that represents the ground state of N.

A)

B)

C)

D)

E)

Answer 1

Question 2

Give the ground state electron configuration for Cd.

A)[Kr] 5s² 5d¹⁰
B)[Kr] 5s² 4d¹⁰ 5p²
C)[Kr] 4d¹⁰
D)[Kr] 5s² 4d⁸
E)[Kr] 5s² 4d¹⁰

Answer 2

[Kr] 5s² 4d¹⁰

Question 3

Give the ground state electron configuration for Pb.

A)[Xe] 6s² 6p²
B)[Xe] 6s² 5d¹⁰ 6p²
C)[Xe] 6s² 5f¹⁴ 6d¹⁰ 6p²
D)[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²
E)[Xe] 6s² 5f¹⁴ 5d¹⁰ 6p²

Answer 3

[Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²

Question 4

Choose the valence orbital diagram that represents the Si.

A)
B)
C)
D)
E)

Question 5

Choose the valence orbital diagram that represents the ground state of Zn.

A)
B)
C)
D)
E)

Question 6

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

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

Question 7

Write out the orbital diagram that represents the ground state of As.How many unpaired electrons are there?

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

Question 8

Give the ground state electron configuration for Sr.

A)[Kr] 5s² 4d²
B)[Kr] 5s² 4d¹⁰ 5p²
C)[Kr] 5s²
D)[Kr] 5s² 5d¹⁰ 5p²
E)[Kr] 5s² 4d¹⁰

Question 9

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

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

Question 10

Give the ground state electron configuration for I.

A)[Kr] 5s² 4d¹⁰ 5p⁶
B)[Kr] 5s² 4d¹⁰ 5p⁵
C)[Kr] 4d¹⁰ 5p⁶
D)[Kr] 5s² 5p⁶
E)[Kr] 5s² 5d¹⁰ 5p⁶

Question 11

Which of the following statements is true?

A)An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
B)An orbital that penetrates into the region occupied by core electrons is more shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
C)It is possible for two electrons in the same atom to have identical values for all four quantum numbers.
D)Two electrons in the same orbital can have the same spin.
E)None of the above are true.

Question 12

When filling degenerate orbitals,electrons fill them singly at first,with parallel spins.This is know as

A)Aufbau principle.
B)Heisenberg uncertainty principle.
C)Hund's rule.
D)Pauli exclusion principle.

Question 13

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle)to the Cl atom.

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

Question 14

Identify the element that has a ground state electronic configuration of [Ar] 4s² 3d¹⁰ 4p¹.

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

Question 15

No two electrons can have the same four quantum number is known as

A)Pauli exclusion principle.
B)Hund's rule.
C)Aufbau principle.
D)Heisenberg uncertainty principle.

Question 16

Give the set of four quantum numbers that represent the last electron added (using the Aufbau principle)to the Zn atom.

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

Question 17

Identify the element that has a ground state electronic configuration of [Kr] 5s² 4d⁵.

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

Question 18

Give the set of four quantum numbers that could represent the last electron added (using the Aufbau principle)to the Sr atom.

A)n = 5,l = 0,m_l = 0,m_s = -
B)n = 4,l = 1,m_l = 1,m_s = -
C)n = 5,l = 1,m_l = 0,m_s = +
D)n = 4,l = 1,m_l = -1,m_s = +
E)n = 5,l = 1,m_l =1 ,m_s = -

Question 19

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

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

Question 20

Give the ground state electron configuration for Se.

A)[Ar] 4s² 3d¹⁰ 4p⁴
B)[Ar] 4s² 4d¹⁰ 4p⁴
C)[Ar] 4s² 3d¹⁰ 4p⁶
D)[Ar] 4s² 3d¹⁰
E)[Ar] 3d¹⁰ 4p⁴

Question 21

How many of the following elements have 2 unpaired electrons in the ground state?
C O Ti Si

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

Question 22

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 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 23

How many valence electrons does an atom of Ti possess?

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

Question 24

Give the complete electronic configuration for Mn.

A)1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4d⁵
B)1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁶
C)1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵
D)1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁵

Question 25

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

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

Question 26

Predict the charge for the most stable ion of nitrogen.

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

Question 27

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 28

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 29

How many valence electrons do the alkali metals possess?

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

Question 30

Identify the number of valence electrons for Mg.

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

Question 31

Place the following in order of decreasing radius.
Te^2⁻ F^⁻ O^2⁻

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

Question 32

How many valence electrons does an atom of S have?

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

Question 33

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

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

Question 34

How many valence electrons does an atom of C have?

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

Question 35

How many valence electrons does an atom of Ba possess?

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

Question 36

How many valence electrons does an atom of Cu possess?

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

Question 37

Place the following in order of increasing radius.
Ca²⁺ S^2⁻ Cl^⁻

A)Ca²⁺ < Cl⁻ < S^2-
B)Cl⁻ < Ca²⁺ < S²⁻
C)S²⁻ < Cl⁻ < Ca²⁺
D)Ca²⁺ < S²⁻ < Cl⁻
E)Cl⁻ < S²⁻ < Ca²⁺

Question 38

How many valence electrons does an atom of Al possess?

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

Question 39

How many valence electrons do the halogens possess?

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

Question 40

How many of the following elements have 1 unpaired electron in the ground state?
B Al S Cl

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

Question 41

Choose the ground state electron configuration for Ti²⁺.

A)[Ar] 3d²
B)[Ar] 4s²
C)[Ar] 4s² 3d²
D)[Ar] 4s² 3d⁴
E)[Ar] 3d⁴

Question 42

Give the ground state electron configuration for the ion of Ba.

A)[Kr] 5s² 5p⁶
B)[Kr] 5s² 4d¹⁰ 5p⁶ 6s² 6p²
C)[Kr] 5s² 4d¹⁰ 5p⁶ 6s¹
D)[Kr] 5s² 4d¹⁰ 5p⁶ 6s²
E)[Kr] 5s² 4d¹⁰ 5p⁶

Question 43

Refer to the figure.Place the following in order of decreasing IE₁.
Cs Mg Ar

A)Cs > Mg > Ar
B)Mg > Ar > Cs
C)Ar > Mg > Cs
D)Cs > Ar > Mg
E)Mg > Cs > Ar

Question 44

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

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

Question 45

Refer to the figure.Place the following in order of increasing IE₁.
N F As

A)N < As < F
B)As < N < F
C)F < N < As
D)As < F < N
E)F < AS < N

Question 46

How many of the following species are diamagnetic?
Cs Zr²⁺ Al³⁺ Hg²⁺

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

Question 47

Choose the paramagnetic species from below.

A)Ca
B)O²⁻
C)Cd²⁺
D)Zn
E)Nb³⁺

Question 48

Choose the ground state electron configuration for Zn²⁺.

A)[Ar] 4s² 3d⁸
B)[Ar] 3d¹⁰
C)[Ar] 4s² 3d⁶
D)[Ar]
E)[Ar] 3d⁸

Question 49

Refer to the figure.Place the following in order of increasing IE₁.
K Ca Rb

A)Ca < K < Rb
B)Rb < Ca < K
C)Ca < Rb < K
D)Rb < K < Ca
E)K < Ca < Rb

Question 50

Give the ground state electron configuration for Mg²⁺.

A)1s² 2s² 2p⁶ 3s²
B)1s² 2s² 2p⁶
C)1s² 2s² 2p⁶ 3s² 3p²
D)1s² 2s² 2p⁶ 3s² 3p⁶
E)1s² 2s² 2p⁶ 3s¹

Question 51

Choose the ground state electron configuration for Zr²⁺.

A)[Kr] 5s²
B)[Kr] 5s² 4d²
C)[Kr] 4d²
D)[Kr]
E)[Kr] 5s² 4d⁴

Question 52

How many of the following species are paramagnetic?
Sc³⁺ Br^⁻ Mg²⁺ Se

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

Question 53

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 54

Give the ground state electron configuration for Se^2⁻.

A)[Ar] 4s² 3d¹⁰ 4p⁴
B)[Ar] 4s² 3d¹⁰ 4p²
C)[Ar] 4s² 4p⁶
D)[Ar] 4s² 3d¹⁰ 4p⁶
E)[Ar] 4s² 3d⁸ 4p⁶

Question 55

Place the following in order of decreasing metallic character.
P As K

A)P > As > K
B)As > P > K
C)K > P > As
D)As > K > P
E)K > As > P

Question 56

Choose the paramagnetic species from below.

A)Ti⁴⁺
B)O
C)Ar
D)All of the above are paramagnetic.
E)None of the above are paramagnetic.

Question 57

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)

Question 58

Choose the diamagnetic species from below.

A)Sn²⁺
B)Br
C)P
D)Cr
E)None of the above are diamagnetic.

Question 59

Give the ground state electron configuration for Br⁻.

A)[Ar] 4s² 3d¹⁰ 4p⁶
B)[Ar] 4s² 3d¹⁰ 4p⁵
C)[Ar] 4s² 4p⁶
D)[Ar] 4s² 4d¹⁰ 4p⁶
E)[Ar] 4s² 3d¹⁰ 4p⁴

Question 60

Give the ground state electron configuration for Rb⁺.

A)[Ar ]4s² 4p⁶
B)[Kr] 5s¹
C)[Ar] 4s² 3d¹⁰ 4p⁶
D)[Kr] 5s²
E)[Kr] 5s² 4d²

Question 61

Match the following.

-number of unpaired electrons in Cr²⁺

A)0
B)2
C)electrons in the outermost shell
D)1
E)electrons in completed shells

Question 62

Match the following.
number of unpaired electrons in Na

A)0
B)2
C)electrons in the outermost shell
D)1
E)electrons in completed shells

Question 63

Choose the valence orbital diagram that represents the ground state of Zr.

A)
B)
C)
D)
E)

Question 64

Why does the size of the transition elements stay roughly the same as you move across a period?

Question 65

Match the following.
core electrons

A)0
B)2
C)electrons in the outermost shell
D)1
E)electrons in completed shells

Question 66

Which reaction below represents the second electron affinity of S?

A)S(g)+ e⁻ → S⁻(g)
B)S⁻(g)+ e⁻ → S²⁻(g)
C)S(g)→ S⁺(g)+ e⁻
D)S⁻(g)→ S(g)+ e⁻
E)S²⁻(g)→ S⁻(g)+ e⁻

Question 67

Choose the valence orbital diagram that represents the ground state of Se²⁻.

A)
B)
C)
D)
E)

Question 68

Choose the ground state electron configuration for Cr³⁺.

A)[Ar] 4s¹ 3d²
B)[Ar]
C)[Ar] 4s² 3d⁶
D)[Ar] 3d³
E)[Ar] 4s² 3d¹

Question 69

Give the set of four quantum numbers that could represent the electron lost to form the K⁺ ion from the K atom.

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

Question 70

Place the following in order of increasing metallic character.
Br Cs Se

A)Br < Se < Cs
B)Se < Br < Cs
C)Cs < Br < Se
D)Cs < Se < Br
E)Br < Cs < Se

Question 71

Give the set of four quantum numbers that could represent the electron gained to form the Br^- ion from the Br atom.

A)n = 4,l = 2,m_l = 1,m_s = -
B)n = 4,l = 0,m_l = 1,m_s = +
C)n = 4,l = 1,m_l = 1,m_s = -
D)n = 3,l = 2,m_l = 2,m_s = +
E)n = 5,l = 1,m_l = -1 ,m_s = +

Question 72

Give the set of four quantum numbers that could represent the electron lost to form the Rb⁺ ion from the Rb atom.

A)n = 6,l = 0,m_l = 0,m_s = -
B)n = 4,l = 1,m_l = 1,m_s = -
C)n = 5,l = 1,m_l = 0,m_s = +
D)n = 4,l = 1,m_l = 0,m_s = -
E)n = 5,l = 0,m_l = 0,m_s = +

Question 73

Below is a list of successive ionization energies (in kJ/mol)for a period 3 element.Identify the element and explain how you came to that conclusion.
IE₂ = 2250 IE₃ = 3360 IE₄= 4560 IE₅= 7010 IE₆= 8500 IE₇ = 27,100

Question 74

List the noble gas that has the highest ionization energy.

Question 75

Why do Li,Na,and K have similar chemical properties?

Question 76

Match the following.
valence electrons

A)0
B)2
C)electrons in the outermost shell
D)1
E)electrons in completed shells

Question 77

Which reaction below represents the electron affinity of Li?

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

Question 78

Why is the first ionization energy of sulfur smaller than the first ionization energy of phosphorus?

Question 79

Match the following.
number of unpaired electrons in Zn²⁺

A)0
B)2
C)electrons in the outermost shell
D)1
E)electrons in completed shells

Question 80

Define ionization energy.