Deck 8: Periodic Properties of the Elements

Question 1

When filling degenerate orbitals,electrons fill them singly first,with parallel spins.This is known as (the)

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

Answer 1

Hund's rule.

Question 2

The element that corresponds to the electron configuration 1s²2s²2p⁶3s²3p⁶4s¹3d⁵ is

A) titanium.
B) vanadium.
C) chromium.
D) manganese.
E) iron.

Answer 2

chromium.

Question 3

Give the ground state electron configuration for Sr.

A) [Kr]5s²4d²
B) [Kr]5s²4d¹⁰5p²
C) [Kr]5s²
D) [Kr]5s²5d¹⁰5p²
E) [Kr]5s²4d¹⁰

Answer 3

[Kr]5s²

Question 4

How many valence electrons do the alkaline earth metals possess?

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

Question 5

Give the ground state electron configuration for Se.

A) [Ar]4s²3d¹⁰4p⁴
B) [Ar]4s²4d¹⁰4p⁴
C) [Ar]4s²3d¹⁰4p⁶
D) [Ar]4s²3d¹⁰
E) [Ar]3d¹⁰4p⁴

Question 6

Electrons filling up the orbitals from low to high is known as (the)

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

Question 7

Give the number of core electrons for Cd.

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

Question 8

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

A)

B)

C)

D)

E)

Question 9

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

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

Question 10

No two electrons can have the same four quantum numbers is known as (the)

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

Question 11

Give the complete electronic configuration for oxygen.

A) 1s²2s²2p_y²2p_z²
B) 1s²2s²2p_x²2p_y¹2p_z¹
C) 1s²2s²2p_x²2p_z²
D) 1s²2s²2p_x²2p_y²
E) 1s²2s²2p_x⁴

Question 12

How many valence electrons do the halogens possess?

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

Question 13

Give the complete electronic configuration for nitrogen.

A) 1s²2s²2p_y¹2p_z²
B) 1s²2s²2p_x³
C) 1s²2s²2p_x²2p_y¹
D) 1s²2s²2p_x¹2p_y¹2p_z¹
E) 1s²2s²2p_y²2p_z¹

Question 14

Give the ground state electron configuration for Cd.

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

Question 15

How many valence electrons do the noble gases possess?

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

Question 16

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 is true.

Question 17

Give the complete electronic configuration for Mn.

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

Question 18

Give the ground state electron configuration for Pb.

A) [Xe]6s²6p²
B) [Xe]6s²5d¹⁰6p²
C) [Xe]6s²5f¹⁴6d¹⁰6p²
D) [Xe]6s²4f¹⁴5d¹⁰6p²
E) [Xe]6s²4f¹⁴5d¹⁰6s²6p²

Question 19

How many valence electrons do the alkali metals possess?

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

Question 20

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

A)

B)

C)

D)

E)

Question 21

Which reaction below represents the 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 22

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

A) [Kr]5s²5p⁶
B) [Kr]5s²4d¹⁰5p⁶6s²6p²
C) [Kr]5s²4d¹⁰5p⁶6s¹
D) [Kr]5s²4d¹⁰5p⁶6s²
E) [Kr]5s²4d¹⁰5p⁶

Question 23

For a particular element,identify the species that has the smallest radius.

A) cation
B) anion
C) neutral
D) radical
E) They are all the same size.

Question 24

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 25

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 26

Place the following in order of increasing metallic character. Rb Cs K Na

A) K < Cs < Na < Rb
B) Na < K < Rb < Cs
C) Cs < Rb < K < Na
D) K < Cs < Rb < Na
E) Na < Rb < Cs < K

Question 27

Choose the ground state electron configuration for Ti²⁺.

A) [Ar]3d²
B) [Ar]4s²
C) [Ar]4s²3d²
D) [Ar]4s²3d⁴
E) [Ar]3d⁴

Question 28

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 29

A cation of +2 indicates that an element has

A) lost two electrons.
B) lost two protons.
C) lost two neutrons.
D) gained two electrons.
E) gained two protons.

Question 30

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

A)

B)

C)

D)

E)

Question 31

Choose the ground state electron configuration for Cr³⁺.

A) [Ar]4s¹3d²
B) [Ar]
C) [Ar]4s²3d⁶
D) [Ar]3d³
E) [Ar]4s²3d¹

Question 32

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 33

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 34

Choose the valence orbital diagram that represents the ground state of Sr^2⁺.

A)

B)

C)

D)

E)

Question 35

Identify the isoelectronic elements.

A) Cl^-, F^-, Br^-, I^-, At^-
B) N^3-, S^2-, Br^-, Cs⁺, Sr²⁺
C) P^3-, S^2-, C1^-, K⁺, Ca²⁺
D) Zn²⁺, Co²⁺, Cu²⁺, Cr²⁺, Cd²⁺
E) Ne, Ar, Kr, Xe, He

Question 36

Choose the ground state electron configuration for Zn²⁺.

A) [Ar]4s²3d⁸
B) [Ar]3d¹⁰
C) [Ar]4s²3d⁶
D) [Ar]
E) [Ar]3d⁸

Question 37

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 38

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 39

Give the ground state electron configuration for F⁻.

A) 1s²2s²2p⁶
B) 1s²2s²2p⁵
C) 1s²2s²2p⁴
D) 1s²2s²2p³
E) 1s²2s²2p²

Question 40

Identify the elements correctly shown by decreasing radii size.

A) N^3- > N
B) K⁺ > K
C) N > N^3-
D) Cu²⁺ > Cu⁺
E) S^- > S^2-

Question 41

Describe the reaction of the alkali metals with non-metals.

A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves

Question 42

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 = 2, m_l = 2, m_s = +
E) n = 4, l = 2 m_l = 0, m_s = -

Question 43

Which element has the ground-state electron configuration [Xe]6s²?

A) Re
B) Ir
C) Eu
D) Gd

Question 44

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 = 0, 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 45

Identify the most reactive alkali metal with water.

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

Question 46

Identify the element that has a ground state electronic configuration of [Ar]4s²3d¹⁰4p⁶.

A) Ar
B) Xe
C) Kr
D) N

Question 47

The complete electron configuration of silicon,element 14,is ________.

A)

3s²3p²
B)
2p¹⁰
C)
2p6
D) 1p⁶2s⁴
E) 2s6_2p2

Question 48

The element that corresponds to the electron configuration 1s²2s¹ is

A) nitrogen.
B) carbon.
C) boron.
D) beryllium.
E) lithium.

Question 49

The condensed electron configuration of gallium,element 31,is ________.

A) [Kr]4s²3d³
B) [Ne]3s⁴3p⁹
C) [Kr]4s⁴3d³
D) [Ar]3d¹⁰4s²4p¹
E) [Ar]4s³

Question 50

Give the electron configuration for O.

A) 1s²2s²2p⁴
B) 1s²2p⁴
C) 1s²2s²2p³
D) 1s²2s¹2p⁵
E) 1s²2s²2p²

Question 51

Identify a characteristic of halogens.

A) powerful reducing agents
B) forms water in reactions
C) powerful oxidizing agents
D) absorbs water in reactions
E) inert

Question 52

Identify the noble gas that is used by researchers to cool down samples for analysis.

A) radon
B) neon
C) helium
D) iodine
E) oxygen

Question 53

Halogens can react with each other to form

A) covalent bonds.
B) ionic bonds.
C) salts.
D) hydrogen halides.
E) metal halides.

Question 54

Give the ground state electron configuration for Te.

A) [Kr]5s²4d¹⁰5p⁶
B) [Kr]5s²4d¹⁰5p⁴
C) [Kr]4d¹⁰5p⁴
D) [Kr]5s¹5p⁴
E) [Kr]5s²5d⁸5p⁶

Question 55

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 =1, m_l = 1, m_s = -

Question 56

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

A) n = 2, l = 1, m_l = 1, m_s = +
B) n = 3, l = 1, 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 57

The condensed electron configuration of magnesium,element 12,is ________.

A) [He]2s⁴2p⁴
B) [Ne]2p⁸
C) [Ne]3s²
D) [He]2s²
E) [He]2s⁶

Question 58

Describe the reaction of the noble gases with metals.

A) inert
B) vigorous
C) mild reaction
D) forms water
E) dissolves

Question 59

The complete electron configuration of titanium,element 22,is ________.

A)


3p6
B)



3d²4s²
C)


3p4
D)

3s4
E)


3p²

Question 60

The element that corresponds to the electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹ is

A) iron.
B) titanium.
C) scandium.
D) vanadium.
E) manganese.

Question 61

How many valence electrons does an atom of Tl possess?

A) 3
B) 5
C) 0
D) 4
E) 7

Question 62

Give the number of valence electrons for Pb.

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

Question 63

Give the number of core electrons for phosphorus.

A) 3
B) 6
C) 10
D) 7
E) 11

Question 64

How many valence electrons does an atom of Na possess?

A) 1
B) 3
C) 4
D) 7
E) 0

Question 65

How many valence electrons does an atom of Ar possess?

A) 2
B) 4
C) 7
D) 0
E) 8

Question 66

How many valence electrons does an atom of N have?

A) 3
B) 5
C) 2
D) 1
E) 7

Question 67

Give the number of valence electrons for Zr.

A) 0
B) 11
C) 4
D) 2
E) 14

Question 68

Give the number of valence electrons for Cl.

A) 8
B) 9
C) 2
D) 3
E) 7

Question 69

How many valence electrons does an atom of Ca possess?

A) 2
B) 4
C) 8
D) 6
E) 3

Question 70

Which of the following have their valence electrons in the same shell?

A) Rb, Sb, I
B) Al, Ge, Sb
C) P, As, Sb
D) He, Ne, F
E) Zn, Cd, Hg

Question 71

An element that has the valence electron configuration 5s²5p⁵ belongs to which period and group?

A) period 5; group 5A
B) period 5; group 7A
C) period 6; group 5A
D) period 6; group 7A

Question 72

Identify the number of valence electrons for Li.

A) 8
B) 6
C) 4
D) 1
E) 0

Question 73

Which of the following have the same number of valence electrons?

A) Cs, Bi, At
B) Al, Ge, Sb
C) P, As, Sb
D) Xe, Rn, At
E) Fr, Ra, Lr

Question 74

What is the general valence-electron ground-state electron configuration for neutral alkali metals?

A) ns²
B) ns¹
C) (n-1)s²ns¹
D) (n-1)s²ns²np²
E) np⁵

Question 75

Give the number of core electrons for Te.

A) 2
B) 6
C) 46
D) 50
E) 11

Question 76

How many valence electrons does a neutral lanthanide atom have?

A) 4
B) 3
C) 6
D) 64
E) 14

Question 77

Give the number of core electrons for S.

A) 8
B) 12
C) 10
D) 14
E) 16

Question 78

Give the number of valence electrons for Te.

A) 1
B) 7
C) 3
D) 5
E) 6

Question 79

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

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

Question 80

How many valence shell electrons does an atom of thallium have?

A) 1
B) 4
C) 3
D) 81
E) 7