Deck 4: Periodic Properties of the Elements

Question 1

When filling degenerate orbitals,electrons fill them singly first,with parallel spins is known as

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

Answer 1

Hund's rule.

Question 2

Which of the following elements is a actinide?

A) Ce
B) Na
C) U
D) Ar
E) Rg

Answer 2

U

Question 3

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.

Answer 3

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.

Question 4

Predict the charge that an ion formed from sodium would have.

A) 1-
B) 6+
C) 3-
D) 1+
E) 2-

Question 5

Which of the following statements is FALSE?

A) Halogens are very reactive elements.
B) The alkali metals are fairly unreactive.
C) Sulfur is a main group element.
D) Noble gases do not usually form ions.
E) Zn is a transition metal.

Question 6

Predict the charge that a calcium ion would have.

A) 6-
B) 2-
C) 3+
D) 2+
E) 1+

Question 7

Which of the following elements is a lanthanide?

A) Ce
B) Na
C) U
D) Ar
E) Rg

Question 8

Only two electrons,with opposing spins,are allowed in each orbital is known as the

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

Question 9

Identify the green-yellowish gas that is used as a disinfecting agent.

A) chlorine
B) bromine
C) iodine
D) fluorine

Question 10

Which of the following elements is NOT a metal?

A) Ba
B) Mg
C) Xe
D) Pb
E) Ga

Question 11

Which of the following does NOT describe a metal?

A) good conductor of heat
B) good conductor of electricity
C) tends to gain electrons
D) forms ionic compounds with nonmetals
E) found on the left side of the periodic table

Question 12

Predict the charge that an aluminum ion would have.

A) 5-
B) 1+
C) 1-
D) 2+
E) 3+

Question 13

Predict the charge that an ion formed from sulfur would have.

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

Question 14

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 15

Semiconductors are

A) metalloids.
B) noble gases.
C) nonmetals.
D) metals.

Question 16

Which of the following statements is FALSE?

A) An anion is usually larger than its corresponding atom.
B) Metals tend to form cations.
C) An atoms is usually larger than its corresponding cation.
D) The halogens tend to form 1+ ions.
E) Nonmetals tend to gain electrons.

Question 17

Which of the following does NOT describe a nonmetal?

A) tend to gain electrons
B) found in the upper right hand corner of the periodic table
C) poor conductor of electricity
D) relatively unreactive
E) poor conductor of heat

Question 18

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

A)
B)
C)
D)
E)

Question 19

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

A)
B)
C)
D)
E)

Question 20

The element that corresponds to the electron configuration 1s²2s²2p⁶3s²3p⁶4s¹3d⁵ is

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

Question 21

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 22

How many valence electrons do the noble gases possess?

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

Question 23

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 24

Give the ground state electron configuration for Se.

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

Question 25

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 26

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 27

Give the number of valence electrons for Cd.

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

Question 28

Give the ground state electron configuration for Cd.

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

Question 29

Give the ground state electron configuration for I.

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

Question 30

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

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

Question 31

How many valence electrons do the halogens possess?

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

Question 32

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 33

How many valence electrons do the alkali metals possess?

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

Question 34

Give the ground state electron configuration for Sr.

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

Question 35

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 36

How many valence electrons does an atom of Al possess?

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

Question 37

How many valence electrons do alkali earth metals possess?

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

Question 38

Give the complete electronic configuration for Mn.

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

Question 39

Give the ground state electron configuration for Pb.

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

Question 40

Give the number of core electrons for Cd.

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

Question 41

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 42

Identify the species that has the smallest radius.

A) N^-5
B) N^-2
C) N⁰
D) N⁺¹
E) N⁺³

Question 43

Choose the ground state electron configuration for Ti²⁺.

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

Question 44

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 45

Give the ground state electron configuration for Mg²⁺.

A) 1s²2s²2p⁶3s²
B) 1s²2s²2p⁶
C) 1s²2s²2p⁶3s²3p²
D) 1s²2s²2p⁶3s²3p⁶
E) 1s²2s²2p⁶3s¹

Question 46

Give the ground state electron configuration for Se²⁻.

A) [Ar]4s²3d¹⁰4p⁴
B) [Ar]4s²3d¹⁰4p²
C) [Ar]4s²4p⁶
D) [Ar]4s²3d¹⁰4p⁶
E) [Ar]4s²3d⁸4p⁶

Question 47

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 48

Give the ground state electron configuration for Rb⁺.

A) [Ar]4s²4p⁶
B) [Kr]5s¹
C) [Ar]4s²3d¹⁰4p⁶
D) [Kr]5s²
E) [Kr]5s²4d²

Question 49

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

A)
B)
C)
D)
E)

Question 50

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

A)
B)
C)
D)
E)

Question 51

Give the ground state electron configuration for Br⁻.

A) [Ar]4s²3d¹⁰4p⁶
B) [Ar]4s²3d¹⁰4p⁵
C) [Ar]4s²4p⁶
D) [Ar]4s²4d¹⁰4p⁶
E) [Ar]4s²3d¹⁰4p⁴

Question 52

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 53

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 54

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 55

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 56

Identify the number of valence electrons in Cl^-.

A) 6
B) 7
C) 8
D) 5
E) 4

Question 57

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 58

For a given atom,identify the species that has the smallest radius.

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

Question 59

Choose the ground state electron configuration for Cr³⁺.

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

Question 60

Choose the ground state electron configuration for Zn²⁺.

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

Question 61

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 62

Describe the reaction of the noble gases with metals.

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

Question 63

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 64

Which element has the highest first ionization energy?

A) Cl
B) S
C) I
D) P
E) Ca

Question 65

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 66

Which species has the highest ionization energy?

A) Mg
B) Mg⁺
C) Mg²⁺
D) Al⁺
E) Al²⁺

Question 67

Which describes the valance electrons of magnesium?

A) 3s⁰
B) 3s¹
C) 3s²
D) 3s²d¹
E) 3s²d²

Question 68

Halogens can react with each other to form

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

Question 69

Give the complete electronic configuration for Br^-.

A) 1s²2s²2p⁶3s²3p⁶4s²4p⁶
B) 1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁶
C) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶
D) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵
E) 1s²2s²p⁶3s²p⁶4s²3d¹⁰4p⁶

Question 70

Give the complete electronic configuration for Ca²⁺.

A) 1s²2s²2p⁶3s²4p⁶
B) 1s²2s²2p⁶3s²3p⁶
C) 1s²2s²2p⁶3s²3p⁵
D) 1s²2s²3p⁶4s²5p⁶
E) 1s²2s²p⁶3s²p⁶

Question 71

The ________ is a change in energy associated with gaining an electron in the gaseous state for an atom or ion.

A) first ionization energy
B) electron affinity
C) binding energy
D) metallic nature
E) shielding

Question 72

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 73

Which ion has the largest radius?

A) Na⁺
B) Ga³⁺
C) K⁺
D) Mg²⁺
E) Ca²⁺

Question 74

Which element would most likely form an ion with a charge of -2?

A) Te
B) I
C) N
D) Na
E) Al

Question 75

According to Hund's Rule

A) electrons pair off first, then fill orbitals.
B) electrons fill orbitals of the same energy singly and pair up only after the orbitals are all half filled.
C) orbitals of the same energy level have the same energy.
D) no two electrons in the same atom can have the same four quantum numbers.
E) electrons found in the same orbital must have the same spin.

Question 76

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

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

Question 77

Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?

A) Electrons in the 2s orbital are shielded by electrons in the 2p.
B) There are more nodes found in the 2s orbital.
C) Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus.
D) The larger number of electrons found in the 2p orbital leads to greater repulsion.
E) The shape of the orbital ultimately determines the energy of the electrons.

Question 78

The Pauli Exclusion Principle states that

A) s orbitals are always lower in energy than p orbitals.
B) electrons spin around the nucleus.
C) you can never know the precise position and energy of an electron.
D) The potential energy of two charges particles depends on their distance.
E) no two electrons in the same atom can have the same four quantum numbers.

Question 79

Which element is diamagnetic?

A) Li
B) F
C) Rb
D) V
E) Zn

Question 80

Identify the alkali metal that is most reactive with water.

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