Deck 8: The Structure of Atoms and Periodic Trends

Question 1

The procedure by which electrons are assigned to (or built up into) orbitals is known as the ____ principle.

A) Aufbau
B) Bohr
C) Planck
D) Hund
E) Pauli

Answer 1

Aufbau

Question 2

Which of the following statements concerning the Pauli exclusion principle is/are CORRECT?

Question 3

The small, but important, energy differences between 3s, 3p, and 3d electrons is a consequence of

A) the number of electrons they can hold
B) their principal quantum number
C) the Heisenberg uncertainty principle
D) thier effective nuclear charge
E) Hund's rule

Answer 3

thier effective nuclear charge

Question 4

What is the maximum number of electrons that can occupy the n = 3 shell?

A) 2
B) 8
C) 18
D) 32
E) 50

Question 5

How many electrons can be described by the quantum numbers n= 3 and l= 2?

A) 14
B) 6
C) 2
D) 18
E) 10

Question 6

Which of the following statements is true concerning the electron configuration [Xe]6p²?

A) This configuration cannot be the ground-state electron configuration for a Ba atom because it violates the Pauli exclusion principle.
B) This configuration cannot be the ground-state electron configuration for a Ba atom because it violates Hund's rule.
C) This configuration is the ground-state electron configuration for a Ba atom.
D) This configuration cannot be the ground-state electron configuration for a Ba atom because it violates the Heisenberg uncertainty principle.
E) This configuration cannot be the ground-state electron configuration for a Ba atom because it violates the Aufbau principle.

Question 7

What is the maximum number of electrons that can occupy one s orbital?

A) 1
B) 2
C) 6
D) 10
E) 14

Question 8

Which of the following orbital occupancy designations is incorrect?

A) 2s²
B) 3d⁶
C) 1s²
D) 4p³
E) 3d¹²

Question 9

Which of the following statements 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 have the lowest ionization energies of all electrons.
E) Valence electrons in the outermost shell of all elements have the highest ionization energy.

Question 10

Which of the following elements is found in the d-block of the periodic table?

A) Ir
B) Tb
C) Li
D) Cl
E) None of these

Question 11

According to the Aufbau principle, which of the following subshells is typically filled next after the 4s subshell?

A) 3d
B) 4s
C) 3p
D) 2p
E) 2s

Question 12

Which of the following sets of quantum numbers is allowed?

A) n = 2, $\ell$ = 1, $m _ { \ell }$ = +1/2, m_s = -1/2
B) n = 3, $\ell$ = 2, $m _ { \ell }$ = +1, m_s = +1
C) n = 4, $\ell$ = 1, $m _ { \ell }$ = 0, m_s = -1/2
D) n = 4, $\ell$ = 3, $m _ { \ell }$ = -1, m_s = 0
E) n = 5, $\ell$ = 2, $m _ { \ell }$ = +2, m_s = -1

Question 13

An element that has the same ground state valence-shell electron configuration as thallium is

A) gallium.
B) carbon.
C) krypton.
D) cesium.
E) magnesium.

Question 14

How many unpaired electrons are found in the ground state electron configuration of barium (ba)?

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

Question 15

How many electrons can be described by the following quantum numbers: n = 3, $\ell$ = 2, $m _ { \ell }$ = 1?

A) 1
B) 2
C) 6
D) 10
E) 18

Question 16

How many electrons can be described by the following quantum numbers: n = 4, $\ell$ = 2, $m _ { \ell }$ = 2, m_s = -1/2?

A) 1
B) 2
C) 6
D) 10
E) 18

Question 17

Which of the following statements concerning the Pauli exclusion principle is/are CORRECT?
1. If two electrons occupy the same orbital they must have opposite spins.
2. No two electrons in an atom can have the same four quantum numbers.
3. Electrons with opposing spins are attracted to each other.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3

Question 18

How many valence electrons does an arsenic atom have?

A) 5
B) 8
C) 7
D) 2
E) 33

Question 19

Which of the following elements in its 1+ ionic state has the ground state electron configuration [Kr]4d¹⁰?

A) Ru
B) Au
C) Ag
D) In
E) Cd

Question 20

The complete electron configuration of tin is _____.

A) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p²
B) 1s²2s²2p⁶3s²3p⁶4s²4p⁶5s²4d¹⁰5d¹⁰5p²
C) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4d¹⁰4p²
D) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5d¹⁰5p²
E) None of these

Question 21

Which ground-state electron configuration is incorrect?

A) Br: [Ar]3d¹⁰4s²4p⁵
B) K: [Ar]4s¹
C) Ni: [Ar]3d⁵
D) Mg: 1s²2s²2p⁶3s²
E) Co: [Ar]3d⁷4s²

Question 22

Which of the following electron configurations corresponds to the ground state of an atom of a transition element?

A) 1s²2s²2p¹
B) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p³
C) 1s²2s²2p⁶3s²3p⁶3d¹4s²
D) 1s²2s²2p⁶3s²3p⁶4s¹
E) 1s²2s²2p⁶3s²3p⁴

Question 23

Which of the following atoms is diamagnetic in its ground state?

A) mercury (Hg)
B) tin (Sn)
C) rhenium (Re)
D) berkelium (Bk)
E) phosphorus (P)

Question 24

Which of the following orbital diagrams represents a diamagnetic atom? 1s 2s 2p

A)
B)
C)
D)
E)

Question 25

Which atom has the ground state electronic configuration 1s²2s²2p⁶3s²3p⁶4s²3d³?

A) Ga
B) V
C) As
D) Nb
E) none

Question 26

Which element has the following ground state electron configuration?

A) In
B) Y
C) Nb
D) Tl
E) Ga

Question 27

What is the ground-state electron configuration of sulfur (S)?

A) [Ne]3s³3p³
B) [Ar]3s²3p⁴
C) [Ar]3p⁶
D) [Ne]3s²3p⁴
E) [Ar]3p⁶..

Question 28

If the ground state electron configuration of an element is [Ar]3d¹⁰4s²4p⁵, what is the typical charge on the monatomic anion of the element?

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

Question 29

Which of the following orbital diagrams represents a paramagnetic atom? 1s 2s 2p
1) 2. 3.

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

Question 30

For which of the following atoms is the 2+ ion diamagnetic in the ground state?

A) Ni
B) Fe
C) Zn
D) Mn
E) Cu

Question 31

Which of the following elements has the ground state electron configuration [Ar]3d¹⁰4s¹?

A) Cu
B) Zn
C) Ge
D) Ag
E) Cd

Question 32

What is a possible set of quantum numbers for an unpaired electron in the orbital box diagram below?

A) n = 1, $\ell$ = 1, $m _ { \ell }$ = -1, m_s = +1/2
B) n = 4, $\ell$ = 2, $m _ { \ell }$ = -1, m_s = -1/2
C) n = 5, $\ell$ = 2, $m _ { \ell }$ = -2, m_s = +1/2
D) n = 5, $\ell$ = 0, $m _ { \ell }$ = 0, m_s = -1/2
E) n = 5, $\ell$ = 1, $m _ { \ell }$ = -1, m_s = +1/2

Question 33

What noble gas core precedes the valence shell ground state electron configuration for potassium (K)?

A) [Ar]
B) [Rn]
C) [Kr]
D) [Ne]
E) [Xe]

Question 34

Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)

A) has a filled valence shell of electrons.
B) has three electrons per orbital, each with identical spins.
C) has $m _ { \ell }$ values greater than or equal to +1.
D) has the maximum number of unpaired electrons, all with the same spin.
E) has two electrons per orbital, each with opposing spins.

Question 35

Which is the correct valence shell orbital box notation for the ground state electron configuration of Fe?
$3 d$$\quad4 s$

A)
B)
C)
D)
E)

Question 36

Which element has the following ground state electron configuration?

A) Be
B) O
C) Li
D) Si
E) N

Question 37

All of the following ground-state electron configurations are correct except

A) V: [Ar]4s²4d³
B) K: [Ar]4s¹
C) Sb: [Kr]4d¹⁰5s²5p³
D) Cr: [Ar]3d⁵4s¹
E) Te: [Kr]4d¹⁰5s²5p⁴

Question 38

Which element has the following ground state electron configuration? 3d 4s
[Ar]

A) Sc
B) Ni
C) Co
D) Fe
E) V

Question 39

Place the following atoms in order of increasing atomic radii: Se, Sb, Br, and Te.

A) Br < Se < Te < Sb
B) Se < Br < Sb < Te
C) Se < Br < Te < As
D) Sb < Te < Se < Br
E) Te < Sb < Se < Br

Question 40

Which of the following equations corresponds to the second ionization of magnesium?

A) Mg(g) → Mg⁺(g) + e^-..
B) Mg(g) → Mg⁺(g) + e^-.
C) Mg(g) → Mg⁺(g) + e^-
D) Mg(g) → Mg²⁺(g) + 2e^-
E) Mg(g) + e^- → Mg^-(g)

Question 41

The change in energy for which of the following processes corresponds to the first ionization energy of beryllium?

A) Be(g) → Be⁺(g) + e^-
B) Be(s) → Be⁺(s) + e^-
C) Be(s) → Be⁺(g) + e^-
D) Be(g) → Be²⁺(g) + 2e^-
E) Be(s) + e^- → Be^-(s)

Question 42

Which of the following atoms of elements has the largest atomic radius?

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

Question 43

An atom of which of the following elements has the smallest ionization energy?

A) At
B) Bi
C) Pb
D) Cs
E) Po

Question 44

Rank the following atoms in order decreasing atomic radii: Be, Be, Be, B.

A) B > Be > Be > Be
B) Be > B > Be > Be
C) Be > Be > B > Be
D) Be > Be > Be > B
E) B > Be > Be > Be..

Question 45

What 2+ ion has the following ground state electron configuration?

A) Mn²⁺
B) Co²⁺
C) Ni²⁺
D) Cu²⁺
E) Ge²⁺

Question 46

Which of the following ions has the given ground state electron configuration?

A) Cd²⁺
B) Sr²⁺
C) Zn²⁺
D) Sn²⁺
E) None of these

Question 47

Which of the following has the same (total) number of electrons as Ar?

A) Na⁺
B) Ca²⁺
C) Ga³⁺
D) O^2-
E) none

Question 48

What is the ground state electron configuration for Sn²⁺?

A) [Kr]4d¹⁰5s²
B) [Kr]4d¹⁰5p²
C) [Kr]5s²
D) [Kr]4d¹⁰5s²5p²
E) [Kr]4d¹⁰5s²5p⁴

Question 49

Which of the following statements is true of atomic radii?

A) They decrease down a group and remain constant across a period.
B) They decrease down a group and increase across a period.
C) They increase down a group and increase across a period.
D) They increase down a group and remain constant across a period.
E) They increase down a group and decrease across a period.

Question 50

Arrange F, Cl, and Br in order of their increasing first ionization energies.

A) F < Cl < Br
B) Cl < F < Br
C) Cl < Br < F
D) Br < F < Cl
E) Br < Cl < F

Question 51

For which one of the following elements is the second ionization energy over ten times larger than its first ionization energy?

A) B
B) N
C) Li
D) Ne
E) Cu

Question 52

The ground-state electron configuration of a Ni²⁺ ion is 1s²2s²2p⁶3s²3p⁶3d⁸ . Therefore, Ni²⁺ is

A) paramagnetic with two unpaired electrons.
B) diamagnetic.
C) paramagnetic with one unpaired electron.
D) paramagnetic with four unpaired electrons.
E) paramagnetic with five unpaired electrons.

Question 53

What is the ground-state electron configuration of the chloride ion?

A) $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 }$
B) $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 2 }$
C) $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 }$
D) $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 }$
E) $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 4 }$

Question 54

An atom of which of the following elements has the smallest atomic radius?

A) F
B) Rb
C) Ca
D) Ge
E) P

Question 55

What is the ground state electron configuration for Cr³⁺?

A) [Ar]
B) [Ar]3d⁷4s²
C) [Ar]3d¹4s²
D) [Ar]3d²4s¹
E) [Ar]3d³

Question 56

Which of the given ions have the same ground state electron configuration: S^2-, N^3-, Mg²⁺, and Br^-?

A) N^3- and Mg²⁺
B) S^2-, N^3-, and Br^-
C) S^2- and Br^-
D) Mg²⁺ and Br^-
E) S^2-, N^3-, Mg²⁺, and Br^-

Question 57

What 2- ion has the following ground state electron configuration?

A) oxide ion
B) nitride ion
C) fluoride ion
D) sulfide ion
E) magnesium ion

Question 58

Which of the following cations has the same number of unpaired electrons as Fe²⁺?

A) Ni²⁺
B) Fe³⁺
C) Cr²⁺
D) Mn²⁺
E) Co²⁺

Question 59

Electron ________ is defined as the energy change for a process in which a gas phase atom acquires an electron.

Question 60

Explain the difference between paramagnetic and ferromagnetic materials.

Question 61

An atom of which of the following elements has the most negative electron affinity?

A) K
B) Sb
C) Cl
D) Br
E) O

Question 62

_____ have no affinity for electrons.

A) Transition metals
B) s-block elements
C) Main group nonmetals
D) Noble gases
E) Semiconductors

Question 63

Place the following ions in order from smallest to largest ionic radii: K⁺, Na⁺, Mg²⁺, and Al³⁺.

A) Al³⁺ < Mg²⁺ < Na⁺ < K⁺
B) Na⁺ < Mg²⁺ < Al³⁺ < K⁺
C) K⁺ < Mg²⁺ < Na⁺ < Al³⁺
D) K⁺ < Al³⁺ < Mg²⁺ < Na⁺
E) Mg²⁺ < Al³⁺ < Na⁺ < K⁺

Question 64

A metal halide forms when potassium reacts with elemental chlorine. What is the most likely formula of this metal halide?

A) KCl
B) KCl₂
C) K₂Cl
D) KCl₃
E) K3Cl₂

Question 65

Which of the following elements would be expected to have chemical and physical properties most similar to Iodine (I)?

A) Fluorine (F)
B) Aluminum (Al)
C) Magnesium (Mg)
D) Rubidium (Rb)
E) Krypton (Kr)

Question 66

The change in energy for the following reaction is referred to as the ____ for boron. B(g) + e^- → B^-(g)

A) oxidation number
B) electron affinity
C) electronegativity energy
D) first ionization energy
E) second ionization energy

Question 67

The f-block elements are also referred to as the ________ and actinides.

Question 68

________ rule states that the most stable arrangement of electrons is that which contains the maximum number of unpaired electrons, all with the same spin direction.

Question 69

What is the charge formed by alkaline earth metals when they react with nonmetals?

A) +1
B) −1
C) +2
D) −2
E) +3

Question 70

Rank the following ions in order of decreasing ionic radii: Al3+, Mg2+, Al3+, Al3+.

A) Al3+ > Al3+ > Mg2+ > Al3+
B) Al3+ > Al3+ > Mg2+ > Al3+..
C) Al3+> Mg2+ > Al3+ > Al3+
D) Al3+ > Mg2+ > Al3+ > Al3+..
E) Mg2+ > Al3+ > Al3+ > Al3+

Question 71

As one moves horizontally from left to right across a period, the effective ________ charge increases, resulting in decreasing atomic radii.

Question 72

A metal phosphide forms when potassium reacts with elemental phosphorus. What is the most likely formula of this metal phosphide?

A) KP
B) K₃P
C) K₂P₃
D) K₃P₂
E) KP₃

Question 73

The element _____ has the electron configuration [Rn]5f¹²7s².

Question 74

Which of the following species has the largest radius?

A) Cl^-
B) P
C) K^-
D) Br^-
E) Ca²⁺

Question 75

A metal oxide forms when potassium reacts with oxygen. What is the most likely formula of this metal oxide?

A) KO
B) K₂O
C) K₂O₃
D) KO₂
E) KO₃

Question 76

Which group of the periodic table of elements forms only 2+ ions?

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

Question 77

Explain why the first ionization energy for oxygen is lower than that for nitrogen.

Question 78

According to the general trend in electron affinities, which group (or family) of elements tends to form the most stable anions in the gas phase?

A) Noble gases
B) Halogens
C) Transition metals
D) Alkaline earth metals
E) Alkali metals

Question 79

Which of the following groups is a part of the s-block elements?

A) Group 2A
B) Group 6A
C) Group 8A
D) Group 7A
E) Group 5A

Question 80

In the context of magnetism, Cu²⁺ is _____.

A) diamagnetic
B) paramagnetic
C) ferromagnetic
D) ferrimagnetic
E) antiferromagnetic