Deck 8: The Structure of Atoms and Periodic Trends

Question 1

Which of the following statements is/are CORRECT for an oxygen atom?
1)The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s electron.
2)The effective nuclear charges felt by 2s and 2p electrons are identical.
3)The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron.

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

Answer 1

3 only

Question 2

What is the maximum number of electrons that can occupy the n = 1 shell?

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

Answer 2

2

Question 3

How many electrons can be described by the quantum numbers n= 3 and l= 1?

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

Answer 3

6

Question 4

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 5

Which of the following electron configurations is not allowed?

A)
B)
C)
D)
E)

Question 6

How many valence electrons does a nitrogen atom have?

A) 5
B) 8
C) 7
D) 3
E) 15

Question 7

Choose the statement that is $\textbf{ true: }$

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 have the lowest ionization energies of all electrons
E) Two of the above are true.

Question 8

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

Question 9

What is the maximum number of electrons that can occupy $\underline{\text{ one }}$ d orbital?

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

Question 10

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

A) tin.
B) krypton.
C) potassium.
D) beryllium.
E) boron.

Question 11

Which of the following orbital occupancy designations is $\underline{\text{ incorrect? }}$

A) 2s²
B) 3s²
C) 1s²
D) 4d³
E) 1s⁶

Question 12

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

Question 13

The maximum number of electrons that can be accommodated in an s subshell is

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

Question 14

According to the building-up principle or aufbau principle,which subshell is typically filled next after the 5p subshell?

A) 6s
B) 5d
C) 3p
D) 6d
E) 5f

Question 15

Which of the following statements concerning ground state electron configurations is/are CORRECT?
1)For a hydrogen atom with one electron,the 2s and 2p orbitals have identical energies.
2)For a lithium atom with three electrons,the 2s and 2p orbitals have different energies.
3)The effective nuclear charge felt by an electron in a 2p orbital is greater for a carbon atom than for a boron atom.

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

Question 16

How many electrons can be described by the following quantum numbers: n = 5, = 0, = 0,m_s = -1/2?

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

Question 17

Which element is found in the p-block of the periodic table?

A) Al
B) Ni
C) Tb
D) Fr
E) none of the above

Question 18

How many electrons can be described by the following quantum numbers: n = 6, = 4, = -4?

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

Question 19

Which of the following statements is true concerning the electron configuration [Ar]4p²?

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

Question 20

Which of the following sets of quantum numbers is allowed?

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

Question 21

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

A)
B)
C)
D)
E)

Question 22

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

A) 1s²2s²2p³
B) 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p¹
C) 1s²2s²2p⁶3s²3p⁶3d²4s²
D) 1s²2s²2p⁶3s²3p⁶4s²
E) 1s²2s²2p⁶3s²3p⁴

Question 23

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 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 24

The complete electron configuration of tin is

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

Question 25

Which atom has the ground state electronic configuration 1s²2s²2p⁶3s²3p⁶4s²3d³?

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

Question 26

Which of the following orbital diagrams represent(s)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 27

Which element has the following ground state electron configuration?

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

Question 28

Which element has the following ground state electron configuration?

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

Question 29

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

A) Sc
B) Mn
C) Co
D) Zn
E) Fe

Question 30

Which ground-state electron configuration is $\underline{\text{ incorrect? }}$

A)
B)
C)
D)
E)

Question 31

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

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

Question 32

Which element has the ground state electron configuration [Ar]3d¹⁰4s¹?

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

Question 33

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

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

Question 34

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

A) .
B) .
C) .
D) .
E) .

Question 35

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

A)
B)
C)
D)
E)

Question 36

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

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

Question 37

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

A) ytterbium (Yb)
B) holmium (Ho)
C) tantalum (Ta)
D) aluminum (Al)
E) germanium (Ge)

Question 38

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 39

Which 1+ ion has the ground state electron configuration [Kr]4d¹⁰?

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

Question 40

Which is the correct valence shell orbital box notation for the ground state electron configuration of Co?
$~~~~~~~~$ 3d $~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$ 4s

A)
B)
C)
D)
E)

Question 41

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

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

Question 42

Which of the following statements is/are CORRECT?
1)For any element,the second ionization energy is larger than the first ionization energy.
2)Ionization energy is a positive value for all elements.
3)Ionization energy increases down a group of the periodic table.

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

Question 43

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

A)
B)
C)
D)
E) none

Question 44

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 45

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 46

Which of the following 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 47

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 48

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

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

Question 49

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 50

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

A)
B)
C)
D)
E)

Question 51

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

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

Question 52

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

A) Se
B) Te
C) S
D) Po
E) O

Question 53

What is the ground state electron configuration for Cr³⁺?

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

Question 54

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

A)
B)
C)
D)
E)

Question 55

The ground-state electron configuration of a .Therefore, Is

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

Question 56

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

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

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

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

A)
B)
C)
D)
E)

Question 59

In general,atomic radii

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

Question 60

Rank the following atoms in order decreasing atomic radii: C,N,B,Al.

A) Al > B > C > N
B) B > Al > C > N
C) C > B > Al > N
D) B > C > N > Al
E) Al > C > B > N

Question 61

Which of the following species would you expect to have the largest radius?

A)
B) P
C)
D)
E)

Question 62

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

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

Question 63

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 64

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 65

According to the general trend in electron affinities,which group (or family)of elements tend 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 66

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

A) SrI
B) SrI₂
C) Sr₂I
D) SrI₃
E) Sr₃I₂

Question 67

Which elements have no affinity for electrons?

A) transition metals
B) s-block elements
C) main group nonmetals
D) noble gases
E) semiconductors

Question 68

Which of the following elements would be expected to have chemical and physical properties most similar to those of the barium (Ba)?

A) magnesium (Mg)
B) argon (Ar)
C) aluminum (Al)
D) tin (Sn)
E) potassium (K)

Question 69

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 70

________ 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 71

A metal nitride forms when sodium reacts with elemental nitrogen.What is the most likely formula of this metal nitride?

A) NaN
B) Na₃N
C) Na₂N₃
D) Na₃N₂
E) NaN₃

Question 72

Rank F,Cl,and Br in order of increasing first ionization energy.

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

Question 73

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 74

The element ________ has the following electron configuration: [Rn]5f¹²7s².

Question 75

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

Question 76

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

Question 77

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

A) Rb
B) As
C) Cl
D) Br
E) Se

Question 78

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

Question 79

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

A) SrO
B) Sr₂O
C) Sr₂O₃
D) SrO₂
E) SrO₃

Question 80

Rank the following ions in order of decreasing ionic radii: Rb^-,Br^-,Te^2-,I^-.

A) I^- > Te^2-> Br^- > Rb^-
B) Te^2- > I^- > Br^- > Rb^-
C) Rb^-> Br^- > Te^2- > I^-
D) I^- > Br^- > Te^2- > Rb^-
E) Br^- > Te^2- > Rb^- > I^-