Question 1

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

Accepted Answer

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) 
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 2

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

Accepted Answer

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

Question 3

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

Accepted Answer

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)  $1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 4 }$ 
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 4

_____ have no affinity for electrons.

Accepted Answer

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

Question 5

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

Accepted Answer

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

Question 6

Explain the difference between paramagnetic and ferromagnetic materials.

Accepted Answer

Elements with unpaired electrons are par

Question 7

Which of the following orbital occupancy designations is incorrect?

Accepted Answer

A)  2s2 
B)  3d6 
C)  1s2 
D)  4p3 
E)  3d12 
A)  2s2 
B)  3d6 
C)  1s2 
D)  4p3 
E)  3d12

Question 8

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

Accepted Answer

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

Question 9

Which element has the following ground state electron configuration?

Accepted Answer

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

Question 10

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

Accepted Answer

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

Question 11

Which of the following species has the largest radius?

Accepted Answer

A)  Cl- 
B)  P 
C)  K- 
D)  Br- 
E)  Ca2+ 
A)  Cl- 
B)  P 
C)  K- 
D)  Br- 
E)  Ca2+

Question 12

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

Accepted Answer

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

Question 13

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

Accepted Answer

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

Question 14

What is the ground state electron configuration for Sn2+?

Accepted Answer

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

Question 15

How many valence electrons does an arsenic atom have?

Accepted Answer

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

Question 16

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

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

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

Accepted Answer

Oxygen has a 1s²2s²2p⁴ electron configurati

Question 19

Which of the following statements is true of atomic radii?

Accepted Answer

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. 
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 20

Which of the following statements is true?

Accepted Answer

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. 
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.

Exam 8: The Structure of Atoms and Periodic Trends

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

Which is the correct valence shell orbital box notation for the ground state electron configuration of Fe? 3d3 d3d4s\quad4 s4s

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

_____ have no affinity for electrons.

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

Explain the difference between paramagnetic and ferromagnetic materials.

Which of the following orbital occupancy designations is incorrect?

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

Which element has the following ground state electron configuration?

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

Which of the following species has the largest radius?

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

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

What is the ground state electron configuration for Sn2+?

How many valence electrons does an arsenic atom have?

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

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

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

Which of the following statements is true of atomic radii?

Which of the following statements is true?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

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

What is the ground state electron configuration for Sn²⁺?

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