Question 1

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 2

In the context of magnetism,Cu2+ is _____.

Accepted Answer

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

Question 3

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

Accepted Answer

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

Question 4

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

Accepted Answer

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. 
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 5

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

Accepted Answer

Oxygen has a 1s²2s²2p⁴ electron configurati

Question 6

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 7

Electrons with opposing spins are attracted to each other.

Accepted Answer

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

Question 8

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 9

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 10

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 11

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

Accepted Answer

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) 
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 12

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

Accepted Answer

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

Question 13

Which ground-state electron configuration is incorrect?

Accepted Answer

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

Question 14

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 15

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

Accepted Answer

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

Question 16

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 17

Explain the difference between paramagnetic and ferromagnetic materials.

Accepted Answer

Elements with unpaired electrons are par

Question 18

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

Accepted Answer

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

Question 19

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

Accepted Answer

A)  Al3+ 2+ + + 
B)  Na+ 2+ 3+ + 
C)  K+ 2+ + 3+ 
D)  K+ 3+ 2+ + 
E)  Mg2+ 3+ + + 
A)  Al3+ 2+ + + 
B)  Na+ 2+ 3+ + 
C)  K+ 2+ + 3+ 
D)  K+ 3+ 2+ + 
E)  Mg2+ 3+ + +

Question 20

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

Accepted Answer

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

Exam 8: The Structure of Atoms and Periodic Trends

How many valence electrons does an arsenic atom have?

In the context of magnetism,Cu2+ is _____.

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

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

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

What is the ground state electron configuration for Sn2+?

Electrons with opposing spins are attracted to each other.

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

Which of the following statements is true of atomic radii?

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

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

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

Which ground-state electron configuration is incorrect?

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

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

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

Explain the difference between paramagnetic and ferromagnetic materials.

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

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

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

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

In the context of magnetism,Cu²⁺ is _____.

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

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?

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