Question 1

Which ground-state ion does not have an electron configuration described by the following orbital diagram?

Accepted Answer

A)  V+ 
B)  Cr2+ 
C)  Mn3+ 
D)  Co5+ 
E)  Fe4+ 
A)  V+ 
B)  Cr2+ 
C)  Mn3+ 
D)  Co5+ 
E)  Fe4+

Question 2

How does atomic radius change as you move across the periodic table?

Accepted Answer

A)  Atomic radius decreases moving from left to right across a period and increases from top to bottom. 
B)  Atomic radius increases moving left to right across a period and decreases from top to bottom. 
C)  Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D)  Atomic radius increases diagonally across the periodic table. 
E)  None of the answers is correct. 
A)  Atomic radius decreases moving from left to right across a period and increases from top to bottom. 
B)  Atomic radius increases moving left to right across a period and decreases from top to bottom. 
C)  Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D)  Atomic radius increases diagonally across the periodic table. 
E)  None of the answers is correct.

Question 3

Which species have the most similar atomic radii?

Accepted Answer

A)  S2- and Cl- 
B)  Ar and As 
C)  Rb+ and K+ 
D)  I- and Br - 
E)  Br and Cs 
A)  S2- and Cl- 
B)  Ar and As 
C)  Rb+ and K+ 
D)  I- and Br - 
E)  Br and Cs

Question 4

Which of the species listed below is not isoelectronic with the others?

Accepted Answer

A)  O- 
B)  F- 
C)  Mg2+ 
D)  Na+ 
E)  N3- 
A)  O- 
B)  F- 
C)  Mg2+ 
D)  Na+ 
E)  N3-

Question 5

Explain why the trend in electron affinity increases in general as you move from left to right across a period (row) of the periodic table.

Accepted Answer

The trend in electron affinity is due to

Question 6

How many protons and electrons are present in one Br- ion?

Accepted Answer

A)  35 protons, 35 electrons 
B)  80 protons, 81 electrons 
C)  35 protons, 34 electrons 
D)  35 protons, 36 electrons 
E)  80 protons, 34 electrons 
A)  35 protons, 35 electrons 
B)  80 protons, 81 electrons 
C)  35 protons, 34 electrons 
D)  35 protons, 36 electrons 
E)  80 protons, 34 electrons

Question 7

Which of these elements has the greatest metallic character?

Accepted Answer

A)  Br 
B)  Se 
C)  Ni 
D)  As 
E)  Si 
A)  Br 
B)  Se 
C)  Ni 
D)  As 
E)  Si

Question 8

The electron configuration of a cobalt(III) ion is

Accepted Answer

A)  [Ar]3d5. 
B)  [Ar]4s13d5. 
C)  [Ar]4s23d4. 
D)  [Ar]3d6. 
E)  [Ar]4s23d9. 
A)  [Ar]3d5. 
B)  [Ar]4s13d5. 
C)  [Ar]4s23d4. 
D)  [Ar]3d6. 
E)  [Ar]4s23d9.

Question 9

In what groups are transition metals located?

Accepted Answer

A)  1A, 7A, and 1B 
B)  2A, 4A, and 7A 
C)  1B through 8B 
D)  2B and 3B through 6B 
E)  3A through 6A 
A)  1A, 7A, and 1B 
B)  2A, 4A, and 7A 
C)  1B through 8B 
D)  2B and 3B through 6B 
E)  3A through 6A

Question 10

Which element in Group 6A has the highest electron affinity?

Accepted Answer

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

Question 11

Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

Accepted Answer

A)  A2- > B- > C > D+ > E2+ 
B)  E2+ > D+ > C > B- > A2- 
C)  A2- > B- > C + 2+  
D)  A2- -  D+ > E2+ 
E)  None of these relative radii statements is correct. 
A)  A2- > B- > C > D+ > E2+ 
B)  E2+ > D+ > C > B- > A2- 
C)  A2- > B- > C + 2+  
D)  A2- -  D+ > E2+ 
E)  None of these relative radii statements is correct.

Question 12

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

Accepted Answer

A)  X has a larger electron affinity than Y does. 
B)  X has a larger effective nuclear charge than Y does. 
C)  X has greater metallic character than Y does. 
D)  X has a larger first ionization energy than Y does. 
E)  X is a poorer conductor of electricity than Y when in the solid state. 
A)  X has a larger electron affinity than Y does. 
B)  X has a larger effective nuclear charge than Y does. 
C)  X has greater metallic character than Y does. 
D)  X has a larger first ionization energy than Y does. 
E)  X is a poorer conductor of electricity than Y when in the solid state.

Question 13

The energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Accepted Answer

A)  Larger nuclear charge lowers energy; more electrons in an orbital lowers energy. 
B)  Larger nuclear charge lowers energy; more electrons in an orbital increases energy. 
C)  Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D)  Smaller nuclear charge lowers energy; more electrons in an orbital increases energy. 
E)  None of these statements is generally correct. 
A)  Larger nuclear charge lowers energy; more electrons in an orbital lowers energy. 
B)  Larger nuclear charge lowers energy; more electrons in an orbital increases energy. 
C)  Smaller nuclear charge lowers energy; more electrons in an orbital lowers energy. 
D)  Smaller nuclear charge lowers energy; more electrons in an orbital increases energy. 
E)  None of these statements is generally correct.

Question 14

Select the element with the greatest metallic character.

Accepted Answer

A)  Li 
B)  Ca 
C)  Al 
D)  Pb 
E)  Cs 
A)  Li 
B)  Ca 
C)  Al 
D)  Pb 
E)  Cs

Question 15

What is the definition of electron affinity?

Accepted Answer

The energy released (the negat

Question 16

In 1864, the English chemist John Newlands noticed that when the elements were arranged in order of increasing atomic mass, every eighth element had similar properties. Newlands referred to this relationship as the

Accepted Answer

A)  law of periodicity. 
B)  law of loopholes. 
C)  law of octaves. 
D)  law of orbitals. 
E)  law of proportionality. 
A)  law of periodicity. 
B)  law of loopholes. 
C)  law of octaves. 
D)  law of orbitals. 
E)  law of proportionality.

Question 17

What is the definition of nuclear charge, labeled Z?

Accepted Answer

The number

Question 18

Who noticed that the periodic table was arranged in order of atomic mass, where every eighth element had similar properties, and called this the law of octaves?

Accepted Answer

A)  Meyer 
B)  Newlands 
C)  Moseley 
D)  Mendeleev 
E)  Thomson 
A)  Meyer 
B)  Newlands 
C)  Moseley 
D)  Mendeleev 
E)  Thomson

Question 19

How many total electrons are present in chloride ion?

Accepted Answer

A)  16 
B)  17 
C)  18 
D)  19 
E)  21 
A)  16 
B)  17 
C)  18 
D)  19 
E)  21

Question 20

A sulfide ion, S2-, has

Accepted Answer

A)  16 protons and 16 electrons. 
B)  32 protons and 16 electrons. 
C)  16 protons and 14 electrons. 
D)  16 protons and 18 electrons. 
E)  32 protons and 18 electrons. 
A)  16 protons and 16 electrons. 
B)  32 protons and 16 electrons. 
C)  16 protons and 14 electrons. 
D)  16 protons and 18 electrons. 
E)  32 protons and 18 electrons.

Exam 7: Electron Configuration and the Periodic Table

Which ground-state ion does not have an electron configuration described by the following orbital diagram?

How does atomic radius change as you move across the periodic table?

Which species have the most similar atomic radii?

Which of the species listed below is not isoelectronic with the others?

Explain why the trend in electron affinity increases in general as you move from left to right across a period (row) of the periodic table.

How many protons and electrons are present in one Br- ion?

Which of these elements has the greatest metallic character?

The electron configuration of a cobalt(III) ion is

In what groups are transition metals located?

Which element in Group 6A has the highest electron affinity?

Consider the set of isoelectronic atoms and ions A2-, B-, C, D+, and E2+. Which arrangement of relative radii is correct?

If the radius of atom X is greater than the radius of atom Y, then it is also likely that

The energy states of atoms containing more than one electron arise from nucleus-electron and electron-electron interactions. Which of the following statements correctly describes these effects?

Select the element with the greatest metallic character.

What is the definition of electron affinity?

In 1864, the English chemist John Newlands noticed that when the elements were arranged in order of increasing atomic mass, every eighth element had similar properties. Newlands referred to this relationship as the

What is the definition of nuclear charge, labeled Z?

Who noticed that the periodic table was arranged in order of atomic mass, where every eighth element had similar properties, and called this the law of octaves?

How many total electrons are present in chloride ion?

A sulfide ion, S2-, has

Chemistry: the Central Science

Atoms, Molecules, and Ions

Stoichiometry: Ratios of Combination

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

How many protons and electrons are present in one Br^- ion?

Consider the set of isoelectronic atoms and ions A^2-, B^-, C, D⁺, and E²⁺. Which arrangement of relative radii is correct?

A sulfide ion, S^2-, has