Question 1

Elements with the highest first ionization energies are found in the ___________ region of the periodic table.

Accepted Answer

A)  lower left 
B)  upper left 
C)  center 
D)  lower right 
E)  upper right 
A)  lower left 
B)  upper left 
C)  center 
D)  lower right 
E)  upper right

Question 2

Which one of the following equations correctly represents the process relating to the ionization energy of X?

Accepted Answer

A)  X(s) → X+(g) + e- 
B)  X2(g) → X+(g) + X-(g) 
C)  X(g) + e- → X-(g) 
D)  X-(g) → X(g) + e- 
E)  X(g) → X+(g) + e- 
A)  X(s) → X+(g) + e- 
B)  X2(g) → X+(g) + X-(g) 
C)  X(g) + e- → X-(g) 
D)  X-(g) → X(g) + e- 
E)  X(g) → X+(g) + e-

Question 3

In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

Accepted Answer

A)  16 
B)  18 
C)  32 
D)  36 
E)  None of these choices are correct. 
A)  16 
B)  18 
C)  32 
D)  36 
E)  None of these choices are correct.

Question 4

Which of the following atoms will be diamagnetic?

Accepted Answer

A)  Cr 
B)  Ru 
C)  Fe 
D)  Pt 
E)  Cd 
A)  Cr 
B)  Ru 
C)  Fe 
D)  Pt 
E)  Cd

Question 5

Select the correct electron configuration for Cu (Z = 29).

Accepted Answer

A)  [Ar]4s23d9 
B)  [Ar]4s13d10 
C)  [Ar]4s24p63d3 
D)  [Ar]4s24d9 
E)  [Ar]5s24d9 
A)  [Ar]4s23d9 
B)  [Ar]4s13d10 
C)  [Ar]4s24p63d3 
D)  [Ar]4s24d9 
E)  [Ar]5s24d9

Question 6

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of potassium, K.

Accepted Answer

A)  4, 1, -1, ½ 
B)  4, 1, 0, ½ 
C)  4, 0, 1, ½ 
D)  4, 0, 0, ½ 
E)  4, 1, 1, ½ 
A)  4, 1, -1, ½ 
B)  4, 1, 0, ½ 
C)  4, 0, 1, ½ 
D)  4, 0, 0, ½ 
E)  4, 1, 1, ½

Question 7

First ionization energies of neutral atoms may be positive or negative.

Accepted Answer

A) True 
 B)False

Question 8

In the electron configuration [Ar]4s23d104p4, which are valence electrons?

Accepted Answer

A)  all of the electrons after the [Ar] 
B)  only the 4s2 electrons 
C)  only the 3d10 electrons 
D)  only the 4p4 electrons 
E)  both the 4s2 and the 4p4 electrons 
A)  all of the electrons after the [Ar] 
B)  only the 4s2 electrons 
C)  only the 3d10 electrons 
D)  only the 4p4 electrons 
E)  both the 4s2 and the 4p4 electrons

Question 9

Which of the following electron configurations is not possible for an atom in an excited state?

Accepted Answer

A)  1s22s22p63s23p63d104s14p1 
B)  1s22s22p63s13p5 
C)  1s22s22p63s23p23d2 
D)  1s22s22p63s23p63d104s2 
E)  1s22s22p63s23p63d104s14p3 
A)  1s22s22p63s23p63d104s14p1 
B)  1s22s22p63s13p5 
C)  1s22s22p63s23p23d2 
D)  1s22s22p63s23p63d104s2 
E)  1s22s22p63s23p63d104s14p3

Question 10

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of

Accepted Answer

A)  the aufbau principle. 
B)  the Pauli exclusion principle. 
C)  Hund's rule. 
D)  the periodic law. 
E)  Heisenberg's principle. 
A)  the aufbau principle. 
B)  the Pauli exclusion principle. 
C)  Hund's rule. 
D)  the periodic law. 
E)  Heisenberg's principle.

Question 11

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Accepted Answer

A)  Kr. 
B)  Ni. 
C)  Fe. 
D)  Pd. 
E)  None of these choices are correct. 
A)  Kr. 
B)  Ni. 
C)  Fe. 
D)  Pd. 
E)  None of these choices are correct.

Question 12

Select the correct electron configuration for Te (Z = 52).

Accepted Answer

A)  [Kr]5s25p64d8 
B)  [Kr]5s25d105p4 
C)  [Kr]5s24d105p6 
D)  [Kr]5s24f14 
E)  [Kr]5s24d105p4 
A)  [Kr]5s25p64d8 
B)  [Kr]5s25d105p4 
C)  [Kr]5s24d105p6 
D)  [Kr]5s24f14 
E)  [Kr]5s24d105p4

Question 13

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 choices are 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 choices are correct.

Question 14

Electron affinities become increasingly positive toward the right hand end of a period.

Accepted Answer

A) True 
 B)False

Question 15

What is the correct order of decreasing size of the following ions?

Accepted Answer

A)  P3- > Cl- > K+ > Ca2+ 
B)  Ca2+ > K+ > Cl- > P3- 
C)  K+ > Cl- > Ca2+ > P3- 
D)  K+ > Cl- > P3- > Ca2+ 
E)  None of these choices are correct. 
A)  P3- > Cl- > K+ > Ca2+ 
B)  Ca2+ > K+ > Cl- > P3- 
C)  K+ > Cl- > Ca2+ > P3- 
D)  K+ > Cl- > P3- > Ca2+ 
E)  None of these choices are correct.

Question 16

Which of the following electron configurations is correct for the excited state of an element?

Accepted Answer

A)  [He]2s22p5 
B)  [Ne]3s23p1 
C)  [Ar]4s14p1 
D)  [Kr]5s24d7 
E)  [He]1p1 
A)  [He]2s22p5 
B)  [Ne]3s23p1 
C)  [Ar]4s14p1 
D)  [Kr]5s24d7 
E)  [He]1p1

Question 17

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of tin, Sn.

Accepted Answer

A)  5, 2, -1, ½ 
B)  5, 2, 0, ½ 
C)  5, 1, 2, ½ 
D)  5, 1, 0, ½ 
E)  5, 2, 1, ½ 
A)  5, 2, -1, ½ 
B)  5, 2, 0, ½ 
C)  5, 1, 2, ½ 
D)  5, 1, 0, ½ 
E)  5, 2, 1, ½

Question 18

How many valence electrons are there in an atom with the electron configuration [noble gas]ns2(n - 1)d8?

Accepted Answer

A)  2 
B)  6 
C)  8 
D)  10 
E)  None of these choices are correct. 
A)  2 
B)  6 
C)  8 
D)  10 
E)  None of these choices are correct.

Question 19

The most basic oxides are formed from elements found in the __________________ region of the periodic table.

Accepted Answer

A)  upper right 
B)  upper left 
C)  center 
D)  lower right 
E)  lower left 
A)  upper right 
B)  upper left 
C)  center 
D)  lower right 
E)  lower left

Question 20

Which of the following elements has the smallest atomic size?

Accepted Answer

A)  Na 
B)  Ar 
C)  K 
D)  Ca 
E)  Kr 
A)  Na 
B)  Ar 
C)  K 
D)  Ca 
E)  Kr

Exam 8: Electron Configuration and Chemical Periodicity

Elements with the highest first ionization energies are found in the ___________ region of the periodic table.

Which one of the following equations correctly represents the process relating to the ionization energy of X?

In a single atom, what is the maximum number of electrons which can have quantum number n = 4?

Which of the following atoms will be diamagnetic?

Select the correct electron configuration for Cu (Z = 29).

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of potassium, K.

First ionization energies of neutral atoms may be positive or negative.

In the electron configuration [Ar]4s23d104p4, which are valence electrons?

Which of the following electron configurations is not possible for an atom in an excited state?

"Each electron in an atom must have its own unique set of quantum numbers" is a statement of

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Select the correct electron configuration for Te (Z = 52).

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?

Electron affinities become increasingly positive toward the right hand end of a period.

What is the correct order of decreasing size of the following ions?

Which of the following electron configurations is correct for the excited state of an element?

Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of tin, Sn.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns2(n - 1)d8?

The most basic oxides are formed from elements found in the __________________ region of the periodic table.

Which of the following elements has the smallest atomic size?

Keys to Studying Chemistry Definitions, Units, and Problem Solving

The Components of Matter

Stoichiometry of Formulas and Equations

Three Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces Liquids, Solids, and Phase Changes

The Properties of Mixtures Solutions and Colloids

Periodic Patterns in the Main-Group Elements

Organic Compounds and the Atomic Properties of Carbon

Kinetics Rates and Mechanisms of Chemical Reactions

Equilibrium the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics Entropy, Free Energy, and Reaction Direction

Electrochemistry Chemical Change and Electrical Work

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of potassium, K.

In the electron configuration [Ar]4s²3d¹⁰4p⁴, which are valence electrons?

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸ refers to the ground state of

Select the correct set of quantum numbers (n, l, m_l, m_s) for the highest energy electron in the ground state of tin, Sn.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n - 1)d⁸?