Question 1

Which of the following elements has the largest second ionization energy (IE2)?

Accepted Answer

A)  Li 
B)  B 
C)  O 
D)  F 
E)  Na 
A)  Li 
B)  B 
C)  O 
D)  F 
E)  Na

Question 2

Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.

Accepted Answer

A) True 
 B)False

Question 3

Describe how the ionization energies of main group elements vary across a period in the periodic table, using a diagram if necessary.

Accepted Answer

Ionization energies generally

Question 4

"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 5

A negative electron affinity implies that the atom repels an approaching electron.

Accepted Answer

A) True 
 B)False

Question 6

Briefly describe how the atomic radii and ionization energies of group 1A(1) elements compare with those of group 8A(18). Also, explain why the values of these properties are so different between these two groups.

Accepted Answer

Group 1A (1) atoms are much la

Question 7

Which one of the following statements about atomic structure and quantum numbers is incorrect?

Accepted Answer

A)  In a given atom, the maximum number of electrons having principal quantum number n = 3, is 18. 
B)  The number of orbitals in a given f subshell is 7. 
C)  For n = 4, the largest possible value of l is 3. 
D)  For n = 4, the largest possible value of ml is 2. 
E)  The following set of quantum numbers for a single orbital is not allowed: n = 3, l = 1, ml = -2. 
A)  In a given atom, the maximum number of electrons having principal quantum number n = 3, is 18. 
B)  The number of orbitals in a given f subshell is 7. 
C)  For n = 4, the largest possible value of l is 3. 
D)  For n = 4, the largest possible value of ml is 2. 
E)  The following set of quantum numbers for a single orbital is not allowed: n = 3, l = 1, ml = -2.

Question 8

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Accepted Answer

A) True 
 B)False

Question 9

Electron affinities of neutral atoms may be positive or negative.

Accepted Answer

A) True 
 B)False

Question 10

Which of the following fourth-period elements has the smallest atomic radius?

Accepted Answer

A)  K 
B)  Ti 
C)  Cu 
D)  Ge 
E)  Kr 
A)  K 
B)  Ti 
C)  Cu 
D)  Ge 
E)  Kr

Question 11

Which of the following elements has the greatest atomic radius?

Accepted Answer

A)  Li 
B)  Ne 
C)  Rb 
D)  Sr 
E)  Xe 
A)  Li 
B)  Ne 
C)  Rb 
D)  Sr 
E)  Xe

Question 12

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 the above 
A)  16 
B)  18 
C)  32 
D)  36 
E)  none of the above

Question 13

Define what is meant by ionization energy, and write a balanced chemical equation to represent the relevant process for element X.

Accepted Answer

Ionization energy is the minim

Question 14

In many-electron atoms, which quantum numbers specify the energy of an electron?

Accepted Answer

A)  n and l 
B)  n and ml 
C)  l and ml 
D)  n and ms 
E)  n, l, and ml 
A)  n and l 
B)  n and ml 
C)  l and ml 
D)  n and ms 
E)  n, l, and ml

Question 15

Bigger atoms generally have smaller ionization energies.

Accepted Answer

A) True 
 B)False

Question 16

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

Accepted Answer

A) True 
 B)False

Question 17

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 18

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471
IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

Accepted Answer

A)  Li 
B)  B 
C)  O 
D)  Ne 
E)  none of the above 
A)  Li 
B)  B 
C)  O 
D)  Ne 
E)  none of the above

Question 19

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Accepted Answer

A)  the first valence electron is removed. 
B)  the second valence electron is removed. 
C)  the eighth electron of is removed. 
D)  the first core electron is removed. 
E)  the last valence electron is removed. 
A)  the first valence electron is removed. 
B)  the second valence electron is removed. 
C)  the eighth electron of is removed. 
D)  the first core electron is removed. 
E)  the last valence electron is removed.

Question 20

Describe how the atomic radii of main group elements vary with position in the periodic table.

Accepted Answer

Among the main group elements,

Exam 8: Electron Configuration and Chemical Periodicity

Which of the following elements has the largest second ionization energy (IE2)?

Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.

Describe how the ionization energies of main group elements vary across a period in the periodic table, using a diagram if necessary.

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

A negative electron affinity implies that the atom repels an approaching electron.

Briefly describe how the atomic radii and ionization energies of group 1A(1) elements compare with those of group 8A(18). Also, explain why the values of these properties are so different between these two groups.

Which one of the following statements about atomic structure and quantum numbers is incorrect?

The difference in energies between the 1s and 2s orbitals is due to the penetration effect.

Electron affinities of neutral atoms may be positive or negative.

Which of the following fourth-period elements has the smallest atomic radius?

Which of the following elements has the greatest atomic radius?

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

Define what is meant by ionization energy, and write a balanced chemical equation to represent the relevant process for element X.

In many-electron atoms, which quantum numbers specify the energy of an electron?

Bigger atoms generally have smaller ionization energies.

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

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

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE1, 1314 IE2, 3389 IE3, 5298 IE4, 7471 IE5, 10992 IE6, 13329 IE7, 71345 IE8, 84087

When comparing the successive ionization energies of an element, an unusually big increase in ionization energy is seen when

Describe how the atomic radii of main group elements vary with position in the periodic table.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The 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: Bonding, Structure, and Reactivity

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 the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Which of the following elements has the largest second ionization energy (IE₂)?

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

Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. IE₁, 1314 IE₂, 3389 IE₃, 5298 IE₄, 7471 IE₅, 10992 IE₆, 13329 IE₇, 71345 IE₈, 84087