Question 1

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 the above 
A)  2 
B)  6 
C)  8 
D)  10 
E)  none of the above

Question 2

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 3

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Accepted Answer

A)  Kr. 
B)  Ni. 
C)  Fe. 
D)  Pd. 
E)  none of the above. 
A)  Kr. 
B)  Ni. 
C)  Fe. 
D)  Pd. 
E)  none of the above.

Question 4

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

Accepted Answer

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

Question 5

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

Question 6

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 the above 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 the above statements is generally correct.

Question 7

Which of the following elements has the smallest first ionization energy?

Accepted Answer

A)  Rb 
B)  Mg 
C)  I 
D)  As 
E)  F 
A)  Rb 
B)  Mg 
C)  I 
D)  As 
E)  F

Question 8

Select the element with the least metallic character.

Accepted Answer

A)  Sn 
B)  Sr 
C)  Tl 
D)  Ge 
E)  Ga 
A)  Sn 
B)  Sr 
C)  Tl 
D)  Ge 
E)  Ga

Question 9

Elements with _______________ first ionization energies and ___________ electron affinities generally form anions.

Accepted Answer

A)  low, very negative 
B)  high, positive or slightly negative 
C)  low, positive or slightly negative 
D)  high, very negative 
E)  None of the above is generally correct. 
A)  low, very negative 
B)  high, positive or slightly negative 
C)  low, positive or slightly negative 
D)  high, very negative 
E)  None of the above is generally correct.

Question 10

In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

Accepted Answer

A) True 
 B)False

Question 11

State Hund's rule, and show how it applies to the ground state of phosphorus atoms.

Accepted Answer

Electrons occupy orbitals within the sam

Question 12

Define what is meant by electron affinity, and write a balanced chemical equation to represent the relevant process for element Y.

Accepted Answer

Electron affinity is the energ

Question 13

Select the most basic compound from the following:

Accepted Answer

A)  Bi2O3 
B)  SiO2 
C)  Cs2O 
D)  Na2O 
E)  H2O 
A)  Bi2O3 
B)  SiO2 
C)  Cs2O 
D)  Na2O 
E)  H2O

Question 14

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Accepted Answer

A)  n = 2 l = 1 ml = -1 ms = +   
B)  n = 3 l = 0 ml = 0 ms = -   
C)  n = 3 l = 2 ml = -2 ms = -   
D)  n = 4 l = 0 ml = 0 ms = -   
E)  n = 4 l = 2 ml = 1 ms = +   
A)  n = 2 l = 1 ml = -1 ms = +   
B)  n = 3 l = 0 ml = 0 ms = -   
C)  n = 3 l = 2 ml = -2 ms = -   
D)  n = 4 l = 0 ml = 0 ms = -   
E)  n = 4 l = 2 ml = 1 ms = +

Question 15

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

Accepted Answer

A) True 
 B)False

Question 16

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Accepted Answer

A)  X(g) F1F1F1S1F1F1F10 X+(g) + e- 
B)  X+(g) F1F1F1S1F1F1F10 X+(aq) 
C)  X+(g) + e- F1F1F1S1F1F1F10 X(g) 
D)  X(g) + e- F1F1F1S1F1F1F10 X-(g) 
E)  X+(g) + Y-(g) F1F1F1S1F1F1F10 XY(s) 
A)  X(g) F1F1F1S1F1F1F10 X+(g) + e- 
B)  X+(g) F1F1F1S1F1F1F10 X+(aq) 
C)  X+(g) + e- F1F1F1S1F1F1F10 X(g) 
D)  X(g) + e- F1F1F1S1F1F1F10 X-(g) 
E)  X+(g) + Y-(g) F1F1F1S1F1F1F10 XY(s)

Question 17

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

Question 18

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 the above 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 the above is correct.

Question 19

The most acidic 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

Hund's rule is used to predict the electron configuration of atoms in excited states.

Accepted Answer

A) True 
 B)False

Exam 8: Electron Configuration and Chemical Periodicity

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

Which of the following atoms will be diamagnetic?

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed in the formation of a cation for strontium, Sr.

Which of the following elements has the smallest atomic size?

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?

Which of the following elements has the smallest first ionization energy?

Select the element with the least metallic character.

Elements with _______________ first ionization energies and ___________ electron affinities generally form anions.

In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

State Hund's rule, and show how it applies to the ground state of phosphorus atoms.

Define what is meant by electron affinity, and write a balanced chemical equation to represent the relevant process for element Y.

Select the most basic compound from the following:

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

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

Which one of the following equations correctly represents the process involved in the electron affinity of X?

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

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

The most acidic oxides are formed from elements found in the _________________ region of the periodic table.

Hund's rule is used to predict the electron configuration of atoms in excited states.

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

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

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 first electron removed in the formation of a cation for strontium, Sr.

Elements with _____ first ionization energies and _ electron affinities generally form anions.

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.

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