Question 1

Which of the following has the largest radius?

Accepted Answer

A)  As3- 
B)  Br 
C)  Sr2+ 
D)  Cl- 
E)  Se2- 
A)  As3- 
B)  Br 
C)  Sr2+ 
D)  Cl- 
E)  Se2-

Question 2

Which of the following occurs for the representative elements going left to right across the period?

Accepted Answer

A)  Electronegativity decreases. 
B)  Atomic size increases. 
C)  Forces of attraction between electron and nucleus increase because nuclear charge increases. 
D)  The outer electrons are held more weakly. 
E)  none of these 
A)  Electronegativity decreases. 
B)  Atomic size increases. 
C)  Forces of attraction between electron and nucleus increase because nuclear charge increases. 
D)  The outer electrons are held more weakly. 
E)  none of these

Question 3

Which of the following species is most likely to be diamagnetic?

Accepted Answer

A)  Fe 
B)  I 
C)  Mn+ 
D)  W3+ 
E)  Zn2+ 
A)  Fe 
B)  I 
C)  Mn+ 
D)  W3+ 
E)  Zn2+

Question 4

The first ionization energy for rubidium is +403.0 kJ/mol. How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

Accepted Answer

A)  185 kJ 
B)  80.6 kJ 
C)  68.9 kJ 
D)  40.4 kJ 
E)  34.5 kJ 
A)  185 kJ 
B)  80.6 kJ 
C)  68.9 kJ 
D)  40.4 kJ 
E)  34.5 kJ

Question 5

List in order of increasing ionization potential: O, Mg, Rb, S, Si.

Accepted Answer

A)  Si < O < Mg < Rb < S 
B)  Si < S < Rb < Mg < O 
C)  Mg < O < Rb < S < Si 
D)  Rb < Mg < Si < S < O 
E)  S < Si < Mg < O < Rb 
A)  Si < O < Mg < Rb < S 
B)  Si < S < Rb < Mg < O 
C)  Mg < O < Rb < S < Si 
D)  Rb < Mg < Si < S < O 
E)  S < Si < Mg < O < Rb

Question 6

Which of the following elements form amphoteric oxides?

Accepted Answer

A)  Sn 
B)  Mg 
C)  P 
D)  B 
E)  Na 
A)  Sn 
B)  Mg 
C)  P 
D)  B 
E)  Na

Question 7

Which ground state electronic configuration will most readily produce an ion with a charge of 2+?

Accepted Answer

A)  1s22s22p63s23p63d104s2 
B)  1s22s22p63s23p64s1 
C)  1s22s22p63s23p4 
D)  1s22s22p63s23p63d104s24p2 
E)  1s2s22p63s23p63d104s24p6 
A)  1s22s22p63s23p63d104s2 
B)  1s22s22p63s23p64s1 
C)  1s22s22p63s23p4 
D)  1s22s22p63s23p63d104s24p2 
E)  1s2s22p63s23p63d104s24p6

Question 8

Which of the following pairs of elements are classified as metalloids?

Accepted Answer

A)  aluminum and silicon 
B)  argon and neon 
C)  arsenic and germanium 
D)  bromine and sulfur 
E)  copper and silver 
A)  aluminum and silicon 
B)  argon and neon 
C)  arsenic and germanium 
D)  bromine and sulfur 
E)  copper and silver

Question 9

The electron affinity is the energy for an atom in its standard state to gain an electron.

Accepted Answer

A) True 
 B)False

Question 10

Complete 2 Na(s) + 2 H2O →

Accepted Answer

A)  2 NaH(s) + 2 OH- 
B)  2 H2O(l) + 2 Na(s) 
C)  O2(g) + 2NaH2 
D)  2 Na+ + 2 OH- + H2(g) 
E)  2 NaH(s) + O2(g) + H2(g) 
A)  2 NaH(s) + 2 OH- 
B)  2 H2O(l) + 2 Na(s) 
C)  O2(g) + 2NaH2 
D)  2 Na+ + 2 OH- + H2(g) 
E)  2 NaH(s) + O2(g) + H2(g)

Question 11

The effective nuclear charge for sodium is:

Accepted Answer

A)  10 
B)  9 
C)  1 
D)  0 
E)  0 
A)  10 
B)  9 
C)  1 
D)  0 
E)  0

Question 12

Which statement best describes relationships in a modern periodic table?

Accepted Answer

A)  Each transition element is placed in the column of the main group element that it most closely resembles. 
B)  The fourteen elements in the "lanthanide" series form a new independent period. 
C)  Metalloids usually are the cations in ionic compounds. 
D)  Nonmetallic properties tend to predominate for elements at the far right portion of the table. 
E)  Elements are always arranged in order of increasing atomic weights. 
A)  Each transition element is placed in the column of the main group element that it most closely resembles. 
B)  The fourteen elements in the "lanthanide" series form a new independent period. 
C)  Metalloids usually are the cations in ionic compounds. 
D)  Nonmetallic properties tend to predominate for elements at the far right portion of the table. 
E)  Elements are always arranged in order of increasing atomic weights.

Question 13

The ionization energy is the energy for a gaseous atom to lose an electron.

Accepted Answer

A) True 
 B)False

Question 14

Why is the electron affinity so positive for the group 2 elements?

Accepted Answer

A)  The added electron would have to go into a new shell. 
B)  The added electron would have to be added into the half-filled p subshell. 
C)  The added electron would have to be added into the p subshell. 
D)  The groups 2 elements are diatomic elements. 
E)  Electrons can't be added to gases. 
A)  The added electron would have to go into a new shell. 
B)  The added electron would have to be added into the half-filled p subshell. 
C)  The added electron would have to be added into the p subshell. 
D)  The groups 2 elements are diatomic elements. 
E)  Electrons can't be added to gases.

Question 15

How much energy, in joules, must be absorbed to convert to Na+ all the atoms present in 1.00 mg of gaseous Na? The first ionization energy of Na is 495.8 kJ/mol.

Accepted Answer

A)  21.6 J 
B)  0.0464 J 
C)  46.4 J 
D)  0.0216 J 
E)  1.14 × 104 J 
A)  21.6 J 
B)  0.0464 J 
C)  46.4 J 
D)  0.0216 J 
E)  1.14 × 104 J

Question 16

Which of the following elements is likely to have the largest second ionization energy?

Accepted Answer

A)  Na 
B)  Mg 
C)  Al 
D)  Si 
A)  Na 
B)  Mg 
C)  Al 
D)  Si

Question 17

The first ionization potential for S is lower than the first ionization potential for P because:

Accepted Answer

A)  Hund's rule is violated 
B)  P has a p3 configuration 
C)  ionization potentials decrease across a representative period 
D)  P is to the right of S on the periodic table 
E)  P is below S on the periodic table 
A)  Hund's rule is violated 
B)  P has a p3 configuration 
C)  ionization potentials decrease across a representative period 
D)  P is to the right of S on the periodic table 
E)  P is below S on the periodic table

Question 18

Which of the following has the highest first ionization potential: Sb, I, In, Xe, Rb?

Accepted Answer

A)  Sb 
B)  I 
C)  In 
D)  Xe 
E)  Rb 
A)  Sb 
B)  I 
C)  In 
D)  Xe 
E)  Rb

Question 19

Complete Br2 + Cl- →

Accepted Answer

A)  BrCl + Br- 
B)  Br- + Cl2 
C)  Br2Cl- 
D)  Br3- 
E)  no reaction 
A)  BrCl + Br- 
B)  Br- + Cl2 
C)  Br2Cl- 
D)  Br3- 
E)  no reaction

Question 20

Elements in the first two groups are part of the main-group elements along with which of the following groups?

Accepted Answer

A)  d-block elements 
B)  s-block elements 
C)  actinides 
D)  lanthanides 
E)  p-block elements 
A)  d-block elements 
B)  s-block elements 
C)  actinides 
D)  lanthanides 
E)  p-block elements

Exam 9: The Periodic Table and Some Atomic Properties

Which of the following has the largest radius?

Which of the following occurs for the representative elements going left to right across the period?

Which of the following species is most likely to be diamagnetic?

The first ionization energy for rubidium is +403.0 kJ/mol. How much energy would be required to convert 17.1 g of gaseous rubidium to its gaseous +1 monatomic ion at constant temperature?

List in order of increasing ionization potential: O, Mg, Rb, S, Si.

Which of the following elements form amphoteric oxides?

Which ground state electronic configuration will most readily produce an ion with a charge of 2+?

Which of the following pairs of elements are classified as metalloids?

The electron affinity is the energy for an atom in its standard state to gain an electron.

Complete 2 Na(s) + 2 H2O →

The effective nuclear charge for sodium is:

Which statement best describes relationships in a modern periodic table?

The ionization energy is the energy for a gaseous atom to lose an electron.

Why is the electron affinity so positive for the group 2 elements?

How much energy, in joules, must be absorbed to convert to Na+ all the atoms present in 1.00 mg of gaseous Na? The first ionization energy of Na is 495.8 kJ/mol.

Which of the following elements is likely to have the largest second ionization energy?

The first ionization potential for S is lower than the first ionization potential for P because:

Which of the following has the highest first ionization potential: Sb, I, In, Xe, Rb?

Complete Br2 + Cl- →

Elements in the first two groups are part of the main-group elements along with which of the following groups?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

Filters

Complete 2 Na(s) + 2 H₂O →

Complete Br₂ + Cl- →