Question 1

What are the products of the following reaction
H2(g) + Cl2(g) $\rarr$

Accepted Answer

A)  H2O(l) + 2HCl(g) 
B)  H2(g) + Cl2(g) 
C)  H2Cl(g) + Cl-(aq) 
D)  2HCl(g) 
E)  HCl2(g) + H+(aq) 
A)  H2O(l) + 2HCl(g) 
B)  H2(g) + Cl2(g) 
C)  H2Cl(g) + Cl-(aq) 
D)  2HCl(g) 
E)  HCl2(g) + H+(aq)

Question 2

Which one of the following does not have [Xe] as its electronic configuration

Accepted Answer

A)  Te2- 
B)  I- 
C)  Cs+ 
D)  Ba2+ 
E)  Sn4+ 
A)  Te2- 
B)  I- 
C)  Cs+ 
D)  Ba2+ 
E)  Sn4+

Question 3

Which of the following elements has the greatest metallic character

Accepted Answer

A)  Ca 
B)  Mg 
C)  Ba 
D)  As 
E)  Se 
A)  Ca 
B)  Mg 
C)  Ba 
D)  As 
E)  Se

Question 4

Which pair of elements from different groups resemble each other the most in their chemical properties

Accepted Answer

A)  Be and B 
B)  Al and Si 
C)  Li and Be 
D)  Al and Be 
E)  Be and C 
A)  Be and B 
B)  Al and Si 
C)  Li and Be 
D)  Al and Be 
E)  Be and C

Question 5

The electron configuration of the outermost electrons of atoms of the halogen group is ns2np7.

Accepted Answer

A) True 
 B)False

Question 6

Which of the atoms listed below has the largest radius

Accepted Answer

A)  Cl 
B)  I 
C)  P 
D)  Sb 
E)  Se 
A)  Cl 
B)  I 
C)  P 
D)  Sb 
E)  Se

Question 7

Which of the following is the general electron configuration for the outermost electrons of elements in the alkaline earth group

Accepted Answer

A)  ns1 
B)  ns2 
C)  ns2np4 
D)  ns2np5 
E)  ns2np6(n -1)d6 
A)  ns1 
B)  ns2 
C)  ns2np4 
D)  ns2np5 
E)  ns2np6(n -1)d6

Question 8

Electron affinity is always a positive quantity.

Accepted Answer

A) True 
 B)False

Question 9

Consider the element with the electron configuration [Kr]5s24d7. This element is

Accepted Answer

A)  a representative element. 
B)  a transition metal. 
C)  a nonmetal. 
D)  an actinide element. 
E)  a noble gas. 
A)  a representative element. 
B)  a transition metal. 
C)  a nonmetal. 
D)  an actinide element. 
E)  a noble gas.

Question 10

Which of the following elements has the greatest metallic character

Accepted Answer

A)  Br 
B)  F 
C)  Ge 
D)  Mn 
E)  Sc 
A)  Br 
B)  F 
C)  Ge 
D)  Mn 
E)  Sc

Question 11

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) $\rarr$Hg+(g) + e- is therefore

Accepted Answer

A)  1006 kJ/mol. 
B)  greater than 1006 kJ/mol. 
C)  less than 1006 kJ/mol. 
D)  is equal to the electron affinity of mercury. 
E)  is equal to the second ionization energy of mercury. 
A)  1006 kJ/mol. 
B)  greater than 1006 kJ/mol. 
C)  less than 1006 kJ/mol. 
D)  is equal to the electron affinity of mercury. 
E)  is equal to the second ionization energy of mercury.

Question 12

Which, if any, is the ground-state electron configuration for K+

Accepted Answer

A)  [Ar] or 1s22s22p63s23p6 
B)  1s22s22p63s23p5 
C)  1s22s22p63s23p64s2 
D)  [Ar] or 1s22s22p63s23p4 
E)  None of the above 
A)  [Ar] or 1s22s22p63s23p6 
B)  1s22s22p63s23p5 
C)  1s22s22p63s23p64s2 
D)  [Ar] or 1s22s22p63s23p4 
E)  None of the above

Question 13

Concerning the electron configuration of S2-, 1s22s22p63s23p6, which, if any, is the configuration for the valence shell electrons only

Accepted Answer

A)  1s22s22p63s23p6 
B)  2s22p63s23p6 
C)  1s22s22p6 
D)  3s23p6 
E)  None of the above 
A)  1s22s22p63s23p6 
B)  2s22p63s23p6 
C)  1s22s22p6 
D)  3s23p6 
E)  None of the above

Question 14

Which of the following is the electron configuration for the aluminum ion

Accepted Answer

A)  1s22s22p63s2 
B)  1s22s22p63s23p2 
C)  1s22s22p63s23p1 
D)  1s22s22p6 
E)  1s22s22p63s23p4 
A)  1s22s22p63s2 
B)  1s22s22p63s23p2 
C)  1s22s22p63s23p1 
D)  1s22s22p6 
E)  1s22s22p63s23p4

Question 15

How many electrons are in the 4p subshell of vanadium

Accepted Answer

A)  0 
B)  2 
C)  4 
D)  5 
E)  6 
A)  0 
B)  2 
C)  4 
D)  5 
E)  6

Question 16

For Mg atoms a very large jump in the magnitudes of the ionization energies will occur between the second and the third ionization energies.

Accepted Answer

A) True 
 B)False

Question 17

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Accepted Answer

A)  nuclear binding energy. 
B)  number of neutrons. 
C)  atomic mass. 
D)  atomic number. 
E)  atomic size. 
A)  nuclear binding energy. 
B)  number of neutrons. 
C)  atomic mass. 
D)  atomic number. 
E)  atomic size.

Question 18

Which of the following make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+

Accepted Answer

A)  Ca2+ and Fe3+ 
B)  O2- and F 
C)  F and Cl- 
D)  Cl- and Ca2+ 
E)  None of the above. 
A)  Ca2+ and Fe3+ 
B)  O2- and F 
C)  F and Cl- 
D)  Cl- and Ca2+ 
E)  None of the above.

Question 19

The successive ionization energies of a certain element are I1= 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900 kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

Accepted Answer

A)  K 
B)  Si 
C)  As 
D)  Ca 
E)  S 
A)  K 
B)  Si 
C)  As 
D)  Ca 
E)  S

Question 20

Which one of the following is not isoelectronic with Kr

Accepted Answer

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

Exam 8: Periodic Relationships Among the Elements

What are the products of the following reaction H2(g) + Cl2(g) →\rarr→

Which one of the following does not have [Xe] as its electronic configuration

Which of the following elements has the greatest metallic character

Which pair of elements from different groups resemble each other the most in their chemical properties

The electron configuration of the outermost electrons of atoms of the halogen group is ns2np7.

Which of the atoms listed below has the largest radius

Which of the following is the general electron configuration for the outermost electrons of elements in the alkaline earth group

Electron affinity is always a positive quantity.

Consider the element with the electron configuration [Kr]5s24d7. This element is

Which of the following elements has the greatest metallic character

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) →\rarr→ Hg+(g) + e- is therefore

Which, if any, is the ground-state electron configuration for K+

Concerning the electron configuration of S2-, 1s22s22p63s23p6, which, if any, is the configuration for the valence shell electrons only

Which of the following is the electron configuration for the aluminum ion

How many electrons are in the 4p subshell of vanadium

For Mg atoms a very large jump in the magnitudes of the ionization energies will occur between the second and the third ionization energies.

As opposed to early periodic tables based on the law of octaves, modern periodic tables arrange the elements in order of increasing

Which of the following make an isoelectronic pair: Cl-, O2-, F, Ca2+, Fe3+

The successive ionization energies of a certain element are I1= 589.5 kJ/mol, I2 =1145 kJ/mol, I3= 4900 kJ/mol, I4 = 6500 kJ/mol, and I5 = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is

Which one of the following is not isoelectronic with Kr

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

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Quantum Theory and the Electronic Structure of Atoms

Chemical Bonding I: Basic Concepts

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Acid-Base Equilibria and Solubility Equilibria

Entropy Free Energy and Equilibrium

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Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

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Filters

What are the products of the following reaction H₂(g) + Cl₂(g) $\rarr$

The electron configuration of the outermost electrons of atoms of the halogen group is ns²np⁷.

Consider the element with the electron configuration [Kr]5s²4d⁷. This element is

The first ionization energy of mercury is 1006 kJ/mol. The energy change for the reaction Hg(l) $\rarr$ Hg⁺(g) + e^- is therefore

Which, if any, is the ground-state electron configuration for K⁺

Concerning the electron configuration of S^2-, 1s²2s²2p⁶3s²3p⁶, which, if any, is the configuration for the valence shell electrons only

Which of the following make an isoelectronic pair: Cl^-, O^2-, F, Ca²⁺, Fe³⁺

The successive ionization energies of a certain element are I₁= 589.5 kJ/mol, I₂ =1145 kJ/mol, I₃= 4900 kJ/mol, I₄ = 6500 kJ/mol, and I₅ = 8100 kJ/mol. This pattern of ionization energies suggests that the unknown element is