Question 1

The reaction of potassium metal with elemental hydrogen produces ________.

Accepted Answer

A) KH 
B) KH2 
C) K2H 
D) None of the above; potassium will not react directly with hydrogen. 
E) KOH 
A) KH 
B) KH2 
C) K2H 
D) None of the above; potassium will not react directly with hydrogen. 
E) KOH

Question 2

Which of the following correctly represents the second ionization of phosphorus?

Accepted Answer

A) P+ (g) + e- → P2+ (g) 
B) P (g) → P+ (g) + e- 
C) P- (g) + e-  → P2- (g) 
D) P+ (g) → P2+ (g) + e- 
E) P+ (g) + e- → P (g) 
A) P+ (g) + e- → P2+ (g) 
B) P (g) → P+ (g) + e- 
C) P- (g) + e-  → P2- (g) 
D) P+ (g) → P2+ (g) + e- 
E) P+ (g) + e- → P (g)

Question 3

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________.

Accepted Answer

A) Na 
B) Rb 
C) Ca 
D) Be 
E) Fr 
A) Na 
B) Rb 
C) Ca 
D) Be 
E) Fr

Question 4

Which ion below has the largest radius?

Accepted Answer

A) Cl- 
B) K+ 
C) Br- 
D) F- 
E) Na+ 
A) Cl- 
B) K+ 
C) Br- 
D) F- 
E) Na+

Question 5

In nature, sulfur is most commonly found in ________.

Accepted Answer

A) pure elemental sulfur 
B) sulfur oxides 
C) metal sulfides 
D) sulfuric acid 
E) H2S 
A) pure elemental sulfur 
B) sulfur oxides 
C) metal sulfides 
D) sulfuric acid 
E) H2S

Question 6

Consider the following electron configurations to answer the questions that follow:
(i)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P11S1S1P0
(ii)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0
(iii)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P11S1S1P0
(iv)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P14S1S1P0
(v)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P15S1S1P0
-The electron configuration of the atom that is expected to have a positive electron affinity is ________.

Accepted Answer

A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v) 
A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v)

Question 7

An added electron to the element bromine goes into which orbital?

Accepted Answer

The answer of An added electron to the element bromine...

Question 8

Consider the following electron configurations to answer the questions that follow:
(i)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P11S1S1P0
(ii)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0
(iii)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P11S1S1P0
(iv)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P14S1S1P0
(v)1sS1U1P12S1S1P0 2sS1U1P12S1S1P0 2pS1U1P16S1S1P0 3sS1U1P12S1S1P0 3pS1U1P15S1S1P0
-The electron configuration belonging to the atom with the highest second ionization energy is ________.

Accepted Answer

A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v) 
A) (i) 
B) (ii) 
C) (iii) 
D) (iv) 
E) (v)

Question 9

Which element would be expected to have chemical and physical properties closest to those of rubidium?

Accepted Answer

A) Cu 
B) Fe 
C) S 
D) Ca 
E) K 
A) Cu 
B) Fe 
C) S 
D) Ca 
E) K

Question 10

The alkali metal that is naturally radioactive is ________.

Accepted Answer

A) rubidium 
B) cesium 
C) lithium 
D) francium 
E) sodium 
A) rubidium 
B) cesium 
C) lithium 
D) francium 
E) sodium

Question 11

The atomic radius of main-group elements generally increases down a group because ________.

Accepted Answer

A) effective nuclear charge increases down a group 
B) effective nuclear charge decreases down a group 
C) effective nuclear charge zigzags down a group 
D) the principal quantum number of the valence orbitals increases 
E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases 
A) effective nuclear charge increases down a group 
B) effective nuclear charge decreases down a group 
C) effective nuclear charge zigzags down a group 
D) the principal quantum number of the valence orbitals increases 
E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases

Question 12

Of the following oxides, ________ is the most acidic.

Accepted Answer

A) CaO 
B) CO2 
C) Al2O3 
D) Li2O 
E) Na2O 
A) CaO 
B) CO2 
C) Al2O3 
D) Li2O 
E) Na2O

Question 13

Oxides of the active metals combine with acid to form ________.

Accepted Answer

A) hydrogen gas 
B) metal hydrides 
C) water and a salt 
D) oxygen gas 
E) metal hydroxides 
A) hydrogen gas 
B) metal hydrides 
C) water and a salt 
D) oxygen gas 
E) metal hydroxides

Question 14

Which one of the following is a metal?

Accepted Answer

A) Li 
B) S 
C) I 
D) He 
E) Si 
A) Li 
B) S 
C) I 
D) He 
E) Si

Question 15

Of the compounds below, ________ has the smallest ionic separation.

Accepted Answer

A) KF 
B) K2S 
C) RbCl 
D) SrBr2 
E) RbF 
A) KF 
B) K2S 
C) RbCl 
D) SrBr2 
E) RbF

Question 16

Write the balanced equation for the reaction of elemental fluorine with liquid water.

Accepted Answer

2H₂O (l) +

The reaction of potassium metal with elemental hydrogen produces ________.

Which of the following correctly represents the second ionization of phosphorus?

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________.

Which ion below has the largest radius?

In nature, sulfur is most commonly found in ________.

An added electron to the element bromine goes into which orbital?

Which element would be expected to have chemical and physical properties closest to those of rubidium?

The alkali metal that is naturally radioactive is ________.

The atomic radius of main-group elements generally increases down a group because ________.

Of the following oxides, ________ is the most acidic.

Oxides of the active metals combine with acid to form ________.

Which one of the following is a metal?

Of the compounds below, ________ has the smallest ionic separation.

Write the balanced equation for the reaction of elemental fluorine with liquid water.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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Exam 7: Periodic Properties of the Elements

The reaction of potassium metal with elemental hydrogen produces ________.

Which of the following correctly represents the second ionization of phosphorus?

This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ________.

Which ion below has the largest radius?

In nature, sulfur is most commonly found in ________.

An added electron to the element bromine goes into which orbital?

Consider the following electron configurations to answer the questions that follow: (i)1s2 2s2 2p6 3s1 (ii)1s2 2s2 2p6 3s2 (iii)1s2 2s2 2p6 3s2 3p1 (iv)1s2 2s2 2p6 3s2 3p4 (v)1s2 2s2 2p6 3s2 3p5 -The electron configuration belonging to the atom with the highest second ionization energy is ________.

Which element would be expected to have chemical and physical properties closest to those of rubidium?

The alkali metal that is naturally radioactive is ________.

The atomic radius of main-group elements generally increases down a group because ________.

Of the following oxides, ________ is the most acidic.

Oxides of the active metals combine with acid to form ________.

Which one of the following is a metal?

Of the compounds below, ________ has the smallest ionic separation.

Write the balanced equation for the reaction of elemental fluorine with liquid water.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

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