Question 1

In the following reaction: 2 Mn+2 + Br2 $\rightarrow$ 2 Mn+3 + 2 Br- the species that is oxidized is ________.

Accepted Answer

A)  Mn2+ 
B)  Br- 
C)  Mn+3 
D)  Br2 
A)  Mn2+ 
B)  Br- 
C)  Mn+3 
D)  Br2

Question 2

Which of the following equations is incorrectly classified as to type of chemical reaction?

Accepted Answer

A)  NaHCO3 + HCl $\rightarrow$ NaCl + H2O + CO2 double-replacement/nonredox 
B)  2 Na + H2 $\rightarrow$2 NaH synthesis/redox 
C)  PbO + C$\rightarrow$ Pb + CO single-replacement/nonredox 
D)  2 Na + 2 HCl $\rightarrow$ 2 NaCl + H2 single-replacement/redox 
A)  NaHCO3 + HCl $\rightarrow$ NaCl + H2O + CO2 double-replacement/nonredox 
B)  2 Na + H2 $\rightarrow$2 NaH synthesis/redox 
C)  PbO + C$\rightarrow$ Pb + CO single-replacement/nonredox 
D)  2 Na + 2 HCl $\rightarrow$ 2 NaCl + H2 single-replacement/redox

Question 3

In the disproportion equation below, what species is undergoing disproportionation?
3 Br2 + 6 OH- $\rightarrow$BrO3- + 5 Br- + 3 H2O

Accepted Answer

A)  OH- 
B)  Br- 
C)  H2O 
D)  Br2 
A)  OH- 
B)  Br- 
C)  H2O 
D)  Br2

Question 4

In a redox reaction, the substance reduced ________.

Accepted Answer

A)  contains an element which increases in oxidation number 
B)  is also the reducing agent 
C)  always gains electrons 
D)  always loses electrons 
A)  contains an element which increases in oxidation number 
B)  is also the reducing agent 
C)  always gains electrons 
D)  always loses electrons

Question 5

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word
-Ag+(aq) + Cl-(aq) $\rightarrow$AgCl(s) ____________________

Accepted Answer

A)  non-redox 
B)  redox 
A)  non-redox 
B)  redox

Question 6

The anode in a galvanic or electrolysis cell is ________.

Accepted Answer

A)  the compartment where solution is placed 
B)  the electrode where electrons leave the cell 
C)  the electrode where reduction takes place 
D)  always the oxidizing agent for the reaction 
A)  the compartment where solution is placed 
B)  the electrode where electrons leave the cell 
C)  the electrode where reduction takes place 
D)  always the oxidizing agent for the reaction

Question 7

The balanced full-equation obtained by adding the following two balanced half-reactions is ________.
2H2O + PH3 $\rightarrow$H3PO2 + 4H+ + 4e-
I2 + 2e- $\rightarrow$2I-

Accepted Answer

A)  2 H2O + PH3 + I2 $\rightarrow$ H3PO2 + 4 H+ + 2 I- + 2 e- 
B)  4 H2O + 2 PH3 + I2 $\rightarrow$ 2 H3PO2 + 8 H+ + 2 I- 
C)  2 H2O + PH3 + 2 I2 $\rightarrow$ H3PO2 + 8 I- + 8 H+ 
D)  2 H2O + PH3 + 2 I2 $\rightarrow$ H3PO2 + 4 I- + 4 H+ 
A)  2 H2O + PH3 + I2 $\rightarrow$ H3PO2 + 4 H+ + 2 I- + 2 e- 
B)  4 H2O + 2 PH3 + I2 $\rightarrow$ 2 H3PO2 + 8 H+ + 2 I- 
C)  2 H2O + PH3 + 2 I2 $\rightarrow$ H3PO2 + 8 I- + 8 H+ 
D)  2 H2O + PH3 + 2 I2 $\rightarrow$ H3PO2 + 4 I- + 4 H+

Question 8

Which substance is serving as the oxidizing agent in the following reaction?
14H+ + Cr2O7-2 + 3 Ni $\rightarrow$ 3 Ni2+ + 2 Cr+3 + 7 H2O

Accepted Answer

A)  Ni 
B)  H+ 
C)  Cr2O7-2 
D)  H2O 
A)  Ni 
B)  H+ 
C)  Cr2O7-2 
D)  H2O

Question 9

What is the cathode material in a common dry cell such as a flashlight battery?

Accepted Answer

A)  lead 
B)  graphite 
C)  zinc 
D)  magnesium 
A)  lead 
B)  graphite 
C)  zinc 
D)  magnesium

Question 10

In the redox reaction: 2 HNO2 + 2 HI $\rightarrow$ 2 NO + I2 + 2 H2O, ________.

Accepted Answer

A)  HNO2 is the oxidizing agent. 
B)  HNO2 is the substance oxidized. 
C)  I undergoes an oxidation number increase of 2 units per atom. 
D)  N undergoes an oxidation number increase of 2 units per atom. 
A)  HNO2 is the oxidizing agent. 
B)  HNO2 is the substance oxidized. 
C)  I undergoes an oxidation number increase of 2 units per atom. 
D)  N undergoes an oxidation number increase of 2 units per atom.

In the following reaction: 2 Mn⁺² + Br₂ $\rightarrow$ 2 Mn⁺³ + 2 Br^- the species that is oxidized is ________.

Which of the following equations is incorrectly classified as to type of chemical reaction?

In the disproportion equation below, what species is undergoing disproportionation? 3 Br₂ + 6 OH^- $\rightarrow$ BrO₃^- + 5 Br^- + 3 H₂O

In a redox reaction, the substance reduced ________.

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -Ag⁺(aq) + Cl^-(aq) $\rightarrow$ AgCl(s) ____________________

The anode in a galvanic or electrolysis cell is ________.

The balanced full-equation obtained by adding the following two balanced half-reactions is ________. 2H₂O + PH₃ $\rightarrow$ H₃PO₂ + 4H⁺ + 4e^- I₂ + 2e^- $\rightarrow$ 2I^-

Which substance is serving as the oxidizing agent in the following reaction? 14H⁺ + Cr₂O₇^-2 + 3 Ni $\rightarrow$ 3 Ni²⁺ + 2 Cr⁺³ + 7 H₂O

What is the cathode material in a common dry cell such as a flashlight battery?

In the redox reaction: 2 HNO₂ + 2 HI $\rightarrow$ 2 NO + I₂ + 2 H₂O, ________.

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

States of Matter

Gas Laws

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Exam 15: Oxidation and Reduction

In the following reaction: 2 Mn+2 + Br2 →\rightarrow→ 2 Mn+3 + 2 Br- the species that is oxidized is ________.

Which of the following equations is incorrectly classified as to type of chemical reaction?

In the disproportion equation below, what species is undergoing disproportionation? 3 Br2 + 6 OH- →\rightarrow→ BrO3- + 5 Br- + 3 H2O

In a redox reaction, the substance reduced ________.

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -Ag+(aq) + Cl-(aq) →\rightarrow→ AgCl(s) ____________________

The anode in a galvanic or electrolysis cell is ________.

The balanced full-equation obtained by adding the following two balanced half-reactions is ________. 2H2O + PH3 →\rightarrow→ H3PO2 + 4H+ + 4e- I2 + 2e- →\rightarrow→ 2I-

Which substance is serving as the oxidizing agent in the following reaction? 14H+ + Cr2O7-2 + 3 Ni →\rightarrow→ 3 Ni2+ + 2 Cr+3 + 7 H2O

What is the cathode material in a common dry cell such as a flashlight battery?

In the redox reaction: 2 HNO2 + 2 HI →\rightarrow→ 2 NO + I2 + 2 H2O, ________.

The Science of Chemistry

Numbers From Measurements

Unit Systems and Dimensional Analysis

Basic Concepts About Matter

Atoms, Molecules, Formulas, and Subatomic Particles

Electronic Structure and Chemical Periodicity

Chemical Bonds

Chemical Nomenclature

Chemical Calculations: the Mole Concept and Chemical Formulas

Chemical Calculations Involving Chemical Equations

States of Matter

Gas Laws

Solutions

Acids, Bases and Salts

Reaction Rates and Chemical Equilibrium

Nuclear Chemistry

Filters

In the following reaction: 2 Mn⁺² + Br₂ $\rightarrow$ 2 Mn⁺³ + 2 Br^- the species that is oxidized is ________.

In the disproportion equation below, what species is undergoing disproportionation? 3 Br₂ + 6 OH^- $\rightarrow$ BrO₃^- + 5 Br^- + 3 H₂O

Indicate whether each of the following formula unit or net ionic equations is or is not a redox reaction by writing the word -Ag⁺(aq) + Cl^-(aq) $\rightarrow$ AgCl(s) ____________________

The balanced full-equation obtained by adding the following two balanced half-reactions is ________. 2H₂O + PH₃ $\rightarrow$ H₃PO₂ + 4H⁺ + 4e^- I₂ + 2e^- $\rightarrow$ 2I^-

Which substance is serving as the oxidizing agent in the following reaction? 14H⁺ + Cr₂O₇^-2 + 3 Ni $\rightarrow$ 3 Ni²⁺ + 2 Cr⁺³ + 7 H₂O

In the redox reaction: 2 HNO₂ + 2 HI $\rightarrow$ 2 NO + I₂ + 2 H₂O, ________.