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Questions and Answers
What is the primary function of an oxidizing agent in a reduction half reaction?
What is the primary function of an oxidizing agent in a reduction half reaction?
- To inhibit the reaction and prevent electron transfer
- To gain electrons and become reduced
- To lose electrons and become oxidized
- To facilitate the transfer of electrons from another species (correct)
Which of the following statements is true about the organization of the reduction half reaction table?
Which of the following statements is true about the organization of the reduction half reaction table?
- The strongest reducing agents are listed at the bottom right corner (correct)
- The weakest oxidizing agents are listed at the bottom left corner
- The weakest reducing agents are listed at the top right corner
- The strongest oxidizing agents are listed at the top left corner
What determines whether a reaction is spontaneous or non-spontaneous?
What determines whether a reaction is spontaneous or non-spontaneous?
- The presence of a reducing agent
- The combination of a reduction half reaction and an oxidation half reaction
- The presence of an oxidizing agent
- The relative reactivity of the species involved (correct)
What is the oxidizing agent in the reaction: Cu(s) / H +(aq) / NO3–(aq) / H2O(l)?
What is the oxidizing agent in the reaction: Cu(s) / H +(aq) / NO3–(aq) / H2O(l)?
What is the net result of combining a reduction half reaction and an oxidation half reaction?
What is the net result of combining a reduction half reaction and an oxidation half reaction?
Which species loses electrons in the reaction Pb(s) + 2 Ag+(aq) → 2 Ag(s) + Pb2+(aq)?
Which species loses electrons in the reaction Pb(s) + 2 Ag+(aq) → 2 Ag(s) + Pb2+(aq)?
In a redox reaction, what is the purpose of multiplying the half-reactions by simple whole numbers?
In a redox reaction, what is the purpose of multiplying the half-reactions by simple whole numbers?
What is the oxidation half reaction for the reaction Pb(s) + 2 Ag+(aq) → 2 Ag(s) + Pb2+(aq)?
What is the oxidation half reaction for the reaction Pb(s) + 2 Ag+(aq) → 2 Ag(s) + Pb2+(aq)?
What is the reduction half-reaction in the reaction: O2(g) + 4 H +(aq) + 4e – → 2 H2O(l)?
What is the reduction half-reaction in the reaction: O2(g) + 4 H +(aq) + 4e – → 2 H2O(l)?
What is the net ionic equation for the reaction: Fe(s) / H2O(l) / H +(aq) / O2(g)?
What is the net ionic equation for the reaction: Fe(s) / H2O(l) / H +(aq) / O2(g)?
Why does a strip of zinc react with a solution of copper(II) nitrate, but a strip of copper does not react with a solution of zinc nitrate?
Why does a strip of zinc react with a solution of copper(II) nitrate, but a strip of copper does not react with a solution of zinc nitrate?
Which of the following is a characteristic of a spontaneous redox reaction?
Which of the following is a characteristic of a spontaneous redox reaction?
What is the purpose of the reduction half reaction table?
What is the purpose of the reduction half reaction table?
What is the role of the species being oxidized in a redox reaction?
What is the role of the species being oxidized in a redox reaction?
Which of the following species is most likely to be a reducing agent in a reaction?
Which of the following species is most likely to be a reducing agent in a reaction?
What is the purpose of constructing half-reactions in predicting balanced redox equations?
What is the purpose of constructing half-reactions in predicting balanced redox equations?
In a disproportionation reaction, what happens to the species being reacted?
In a disproportionation reaction, what happens to the species being reacted?
What determines the spontaneity of a redox reaction?
What determines the spontaneity of a redox reaction?
What is the purpose of a reductions table in redox reactions?
What is the purpose of a reductions table in redox reactions?
When creating a net ionic equation, what is the first step?
When creating a net ionic equation, what is the first step?
Which of the following is an example of an oxidation half reaction?
Which of the following is an example of an oxidation half reaction?
What is the relationship between the position of an oxidizing agent on the reductions table and its reactivity?
What is the relationship between the position of an oxidizing agent on the reductions table and its reactivity?
What is necessary for a redox reaction to occur?
What is necessary for a redox reaction to occur?
Which of the following is an example of a spontaneous redox reaction?
Which of the following is an example of a spontaneous redox reaction?
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Study Notes
Using the Reductions Table
- A reduction half-reaction table shows all reactions with electrons being gained, and the species gaining electrons is the oxidizing agent.
- If the table were written in reverse, it would show a loss of electrons and be called an oxidation half-reaction table.
Reduction and Oxidation Half-Reactions
- In a reduction half-reaction, electrons are gained, and the species gaining electrons is the oxidizing agent.
- In an oxidation half-reaction, electrons are lost, and the species losing electrons is the reducing agent.
Characteristics of the Reductions Table
- The most reactive or strongest oxidizing agents are found at the upper left corner of the table.
- The most reactive or strongest reducing agents are found at the lower right side of the table.
- When a reduction half-reaction is added to an oxidation half-reaction, a REDOX (reduction-oxidation) reaction is formed.
Determining Spontaneous or Non-Spontaneous Reactions
- A reaction is spontaneous if an oxidizing agent (OA) reacts with a reducing agent (RA) where the OA is positioned higher on the table than the RA.
- A reaction is non-spontaneous if an OA reacts with an RA where the OA is positioned lower on the table than the RA.
Disproportionation
- Disproportionation is a reaction where a species is both oxidized and reduced.
- Example: Two iron(II) ions colliding in a solution, resulting in one iron(II) ion being oxidized to iron(III) and another iron(II) ion being reduced to iron(s).
Predicting Redox Reactions
- Steps to predict balanced redox equations:
- Start with two half-reaction equations
- Balance each half-reaction equation
- Multiply each half-reaction equation by simple whole numbers to balance electrons lost and gained
- Add the two half-reaction equations, cancelling electrons and identical species
Constructing Half-Reactions
- Identify all species present
- Identify which species are oxidizing agents (OA) and reducing agents (RA)
- Use the Reductions Table to create net ionic (redox) equations
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