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Questions and Answers
In a redox reaction, what happens to the oxidation number of a substance when it is reduced?
In a redox reaction, what happens to the oxidation number of a substance when it is reduced?
- The oxidation number becomes zero.
- The oxidation number decreases. (correct)
- The oxidation number increases.
- The oxidation number remains the same.
Oxidation and reduction always occur independently of each other.
Oxidation and reduction always occur independently of each other.
False (B)
What mnemonic is used to remember that oxidation is loss and reduction is gain of electrons?
What mnemonic is used to remember that oxidation is loss and reduction is gain of electrons?
OIL RIG
The substance that accepts electrons in a redox reaction is called the ______ agent.
The substance that accepts electrons in a redox reaction is called the ______ agent.
Match the terms with their correct definitions in the context of redox reactions:
Match the terms with their correct definitions in the context of redox reactions:
Which of the following is true regarding the oxidation state of an individual atom?
Which of the following is true regarding the oxidation state of an individual atom?
The oxidation state of oxygen is always -2 in all compounds.
The oxidation state of oxygen is always -2 in all compounds.
What is the oxidation number of Group 1 metals in compounds?
What is the oxidation number of Group 1 metals in compounds?
In the reaction $Zn + 2H^+ \rightarrow Zn^{2+} + H_2$, zinc acts as the ______ agent.
In the reaction $Zn + 2H^+ \rightarrow Zn^{2+} + H_2$, zinc acts as the ______ agent.
Match the following elements with their typical oxidation states in compounds:
Match the following elements with their typical oxidation states in compounds:
In the balanced redox reaction, what must be true about the number of electrons?
In the balanced redox reaction, what must be true about the number of electrons?
The oxidation number method is used to balance only simple redox reactions; complex reactions require other methods.
The oxidation number method is used to balance only simple redox reactions; complex reactions require other methods.
In the balanced equation $2Al(s) + 3H_2SO_4(aq) \rightarrow Al_2(SO_4)_3(aq) + 3H_2(g)$, which element is reduced?
In the balanced equation $2Al(s) + 3H_2SO_4(aq) \rightarrow Al_2(SO_4)_3(aq) + 3H_2(g)$, which element is reduced?
In the reaction $PbS(s) + O_2(g) \rightarrow PbO(s) + SO_2(g)$, the oxidizing agent is ______.
In the reaction $PbS(s) + O_2(g) \rightarrow PbO(s) + SO_2(g)$, the oxidizing agent is ______.
Match the half-reactions with the correct step in balancing redox reactions:
Match the half-reactions with the correct step in balancing redox reactions:
Flashcards
Oxidation-reduction reaction
Oxidation-reduction reaction
A reaction where electrons are exchanged between chemical compounds.
Oxidizing agent
Oxidizing agent
Substance that accepts electrons and oxidizes another species.
Reducing agent
Reducing agent
Substance that donates electrons and reduces another species.
Oxidation State (OS)
Oxidation State (OS)
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Oxidation state of individual atom
Oxidation state of individual atom
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Total oxidation state
Total oxidation state
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Oxidation state of Group 1 metals
Oxidation state of Group 1 metals
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Oxidation state of Group 2 metals
Oxidation state of Group 2 metals
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Fluorine Oxidation State
Fluorine Oxidation State
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OIL RIG meaning
OIL RIG meaning
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Study Notes
- Redox reactions include corrosion, combustion, photosynthesis, and decay.
- Fuel combustion, metal degradation, photosynthesis, and cellular respiration all involve redox reactions.
- This study material explores how redox reactions function and their effects on cells.
Learning Objectives
- Define oxidation and reduction reactions.
- Identify oxidizing and reducing agents.
- Apply rules for assigning oxidation numbers.
- Balance redox reactions using the change in oxidation number method.
Oxidation and Reduction Reactions
- Redox reactions involve electron exchange between chemical compounds.
- Redox reactions consist of a reduced half and an oxidized half.
- The oxidation number decreases in the reduced half as it absorbs electrons.
- The oxidation number increases in the oxidized half as it loses electrons.
OIL RIG
- "Oxidation is loss, reduction is gain (OIL RIG)" is a mnemonic to remember what happens in each process.
- In a redox reaction, the number of electrons remains constant.
- Electrons released in the oxidation half-reaction are captured in the reduction half-reaction.
Oxidizing and Reducing Agents
- The oxidizing agent accepts electrons and oxidizes another species.
- The reducing agent donates electrons and reduces another species.
- COâ‚‚ is reduced when reacting with hydrogen, decreasing carbon's oxidation number from +4 to +2.
- Hydrogen is oxidized, with its oxidation number increasing from 0 to +1.
Rules for Assigning Oxidation State
- Oxidation state reflects the number of electrons an atom loses, gains, or appears to use in compounds.
- The oxidation state of an individual atom is 0.
- The total oxidation state of all atoms in a neutral species is 0, while in an ion, it equals the ion charge.
- Group 1 metals have an oxidation state of +1, and Group 2 metals have +2.
- Fluorine's oxidation state is -1 in compounds.
- Hydrogen generally has an oxidation state of +1 in compounds.
- Oxygen generally has an oxidation state of -2 in compounds.
- In binary metal compounds, Group 17 elements have an oxidation state of -1, Group 16 elements of -2, and Group 15 elements of -3.
- Group 1A(1) elements have an oxidation number of +1 in all compounds.
- Group 2A(2) elements have an oxidation number of +2 in all compounds.
- Hydrogen's oxidation number is +1 with nonmetals and -1 with metals and boron.
- Fluorine's oxidation number is always -1.
- Oxygen's oxidation number is -1 in peroxides and -2 in other compounds (except with fluorine).
- Group 7A(17) elements have an oxidation number of -1 with metals and nonmetals (except oxygen).
Identifying Oxidation State
- Example: CaCO3 (s) has a total oxidation state of 0, C = 0-(+2)-3(-2) = +4
Identifying Oxidizing and Reducing Agents
- In the reaction Zn + 2H+ → Zn2+ + H2, Zn is oxidized and acts as the reducing agent; H+ is reduced and acts as the oxidizing agent.
Balancing Redox Equations
- Ensure the number of electrons lost by the reducing agent equals those gained by the oxidizing agent.
- Two methods to balance redox reactions include:
- Oxidation number method
- Half-reaction method
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