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Questions and Answers
What happens to the oxidation number of iron during the reaction?
What happens to the oxidation number of iron during the reaction?
- It remains the same at (2+).
- It fluctuates between (2+) and (3+).
- It increases from (2+) to (3+). (correct)
- It decreases from (3+) to (2+).
How many electrons are added to balance the charges in the reduction half-reaction?
How many electrons are added to balance the charges in the reduction half-reaction?
- Four electrons.
- Six electrons. (correct)
- One electron.
- Two electrons.
What is the first step when balancing the half-reactions?
What is the first step when balancing the half-reactions?
- Adding electrons to balance the charges.
- Balancing charges last.
- Balancing oxygen atoms with water. (correct)
- Balancing hydrogen atoms.
What must occur after balancing the half-reactions before combining them?
What must occur after balancing the half-reactions before combining them?
In what medium does the described reaction occur initially?
In what medium does the described reaction occur initially?
What is the primary process involved in redox reactions?
What is the primary process involved in redox reactions?
What occurs to the oxidation state of an atom during oxidation?
What occurs to the oxidation state of an atom during oxidation?
In the reaction of zinc and copper, what role does zinc play?
In the reaction of zinc and copper, what role does zinc play?
What are the two general types of electrochemical cells?
What are the two general types of electrochemical cells?
To balance a redox reaction in a half-reaction method, which step should be taken first?
To balance a redox reaction in a half-reaction method, which step should be taken first?
What is the purpose of balancing charges in a redox reaction?
What is the purpose of balancing charges in a redox reaction?
In an electrochemical process, what happens to the energy during a spontaneous redox reaction?
In an electrochemical process, what happens to the energy during a spontaneous redox reaction?
Which of the following accurately describes the reduction reaction in a redox process?
Which of the following accurately describes the reduction reaction in a redox process?
Flashcards
Oxidation
Oxidation
A chemical reaction where an element or ion loses electrons, increasing its oxidation number.
Reduction
Reduction
A chemical reaction where an element or ion gains electrons, decreasing its oxidation number.
Half-Reaction Method
Half-Reaction Method
A method of balancing chemical equations by separating the reaction into two half-reactions, one for oxidation and one for reduction. Each half-reaction is then balanced separately for atoms and charges.
Electron Balance
Electron Balance
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Acidic Medium
Acidic Medium
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Redox Reactions
Redox Reactions
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Redox Reaction Equation
Redox Reaction Equation
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Voltaic Cell
Voltaic Cell
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Electrolytic Cell
Electrolytic Cell
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Balancing Redox Reactions
Balancing Redox Reactions
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Cell Notation
Cell Notation
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Study Notes
Electrochemistry Fundamentals
- Electrochemistry studies the interconversion of chemical and electrical energy.
- Redox reactions involve electron transfer. Oxidation is loss of electrons, reduction is gain of electrons.
- Oxidation states change during redox reactions. Oxidation increases the oxidation state (more positive), reduction decreases it (more negative).
- Balancing redox reactions involves identifying oxidation and reduction half-reactions and balancing atoms and charges.
- Balancing half-reactions: First balance atoms other than H and O. Balance O atoms by adding H2O. Balance H atoms by adding H+. Balance charges by adding electrons.
Voltaic Cells
- Voltaic cells are electrochemical cells that produce electricity from a spontaneous chemical reaction.
- Anode: electrode where oxidation occurs (electrons released)
- Cathode: electrode where reduction occurs (electrons received)
- Salt bridge: completes the circuit, maintains charge neutrality by allowing ion movement between half-cells.
- Cell notation: Anode | anode solution || cathode solution | cathode
- Example: Zn(s) | Zn2+(aq) || Cu2+ (aq) | Cu(s)
Cell Notation Details
- The anode is always written on the left, followed by the anode species, then a double vertical bar ( || ), followed by the cathode species, then the cathode.
- Phases must be specified in the cell notation (i.e., solid, aqueous, gas).
- Concentrations or pressures (for gases) of species are given in parentheses (e.g. 1.0M, 1.0 atm).
- Inert electrodes (like Pt or graphite) are included in the notation.
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