Podcast
Questions and Answers
Which process involves the metal cation dissolving from the metal to the solution?
Which process involves the metal cation dissolving from the metal to the solution?
Ionic Pressure (I.P.) refers to the tendency for the metal cation to deposit onto the metal rod.
Ionic Pressure (I.P.) refers to the tendency for the metal cation to deposit onto the metal rod.
True
What is formed when the metal rod acquires charge and is surrounded by opposite charge?
What is formed when the metal rod acquires charge and is surrounded by opposite charge?
Double Electric Layer
In the Zno / Zn2+ system, the process is __________, meaning Zn dissolves into solution.
In the Zno / Zn2+ system, the process is __________, meaning Zn dissolves into solution.
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Match the following metal systems with their dominant process:
Match the following metal systems with their dominant process:
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Which of the following statements about Standard Electrode Potential (Eo) is true?
Which of the following statements about Standard Electrode Potential (Eo) is true?
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The Standard Hydrogen Electrode (NHE) has an Eo value of -1.00.
The Standard Hydrogen Electrode (NHE) has an Eo value of -1.00.
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What does a more negative Eo value indicate about a metal's tendency to oxidize?
What does a more negative Eo value indicate about a metal's tendency to oxidize?
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The electrode potential of the lithium half-cell is __________.
The electrode potential of the lithium half-cell is __________.
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Match the following systems with their Standard Electrode Potentials (Eo):
Match the following systems with their Standard Electrode Potentials (Eo):
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Study Notes
Standard Electrode Potential (Eo)
- The standard electrode potential (Eo) is a measure of the tendency of a metal to lose electrons and get oxidized.
- The greater the negative value of the Eo, the greater the tendency of the metal to form its ionic state.
- The standard electrode potential is also a measure of the reducing strength of the metal.
- The standard hydrogen electrode (NHE) has a potential of zero.
Solution Pressure (S.P.) and Ionic Pressure (I.P.)
- Solution Pressure is the tendency of a metal to dissolve and form cations.
- Ionic Pressure is the tendency of metal cations in a solution to be deposited on the metal rod.
- The predominant process depends on the nature of the metal and the concentration of the solution.
Half-Cell and Single Electrode Potential
- A half-cell consists of a metal rod immersed in a solution of its ions.
- The potential difference between the metal rod and its solution is called the single electrode potential.
- The sign of the potential is the same as the charge on the metal electrode.
- The single electrode potential is a measure of the tendency of the metal to be oxidized or reduced.
Galvanic Cell or Voltaic Cell
- When two half-cells are connected, electrons pass from the half-cell with a higher tendency to oxidize to the half-cell with a higher tendency to reduce.
- This flow of electrons creates an electric current in the cell.
- The potential difference between the two half-cells is called the electromotive force (emf) of the cell.
Redox Reactions
- Oxidation is the loss of electrons.
- Reduction is the gain of electrons.
- Oxidants (oxidizing agents) are electron acceptors.
- Reductants (reducing agents) are electron donors.
- Redox reactions involve the transfer of electrons from a reductant to an oxidant.
- Each redox reaction can be represented by two half-reactions: one for oxidation and one for reduction.
Half-Reactions of Oxidants and Reductants
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Half-reactions of Oxidants:
- MnO4- + 8H+ + 5e- = Mn2+ + 4H2O
- Ce4+ + e- = Ce3+
- Cr2O72- + 14H+ + 6e- = 2Cr3+ + 7H2O
- I2 + 2e- = 2I-
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Half-reactions of Reductants:
- C2O42- = 2CO2 + 2e-
- 2I- = I2 + 2e-
- 2S2O32- = S4O62- + 2e-
- NO2- + H2O = NO3- + 2H+ + 2e-
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Description
Test your knowledge on standard electrode potential, solution pressure, and ionic pressure. This quiz covers key definitions and principles related to half-cell and single electrode potential. Challenge yourself and enhance your understanding of electrochemistry.
