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Oxidize
When a substance LOSES its electrons.
Reduced
When a substance GAINS its electrons.
Redox Reaction
The net reaction of oxidation and reduction.
Oxidation and Reduction
Occur together in ONE reaction.
Oxidizing Agent
A substance that gets reduced causes another substance to be oxidized.
Reducing Agent
A substance that gets oxidized cause another substance to be reduced.
Disproportionation
A reaction in which the same substance functions as both the oxidizing agent and a reducing agent; it is both reduced and oxidized.
Oxidation Number
A positive or negative number that allows you to determine what is happening to the electron in the reaction.
Oxidation Number Increaese
The substance is being OXIDIZED.
Oxidation Number Decrease
The substance is being REDUCED.
Oxidization States Constants
All atoms: 0
Hydrogen: +1, except in hydrides then -1
Oxygen: -2, except in peroxides then -1
Monatomic inons: charge on ion
Spontaneity Rule
If the OA is above the RA pn the redox half reaction table.
5 Step Methode
Step 1: list all entities present and classify as OA and RA and SOA and SRA.
Step 2: Write down the half reactions for the SOA.
Step 3: Write down the half reactions for the SRA.
Step 4: Balance the electrons in both half reactions and put the two half reactions together.
Step 5: Perdict spontinaity.
Voltaic Cell
An electrochemical cell that spontaneously reacts to PRODUCE electricity.
Electrolytic Cell
An electrochemical cell that USES electricity to cause a non-spontanious chemical change.
Electrode
The solid in the half-cell where the wires attach.
Anode
The electrode where oxidization occurs, where the strongest RA reacts.
Cathode
The eletrode where reduction occurs, where the strongest OA reacts.
Anion
A negative ion, moves toward the anode.
Cation
A postive ion, moves toward the cathode.
Salt Bridge
A barrier the keeps the solutions in a voltaic cell apart, but allows the flow of ions between the solutions to prevent an electrical charge build up. Required by Voltaic Cells
Electrolyte
A substance the conducts electricity when dissolved in water.
Power Supply
An electronic device that replaces a battery.
External Circuit
The wires that are used to connect the anode to the cathode.
Electron Flow
Anode to Cathode.
Ion FLow
Anions to Anode; Cations to Cathade.
Cell Spontanaity
Voltaic: yes
Electrolytic: no
Net Electrode Potencial of Cells (E°net )
Voltaic: positve
Electrolytic: negative
Line Notion of Cells
anode / anode electrolyte // cathode electrolyte / cathode
Chloride Anomaly
When chloride acts as the reducing agent when with water in a reaction.
Standard Hydrogen Half-Cell
What is used to measure the standard reduction potentials. It contains 1.00 mol/L of the hydrogen ion.
Standard Cell Difference Equation
E°net= E°r(cathode) - E°r(anode)
Calculating Cell Potential Difference
Step 1: List all entities present
Step 2: Determine OAs and RAs
Step 3: Determine SOAs and SRAs
Step 4: Write down anode and cathode half reactions (redox half reactions)
Step 5: Calculate the cell potential difference
Spontaneity in Electrochemical Cells
If OA is above the RA, it is spontaneous.
If the cell potential is positive, the reactions is spontaneous.
Faraday's Constant
9.65 x 10^4 C/mol → it represents the number of coulombs per mole of electrons.
Moles of an Electron Equation
(I x t)/F
I = amps
t = time in seconds
F = Faraday's constant in C/s