REDOX
This process involves the loss of electrons.
Oxidation
This type of cell produces electrical energy spontaneously.
Galvanic (Voltaic) Cell
The purpose of the salt bridge is to maintain this property of the solutions.
Electrical Neutrality
This equation relates free energy and cell potential.
ΔG=−nFE
In electroplating, the object being coated acts as this electrode.
Cathode
This electrode is where reduction occurs.
Cathode
This type of cell requires an external power source
Electrolytic Cell
In a Zn-Cu galvanic cell, electrons flow from this electrode to the copper electrode.
At equilibrium, this quantity equals zero in a galvanic cell.
Ecell
During silver electroplating, silver ions undergo this process at the SPOON.
Reduction
These particles travel through the external wire in an electrochemical cell
Electrons
A galvanic cell has this sign for ΔG.
Negative
In a Zn-Cu galvanic cell, nitrate ions move toward this half-cell
Anode
When Q increases, this happens to Ecell.
This happens to the mass of the silver anode during electroplating.
Decrease
In an electrolytic cell, this electrode is connected to the positive terminal of the battery
Anode
This is the sign of Ecell∘ in a nonspontaneous reaction.
Negative
These ions move toward the cathode compartment through the salt bridge.
Cations
The x-intercept of a graph of Ecell vs log(Q) corresponds to this quantity.
log(K)
As electroplating continues, the external voltage required generally does this.
Increase
This quantity becomes more positive when an atom loses electrons
Oxidation Number
In BOTH galvanic and electrolytic cells, this process always occurs at the anode
Oxidation
As oxidation occurs at the anode, the solution becomes increasingly ___ without salt bridge ions.
postive
A reaction with a very large K value has this sign for Ecell∘.
This explains why increasing concentration differences make electroplating less favorable over time.
Nernst Equation