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10 Cards in this Set

  • Front
  • Back
Define oxidation and reduction.
Oxidation is the loss of an electron by a substance.
Reduction is the gain of an electron by a substance.
What are the oxidations #s for:
A free element
A monatomic ion
Oxygen
Hydrogen
Fluorine
Group IA elements
Group IIA elements
A free element - 0
A monatomic ion (An ion of only 1 atom) - Equal to the charge on the ion.
Oxygen - -2
Hydrogen - +1
Fluorine - -1
Group IA elements - +1
Group IIA elements - +2
What do the sum of all the oxidation numbers in a compound have to equal?
Zero; 0.
What are the steps in balancing redox reaction equations?
Determine which substances are undergoing oxidation and what substances are undergoing reduction.
Write the half-reaction for each process.
Balance each reaction.
Add the two balanced half-reactions.
What is an eletrolytic cell?
Its a gadget that has non-spontaneous reactions that are driven by an out-side source of electrical energy (electrolysis).
In an electrolytic cell - where is the positive/negative electrode and which one is the location where oxidation/reduction occurs?
The positive electrode (anode) is where oxidation takes place. The negative electrode (cathode) is where reduction takes place.
How much is 1 faraday?
96,485 C = 1 mole electrons = 1 faraday (F)
What is an electromotive force (emf)?
It is the driving force that pushes the electrons through the circuit. It is the potential difference between the electrodes of the cell.
What is the standard electrode potential?
Temp - 25 C
Concentration of each ion - 1 M
Partial pressure of each gas is 1 atm
Metals are in pure state.
What does a positive/negative electromotive force (emf) indicate?
A positive electromotive force (emf) indicates a spontaneous reaction.
A negative electromotive force (emf) indicates a non-spontaneous reaction.