1. Electrochemistry
and
The Chemical Cells

2. Electrochemistry -
A branch of chemistry dealing with the relations between chemical energy and electrical energy.
Examples of technology utilizing electrochemistry:
1. Batteries
2. Electroplating

3. Electricity - The flow of electrons. Electron -
A negatively charged subatomic particle., found orbiting the nucleus of an atom, with an insignificant mass.

4. Volt -
The SI unit of electromotive force, the potential difference of energy that will move one ampere of current across one ohm of resistance.

5. Amp -
The SI unit of current.

6. Ohm -
The SI uit of electrical resistance.

7. Oxidation -
Chemical process where electrons are lost. The oxidation number (charge) gets more positive.

8. Reduction -
Chemical process where electrons are gained. The oxidation state (charge) gets more negative.

9. OIL RIG -
An acronym to help remember the difference between oxidation and reduction.
Oxidation Is Loss, Reduction Is Gain (of electrons).

10. Electrochemical cell -
A system consisting of electrodes that dip into an electrolytic solution and in which a chemical reaction produces an electric current.

11. Electrolytic solution -
An aqueous solution that contains ions (electrolytes) and conducts electric current.
Examples:
1. “Gatorade”, “All-sport”…
2. “Battery acid”
3. Your blood and interstitial fluid

12. There are two types of electrochemical cells:
1. Voltaic cells
(not to be confused with the term “Electrochemical cells”)
2. Electrolytic cells

13. Voltaic cell -
Uses energy from a spontaneous chemical reaction to produce an electric current. These cells are often called a "Galvanic cells".

14. Examples of voltaic cells:
A non-rechargeable battery ("Dry cell")
A car battery
A potato clock
A "plating solution and cell" that does not require additional electricity. (We will copper plate tin this way in the lab.)

15. Electrolytic cell -
Uses energy from a non-spontaneous chemical reaction to produce an electric current. These are often used to plate metals.

16. Examples of electrolytic cells:
Electrolysis of water into Hydrogen and Oxygen.
Electrolysis of brine (concentrated salt water) into Chlorine gas, Hydrogen, and Sodium chloride.

17. Anode - The site that is always the electrode where oxidation occurs.
It is the negative terminal in a voltaic cell.
It is the positive terminal in an electrolytic cell.

18. Cathode -
The site that is always the electrode where reduction occurs.
It is the positive terminal in a voltaic cell.
It is the negative terminal in an electrolytic cell.

19. Remember:
If you alphabetize
“A” precedes “C”
and
“O” precedes “R”
Anodes are oxidized
Cathodes are reduced

20. A Voltaic Cell

21. An Electrolytic cell