1. Oxidation-Reduction Reactions
BATTERIES
Oxidation-Reduction Reactions
TEAM: ATE
Names of Team Members

2. Goals & Purpose Redox Reactions Explain how batteries work
Explain how energy is produced
Explain Battery Arrangements
Different types of batteries

3. Batteries are EVERYWHERE!
Technology in US continuously advancing-smaller batteries w/ more power
flashlights, pagers, cell phones, i-pod, laptops, cars, etc.
dependent on batteries and how long they keep their charge

4. REDOX REACTIONS AKA Oxidation-Reduction Reactions
transfer of electrons between atoms
Oxidation involves a loss of electrons
Reduction involves a gain in electrons

5. BATTERIES Put redox reactions to use
Convenient way of generating electricity
Electrical energy can be obtained from any electrochemical cell
When several cells are connected to provide sufficient power- these cells are known as BATTERIES

6. How batteries work… Every battery has two terminals
Positive + & Negative -
Normal flashlight batteries the ends are the terminals
Large car batteries have two heavy lead posts that act as terminals
Electrons collect on negative end
Connect wire between two terminals & electrons flow through it from the negative to the positive terminal

8. Electrons must flow from battery through wire from the negative to the positive terminal for the chemical reaction to take place
The speed of electron production by this chemical reaction controls how many electrons can flow between the terminals
Unless electrons are flowing reaction does not take place… this is why batteries can sit for years and still work

9. Battery Arrangements
Group together serially to form higher voltage (voltages add up)
Group together parallel to form higher current (currents add up)

11. CURRENT – flow of electric charge
Electronic and electrical things 'work' because electrons are flowing through them
This is current (I) measured in amps.
The more amps, the hotter, faster, louder, etc
Talking of current is always relative to a SINGLE POINT in a circuit... the number of electrons passing that point

12. VOLTAGE – potential energy
What makes the electrons move
Voltage is always a comparison between two points
one point is assumed to be the 'zero voltage' point

13. Types of Batteries
Zinc-Carbon- standard carbon battery used in all inexpensive AA, C, & D dry cell batteries
Alkaline- Common in Duracell & Energizer batteries – zinc & manganese-oxide
Lithium Photo- lithium, lithium iodide, and lead-iodide used – ability to supply power surges
Lead-acid-automobiles – oxide electrodes – (rechargeable)
Nickel-cadmium- nickel-hydroxide & potassium-hydroxide electrodes (rechargeable)

14. Types continued…
Nickel-metal hydride- rapidly replacing nickel due to not suffering from memory effect (rechargeable)
Lithium-ion-very good power-to-weight ratio – high-end laptop computers and cell phones (rechargeable)
Zinc-air- lightweight and rechargeable
Zinc-mercury oxide- hearing aids
Silver-zinc- aeronautical applications – good power-to-weight ratio
Metal-chloride- electric vehicles - scooter

15. Name seven things that you personally use batteries for:
QUIZ Question…
Name seven things that you personally use batteries for:

16. SOURCES
Baird, Colin and Gloffke, Wendy. (2005). Chemistry in Your Life. New York: W. H. Freeman and Company.