Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
24 Cards in this Set
- Front
- Back
|
Cell
|
Continuously converts chemical energy into electrical energy. Two electrodes and one electrolyte
|
|
|
Battery
|
Pile o cells connected to provide electrical energy
|
|
|
Primary cell
|
Can't be charged
|
|
|
Secondary cell
|
Can be charged
|
|
|
Fuel Cellelecte
|
Can theoretically produce electricity forever as Lin as fuel is supplied.
|
|
|
Electric Potential energy
|
Voltage
Measured in Volts. Energy difference we unit charge. |
|
|
Electric current
|
Rate of flow of charge through a circuit
Amperes (A) Determined by size of battery |
|
|
Power
|
Ate t which it produces electrical energy.
Watts (W) P= V/A |
|
|
Voltaic cells
|
Spontaneous redox reaction.
Two containers |
|
|
Anode
|
Negative electrode (in voltaic cells. Opposite if electrolytic cell)
Oxidation occurs at anode Loses electrons LEOA Metal disappears |
|
|
Cathode
|
Positive electrode if voltaic (opposite of electrolytic)
Reduction at cathode Gains electrons GERC New metal appears |
|
|
Inert electrodes
|
When Hal reaction doesn't have metal use carbon(graphite) rods or platinum rods as electrodes. This is because they don't react. Te facilitate electron transfer.
|
|
|
Cell notation
|
Anode (-)| electrolyte || electrolyte | cathode (+)
|
|
|
Cell potential
|
Differene between cathode and anode cell potential
On data book E• = Er cathode + Eo Anode Or E•= Er cathode - Er Anode |
|
|
Reference Half Cell
|
In data book it's H+ but to put it to something else make that something else potential zero and do the same to all the other elements.
!! This will change the half cell potential b |
|
|
Electrochemistry
|
Study I the interaction o electricity and chemistry
|
|
|
Electrocity
|
Involved in any reaction anytime there is transfer of electrons
|
|
|
Redox reactions
|
Involve transfer of electrons from one substance to another
|
|
|
Disproportionation
|
The same species act as both oxidizing agent and reducing agent.
|
|
|
Element oxidation number rule
|
Have numbers of 0
|
|
|
Mono atomic ion oxidation number
|
Equal to their ion charge
|
|
|
Hydrogen oxidation number rule
|
With nonmetal- +1
With metal - -1 |
|
|
Oxygen oxidation number rule
|
-2
Except peroxides. It equals -1 |
|
|
Conservation of electrons
|
The number of electrons gained must equally be number of electrons lost.
|
