Unit C: Electrochemical Changes Module 6 Flashcards
Voltaic Cell
spontaneous reaction,
converts chemical energy into electrical energy
positive standard cell potential
regular neg/pos for the cathode/anode
Anode
where oxidation occurs
Cathode
where reduction occurs
Cell Notation
anode/electrolyte//electrolyte/cathode
Where do electrons flow in a voltaic cell
anode to cathode
Inert Electrodes
used when the solutions aren’t metals to provide an inert surface for the half reaction to occur and the external wires to be connected to.
Must be conductors
Standard Cell Potential / Equation
max electrical potential difference of a cell
energy difference btw the cathode half cell and anode half cell
Enet= E cathode- E anode
Changing reference half cell
add the reduction potential to other cells, add if neg subtract if pos
won’t effect standard cell potential
Primary Cell
a closed cell that can’t be recharged
Secondary Cell
a closed cell that can be recharged (recharge by adding energy which reverses the reaction)
Fuel Cell
an open cell that requires continuous addition of fuel
Electrochemical basis of corrosion
corrosion is a process that degrades metals electrochemically, it works like a voltaic cell w a spontaneous reaction
Corrosion Prevention
cover with another metal / make an alloy
use a paint oils or grease
cathodic protection by forcing it to become the cathode
Electrolytic Cell
non spontaneous reaction
converts electrical energy into chemical energy
negative standard cell potential
opposite negativity/positive for cathode/anode
Electrolyte notation
anode/electolyte/cathode