Studied by 1 personOxidation state
The charge of an element.
Oxidation
When an element loses electrons. (Becomes more positive)
Reduction
When an element gains electrons. (Becomes more negative)
Redox Reactions
Reactions where both reduction and oxidation are occurring at simultaneously
Reducing Agent
The element which is being Oxidized
Oxidizing Agent
The element which is being Reduced.
Spectator Ions
Ions where the charge does not change during the reaction.
Reduction half-reaction
Equation showing just the element being reduced along with the electrons gained.
Oxidation half-reaction
Equation showing just the element being oxidized with the electrons lost.
Electrodes
either the anode or the cathode. Where electrons are lost from and gained by.
Anode
The negative electrode where oxidation occurs.
Cathode
The positive electrode where Reduction occurs.
A wire (in an electrochemical cell)
Where the electrons flow through (from Anode to Cathode)
Voltaic/Galvanic Cell
Cell which produces electricity. Converts chemical energy to electrical energy.
Salt Bridge
Where the ions flow through in Voltaic/Galvanic cells (Only). the flow is opposite of the electrons.
Electrolytic Cells
Cells that need external energy to force a nonspontaneous reaction. changes electrical energy into chemical energy.
