Electrolytic Cell

• Electrolytic cells


  No flow of e- to produce a current, outside power source must be supplied, converts electrical energy into chemical energy
• Charging a battery


  This is how we charge a battery
• Electroplating


  Process of adding a layer (plate) of metal on the surface of another object
• Electroplating process


  1. Battery forces electrons to travel to the spoon

  2. Spoon is negative & will attract Silver (+) ions

  3. Silver ions will reduce (stick) onto the spoon, plating it

  4. The Ag bar (anode) loses e- & will eventually disappear
• At the anode

  Oxidization, e- loss
• At the cathode

  Reduction, e- gain
• Electrolytic

  Anode oxidation, cathode reduction, e- flow anode->cathode
• Spontaneous


  Chemical energy changes to electricity
• Non-spontaneous


  Electrical energy changes to chemical energy
• Electrolytic cells vs Voltaic cells

  • Electrolytic needs external power source & non-spontaneous, Voltaic is produces its own energy & spontaneous
  • Electrolytic has no salt bridge while Galvanic has a salt bridge
• if a group 17 element is by itself, add a two for the subscript bc it's diatomic. Also, add a 2 in front of the element in the half rxn
• When you write a half rxn, you always start the equation with the element and charge in the diagram, then add e- accordingly
• In electroplating

  The anode will always be the metal
• In electroplating

  The cathode is the one getting plated
• if question is asking why the mass of a specific electrode decreases or increases as the cell operates, in terms of the ion and atoms, if it's oxidation, say the atoms are oxidized to ions and if it's reduction, say the atoms are reduced to ions.