So galvanic cell, also known as a voltaic cell is a spontaneous cell that produces or discharges electricity. Therefore making it a battery. Now we're gonna say it uses stored chemical energy and converts it into electrical energy. Now it has different parts to it. First we're gonna talk about the an ode. The note is known as the negative electrode when it comes to a galvanic or voltaic cell. So it's the metal electrode and compartment where oxidation occurs. Remember oxidation means that you are losing electrons. The cathode is the positive metal electrode and compartment where reduction occurs. Remember that means you're gaining electrons. So if you look at this image here, we have basically the anote here which we labeled in this aqua blue. So it's negatively charged cathode is positively charged. The anna is losing electrons. So it's literally losing electrons from its surface. The electrons are going this way towards the cathode. The cathode is this metal electrode here. So this electrode is gaining electrons. This one here is losing electrons. The one that's losing is zinc, zinc solid. In this case it also has dissolved in it, zinc two plus ions which are originating from the cap on the electrode itself. Over here we have copper two plus ions in the solution which are originating from this electrode as well. Now we also have what's called a salt bridge. A salt bridge is a tube that connects both half cells. So a half cell is this jar and this jar, both half cells to one another and allows for the flowing of neutral ions. Now, neutral ion sounds a little bit like an oxymoron, like ions have a charge. So why would they be neutral? Well when we say the term neutral ions were basically saying these are ions within solution that possess no acidic or basic properties. Okay so ions when we're getting to this electrochemical stuff, they can be acidic, basic or neutral here. When it comes to our galvanic or voltaic cell we use neutral ions within this salt bridge this tube here. This tube here has within it negative ions and positive ions that are neutral ions. The negative ones will flow towards the annual compartment. The positive ones will flow towards the cathode department compartment. Now besides that, we have one more piece the volt meter. The volt meter which is this portion right here. This is device that records the amount of electricity generated by the galvanic cell. So this thing here is actually producing electricity which is pretty cool. It does it by a spontaneous redox reaction. So just remember when it comes to galvanic or voltaic cells, same thing. These are the important portions of it. And it also depicts the flow of electrons as we move from the an ode to the cathode

And electrolytic cell is a non spontaneous cell that utilizes electrolysis in order to operate. Now, electrolysis is when we have chemical reactions that consume external cam electrical electrical energy in order to occur. Now we're going to stay here no matter the cell, whether it be an electrolytic cell, a galvanic slash voltaic cell, it doesn't matter. The cathode is always the site of reduction and the A note is always the site of oxidation. However, because electrolytic cells are non spontaneous, their signs will be different here. Since the process is non spontaneous, the cathode is now negatively charged, indiana is now positively charged. So basically our understanding here is that when it comes to electrolytic cells, they are the opposites of galvanic cells. So just remember this fundamental idea, they're opposites of one another.

So when it comes to an electrolytic cell it has to consume electrical energy and then it converts that energy into chemical energy. Now because an electrolytic cell requires electrical energy. You typically see a battery being installed with an electronic self so they can draw this electrical energy out and quickly converted into chemical energy. Now remember in electrolytic cell are cathode is now negatively charged and the A note is positively charged. But even though their signs are different, we still have to realize that when it comes to the cathode, that is where reduction occurs. So here 10 2 plus ion is still reduced but now to 10 neutral and notice still oxidation. So now copper metal is oxidized to copper two plus. We still have our salt bridge, we still have the movement of electrons now. So electrons will move this way towards my cattle. So that's not going to change. Alright, so now we're going to say that since we're dealing with the cathode, we have R. S. N two plus acquis being reduced to be reduced, it has to absorb electrons. So it's going to have to electrons To give us our 10 neutral solid and then are an ode is being oxidized with losing electron. So we have our copper solid here losing two electrons To produce copper two plus acquis. When we cancel out the electrons, what we get is our overall equation, which is S. N two plus Aquarius plus copper solid, gives me S and solid plus copper two plus acquis. And we're gonna say here, is that the application of an electrolytic cell? Is that we see that it can be used for batteries. So we can have example double A, triple A. Etcetera batteries. We use those batteries to harness electrical energy and convert it into chemical energy. We could also utilize rechargeable lithium batteries. Mhm. So, just remember electrolytic cells are non spontaneous and so requiring outside energy source. This application is in the form of batteries. We utilize the electrical energy that they can produce, converted into chemical energy that we can deal with redox reactions.