Introduction to Galvanic Cells & Voltaic Cells

This chemistry video tutorial provides a basic introduction into electrochemical cells such as galvanic cells also known as voltaic cells. A galvanic cell is device such as a battery which converts chemical energy into electrical energy. A galvanic is made using two electrodes known as the anode and the cathode. Oxidation occurs at the anode and reduction occurs in the cathode. The electrons are written on the right of an oxidation half-reaction and they are located on the left side of a reduction half-reaction. Oxidation involves the loss of electrons and reduction is associated with the gain of electrons. Electrons always flow from the anode to the cathode. The purpose of the salt bridge is to prevent the build up of charge. Cations flow through the salt bridge toward the cathode and anions flow toward the anode. This electrochemistry explains completely how a galvanic cell works. It discusses how to write the overall reaction from the half reactions and how to represent the cell using standard line notation or cell notation. The electromotive force of a galvanic cell is measured in volts and 1 volt is 1 joule per coulomb. Voltage represents the work that can be done per coulomb of electric charge. Electric current is the rate at which electric charge is transferred. This video discusses how to increase the voltage and current delivered by a galvanic cell.
Intro to Galvanic & Voltaic Cells:
• Introduction to Galvan...
How To Draw Galvanic Cells:
• How To Draw Galvanic C...
Standard Reduction Potentials:
• Standard Reduction Pot...
Cell Potential Problems:
• Cell Potential Problem...
Cell Notation Problems:
• Cell Notation Practice...
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Concentration Cells:
• Concentration Cells & ...
Cell Potential & Gibbs Free Energy:
• Cell Potential & Gibbs...
Cell Potential & Equilibrium K:
• Equilibrium Constant K...
Nernst Equation:
• Nernst Equation Explai...
Electrolysis of Water:
• Electrolysis of Water ...
_____________________________________
Electrolysis of Sodium Chloride:
• Electrolysis of Sodium...
Electrolysis & Electroplating Problems:
• Electrolysis & Electro...
Electrochemistry Practice Problems:
• Electrochemistry Pract...
SAT Chemistry Subject Test Review:
• SAT Chemistry Subject ...
Carbon -14 Dating:
• Carbon 14 Dating Probl...
Beer Lambert's Law:
• Beer Lambert's Law, Ab...
______________________________________
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In case someone hasn't already mentioned it, at 9:14 you mistakenly call the Zn 2+ an anion -- you correct yourself in the following discussion.

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Here's a tip from a fellow student to another, there is a good way to remember Oxidation = anode and Reduction = cathode. Using the phrase "an ox cared" You can know an=anode ox=oxidation and cared = ca and red which both respectively means cathode and reduction

[@mosespumpuni2631]

Some books' got anode as positive and cathode as negative... it's so confusing 😕

[@Lightning_Dragon_]

@@mosespumpuni2631I think you might be getting it confused. Theres also a thing where electrons (negative charge) flow to cathode and positive charge flow to anode, which makes sense because anode is negative which attracts positive and vice versa. But the charge of the anode itself is always negative and cathode positive. Hope this helps.

[@rjhick1]

@@mosespumpuni2631 That depends on the cell. Galvanic Cells Anodes are negatiive and positive cathodes. For electrolytic cells is flipped. The anodes are positive and cathodes are negatives. Still regardless dont pay attention to that. Oxidation happens at anodes, and reduction happens at cathodes regardless of its the cell is galvanic or electrolytic. Thats the part to remember

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Thats good. Another good one is Red Cat. Reduction happens at cathode.

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That only applies in galvanic cells right?

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Do the electrons travel only through the wire or will a small amount travel through the salt bridge? Edit: I just found the answer on stack exchange. A small amount of current will leak through the electrolyte. To counter this modern batteries have a membrane called a separator that allows ion exchange but has a much higher resistance to combat the flow of electrons.

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Why nobody discusses the salt bridge in detail.

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It’s used to prevent the mixing of the half reactions and balancing them out :)

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To retain charge balance

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I just have one question. Hypothetically, if we had a Mg and Zn simple cell (one beaker) in a dilute acid, would the electrons on Mg go to Zinc or would the Mg react and reduce the H+ ions in the acid instead. I am presuming Mg would directly reduce H+ because Zinc is more reactive than Hydrogen. Also there is a bigger difference in reactivity between H+ and Mg too. ???????

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Concerning the salt bridge, if the zinc ions flow to the cathode side, will the copper electrode now get coated by zinc metal?

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No. The zinc ions will combine with the sulfate ions from the copper side and form a salt

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So how do you build the salt bridge? And how do you stop the electrons from flowing through it instead of through your load?

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It is the ions from the salt bridge which flow into the two 1/2 cells to maintain electroneutrality.

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Hello! I have a question, how can the zinc ion that left the eletrode, be dissolved in its corresponding solution, yet also pass through the wire towards the cathode? Doesnt it dissolve into the solution? Aswell, how can the anode be negative if it is loosing electrions so there are more protons so it will have to be a cation? 6:03 6:16

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But how do the electrons that leave the zinc metal strip dissolve in the correspoding metal solution and at the same time flow towards the cathode?

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