Anions in Galvanic Cells: Attraction & Dissolution

In summary, a galvanic cell involves the dissolution of atoms at the anode through oxidation and the precipitation of these atoms at the cathode through reduction. The charge carriers in a power supply are electrons, which are more mobile than protons or atoms. The electrode potential is the difference in electronegativity between the two electrodes, which determines which one will be the reductant (anode) and which will be the oxidant (cathode).
  • #1
Mr_Bojingles
79
0
In a galvanic cell is it the anions from the electrolyte which is attracted to the cathode or is it the anions produced from the anode dissolving which flow to the cathode??

Also it mentions that the charges increase in energy as they pass through the power supply and they decrease when they pass through the consumer. What exactly is a charge? Is it just an electron or is it a proton with electrons or what??
 
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  • #2
Mr_Bojingles said:
In a galvanic cell is it the anions from the electrolyte which is attracted to the cathode or is it the anions produced from the anode dissolving which flow to the cathode??
Both species of atoms can be involved depending on the construction of the cell, i.e. whether there is a single or dual electrolyte. However the reactions are dissolution (by oxidation), which occurs at the anode and precipitation (by reduction), which occurs at the cathode. Atoms dissolved from the anode will interact chemically with the electrolyte.

Also it mentions that the charges increase in energy as they pass through the power supply and they decrease when they pass through the consumer. What exactly is a charge? Is it just an electron or is it a proton with electrons or what??
The electrons are the charge carriers through a power supply. Is one thinking of an electrolytic cell in this case?

Electrons and protons have charge. Electrons are negatively charged, while protons (and the atomic nucleus which contains protons and neutrons) are positively charged. Keep in mind that electrons are 'small' with a mass of ~1/1835 of a proton, and so electrons are more mobile than protons or atoms.

These might help in understanding the phenomena involved.

http://en.wikipedia.org/wiki/Galvanic_cell

http://en.wikipedia.org/wiki/Electrolytic_cell

http://en.wikipedia.org/wiki/Electrochemical_cell

http://en.wikipedia.org/wiki/Alkaline_battery

http://en.wikipedia.org/wiki/Electrode_potential
http://en.wikipedia.org/wiki/Nernst_equation


http://chemistry.about.com/library/weekly/aa082003a.htm


http://www.mpoweruk.com/chemistries.htm (some good graphics here)


http://www.science.uwaterloo.ca/~cchieh/cact/c123/battery.html (some bad links on this page)
http://www.science.uwaterloo.ca/~cchieh/cact/c123/emf.html

This is helpful - The Galvanic Cell and the p-n Junction
http://www.rose-hulman.edu/~moloney/BoisePNjunctionOperation.html


Electrochemical and Electrolytic cells
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/electrochem.html
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/electrolyt.html

Electrochemistry concepts
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/electrol.html

Thermodynamic potentials
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/thepot.html

Oxidation/Reduction concepts
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/redoxcon.html


CZ batteries
http://www.eveready.com/pdfs/ever_cz_appman.pdf [Broken]

Zn-MnO2 batteries
http://www.eveready.com/pdfs/ever_alkcylin_appman.pdf [Broken]
 
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  • #3
That pretty much explains it. Thanks alot. One things still unclear to me though.

When the dissolution takes place at the anode do hydrogen ions break off and leave electrons attached to the anode followed by the hydrogen ions precipitating on the cathode? If so does that mean the anode gradually erodes and the cathode gradually expands?

Also is the electrode potential the electronegativity difference of the two electrodes which determines which one will be the reductant(anode) and which will be the oxidant(cathode)?
 

1. What are anions in galvanic cells?

Anions are negatively charged ions that are involved in the electrochemical reactions that occur in galvanic cells. They are attracted to the positively charged anode and help facilitate the flow of electrons through the cell.

2. How do anions contribute to the attraction and dissolution in galvanic cells?

Anions are attracted to the positively charged anode, which is where the oxidation reaction occurs. This attraction helps pull the anions towards the anode and allows for the flow of electrons through the cell. Additionally, anions can also participate in the dissolution of the anode material, aiding in the overall reaction of the cell.

3. What role do anions play in the overall functioning of a galvanic cell?

Anions play a crucial role in the functioning of galvanic cells. They help facilitate the movement of electrons through the cell, contribute to the dissolution of the anode material, and maintain charge balance within the cell. Without anions, the electrochemical reactions that occur in galvanic cells would not be able to proceed efficiently.

4. Can anions be replaced or substituted in a galvanic cell?

In general, anions cannot be easily replaced or substituted in a galvanic cell. This is because the specific type of anion that is involved in the electrochemical reactions is often a key factor in dictating the overall functioning of the cell. However, in some cases, certain anions can be exchanged for others if they have similar properties and do not significantly impact the overall reaction.

5. Are there any potential issues or limitations with anions in galvanic cells?

There can be potential issues or limitations with anions in galvanic cells, depending on the specific type of anion and the composition of the cell. For example, some anions may be more reactive and can cause corrosion of the anode material, leading to decreased efficiency and lifespan of the cell. Additionally, certain anions may not be able to participate in the reactions or may interfere with the functioning of the cell, resulting in reduced overall performance.

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