Understanding Ion and Electron Flow in Galvanic and Electrolytic Cells

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SUMMARY

In galvanic cells, cations move towards the cathode, which is the negative terminal, while anions move towards the anode, the positive terminal. This behavior is due to the inherent differences in charge between the electrodes in galvanic and electrolytic cells. In galvanic cells, the cathode is considered positive because it is where reduction occurs, while in electrolytic cells, the cathode is negative as it attracts cations during the electrolysis process. Understanding these principles is crucial for grasping the fundamental operations of electrochemical cells.

PREREQUISITES
  • Basic knowledge of electrochemistry
  • Understanding of oxidation and reduction reactions
  • Familiarity with galvanic and electrolytic cell configurations
  • Concept of electrode polarity and ion movement
NEXT STEPS
  • Study the Nernst equation for understanding cell potentials
  • Explore the differences between galvanic and electrolytic cells in detail
  • Learn about ion transport mechanisms in electrochemical systems
  • Investigate applications of electrochemical cells in real-world scenarios
USEFUL FOR

Chemistry students, electrochemists, educators, and anyone interested in the principles of electrochemical reactions and their applications.

ajayguhan
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I know that positively charged cation move toward cathode which is the negative terminal and the negatively charged anion move towards anode which is positive terminal

Why does in galvanic cell cations are moving toward cathode which is positively terminal?

And why in galvanic cell cathode is positive and in electrolytic cell cathode is negative?

How could this happen?
 
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