Electrochemical Cells

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Electrochemical Process Noun

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[uh-lek-troh-kem-i-kuhl pros-es]

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Electrochemical Process

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Any process involving the conversion between chemical potential energy and electrical energy through oxidation-reduction reactions.

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Example: This diagram shows an electrochemical cell where a chemical reaction creates electricity. Electrons flow from the zinc anode to the copper cathode, powering a lightbulb.

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Electrochemical Cell Noun

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[uh-lek-troh-kem-i-kuhl sel]

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Electrochemical Cell

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A device that converts chemical energy into electrical energy, or vice versa, by means of redox reactions.

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Example: A zinc anode and a copper cathode in separate solutions are connected, causing electrons to flow and generate electricity, which powers the light bulb.

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Redox Reaction Noun

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[ree-doks ree-ak-shuhn]

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Redox Reaction

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A chemical reaction characterized by the transfer of electrons between reacting chemical species, involving both reduction and oxidation.

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Example: This diagram shows atom A losing an electron (oxidation) to atom B, which gains the electron (reduction), illustrating the electron transfer in a redox reaction.

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Electric Potential Noun

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[uh-lek-trik poh-ten-shuhl]

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Electric Potential

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The amount of work needed to move a unit of electric charge from a reference point to a specific point.

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Example: Pushing a ball uphill stores potential energy, just like a battery stores energy by creating a high electric potential, ready to make electricity flow.

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Voltaic Cell Noun

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[vohl-tey-ik sel]

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Voltaic Cell

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An electrochemical cell that generates electrical energy from a spontaneous redox reaction, converting chemical energy into electrical energy.

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Example: A voltaic cell converts chemical energy into electrical energy. Electrons flow from the zinc electrode (anode) through a wire to the copper electrode (cathode), powering a lightbulb.

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Half-Cell Noun

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[haf-sel]

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Half-Cell

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A distinct part of a voltaic cell where either the oxidation or the reduction half-reaction occurs.

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Example: This diagram shows a half-cell, where an electrode is in a solution. A chemical reaction on the electrode's surface involves ions and electrons.

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Electrode Noun

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[uh-lek-trohd]

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Electrode

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A solid electrical conductor through which an electric current enters or leaves an electrolyte or other medium.

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Example: This diagram shows two electrodes, a positive anode and a negative cathode, placed in a solution, which is a basic setup for an electrochemical cell.

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Anode Noun

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[an-ohd]

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Anode

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The electrode in an electrochemical cell where oxidation takes place, releasing electrons into the external circuit.

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Example: In this simple battery (electrochemical cell), the anode is the negative terminal that releases electrons, creating an electrical current to power the lightbulb.

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Cathode Noun

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[kath-ohd]

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Cathode

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The electrode in an electrochemical cell where reduction takes place, consuming electrons from the external circuit.

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Example: In an electrolytic cell, the cathode is the negative electrode connected to the battery, where positively charged ions (cations) are attracted to undergo reduction.

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Salt Bridge Noun

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[sawlt brij]

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Salt Bridge

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A component connecting the two half-cells of a voltaic cell, allowing ion flow to maintain charge neutrality.

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Example: A salt bridge connects two half-cells in an electrochemical cell, allowing ions to flow between them to maintain charge neutrality and complete the electrical circuit.