Voltaic Cells

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Electrochemistry Noun

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[uh-lek-troh-kem-uh-stree]

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Electrochemistry

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The branch of chemistry studying the relationship between electrical energy and chemical reactions, particularly redox processes.

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Example: This diagram shows a voltaic cell. Chemical reactions cause electrons to flow from the zinc (Zn) electrode to the copper (Cu) electrode, creating electricity.

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Redox Reaction Noun

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[ree-doks ree-ak-shun]

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Redox Reaction

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A type of chemical reaction that involves a transfer of electrons between two species, resulting in changes in oxidation states.

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Example: This diagram shows that in a redox reaction, one substance (A) is oxidized by losing an electron, while another substance (B) is reduced by gaining it.

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Oxidation Noun

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[ok-si-dey-shun]

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Oxidation

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A chemical process that involves the loss of electrons by a molecule, atom, or ion during a redox reaction.

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Example: This image shows the chemical reaction for rusting, where iron (Fe) combines with oxygen (O2) in the presence of water, a common example of oxidation.

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Reduction Noun

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[ri-duhk-shun]

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Reduction

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A chemical process that involves the gain of electrons by a molecule, atom, or ion during a redox reaction.

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Example: This diagram shows that reduction is the gain of an electron. Atom B gains an electron (e+) and becomes negatively charged, illustrating the process.

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Half-reaction Noun

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[haf ree-ak-shun]

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Half-reaction

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The distinct oxidation or reduction part of a redox reaction, showing either the loss or gain of electrons.

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Example: This diagram shows a battery (voltaic cell) where a chemical reaction is split into two parts. One half-reaction shows zinc losing electrons, and the other shows copper gaining those electrons.

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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 generates electrical energy from chemical reactions or uses electrical energy to drive non-spontaneous chemical reactions.

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Example: This diagram shows an electrochemical cell where chemical reactions create electricity. Electrons flow from the zinc anode to the copper cathode, powering a light bulb.

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Voltaic Cell Noun

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[vol-tey-ik sel]

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Voltaic Cell

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An electrochemical cell that uses a spontaneous redox reaction to convert stored chemical energy into electrical energy.

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Example: A voltaic cell converts chemical energy into electrical energy. A zinc anode releases electrons that travel through a wire to a copper cathode.

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Half-cell Noun

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[haf-sel]

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Half-cell

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One of two compartments in an electrochemical cell where either the oxidation or the reduction half-reaction occurs.

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Example: This diagram shows a complete voltaic cell, where each beaker with its electrode and solution (e.g., Zn in ZnSO4) represents one half-cell.

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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 in an electrochemical cell.

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Example: In a battery (a voltaic cell), the anode is the negative electrode where electrons leave, and the cathode is the positive electrode where electrons arrive.

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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 at which the oxidation half-reaction occurs, releasing electrons into the external circuit.

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Example: In a voltaic cell (battery), the anode is the negative electrode where electrons are released, flowing through a circuit to power devices like a lightbulb.