Oxidation and Reduction

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Oxidation-Reduction Reaction Noun

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[ok-si-day-shun ri-duk-shun ree-ak-shun]

Back

Oxidation-Reduction Reaction

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A chemical reaction, also known as a redox reaction, in which electrons are transferred from one substance to another.

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Example: This diagram shows a sodium atom losing an electron (oxidation) and a chlorine atom gaining it (reduction), demonstrating the electron transfer in a redox reaction.

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Oxidation Noun

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[ok-si-day-shun]

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Oxidation

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The complete or partial loss of electrons from a reacting substance, resulting in an increase in its oxidation number.

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Example: This diagram shows that oxidation is the process where an atom (A) loses an electron, becoming positively charged (A+), during a chemical reaction.

Front

Reduction Noun

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[ri-duk-shun]

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Reduction

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The complete or partial gain of electrons by a reacting substance, resulting in a decrease in its oxidation number.

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Example: This diagram shows that reduction is the process where an atom or molecule (B) gains an electron, which is a key part of a redox reaction.

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Oxidizing Agent Noun

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[ok-si-dy-zing ay-jent]

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Oxidizing Agent

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A substance that causes oxidation by accepting electrons from another substance, thereby becoming reduced in the chemical reaction.

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Example: This diagram shows an oxidizing agent (B) taking electrons from a reducing agent (A). By gaining electrons, the oxidizing agent itself becomes reduced.

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Reducing Agent Noun

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[ri-doo-sing ay-jent]

Back

Reducing Agent

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A substance that causes reduction by donating electrons to another substance, thereby becoming oxidized in the chemical reaction.

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Example: Substance A is the reducing agent because it loses electrons and becomes oxidized, causing substance B to gain electrons and become reduced.

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Oxidation Number Noun

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[ok-si-day-shun num-ber]

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Oxidation Number

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A number assigned to an atom or ion to indicate its degree of oxidation or reduction in a chemical species.

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Example: This diagram shows a water molecule (H₂O). The numbers show the oxidation number for each atom: +1 for each hydrogen and -2 for oxygen.

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Electronegativity Noun

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[eh-lek-tro-neg-a-tiv-i-tee]

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Electronegativity

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A measure of the tendency of an atom to attract a bonding pair of electrons when it forms a chemical bond.

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Example: The highly electronegative oxygen atom pulls electrons from the two hydrogen atoms to form shared bonds in a water molecule.

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Rust Noun

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[ruhst]

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Rust

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The common name for iron oxide, a reddish-brown compound formed when iron oxidizes in the presence of oxygen and moisture.

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Example: This diagram shows that iron combines with water and oxygen in a chemical reaction to form iron oxide, a new substance we call rust.

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Electroplating Noun

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[eh-lek-tro-play-ting]

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Electroplating

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A process that uses redox reactions and an electric current to deposit a thin layer of metal onto a conductive object.

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Example: This diagram shows electroplating, where a battery powers a process. The silver bar (anode) loses silver ions (oxidation), which then coat the spoon (cathode) (reduction).

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Monatomic Ion Noun

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[mon-a-tom-ik eye-on]

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Monatomic Ion

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An ion consisting of a single atom that has gained or lost one or more electrons, giving it a net charge.

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Example: A neutral sodium atom loses its single outer electron, resulting in more protons than electrons, which forms a positively charged monatomic ion (Na⁺).