Naming Ionic Compounds

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Ionic Bond Noun

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[eye-on-ik bond]

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Ionic Bond

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An electrostatic attraction that holds oppositely charged ions, typically a metal and a nonmetal, close together in a compound.

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Example: A neutral sodium (Na) atom transfers one electron to a neutral chlorine (Cl) atom, creating a positive sodium ion (Na+) and a negative chloride ion (Cl-).

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Cation Noun

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[kat-eye-on]

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Cation

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A positively charged ion that is formed when a neutral atom, typically a metal, loses one or more electrons.

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Example: A neutral sodium atom (Na) loses its single outer electron, resulting in a positively charged sodium ion (Na+), which is a cation.

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Anion Noun

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[an-eye-on]

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Anion

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A negatively charged ion that is formed when a neutral atom, typically a nonmetal, gains one or more electrons.

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Example: A neutral chlorine atom gains one electron in its outer shell, becoming a negatively charged chloride ion (anion) with more electrons than protons.

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Oxidation-Reduction Reaction Noun

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

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Oxidation-Reduction Reaction

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A type of chemical reaction that involves the transfer of one or more electrons from one reactant to another.

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Example: In a reaction, one atom (A) loses an electron, which is called oxidation. Another atom (B) gains that electron, which is called reduction.

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Oxidation Noun

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[ok-si-day-shun]

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Oxidation

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A chemical process characterized by the full or partial loss of electrons from an atom or ion during a reaction.

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Example: An apple slice turns brown when exposed to air, showing a common example of an oxidation reaction.

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Reduction Noun

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[ree-duk-shun]

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Reduction

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A chemical process characterized by the full or partial gain of electrons by an atom or ion during a reaction.

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Example: This diagram shows that atom B is "reduced" when it gains an electron from atom A, changing it into a negatively charged ion (anion).

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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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An equation showing either the oxidation or the reduction part of a redox reaction, including the electrons gained or lost.

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Example: This image does not illustrate a half-reaction. It shows three complete redox reactions with their corresponding oxidation states, which is a related but different concept.

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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 in a compound to represent its degree of oxidation or the charge it would have.

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Example: This Bohr model of an oxygen atom shows it has 6 electrons in its outer shell. To become stable, it will gain 2 electrons, giving it an oxidation number of -2.

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Transition Metals Noun

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[tran-zish-un met-uls]

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Transition Metals

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A group of elements that can form multiple stable ions, each with a different positive charge or oxidation state.

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Example: Transition metals, like iron and copper, form colorful ionic compounds and require a Roman numeral in their name to show the metal's specific charge.

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Formula Unit Noun

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[for-myoo-luh yoo-nit]

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Formula Unit

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The simplest whole-number ratio of ions present in an ionic compound, representing its empirical formula in a crystal lattice.

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Example: This diagram shows the repeating crystal lattice structure of sodium chloride (NaCl). A formula unit is the simplest ratio of ions, one Na⁺ to one Cl⁻.