Chemical Bonds

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Solute Noun

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[sol-yoot]

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Solute

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A substance whose particles are dissolved in a solvent to create a solution, which can exist as a solid, liquid, or gas.

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Example: This diagram shows a solid ionic compound (the solute) breaking apart into individual ions that become surrounded by water molecules, which is the process of dissolving.

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Solvent Noun

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[sol-vent]

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Solvent

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The substance in which a solute dissolves to form a solution, typically being the component present in the largest amount.

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Example: This diagram shows a solvent, the liquid part of a solution, which dissolves the solute particles that are mixed into it.

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Dissociation Noun

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[dih-soh-see-ay-shun]

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Dissociation

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The process in which an ionic compound separates into its constituent ions when it dissolves in a solvent.

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Example: When an acid like hydrogen chloride (HCl) is in water, it breaks apart, or dissociates, into a positive hydrogen ion and a negative chloride ion.

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Dispersion Noun

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[dih-spur-zhun]

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Dispersion

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The process of dissolving where a substance breaks into smaller pieces that spread evenly throughout the solvent.

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Example: Uneven electron distribution in nonpolar molecules creates temporary dipoles, resulting in a weak attractive force called a dispersion force between them.

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Ionization Noun

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[eye-on-ih-zay-shun]

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Ionization

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The chemical process where neutral molecules react with a solvent to gain or lose electrons, thereby forming ions.

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Example: A neutral sodium atom (Na) loses one electron from its outer shell, resulting in a sodium ion (Na+) with a positive charge.

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Heat of solution Noun

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[heet uv suh-loo-shun]

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Heat of solution

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The net amount of heat energy that is either absorbed or released when a solute dissolves in a solvent.

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Example: This diagram shows a simple calorimeter, a tool used to measure the heat released or absorbed (the heat of solution) when a substance dissolves in a liquid.

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Solubility Noun

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[sol-yuh-bil-i-tee]

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Solubility

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The maximum amount of a solute that can dissolve in a specific amount of solvent at a constant temperature.

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Example: This diagram shows a salt crystal dissolving. Polar water molecules pull the positive (Na+) and negative (Cl-) ions apart, surrounding them and forming a solution.

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Unsaturated solution Noun

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[un-sach-uh-rey-tid suh-loo-shun]

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Unsaturated solution

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A solution containing less solute than the maximum amount that can be dissolved at a specific temperature.

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Example: This diagram shows that when a solute (carbon dioxide) is dissolved in a solvent (water), it forms a solution that is unsaturated because more solute could still be dissolved.

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Saturated solution Noun

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[sach-uh-rey-tid suh-loo-shun]

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Saturated solution

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A solution containing the maximum amount of solute that can be dissolved in the solvent at a given temperature.

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Example: This diagram shows a saturated solution in the middle flask, where the solvent has dissolved the maximum amount of solute and can hold no more.

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Supersaturated solution Noun

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[soo-per-sach-uh-rey-tid suh-loo-shun]

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Supersaturated solution

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An unstable solution containing more dissolved solute than it can normally hold at a specific temperature.

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Example: A supersaturated solution holds more dissolved solute than is normally possible; when disturbed, this unstable solution releases the excess solute to form solid crystals.