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An electride is an ionic compound in which the anion is an electron. The first compounds to be studied in depth that were electrides were solutions of alkali metals in ammonia. For example if sodium metal is disolved in ammonia the resulting blue solution is made up of solvated sodium cations and solvated free electrons. This solution is paramagnetic, conductive and is an excellent reducing agent, as used in a Birch Reduction. It slowly loses it's colour as the electrons reduce ammonia.

Crystalline electride solids are also known, for example $[Cs(2,2,2-crypt)_{2}]e$ , which is blue/black in colour and exibits paramagnetism.

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	An electride is an ionic compound in which the anion is an [[electron]]. The first compounds to be studied in depth that were electrides were solutions of [[alkali metals]] in [[ammonia]]. For example if [[sodium]] metal is disolved in ammonia the resulting blue solution is made up of [[solvated]] sodium cations and solvated free electrons. This solution is [[paramagnetic]], [[conductive]] and is an excellent [[reducing agent]], as used in a [[Birch Reduction]]. It slowly loses it's colour as the electrons reduce ammonia.		An electride is an ionic compound in which the [[anion]] is an [[electron]]. The first compounds to be studied in depth that were electrides were solutions of [[alkali metals]] in [[ammonia]]. For example if [[sodium]] metal is disolved in ammonia the resulting blue solution is made up of [[solvated]] sodium cations and solvated free electrons. This solution is [[paramagnetic]], [[conductive]] and is an excellent [[reducing agent]], as used in a [[Birch Reduction]]. It slowly loses it's colour as the electrons reduce ammonia.

	Crystalline electride solids are also known, for example <math>[Cs(2,2,2-crypt)_2]e</math>, which is blue/black in colour and exibits paramagnetism.		Crystalline electride solids are also known, for example <math>[Cs(2,2,2-crypt)_2]e</math>, which is blue/black in colour and exibits paramagnetism.