Almost all metals are reducing agents but not as powerful as the alkali and alkaline earth...

  

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Almost all metals are reducing agents but not as powerful as the alkali and alkaline earth metals. In most reduction reactions, metals donate electrons to the substrate directly. However, under appropriate conditions it is possible to prepare solutions of electrons (solvated electrons). For example, when Na is dissolved in liquid NH3 a blue colored solution is formed. Na(s) + excess NH3(1) → Na (NH3) + e¯(NH3) To prepare solvated electrons the vessels must be very clean and dry. Presence of impurities like Fe(III) (say, from a rusty spatula) can lead to the formation of NaNH2 and H2 gas. Na(s) + excess NH3(1) Nat (NH3) + NH2 (NH3) + H2(g) Almost all metals are reducing agents but not as powerful as the alkali and alkaline earth metals. In most reduction reactions, metals donate electrons to the substrate directly. However, under appropriate conditions it is possible to prepare solutions of electrons (solvated electrons). For example, when Na is dissolved in liquid NH3 a blue colored solution is formed. Na(s) + excess NH3(1) → Na (NH3) + e¯(NH3) To prepare solvated electrons the vessels must be very clean and dry. Presence of impurities like Fe(III) (say, from a rusty spatula) can lead to the formation of NaNH2 and H2 gas. Na(s) + excess NH3(1) Nat (NH3) + NH2 (NH3) + H2(g)