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What is the oxidation state of the central metal ion in K₂[Cr(CN)₆]?
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6. Chemical Quantities & Aqueous Reactions
Calculate Oxidation Numbers
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In the reaction Zn + 2 H^+ → Zn^{2+} + H_2, what is the oxidizing agent?
A
H^+
B
H_2
C
Zn
D
Zn^{2+}
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Identify the species that undergo oxidation and reduction by examining the changes in oxidation states during the reaction.
Write down the oxidation states of each element in the reactants and products: Zn (0), H^+ (+1), Zn^{2+} (+2), and H_2 (0).
Determine which species is oxidized: Zn goes from 0 to +2, so Zn is oxidized (loses electrons).
Determine which species is reduced: H^+ goes from +1 to 0 in H_2, so H^+ is reduced (gains electrons).
Recall that the oxidizing agent is the species that causes oxidation by accepting electrons, which means it is the species being reduced—in this case, H^+.
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