Consider the following reaction Mg(s)+2HBrO(aq)---> Mg(BrO3)2 (aq) + H2(g) 1. Which reactant atom or ion is being oxidized? 2. Which reactant atom or ion is being reduced. 3. Identify the reactant acting as the oxidizing agent. 4. Identify the reactant acting as the reducing agent. 5. Draw the structural diagram of BrO_3^(1-). 6. Determine the oxidation number of Br in BrO_3^(1-).
Question
Consider the following reaction
Mg(s)+2HBrO(aq)---> Mg(BrO3)2 (aq) + H2(g)
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Which reactant atom or ion is being oxidized?
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Which reactant atom or ion is being reduced.
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Identify the reactant acting as the oxidizing agent.
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Identify the reactant acting as the reducing agent.
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Draw the structural diagram of BrO_3^(1-).
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Determine the oxidation number of Br in BrO_3^(1-).
Solution
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The reactant atom being oxidized is Mg. In the reaction, Mg loses two electrons to form Mg2+, which is a process of oxidation.
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The reactant ion being reduced is HBrO. In the reaction, HBrO gains an electron to form BrO3-, which is a process of reduction.
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The reactant acting as the oxidizing agent is HBrO. An oxidizing agent causes another substance to be oxidized while itself being reduced.
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The reactant acting as the reducing agent is Mg. A reducing agent causes another substance to be reduced while itself being oxidized.
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The structural diagram of BrO3- is a bromine atom in the center surrounded by three oxygen atoms. Each oxygen atom is connected to the bromine atom by a single bond, and each oxygen atom also has two lone pairs of electrons. The bromine atom also has a lone pair of electrons.
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The oxidation number of Br in BrO3- is +5. This is calculated by assigning an oxidation number of -2 to each oxygen atom (for a total of -6) and then solving for the oxidation number of Br that would make the total charge of the ion equal to -1.
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