Questions: For each of the following net ionic equations, which species is being oxidized and which is being reduced? Which species is the reducing agent? Which species is the oxidizing agent? a) Cr^+ + Sn^4+ -> Cr^3+ + Sn^2+ b) 3 Hg^2+ + 2 Fe -> 3 Hg + 2 Fe^3+ c) 2 As + 3 Cl2 -> 2 AsCl3

For each of the following net ionic equations, which species is being oxidized and which is being reduced? Which species is the reducing agent? Which species is the oxidizing agent? a) Cr^+ + Sn^4+ -> Cr^3+ + Sn^2+ b) 3 Hg^2+ + 2 Fe -> 3 Hg + 2 Fe^3+ c) 2 As + 3 Cl2 -> 2 AsCl3
Transcript text: 7) For each of the following net ionic equations, which species is being oxidized and which is being reduced? Which species is the reducing agent? Which species is the oxidizing agent? a) $\mathrm{Cr}^{+}+\mathrm{Sn}^{4+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{Sn}^{2+}$ b) $3 \mathrm{Hg}^{2+}+2 \mathrm{Fe} \longrightarrow 3 \mathrm{Hg}+2 \mathrm{Fe}^{3+}$ c) $2 \mathrm{As}+3 \mathrm{Cl}_{2} \longrightarrow 2 \mathrm{AsCl}_{3}$
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Solution

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Solution Steps

Step 1: Identify Oxidation States

First, we need to determine the oxidation states of each element in the reactants and products.

a) \(\mathrm{Cr}^{+}+\mathrm{Sn}^{4+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{Sn}^{2+}\)

  • \(\mathrm{Cr}^{+}\): Oxidation state of Cr is +1.
  • \(\mathrm{Sn}^{4+}\): Oxidation state of Sn is +4.
  • \(\mathrm{Cr}^{3+}\): Oxidation state of Cr is +3.
  • \(\mathrm{Sn}^{2+}\): Oxidation state of Sn is +2.

b) \(3 \mathrm{Hg}^{2+}+2 \mathrm{Fe} \longrightarrow 3 \mathrm{Hg}+2 \mathrm{Fe}^{3+}\)

  • \(\mathrm{Hg}^{2+}\): Oxidation state of Hg is +2.
  • \(\mathrm{Fe}\): Oxidation state of Fe is 0.
  • \(\mathrm{Hg}\): Oxidation state of Hg is 0.
  • \(\mathrm{Fe}^{3+}\): Oxidation state of Fe is +3.

c) \(2 \mathrm{As}+3 \mathrm{Cl}_{2} \longrightarrow 2 \mathrm{AsCl}_{3}\)

  • \(\mathrm{As}\): Oxidation state of As is 0.
  • \(\mathrm{Cl}_{2}\): Oxidation state of Cl is 0.
  • \(\mathrm{AsCl}_{3}\): Oxidation state of As is +3 and Cl is -1.
Step 2: Determine Changes in Oxidation States

Next, we identify which species are oxidized and reduced by observing changes in their oxidation states.

a) \(\mathrm{Cr}^{+}+\mathrm{Sn}^{4+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{Sn}^{2+}\)

  • Cr: +1 to +3 (oxidized, loses electrons)
  • Sn: +4 to +2 (reduced, gains electrons)

b) \(3 \mathrm{Hg}^{2+}+2 \mathrm{Fe} \longrightarrow 3 \mathrm{Hg}+2 \mathrm{Fe}^{3+}\)

  • Hg: +2 to 0 (reduced, gains electrons)
  • Fe: 0 to +3 (oxidized, loses electrons)

c) \(2 \mathrm{As}+3 \mathrm{Cl}_{2} \longrightarrow 2 \mathrm{AsCl}_{3}\)

  • As: 0 to +3 (oxidized, loses electrons)
  • Cl: 0 to -1 (reduced, gains electrons)
Step 3: Identify Reducing and Oxidizing Agents

The species that is oxidized is the reducing agent, and the species that is reduced is the oxidizing agent.

a) \(\mathrm{Cr}^{+}+\mathrm{Sn}^{4+} \longrightarrow \mathrm{Cr}^{3+}+\mathrm{Sn}^{2+}\)

  • Reducing agent: \(\mathrm{Cr}^{+}\)
  • Oxidizing agent: \(\mathrm{Sn}^{4+}\)

b) \(3 \mathrm{Hg}^{2+}+2 \mathrm{Fe} \longrightarrow 3 \mathrm{Hg}+2 \mathrm{Fe}^{3+}\)

  • Reducing agent: \(\mathrm{Fe}\)
  • Oxidizing agent: \(\mathrm{Hg}^{2+}\)

c) \(2 \mathrm{As}+3 \mathrm{Cl}_{2} \longrightarrow 2 \mathrm{AsCl}_{3}\)

  • Reducing agent: \(\mathrm{As}\)
  • Oxidizing agent: \(\mathrm{Cl}_{2}\)

Final Answer

a)

  • Oxidized: \(\mathrm{Cr}^{+}\)
  • Reduced: \(\mathrm{Sn}^{4+}\)
  • Reducing agent: \(\mathrm{Cr}^{+}\)
  • Oxidizing agent: \(\mathrm{Sn}^{4+}\)

\(\boxed{\text{Oxidized: } \mathrm{Cr}^{+}, \text{ Reduced: } \mathrm{Sn}^{4+}, \text{ Reducing agent: } \mathrm{Cr}^{+}, \text{ Oxidizing agent: } \mathrm{Sn}^{4+}}\)

b)

  • Oxidized: \(\mathrm{Fe}\)
  • Reduced: \(\mathrm{Hg}^{2+}\)
  • Reducing agent: \(\mathrm{Fe}\)
  • Oxidizing agent: \(\mathrm{Hg}^{2+}\)

\(\boxed{\text{Oxidized: } \mathrm{Fe}, \text{ Reduced: } \mathrm{Hg}^{2+}, \text{ Reducing agent: } \mathrm{Fe}, \text{ Oxidizing agent: } \mathrm{Hg}^{2+}}\)

c)

  • Oxidized: \(\mathrm{As}\)
  • Reduced: \(\mathrm{Cl}_{2}\)
  • Reducing agent: \(\mathrm{As}\)
  • Oxidizing agent: \(\mathrm{Cl}_{2}\)

\(\boxed{\text{Oxidized: } \mathrm{As}, \text{ Reduced: } \mathrm{Cl}_{2}, \text{ Reducing agent: } \mathrm{As}, \text{ Oxidizing agent: } \mathrm{Cl}_{2}}\)

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