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Chapter 19: Q6 E (page 1092)

Which of the following is the strongest oxidizing agent: \(VO_4^3,CrO_4^{2 - },\)or \(MnO_4^ - \)?

Short Answer

Expert verified

The strongest oxidation agent is \(MnO_4^ - \)

Step by step solution

01

Oxidation agent:

An oxidizing agent is usually a chemical species that tends to oxidize other substances, by increasing oxidation state of the substance by making it lose electrons.

02

Compairing the given oxidation agent:

The strongest oxidation agent can easily accept electron;

  1. \(MnO_4^ - + 8{H^ + } + 5{e^ - } \to M{n^{2 + }} + 4{H_2}O\) E = +1.507V
  2. \(CrO_4^{2 - } + 4{H_2}O + 3{e^ - } \to Cr{(OH)_3} + 5O{H^ - }\) E = -0.13V
  3. \(VO_4^{3 - } + 6{H^ + } + 2{e^ - } \to V{O^ - } + 3{H_2}O\) E = +1.256V

Hence, the strongest oxidation agent is \(MnO_4^ - \)

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Most popular questions from this chapter

Indicate the coordination number for the central metal atom in each of the following coordination compounds:

\(\begin{aligned}{}(a)\left( {Pt{{\left( {{H_2}O} \right)}_2}B{r_2}} \right)\\(b)\left( {Pt\left( {N{H_3}} \right)(py)(Cl)(Br)} \right)\left( {py = } \right.pyridine,\left. {{C_5}{H_5}\;N} \right)\\(c)\left( {Zn{{\left( {N{H_3}} \right)}_2}C{l_2}} \right)\\(d)\left( {Zn\left( {N{H_3}} \right)(py)(Cl)(Br)} \right)\\(e)\left( {Ni{{\left( {{H_2}O} \right)}_4}C{l_2}} \right)\\(f){\left( {Fe{{(en)}_2}{{(CN)}_2}} \right)^ + }\left( {en = } \right.ethylenediamine,\left. {{C_2}{H_8}\;{N_2}} \right)\end{aligned}\)

Predict whether the carbonate ligand \(C{O_3}^2\)- will coordinate to a metal center as a monodentate, bidentate, or tridentate ligand.

The following reactions all occur in a blast furnace. Which of these are redox reactions?

\(\begin{aligned}{l}(a)3F{e_2}{O_3}(s) + CO(g) \to 2F{e_3}{O_4}(s) + C{O_2}(g)\\(b)F{e_3}{O_4}(s) + CO(g) \to 3FeO(s) + C{O_2}(g)\\(c)FeO(s) + CO(g) \to Fe(l) + C{O_2}(g)\\(d)C(s) + {O_2}(g) \to C{O_2}(g)\\(e)C(s) + C{O_2}(g) \to 2CO(g)\\(f)CaC{O_3}(s) + CaO(s) \to C{O_2}(g)\\(g)CaO(s) + Si{O_2}(s) \to CaSi{O_3}(l)\end{aligned}\)

Sketch the structures of the following complexes. Indicate any cis, trans, and optical isomers.

\(\begin{aligned}{}(a)\left( {Pt{{\left( {{H_2}O} \right)}_2}B{r_2}} \right)\\(b)\left( {Pt\left( {N{H_3}} \right)(py)(Cl)(Br)} \right)\\(c)\left( {Zn{{\left( {N{H_3}} \right)}_3}Cl} \right)\\(d){\left( {Pt{{\left( {N{H_3}} \right)}_3}Cl} \right)^ + }\\(e)\left( {Ni{{\left( {{H_2}O} \right)}_4}C{l_2}} \right)\\(f){\left( {Co{{\left( {{C_2}{O_4}} \right)}_2}C{l_2}} \right)^{3 - }}\end{aligned}\)

Is it possible for a complex of a metal in the transition series to have six unpaired electrons? Explain.
See all solutions

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