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Chapter 23: Problem 12

Complete the following statements for the complex ion \(\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{-}:\) (a) The oxidation number of Cr is _____ (b) The coordination number of Cr is _____ . (c)_____ is a bidentate ligand.

Short Answer

Expert verified
(a) The oxidation number of Cr is +3 (b) The coordination number of Cr is 6 (c) Oxalate (\(C_2O_4^{2-}\)) is a bidentate ligand.

Step by step solution

01

Determine the Oxidation Number of Chromium Cr

The overall charge of the complex ion is -1. The oxalate ion (\(C_2O_4^{2-}\)) has a charge of -2 and there are two of them, contributing -4. The water molecules are neutral, contributing 0. Therefore, the oxidation number of Cr must balance this to -1. If you sum -4 with the oxidation state of Cr and it equals -1, it gives the oxidation state of Cr as +3.
02

Determine the Coordination Number of Chromium Cr

The coordination number is determined by the number of ligand bonds to the metal ion. Here, the oxalate ion (\(C_2O_4^{2-}\)) is a bidentate ligand, which means it can form two bonds. As there are two oxalate ions, they form 4 bonds. Additionally, the two water molecules each form one bond. Thus, the total bonding sites or coordination number come up to 6.
03

Identify the Bidentate Ligand

A bidentate ligand attaches to the central atom at two points. In the given complex ion, the oxalate ion (\(C_2O_4^{2-}\)) is the bidentate ligand as it can bind through two oxygen atoms, making it a bidentate ligand.

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Most popular questions from this chapter

The complex ion \(\left[\mathrm{Ni}(\mathrm{CN})_{2} \mathrm{Br}_{2}\right]^{2-}\) has a squareplanar geometry. Draw the structures of the geometric isomers of this complex.

Which is a stronger oxidizing agent in aqueous solution, \(\mathrm{Mn}^{3+}\) or \(\mathrm{Cr}^{3+} ?\) Explain your choice.

Which of the following hydrated cations are colorless: \(\mathrm{Fe}^{2+}(a q), \mathrm{Zn}^{2+}(a q), \mathrm{Cu}^{+}(a q), \mathrm{Cu}^{2+}(a q)\) \(\mathrm{V}^{5+}(a q), \mathrm{Ca}^{2+}(a q), \mathrm{Co}^{2+}(a q), \mathrm{Sc}^{3+}(a q), \mathrm{Pb}^{2+}(a q) ?\) Explain your choice.

Manganese forms three low-spin complex ions with the cyanide ion with the formulas \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{5-},\) \(\left[\mathrm{Mn (\mathrm{CN})_{6}\right]^{4-},\) and \(\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]^{3-} .\) For each complex ion, determine the oxidation number of Mn and the number of unpaired \(d\) electrons present.

Consider the following two ligand exchange reactions: \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+6 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}+6 \mathrm{H}_{2} \mathrm{O}\) $$ \left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+3 \mathrm{en} \rightleftharpoons\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}+6 \mathrm{H}_{2} \mathrm{O} $$ (a) Which of the reactions should have a larger \(\Delta S^{\circ} ?\) (b) Given that the Co-N bond strength is approximately the same in both complexes, which reaction will have a larger equilibrium constant? Explain your choices.
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