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Chapter 24: Problem 9

Draw plausible structures corresponding to each of the following names. (a) pentamminesulfatochromium(III) ion (b) trioxalatocobaltate(III) ion (c) triamminedichloronitrito-O-cobalt(III)

Short Answer

Expert verified
The detailed structures of the complex ions named are pentamminesulfatochromium(III) ion, trioxalatocobaltate(III) ion and Triamminedichloronitrito-O-cobalt(III) respectively. All structures ensure correct accounting of ionic charges, correct representation of ligands and appropriate labelling of central metal ions.

Step by step solution

01

Draw Pentamminesulfatochromium(III) Ion

The name tells us that the metal is chromium (III) meaning it has a 3+ charge. The ligands are ammonia (NH3 - known as ammine in coordination complexes) and sulfate (SO4 2-). There are 5 ammine and 1 sulfato ligands. Since sulfate has a 2- charge, the five neutral ammine ligands and 3+ Chromium form a complex ion with a net charge of 1+.
02

Draw Trioxalatocobaltate(III) Ion

The metal is cobalt (III) meaning 3+ charge. The ligand is oxalate (C2O4 2-). There are 3 oxalate ligands. The total negative charge from the oxalate ligands is 2- x 3 = -6. Combined with the 3+ charge on cobalt, the overall charge on the entire ion is 3-, so it’s a complex anion.
03

Draw Triamminedichloronitrito-O-cobalt(III)

The metal ion is cobalt (III) meaning 3+ charge. The ligands are ammonia (NH3 - known as ammine in coordination complexes), chloride (Cl-), and nitrite (NO2 -). The nitrito has two different modes of bonding: it can be either nitrito-N or nitrito-O. Here it's nitrito-O as aroused from the name, which means the Oxygen in nitrite bonds to the central cobalt. The entire complex ion has a neutral charge, because the charges of the ligands and the central metal ion balance each other out.

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Most popular questions from this chapter

Write equations to represent the following observations. (a) A quantity of \(\mathrm{CuCl}_{2}(\mathrm{s})\) is dissolved in concentrated HCl(aq) and produces a yellow solution. The solution is diluted to twice its volume with water and assumes a green color. On dilution to ten times its original volume, the solution becomes pale blue. (b) When chromium metal is dissolved in \(\mathrm{HCl}(\mathrm{aq}), \mathrm{a}\) blue solution is produced that quickly turns green. Later the green solution becomes blue-green and then violet.

The most soluble of the following solids in \(\mathrm{NH}_{3}(\mathrm{aq})\) is (a) \(\mathrm{Ca}(\mathrm{OH})_{2} ;\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2} ;\) (c) \(\mathrm{BaSO}_{4} ;\) (d) \(\mathrm{MgCO}_{3}\) (e) \(\overline{\mathrm{Fe}_{2} \mathrm{O}_{3}}\).

Explain the following observations in terms of complex-ion formation. (a) \(\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})\) is soluble in \(\mathrm{NaOH}(\mathrm{aq})\) but insoluble in \(\mathrm{NH}_{3}(\mathrm{aq})\) (b) \(\mathrm{ZnCO}_{3}(\mathrm{s})\) is soluble in \(\mathrm{NH}_{3}(\mathrm{aq}),\) but \(\mathrm{ZnS}(\mathrm{s})\) is not. (c) The molar solubility of AgCl in pure water is about \(1 \times 10^{-5} \mathrm{M} ;\) in \(0.04 \mathrm{M} \mathrm{NaCl}(\mathrm{aq}),\) it is about \(2 \times 10^{-6}; \mathrm{M}\) but in \(1 \mathrm{M} \mathrm{NaCl}(\mathrm{aq}),\) it is about \(8 \times 10^{-5} \mathrm{M}\).

Provide a valence bond description of the bonding in the \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) ion. According to the valence bond description, how many unpaired electrons are there in the \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) complex? How does this prediction compare with that of crystal field theory?

Without performing detailed calculations, show why you would expect the concentrations of the various ammine-aqua complex ions to be negligible compared with that of \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+}\) in a solution having a total \(\mathrm{Cu}(\mathrm{II})\) concentration of \(0.10 \mathrm{M}\) and a total concentration of \(\mathrm{NH}_{3}\) of \(1.0 \mathrm{M}\). Under what conditions would the concentrations of these ammine-aqua complex ions (such as \(\left.\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3} \mathrm{NH}_{3}\right]^{2+}\right)\) become more significant relative to the concentration of \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ?\) Explain.
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