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Chapter 20: Problem 39

A concentrated aqueous copper(II) chloride solution is bright green in color. When diluted with water, the solution becomes light blue. Explain.

Short Answer

Expert verified
The color difference in the copper(II) chloride solution before and after dilution is due to changes in the electronic environment of the copper ion. A concentrated solution results in green colour due to lesser d-d transitions, while dilution causes an increase in the d-d transitions and results in a light blue colour.

Step by step solution

01

Identify the Compound

Firstly, recognize that copper(II) chloride is a transition metal complex. In aqueous solution, it exists as the complex ion [Cu(H2O)6]2+.
02

Determining the Cause of the Color Change

The color of transition metal complexes is based on the d-d transition of electrons. In a concentrated solution, the water molecules are able to move less freely and hence are less able to contribute to the d-d transitions resulting in the green color. As the number of water molecules increases in relation to copper ions (dilution), the water molecules are more able to contribute to the d-d transitions. This results in greater d-d transitions and the observed colour change to light blue.
03

Conclusion

Thus, it can be concluded that the color difference in the copper(II) chloride solution before and after dilution is due to changes in the electronic environment of copper ions in solution. When more water is added, the increased number of water molecules relative to copper ions effects the observed colour change.

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Most popular questions from this chapter

The absorption maximum for the complex ion \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) occurs at \(470 \mathrm{nm}\). (a) Predict the color of the complex and (b) calculate the crystal field splitting in kilojoules per mole.

A student in 1895 prepared three chromium coordination compounds having the same formulas of \(\mathrm{CrCl}_{3}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\) with these properties: Write modern formulas for these compounds and suggest a method for confirming the number of \(\mathrm{Cl}^{-}\) ions present in solution in each case. (Hint: Some of the compounds may exist as hydrates, which are compounds that have a specific number of water molecules attached to them. The \(\mathrm{Cr}\) has a coordination number of 6 in all three compounds.)

How many geometric isomers are in these species: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{-},(\mathrm{b})\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right] ?\)

Give the oxidation numbers of the metals in these species: (a) \(\mathrm{Na}_{2} \mathrm{MoO}_{4}\) (b) \(\mathrm{MgWO}_{4}\), (c) \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\)

Define the terms (a) labile complex, (b) inert complex.
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