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Chapter 21: Problem 7

Figure \(21.17\) shows that the cis isomer of \(\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}^{+}\) is optically active while the trans isomer is not optically active. Is the same true for \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+} ?\) Explain.

Short Answer

Expert verified
Neither the cis nor the trans isomer of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) is optically active, as both isomers lack chiral centers.

Step by step solution

01

Draw the cis and trans isomers

We are given the \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) complex. The compound has a central Co atom surrounded by four NH3 and two Cl ligands. For the cis isomer, the two Cl ligands are adjacent to each other: Cl | NH3-Co-NH3 | \ NH3 NH3 For the trans isomer, the two Cl ligands are opposite to each other: NH3 Cl | \ NH3-Co-NH3 | Cl
02

Identify chiral centers

Now we need to analyze the structures to determine if there are any chiral centers present. In the cis isomer structure, there are no chiral centers because all ligands are not distinct around the cobalt atom, as we have two NH3 ligands. Looking at the trans isomer structure, once again, all the ligands are not distinct around the cobalt atom, as we have two NH3 ligands.
03

Determine if the isomers are optically active

Since neither the cis nor the trans isomers of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) possess any chiral centers, we can conclude that neither of them is optically active. To answer the question: Neither the cis nor the trans isomer of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) is optically active, as both isomers lack chiral centers.

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Most popular questions from this chapter

a. Calculate the molar solubility of AgBr in pure water. \(K_{\text {sp }}\) for AgBr is \(5.0 \times 10^{-13}\) b. Calculate the molar solubility of AgBr in \(3.0 M \mathrm{NH}_{3}\). The overall formation constant for \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) is \(1.7 \times 10^{7}\), that is, \(\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q) \quad K=1.7 \times 10^{7}\) c. Compare the calculated solubilities from parts a and b. Explain any differences. d. What mass of \(\mathrm{AgBr}\) will dissolve in \(250.0 \mathrm{~mL}\) of \(3.0 \mathrm{M} \mathrm{NH}_{3}\) ? e. What effect does adding \(\mathrm{HNO}_{3}\) have on the solubilities calculated in parts a and \(\mathrm{b}\) ?

When aqueous KI is added gradually to mercury(II) nitrate, an orange precipitate forms. Continued addition of KI causes the precipitate to dissolve. Write balanced equations to explain these observations. (Hint: \(\mathrm{Hg}^{2+}\) reacts with \(\mathrm{I}^{-}\) to form \(\mathrm{HgI}_{4}{ }^{2-}\).) Would you expect \(\mathrm{HgL}_{4}{ }^{2-}\) to form colored solutions? Explain.

The complex ion \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) has an absorption maximum at around \(800 \mathrm{~nm}\). When four ammonias replace water, \(\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]^{2+}\), the absorption maximum shifts to around \(600 \mathrm{~nm} .\) What do these results signify in terms of the relative field splittings of \(\mathrm{NH}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}\) ? Explain.

You isolate a compound with the formula \(\mathrm{PtCl}_{4} \cdot 2 \mathrm{KCl}\). From electrical conductance tests of an aqueous solution of the compound, you find that three ions per formula unit are present, and you also notice that addition of \(\mathrm{AgNO}_{3}\) does not cause a precipitate. Give the formula for this compound that shows the complex ion present. Explain your findings. Name this compound.

Would it be better to use octahedral \(\mathrm{Ni}^{2+}\) complexes or octahedral \(\mathrm{Cr}^{2+}\) complexes to determine whether a given ligand is a strong-field or weak-field ligand by measuring the number of unpaired electrons? How else could the relative ligand field strengths be determined?
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