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Chapter 23: Problem 62

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.

Short Answer

Expert verified
The colorless hydrated cations among the given ones are Zn2+, Cu+, V5+, Ca2+, Sc3+, and Pb2+

Step by step solution

01

Assess Transition Metals

Firstly, we need to evaluate the electron configuration of each cation. Those that are not transition metals or which have completely full or completely empty d orbitals will be colorless. The transition metals included in the list are Fe, Zn, Cu, V, and Co. Fe2+, Cu+, Cu2+, V5+, and Co2+ are from transition metals.
02

Evaluate Electron Configuration

Next, examine the electron configurations of these transition metal ions: \n- Fe2+ ([Ar]3d6) has partially filled d orbitals.\n- Cu+ ([Ar]3d10) and Cu1+ ([Ar]3d10) have completely filled d orbitals.\n- Cu2+ ([Ar]3d9) has partially filled d orbitals. \n- V5+ ([Kr]) has empty d orbitals. \n- Co2+ ([Ar]3d7) has partially filled d orbitals.
03

Identify Colorless Cations

Using the obtained information, it can be seen that Cu+, Zn2+, V5+, and Ca2+ are colorless due to completely filled or empty d orbitals. The other non-transition metal cations (Sc3+ and Pb2+) are also colorless.

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Most popular questions from this chapter

Explain the following facts: (a) Copper and iron have several oxidation states, whereas zinc has only one. (b) Copper and iron form colored ions, whereas zinc does not.

The \(K_{\mathrm{f}}\) for the complex ion formation between \(\mathrm{Pb}^{2+}\) and EDTA \(^{4-}\) $$ \mathrm{Pb}^{2+}+\mathrm{EDTA}^{4-} \rightleftharpoons \mathrm{Pb}(\mathrm{EDTA})^{2-} $$ is \(1.0 \times 10^{18}\) at \(25^{\circ} \mathrm{C} .\) Calculate \(\left[\mathrm{Pb}^{2+}\right]\) at equilibrium in a solution containing \(1.0 \times 10^{-3} M \mathrm{~Pb}^{2+}\) and \(2.0 \times 10^{-3} M \mathrm{EDTA}^{4-}\)

The \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) complex is more labile than the \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) complex. Suggest an experiment that would prove that \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) is a labile complex.

Explain the following terms: (a) enantiomers, (b) racemic mixtures.

Predict the number of unpaired electrons in the following complex ions: (a) \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4-},(\mathrm{b})\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)
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