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Chapter 23: Problem 18

Write the formulas for each of the following ions and compounds: (a) bis(ethylenediamine)dichlorochromium(III), (b) pentacarbonyliron(0), (c) potassium tetracyanocuprate(II), (d) tetraammin eaquachlorocobalt(III) chloride.

Short Answer

Expert verified
The formulas are: (a) \(\text{[Cr(en)}_2\text{Cl}_2\text{]Cl}\), (b) \(\text{Fe(CO)}_5\), (c) \(\text{K}_2\text{[Cu(CN)}_4\text{]}\), (d) \(\text{[Co(NH}_3\text{)}_4\text{H}_2\text{O Cl]Cl}_2\)

Step by step solution

01

Breaking down the constituents for (a)

In 'bis(ethylenediamine)dichlorochromium(III)', two 'ethylenediamine' ligands and two 'chloride' ligands are surrounding the central 'chromium' atom which is in its +3 oxidation state. The formula for ethylenediamine is \(\text{en}\) and for chloride is \(\text{Cl}^-\). Thus, the chemical formula becomes \(\text{[Cr(en)}_2\text{Cl}_2\text{]Cl}\) to maintain charge balance.
02

Breaking down the constituents for (b)

For 'pentacarbonyliron(0)', the prefix 'penta-' means there are five 'carbonyl' ligands surrounding the 'iron' atom, which is in its 0 oxidation state. The chemical formula for carbonyl is \(\text{CO}\). Thus, the resulting chemical formula is \(\text{Fe(CO)}_5\) .
03

Breaking down the constituents for (c)

In 'potassium tetracyanocuprate(II)', the prefix 'tetra-' indicates there are four 'cyanide' ligands in the complex ion which has a 'copper' atom in a +2 oxidation state at its center. The formula for cyanide is \(\text{CN}^-\). The compound also contains 'potassium' ions. Thus, the full chemical formula is \(\text{K}_2\text{[Cu(CN)}_4\text{]}\) to ensure electrical neutrality as the complex ion carries a -2 charge.
04

Breaking down the constituents for (d)

In 'tetraammineaquachlorocobalt(III) chloride', the 'tetra-' prefix means there are four 'ammine' ligands present, 'aqua' indicates there is one water ligand, and 'chloro' indicates one chloride ligand. These are surrounding the 'cobalt' atom that is in the +3 oxidation state. Moreover, the 'chloride' at the end of the name infers that chloride ions are also present. So, the chemical formula is \(\text{[Co(NH}_3\text{)}_4\text{H}_2\text{O Cl]Cl}_2\), maintaining electrical neutrality.

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Most popular questions from this chapter

Give the oxidation numbers of the metals in the following species: (a) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right],\) (b) \(\mathrm{K}_{3}\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (c) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

For the same type of ligands, explain why the crystal field splitting for an octahedral complex is always greater than that for a tetrahedral complex.

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.

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.

A solution made by dissolving \(0.875 \mathrm{~g}\) of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) in \(25.0 \mathrm{~g}\) of water freezes at \(-0.56^{\circ} \mathrm{C}\) Calculate the number of moles of ions produced when 1 mole of \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{3}\) is dissolved in water and suggest a structure for the complex ion present in this compound.
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