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Chapter 23: Problem 37

Write the names of the following compounds, using the standard nomenclature rules for coordination complexes: (a) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{NO}_{3}\) (b) \(\mathrm{Hg}\left[\mathrm{Co}(\mathrm{SCN})_{4}\right]\) (c) $\left[\mathrm{Ru}\left(\mathrm{PPh}_{3}\right)_{3} \mathrm{Cl}_{3}\right]$ (d) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{CO}_{3}\right]_{2} \mathrm{SO}_{4}$

Short Answer

Expert verified
The names of the coordination complexes are: (a) di_ammine_silver(I) nitrate (b) mercury(II) tetra_thiocyanatocobalt(III) (c) tri_phosphinetriphenyl_tri_chlororuthenium (d) penta_amminecarbonatocobalt(II) sulfate

Step by step solution

01

Naming Complex (a)

The given complex is \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{NO}_{3}\), where 'Ag' is the metal, 'NH3' is the ligand, and 'NO3' is the counter-ion. Naming the complex: 1. Metal name: Silver (for Ag) 2. Ligand name: di_ammine (for two NH3 ligands) 3. Charge: Since Ag has a +1 charge, the entire complex ion has a +1 charge as well. Therefore, we use (I) for the overall charge. 4. Counter-ion name: Nitrate (for NO3) Hence, the name of the compound is: di_ammine_silver(I) nitrate.
02

Naming Complex (b)

The given complex is \(\mathrm{Hg}\left[\mathrm{Co}(\mathrm{SCN})_{4}\right]\), where 'Hg' is the counter-ion and '[Co(SCN)4]' is the coordination complex with 'Co' as the metal and 4 'SCN' ligands. Naming the complex: 1. Metal name: Cobalt (for Co) 2. Ligand name: tetra_thiocyanato (for four SCN ligands) 3. Charge: Cobalt generally has +2 and +3 oxidation states. Since there are 4 negatively charged SCN ligands, the charge on Co in this complex is +3. Therefore, we use (III) for the overall charge. 4. Counter-ion name: Mercury(II) (for Hg with a +2 charge) The name of the compound is: mercury(II) tetra_thiocyanatocobalt(III).
03

Naming Complex (c)

The given complex is \(\left[\mathrm{Ru}\left(\mathrm{PPh}_{3}\right)_{3}\mathrm{Cl}_{3}\right]\), with 'Ru' as the metal, 3 'PPh3' and 3 'Cl' as ligands. Naming the complex: 1. Metal name: Ruthenium (for Ru) 2. Ligand names: tri_phosphinetriphenyl(triPPh3 ligands), tri_chloro (three Cl ligands) 3. Charge: There's no overall charge on the complex. Hence, the name of the compound is: tri_phosphinetriphenyl_tri_chlororuthenium.
04

Naming Complex (d)

The given complex is \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5}\mathrm{CO}_{3}\right]_{2} \mathrm{SO}_{4}\), where 'Co' is the metal, 5 'NH3' and 1 'CO3' are the ligands, and 'SO4' is the counter-ion. Naming the complex: 1. Metal name: Cobalt (for Co) 2. Ligand names: penta_ammine (five NH3 ligands), carbonato (one CO3 ligand) 3. Charge: The sulfate ion has a -2 charge, which means the complex ion has a +2 charge. Thus, we use (II) for the overall charge. 4. Counter-ion name: Sulfate (for SO4) The name of the compound is: penta_amminecarbonatocobalt(II) sulfate.

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Most popular questions from this chapter

Draw the crystal-field energy-level diagrams and show the placement of \(d\) electrons for each of the following: (b) \(\left[\mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\), (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (four unpaired electrons), (a high-spin complex), (c) $\left[\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{5}\left(\mathrm{H}_{2} \mathrm{O}\right)\right]^{2+}$ (a low-spin complex), (d) \(\left[\mathrm{IrCl}_{6}\right]^{2-}\) (a low-spin complex), (e) \(\left[\mathrm{Cr}(\mathrm{en})_{3}\right]^{3+}\), (f) \(\left[\mathrm{NiF}_{6}\right]^{4-}\).

The square-planar complex $\left[\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2}\right]$ only forms in one of two possible geometric isomers. Which isomer is not observed: cis or trans?

Consider the following three complexes: \(\left(\right.\) Complex 1) $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Br}_{2}\right] \mathrm{Cl}$ 2) \(\left[\mathrm{Pd}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{ONO})_{2}\right]\) (Complex (Complex 3) $\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right]^{+},$ Which of the three complexes can have (a) geometric isomers, (b) linkage isomers, (c) optical isomers, (d) coordinationsphere isomers?

Sketch the structure of the complex in each of the following compounds and give the full compound name: (a) $c i s-\left[\operatorname{PtBr} \mathrm{Cl}\left(\mathrm{NO}_{2}\right)_{2}\right]^{2-}$ (b) $\left[\mathrm{Mn}(\mathrm{CO})_{3}\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\right]^{+}$ (c) $\left.c i s-\left[\mathrm{Cr} \mathrm{Cl}_{4}\right)\left(\mathrm{OH}_{2}\right)_{2}\right]^{-}$ (d) trans-[Co(OH)(en) \(\left._{2} \mathrm{Cl}\right]^{+}\)

(a) Sketch a diagram that shows the definition of the crystalfield splitting energy \((\Delta)\) for an octahedral crystal-field. \((\mathbf{b})\) What is the relationship between the magnitude of \(\Delta\) and the energy of the \(d-d\) transition for a \(d^{1}\) complex? (c) Calculate \(\Delta\) in $\mathrm{kJ} / \mathrm{mol}\( if a \)d^{1}\( complex has an absorption maximum at \)545 \mathrm{nm}$.
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