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Chapter 21: Problem 37

Name the following coordination compounds. a. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2}\) b. $\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{I}_{3}$ c. \(\mathrm{K}_{2}\left[\mathrm{PtC}_{4}\right]\) d. \(\mathrm{K}_{4}\left[\mathrm{Pt} \mathrm{C}_{6}\right]\) e. $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}$ f. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\)

Short Answer

Expert verified
a. hexaamminecobalt(III) chloride b. hexaaquacobalt(III) iodide c. potassium tetracyanidoplatinate(II) d. potassium hexacyanidoplatinate(IV) e. pentaamminechloridocobalt(III) chloride f. triamminetrinitritocobalt(III)

Step by step solution

01

1. Identify the cation and anion

The cation is the complex ion \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\), and the anion is \(\mathrm{Cl}^{-}\).
02

2. Name the ligands

The ligand is NH3, which is called ammine.
03

3. Name the complex ion

The complex ion is named as: hexaamminecobalt(III).
04

4. Combine the names

The full name of the compound is: hexaamminecobalt(III) chloride. b. \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{I}_{3}\)
05

1. Identify the cation and anion

The cation is the complex ion \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\), and the anion is \(\mathrm{I}^{-}\).
06

2. Name the ligands

The ligand is H2O, which is called aqua.
07

3. Name the complex ion

The complex ion is named as: hexaaquacobalt(III).
08

4. Combine the names

The full name of the compound is: hexaaquacobalt(III) iodide. c. \(\mathrm{K}_{2}\left[\mathrm{PtC}_{4}\right]\)
09

1. Identify the cation and anion

The cation is \(\mathrm{K}^{+}\), and the anion is the complex ion \(\left[\mathrm{PtC}_{4}\right]^{2-}\).
10

2. Name the ligands

The ligand is cyanide (CN-), which is called cyanido.
11

3. Name the complex ion

The complex ion is named as: tetracyanidoplatinate(II).
12

4. Combine the names

The full name of the compound is: potassium tetracyanidoplatinate(II). d. \(\mathrm{K}_{4}\left[\mathrm{Pt} \mathrm{C}_{6}\right]\)
13

1. Identify the cation and anion

The cation is \(\mathrm{K}^{+}\), and the anion is the complex ion \(\left[\mathrm{PtC}_{6}\right]^{4-}\).
14

2. Name the ligands

The ligand is cyanide (CN-), which is called cyanido.
15

3. Name the complex ion

The complex ion is named as: hexacyanidoplatinate(IV).
16

4. Combine the names

The full name of the compound is: potassium hexacyanidoplatinate(IV). e. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2}\)
17

1. Identify the cation and anion

The cation is the complex ion \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right]^{2+}\), and the anion is \(\mathrm{Cl}^{-}\).
18

2. Name the ligands

The ligands are NH3, called ammine, and Cl-, called chlorido.
19

3. Name the complex ion

The complex ion is named as: pentaamminechloridocobalt(III).
20

4. Combine the names

The full name of the compound is: pentaamminechloridocobalt(III) chloride. f. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3}\left(\mathrm{NO}_{2}\right)_{3}\right]\)
21

1. Name the ligands

The ligands are NH3, called ammine and NO2-, called nitrito.
22

2. Name the complex ion

The complex ion is named as: triamminetrinitritocobalt(III).
23

3. Combine the names

Since the compound is neutral, there is no need to include cation or anion names. The name of the compound is: triamminetrinitritocobalt(III).

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Most popular questions from this chapter

Use standard reduction potentials to calculate $\mathscr{C}^{\circ}, \Delta G^{\circ},\( and \)K$ (at 298 K) for the reaction that is used in production of gold: $$2 \mathrm{Au}(\mathrm{CN})_{2}-(a q)+\mathrm{Zn}(s) \longrightarrow 2 \mathrm{Au}(s)+\mathrm{Zn}(\mathrm{CN})_{4}^{2-}(a q)$$ The relevant half-reactions are $$\begin{aligned} \operatorname{Au}(\mathrm{CN})_{2}^{-}+\mathrm{e}^{-} \longrightarrow \mathrm{Au}+2 \mathrm{CN}^{-} & \mathscr{C}^{\circ}=-0.60 \mathrm{V} \\ \mathrm{Zn}(\mathrm{CN})_{4}^{2-}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn}+4 \mathrm{CN}^{-} & \mathscr{C}^{\circ}=-1.26 \mathrm{V} \end{aligned}$$

Acetylacetone (see Exercise \(45,\) part a), abbreviated acacH, is a bidentate ligand. It loses a proton and coordinates as acac\(^-\) as shown below: Acetylacetone reacts with an ethanol solution containing a salt of europium to give a compound that is 40.1\(\% \mathrm{C}\) and 4.71\(\% \mathrm{H}\) by mass. Combustion of 0.286 \(\mathrm{g}\) of the compound gives 0.112 $\mathrm{g} \mathrm{Eu}_{2} \mathrm{O}_{3} .$ Assuming the compound contains only \(\mathrm{C}, \mathrm{H},\) O, and Eu, determine the formula of the compound formed from the reaction of acetylacetone and the europium salt. (Assume that the compound contains one europium ion.)

Consider aqueous solutions of the following coordination compounds: $\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{I}_{3}, \operatorname{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{4}, \mathrm{Na}_{2} \mathrm{Pt}_{6},$ and \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{3}\) . If aqueous AgNO \(_{3}\) is added to separate beakers containing solutions of each coordination compound, how many moles of AgI will precipitate per mole of transition metal present? Assume that each transition metal ion forms an octahedral complex.

Ammonia and potassium iodide solutions are added to an aqueous solution of \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3} .\) A solid is isolated (compound A), and the following data are collected: i. When 0.105 g of compound A was strongly heated in excess $\mathrm{O}_{2}, 0.0203 \mathrm{g} \mathrm{CrO}_{3}$ was formed. ii. In a second experiment it took 32.93 \(\mathrm{mL}\) of 0.100$M \mathrm{HCl}\( to titrate completely the \)\mathrm{NH}_{3}\( present in \)0.341 \mathrm{g} \mathrm{com}-$ pound A. iii. Compound A was found to contain 73.53\(\%\) iodine by mass. iv. The freezing point of water was lowered by \(0.64^{\circ} \mathrm{C}\) when 0.601 \(\mathrm{g}\) compound A was dissolved in 10.00 $\mathrm{g} \mathrm{H}_{2} \mathrm{O}\left(K_{\mathrm{f}}=\right.\( \)1.86^{\circ} \mathrm{C} \cdot \mathrm{kg} / \mathrm{mol} )$ What is the formula of the compound? What is the structure of the complex ion present? (Hints: \(\mathrm{Cr}^{3+}\) is expected to be six-coordinate, with \(\mathrm{NH}_{3}\) and possibly I- - as ligands. The I- ions will be the counterions if needed.)

The complex ion NiCl \(_{4}^{2-}\) has two unpaired electrons, whereas \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) is diamagnetic. Propose structures for these two complex ions.
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