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Chapter 21: Problem 38

Give formulas for the following complex ions. a. tetrachloroferrate(III) ion b. pentaammineaquaruthenium(III) ion c. tetracarbonyldihydroxochromium(III) ion d. amminetrichloroplatinate(II) ion

Short Answer

Expert verified
The formulas for the given complex ions are as follows: a. Tetrachloroferrate(III) ion: \([FeCl_4]^{-}\) b. Pentaammineaquaruthenium(III) ion: \([Ru(NH_3)_5(H_2O)]^{3+}\) c. Tetracarbonyldihydroxochromium(III) ion: \([Cr(CO)_4(OH)_2]^{+}\) d. Amminetrichloroplatinate(II) ion: \([Pt(NH_3)Cl_3]^{-}\)

Step by step solution

01

a. Tetrachloroferrate(III) ion

The name reveals that the central atom is iron (Fe) with an oxidation state of +3. The ligand here is "tetrachloro," which means there are four chloride ions (Cl-) surrounding the central atom. The net charge of the complex ion will be -1 since the ligands are negatively charged and there are four of them. So, the formula for tetrachloroferrate(III) ion is: \([FeCl_4]^{-}\).
02

b. Pentaammineaquaruthenium(III) ion

In this case, the central atom is ruthenium (Ru) with an oxidation state of +3. The ligands include "pentaammine" and "aqua." Pentaammine signifies that there are five ammine (NH3) ligands, and aqua signifies a single water molecule (H2O) as a ligand. Since both ligands are neutral, the charge of the complex ion will be +3 (as a result of the oxidation state of the central atom). The formula for pentaammineaquaruthenium(III) ion is: \([Ru(NH_3)_5(H_2O)]^{3+}\).
03

c. Tetracarbonyldihydroxochromium(III) ion

The central atom here is chromium (Cr) with an oxidation state of +3. The ligands include "tetracarbonyl" and "dihydroxo," which means there are four carbonyl (CO) ligands and two hydroxo (OH-) ligands. Since there are two negatively charged hydroxo ligands, the net charge of the complex ion will be +1. The formula for tetracarbonyldihydroxochromium(III) ion is: \([Cr(CO)_4(OH)_2]^{+}\).
04

d. Amminetrichloroplatinate(II) ion

In this example, the central atom is platinum (Pt) with an oxidation state of +2. The ligands include "ammine" and "trichloro," which means there is one ammine (NH3) ligand and three chloride (Cl-) ligands. Since there are three negatively charged chloride ligands and the central atom has a +2 oxidation state, the net charge of the complex ion will be -1. The formula for amminetrichloroplatinate(II) ion is: \([Pt(NH_3)Cl_3]^{-}\).

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Most popular questions from this chapter

A certain first-row transition metal ion forms many different colored solutions. When four coordination compounds of this metal, each having the same coordination number, are dissolved in water, the colors of the solutions are red, yellow, green, and blue. Further experiments reveal that two of the complex ions are paramagnetic with four unpaired electrons and the other two are diamagnetic. What can be deduced from this information about the four coordination compounds?

Tetrahedral complexes of \(\mathrm{Co}^{2+}\) are quite common. Use a \(d\) -orbital splitting diagram to rationalize the stability of \(\mathrm{Co}^{2+}\) tetrahedral complex ions.

A blast furnace is used to reduce iron oxides to elemental iron. The reducing agent for this reduction process is carbon monoxide. a. Given the following data: \(\begin{aligned} \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) & \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g) & & \Delta H^{\circ}=-23 \mathrm{~kJ} \\ 3 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) & \longrightarrow 2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}_{2}(g) & & \Delta H^{\circ}=-39 \mathrm{~kJ} \\ \mathrm{Fe}_{3} \mathrm{O}_{4}(s)+\mathrm{CO}(g) & \longrightarrow 3 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g) & & \Delta H^{\circ}=18 \mathrm{~kJ} \end{aligned}\) determine \(\Delta H^{\circ}\) for the reaction $$ \mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) $$ b. The \(\mathrm{CO}_{2}\) produced in a blast furnace during the reduction process actually can oxidize iron into \(\mathrm{FeO}\). To eliminate this reaction, excess coke is added to convert \(\mathrm{CO}_{2}\) into \(\mathrm{CO}\) by the reaction $$ \mathrm{CO}_{2}(g)+\mathrm{C}(s) \longrightarrow 2 \mathrm{CO}(g) $$ Using data from Appendix 4 , determine \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) for this reaction. Assuming \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) do not depend on temperature, at what temperature is the conversion reaction of \(\mathrm{CO}_{2}\) into CO spontaneous at standard conditions?

Write electron configurations for each of the following. a. \(\mathrm{Cr}, \mathrm{Cr}^{2+}, \mathrm{Cr}^{3+}\) b. \(\mathrm{Cu}, \mathrm{Cu}^{+}, \mathrm{Cu}^{2+}\) c. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}\)

Draw all the geometrical isomers of \(\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2} \mathrm{BrCl}^{+} .\) Which of these isomers also have an optical isomer? Draw the various isomers.
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