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Chapter 20: Problem 15

What are the systematic names for these ions and compounds: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right]^{+},\) (b) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3},\) (c) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]^{+},\) (d) \(\mathrm{Fe}(\mathrm{CO})_{5} ?\)

Short Answer

Expert verified
(a) Tetraamminedichlorocobalt(III) ion, (b) Triamminetrichlorochromium(III), (c) Diaminedibromocobalt(III) ion, (d) Pentacarbonyliron(0)

Step by step solution

01

Identify the central metal atom and the ligands

The first step in naming coordination compounds is to identify the central metal atom and the ligands present. In coordination compounds, the ligands are present inside brackets, while in other compounds, they are outside the brackets.
02

Name the ligands

Next, the ligands are named in alphabetical order. It is important to add prefixes (di-, tri-, tetra-, etc.) if there is more than one of a particular type of ligand present.
03

Designate the charge on the complex

For coordination compounds that are ions, the charge on the complex ion is indicated in roman numerals in parentheses at the end of the name of the complex.
04

Name the central atom

Finally, the central atom is named. If the complex ion is a cation, the metal atom is named same as the element. If it is an anion, the name of the central metal atom ends with '-ate'.
05

Apply these steps to the given examples

(a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4}\mathrm{Cl}_{2}\right]^{+}\) is named as Tetraamminedichlorocobalt(III) ion. (b) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{3}\mathrm{Cl}_{3}\) is named as Triamminetrichlorochromium(III). (c) \(\left[\mathrm{Co}(\mathrm{en})_{2} \mathrm{Br}_{2}\right]^{+}\) is named as Diaminedibromocobalt(III) ion. (d) \(\mathrm{Fe}(\mathrm{CO})_{5}\) is named as Pentacarbonyliron(0).

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Most popular questions from this chapter

Chromium exhibits several oxidation states in its compounds, whereas aluminum exhibits only the +3 oxidation state. Explain.

Draw qualitative diagrams for the crystal-field splittings in (a) a linear complex ion \(\mathrm{ML}_{2},\) (b) a trigonalplanar complex ion \(\mathrm{ML}_{3},\) and \((\mathrm{c})\) a trigonalbipyramidal complex ion ML \(_{5}\).

In a dilute nitric acid solution, \(\mathrm{Fe}^{3+}\) reacts with thiocyanate ion \(\left(\mathrm{SCN}^{-}\right)\) to form a dark-red complex: $$\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{SCN}^{-} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}+\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}$$ The equilibrium concentration of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) may be determined by how darkly colored the solution is (measured by a spectrometer). In one such experiment, \(1.0 \mathrm{~mL}\) of \(0.20 \mathrm{M} \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) was mixed with \(1.0 \mathrm{~mL}\) of \(1.0 \times 10^{-3} M \mathrm{KSCN}\) and \(8.0 \mathrm{~mL}\) of dilute \(\mathrm{HNO}_{3}\). The color of the solution quantitatively indicated that the \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) concentration was \(7.3 \times 10^{-5} M\). Calculate the formation constant for \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\)

The complex ion \(\left[\mathrm{Ni}(\mathrm{CN})_{2} \mathrm{Br}_{2}\right]^{2-}\) has a square planar geometry. Draw the structures of the geometric isomers of this 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 \(\mathrm{Co}-\mathrm{N}\) bond strength is approximately the same in both complexes, which reaction will have a larger equilibrium constant? Explain your choices.
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