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Chapter 21: Problem 36

Name the following complex ions. a. \(\operatorname{Ru}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}^{2+}\) b. \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\) c. $\mathrm{Mn}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{3}^{2+}$ d. \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{55} \mathrm{NO}_{2}^{2+}\) e. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) f. \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\) g. \(\mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}^{3-}\) h. $\mathrm{Co}(\mathrm{SCN})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}^{+}$

Short Answer

Expert verified
a. pentaamminechlororuthenium(II) b. hexacyanoferrate(IV) c. tris(ethylenediamine)manganese(II) d. pentaamminenitrocobalt(III) e. tetracyanonickelate(II) f. tetraamminedichlorochromium(III) g. tris(oxalato)ferrate(III) h. tetrakisaquodithiocyanatocobalt(III)

Step by step solution

01

Name the ligands and the central atom

The ligands are 5 ammine (NH₃) and 1 chloro (Cl). The central metal ion is Ruthenium (Ru). The complex has a charge of +2.
02

Name the complex ion

Since the complex ion is cationic, we name the ligands first followed by the name of the central metal ion. The name for this complex ion is: pentaamminechlororuthenium(II) b. \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\)
03

Name the ligands and the central atom

The ligands are 6 cyanide (CN⁻). The central metal ion is Iron (Fe). The complex has a charge of -4.
04

Name the complex ion

Since the complex ion is anionic, we name the ligands first followed by the name of the central metal ion in '-ate' form. The name for this complex ion is: hexacyanoferrate(IV) c. $\mathrm{Mn}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{3}^{2+}$
05

Name the ligands and the central atom

The ligands are 3 ethylenediamine (NH₂CH₂CH₂NH₂). The central metal ion is Manganese (Mn). The complex has a charge of +2.
06

Name the complex ion

Since the complex ion is cationic, we name the ligands first followed by the name of the central metal ion. The name for this complex ion is: tris(ethylenediamine)manganese(II) d. \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{NO}_{2}^{2+}\)
07

Name the ligands and the central atom

The ligands are 5 ammine (NH₃) and 1 nitro (NO₂). The central metal ion is Cobalt (Co). The complex has a charge of +2.
08

Name the complex ion

Since the complex ion is cationic, we name the ligands first followed by the name of the central metal ion. The name for this complex ion is: pentaamminenitrocobalt(III) e. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\)
09

Name the ligands and the central atom

The ligands are 4 cyanide (CN⁻). The central metal ion is Nickel (Ni). The complex has a charge of -2.
10

Name the complex ion

Since the complex ion is anionic, we name the ligands first followed by the name of the central metal ion in '-ate' form. The name for this complex ion is: tetracyanonickelate(II) f. \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}^{+}\)
11

Name the ligands and the central atom

The ligands are 4 ammine (NH₃) and 2 chloro (Cl). The central metal ion is Chromium (Cr). The complex has a charge of +1.
12

Name the complex ion

Since the complex ion is cationic, we name the ligands first followed by the name of the central metal ion. The name for this complex ion is: tetraamminedichlorochromium(III) g. \(\mathrm{Fe}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}^{3-}\)
13

Name the ligands and the central atom

The ligands are 3 oxalate (C₂O₄²⁻). The central metal ion is Iron (Fe). The complex has a charge of -3.
14

Name the complex ion

Since the complex ion is anionic, we name the ligands first followed by the name of the central metal ion in '-ate' form. The name for this complex ion is: tris(oxalato)ferrate(III) h. $\mathrm{Co}(\mathrm{SCN})_{2}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}^{+}$
15

Name the ligands and the central atom

The ligands are 2 thiocyanato (SCN⁻) and 4 aqua (H₂O). The central metal ion is Cobalt (Co). The complex has a charge of +1.
16

Name the complex ion

Since the complex ion is cationic, we name the ligands first followed by the name of the central metal ion. The name for this complex ion is: tetrakisaquodithiocyanatocobalt(III)

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Most popular questions from this chapter

Will 0.10 mol of AgBr completely dissolve in 1.0 \(\mathrm{L}\) of 3.0 \(\mathrm{M} \mathrm{NH}_{3} ?\) The \(K_{\mathrm{sp}}\) value for \(\mathrm{AgBr}(s)\) is \(5.0 \times 10^{-13},\) and the overall formation constant for the complex ion \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}+\) is \(1.7 \times 10^{7}\) , that is, $$\mathrm{Ag}^{+}(a q)+2 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}(a q) \quad K=1.7 \times 10^{7}$$

When 6\(M\) ammonia is added gradually to aqueous copper(II) nitrate, a white precipitate forms. The precipitate dissolves as more 6\(M\) ammonia is added. Write balanced equations to explain these observations. [Hint: \(\mathrm{Cu}^{2+}\) reacts with \(\mathrm{NH}_{3}\) to form \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+} . ]\)

The compound cisplatin, Pt \(\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2},\) has been studied extensively as an antitumor agent. The reaction for the synthesis of cisplatin is: $\mathrm{K}_{2} \mathrm{PtCl}_{4}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow \mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{2}(s)+2 \mathrm{KCl}(a q)$ Write the electron configuration for platinum ion in cisplatin. Most \(d^{8}\) transition metal ions exhibit square planar geometry. With this and the name in mind, draw the structure of cisplatin.

The carbonate ion \(\left(\mathrm{CO}_{3}^{2-}\right)\) can act as either a monodentate or a bidentate ligand. Draw a picture of \(\mathrm{CO}_{3}^{2-}\) coordinating to a metal ion as a monodentate and as a bidentate ligand. The carbonate ion can also act as a bridge between two metal ions. Draw a picture of a \(\mathrm{CO}_{3}^{2-}\) ion bridging between two metal ions.

Draw the \(d\) -orbital splitting diagrams for the octahedral complex ions of each of the following. a. \(\mathrm{Fe}^{2+}\) (high and low spin) b. \(\mathrm{Fe}^{3+}(\text { high spin })\) c. \(\mathrm{Ni}^{2+}\)
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