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Chapter 24: Problem 1

(a) Draw the structure for \(\mathrm{Pt}(\mathrm{en}) \mathrm{Cl}_{2}\). (b) What is the coordination number for platinum in this complex, and what is the coordination geometry? (c) What is the oxidation state of the platinum? [Section 24.1]

Short Answer

Expert verified
(a) Pt(en)Cl鈧� has a structure with a central platinum atom bonded to two Cl鈦� ions and two ethylenediamine (en) groups. (b) The coordination number for platinum is 6, with an octahedral coordination geometry. (c) The oxidation state of platinum is +2.

Step by step solution

01

Draw the structure for Pt(en)Cl鈧�

Ethylenediamine (en) has the formula NH鈧�-CH鈧�-CH鈧�-NH鈧�, which can bond to the platinum center through its two nitrogen atoms. The structure would look like this: 1. Platinum at the center 2. Two Cl鈧� ions bonded to the platinum 3. Two NH鈧�-CH鈧�-CH鈧�-NH鈧� groups bonded to the platinum through their nitrogen atoms
02

Determine the coordination number

The coordination number is the number of coordination bonds a metal ion forms with ligands. In this case, two chlorides each form one coordinate bond with platinum, and each en ligand forms two coordinate bonds. Thus, the coordination number for platinum in this complex is 2 + 2 + 2 = 6.
03

Determine the coordination geometry

A coordination number of 6 typically leads to an octahedral coordination geometry. In this case, the platinum has an octahedral geometry with Cl atoms and N atoms from ethylenediamine groups occupying the vertices.
04

Determine the oxidation state of platinum

To calculate the oxidation state of platinum, we need to consider the charges contributed by the surrounding ligands. Cl鈧� ions each have a charge of -1, while ethylenediamine (en) is a neutral molecule with no charge. Therefore, Pt must have an oxidation state equal to the sum of charges on the ligands to maintain a neutral complex. Thus, the oxidation state of platinum in this complex is +2, as: Pt^(+2) + 2Cl^(-1) + 2(en) = neutral complex. Summarizing the information: (a) The structure of Pt(en)Cl鈧� has a central platinum atom bonded to two Cl鈧� ions and two ethylenediamine (en) groups. (b) The coordination number for platinum is 6, with an octahedral coordination geometry. (c) The oxidation state of platinum is +2.

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Most popular questions from this chapter

Metallic elements are essential components of many important enzymes operating within our bodies. Carbonic anhydrase, which contains \(\mathrm{Zn}^{2+}\), is responsible for rapidly interconverting dissolved \(\mathrm{CO}_{2}\) and bicarbonate ion, \(\mathrm{HCO}_{3}^{-} .\) The zinc in carbonic anhydrase is coordinated by three nitrogen-containing groups and a water molecule. The enzyme's action depends on the fact that the coordinated water molecule is more acidic than the bulk solvent molecules. Explain this fact in terms of Lewis acid-base theory (Section 16.11).

Carbon monoxide is toxic because it binds more strongly to the iron in hemoglobin (Hb) than does \(\mathrm{O}_{2}\), as indicated by these approximate standard free-energy changes in blood: $$ \begin{array}{clrl} \mathrm{Hb}+\mathrm{O}_{2} \longrightarrow \mathrm{HbO}_{2} & & \Delta G^{\circ}=-70 \mathrm{~kJ} \\ \mathrm{Hb}+\mathrm{CO} \longrightarrow \mathrm{HbCO} & \Delta G^{\circ}=-80 \mathrm{~kJ} \end{array} $$ Using these data, estimate the equilibrium constant at \(298 \mathrm{~K}\) for the equilibrium $$ \mathrm{HbO}_{2}+\mathrm{CO} \rightleftharpoons \mathrm{HbCO}+\mathrm{O}_{2} $$

Explain why the \(d_{x y}, d_{x z}\), and \(d_{y z}\) orbitals lie lower in energy than the \(d_{z^{2}}\) and \(d_{x^{2}-y^{2}}\) orbitals in the presence of an octahedral arrangement of ligands about the central metalion.

Write names for the following coordination compounds: (a) \(\left[\mathrm{Cd}(\mathrm{en}) \mathrm{Cl}_{2}\right]\) (b) \(\mathrm{K}_{4}\left[\mathrm{Mn}(\mathrm{CN})_{6}\right]\) (c) \(\left[\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{CO}_{3}\right] \mathrm{Cl}\) (d) \(\left[\mathrm{Ir}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\right]\left(\mathrm{NO}_{3}\right)_{3}\)

(a) Draw the two linkage isomers of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{SCN}\right]^{2+}\). (b) Draw the two geometric isomers of \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right]^{2+}\). (c) Two compounds with the formula \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{ClBr}\) can be prepared. Use structural formulas to show how they differ. What kind of isomerism does this illustrate?
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