/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 1 (a) Draw the structure for \(\ma... [FREE SOLUTION] | 91影视

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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

Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the \(3+\) rather than in the \(2+\) oxidation state. Furthermore, for a given ligand the complexes of the bivalent metal ions of the first transition series tend to increase in stability in the order \(\mathrm{Mn}(\mathrm{II})<\mathrm{Fe}(\mathrm{II})<\mathrm{Co}(\mathrm{II})<\) \(\mathrm{Ni}(\mathrm{II})<\mathrm{Cu}(\mathrm{II})\). Explain how these two observations are consistent with one another and also consistent with a crystal-field picture of coordination compounds.

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) tetraaquadibromomanganese(III) perchlorate (b) bis(bipyridyl)cadmium(II) chloride (c) potassium tetrabromo(ortho-phenanthroline)cobaltate (III) (d) cesium diamminetetracyanochromate(III) (e) tris(ethylenediammine)rhodium(III) tris(oxalato)cobaltate(III)

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 $$ \mathrm{HbO}_{2}+\mathrm{CO} \rightleftharpoons \mathrm{HbCO}+\mathrm{O}_{2} $$

(a) What is the difference between a monodentate ligand and a bidentate ligand? (b) How many bidentate ligands are necessary to fill the coordination sphere of a six-coordinate complex? (c) You are told that a certain molecule can serve as a tridentate ligand. Based on this statement, what do you know about the molecule?

Write balanced chemical equations to represent the following observations. (In some instances the complex involved has been discussed previously in the text.) (a) Solid silver chloride dissolves in an excess of aqueous ammonia. (b) The green complex \(\left[\mathrm{Cr}(\mathrm{en})_{2} \mathrm{Cl}_{2}\right] \mathrm{Cl}\), on treatment with water over a long time, converts to a brown- orange complex. Reaction of \(\mathrm{AgNO}_{3}\) with a solution of the product precipitates 3 mol of \(\mathrm{AgCl}\) per mole of Cr present. (Write two chemical equations.) (c) When an \(\mathrm{NaOH}\) solution is added to a solution of \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{a}\) precipitate forms. Addition of excess \(\mathrm{NaOH}\) solution causes the precipitate to dissolve. (Write two chemical equations.) (d) A pink solution of \(\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}\) turns deep blue on addition of concentrated hydrochloric acid.
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