Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 23: Problem 26

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{K}_{2} \mathrm{PtCl}_{4}\) (b) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right] \mathrm{Br}_{2}\) (c) \(\mathrm{OsO}_{4}\) (d) \(\left[\mathrm{Mn}(\mathrm{en})_{3}\right]\left(\mathrm{NO}_{3}\right)_{2}\) (e) $\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{3}$ (f) \(\left[\mathrm{Zn}(\mathrm{bipy})_{2}\right]\left(\mathrm{ClO}_{4}\right)_{2}\)

Short Answer

Expert verified
(a) Coordination number: 4, Oxidation number: +2 (b) Coordination number: 4, Oxidation number: 0 (c) Coordination number: 4, Oxidation number: +8 (d) Coordination number: 6, Oxidation number: +2 (e) Coordination number: 6, Oxidation number: +3 (f) Coordination number: 4, Oxidation number: +2

Step by step solution

01

Coordination Number

We must count the number of ligands surrounding Pt. There are four Cl ligands, therefore the coordination number is 4.
02

Oxidation Number

In this complex, Pt has an oxidation state of +2 because the overall charge of \(\mathrm{PtCl}_{4}\) is -2 and there are two \(\mathrm{K}\) ions, each with a charge of +1 to balance it. Therefore, Pt has an oxidation number of +2. (b) \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\mathrm{Br}_{2}\)
03

Coordination Number

There are four CO ligands surrounding the Ni atom, so the coordination number for Ni is 4.
04

Oxidation Number

The overall charge of the Ni(CO)4 complex is 0, since the Br2 has no charge. Considering that CO is a neutral ligand, the Ni atom has an oxidation number of 0. (c) \(\mathrm{OsO}_{4}\)
05

Coordination Number

Os has four O atoms bonded to it, making its coordination number 4.
06

Oxidation Number

Considering that each O atom has an oxidation number of -2, to balance the charge, Os must have an oxidation number of +8. (d) \(\left[\mathrm{Mn}(\mathrm{en})_{3}\right]\left(\mathrm{NO}_{3}\right)_{2}\)
07

Coordination Number

There are three en (ethylenediamine) ligands surrounding the Mn atom. Each en ligand has two donor atoms. Therefore, the coordination number for Mn is 3 x 2 = 6.
08

Oxidation Number

The overall charge of the Mn(en)3 complex is +2 due to the presence of two NO3- ions. The en ligands are neutral, so Mn must have an oxidation number of +2 to balance the charge. (e) \(\left[\mathrm{Cr}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]\mathrm{Cl}_{3}\)
09

Coordination Number

There is one en ligand and four NH3 ligands surrounding the Cr atom. Since en has two donor atoms, the coordination number for Cr is 1 x 2 + 4 = 6.
10

Oxidation Number

Considering the overall charge of the complex is +3 due to the three Cl- ions; the en and NH3 ligands are neutral, so the oxidation number of Cr is +3. (f) \(\left[\mathrm{Zn}(\mathrm{bipy})_{2}\right]\left(\mathrm{ClO}_{4}\right)_{2}\)
11

Coordination Number

There are two bipy (bipyridine) ligands surrounding the Zn atom. Each bipy ligand has two donor atoms, so the coordination number for Zn is 2 x 2 = 4.
12

Oxidation Number

Considering that the overall charge of the Zn(bipy)2 complex is +2, due to the presence of two ClO4- ions, since bipy ligands are neutral, the Zn atom must have an oxidation number of +2.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Consider the tetrahedral anions \(\mathrm{VO}_{4}^{3-}\) (orthovanadate ion), \(\mathrm{CrO}_{4}^{2-}\) (chromate ion), and \(\mathrm{MnO}_{4}^{-}\) (permanganate ion). (a) These anions are isoelectronic. What does this statement mean? (b) Would you expect these anions to exhibit d-d transitions? Explain. (c) As mentioned in "A Closer Look" on charge-transfer color, the violet color of \(\mathrm{MnO}_{4}\) is due to a ligand-to-metal charge transfer (LMCT) transition. What is meant by this term? (d) The LMCT transition in \(\mathrm{MnO}_{4}^{-}\) occurs at a wavelength of \(565 \mathrm{nm}\). The \(\mathrm{CrO}_{4}^{2-}\) ion is yellow. Is the wavelength of the LMCT transition for chromate larger or smaller than that for \(\mathrm{MnO}_{4}^{-}\) ? Explain. (e) The \(\mathrm{VO}_{4}^{3-}\) ion is colorless. Do you expect the light absorbed by the LMCT to fall in the UV or the IR region of the electromagnetic spectrum? Explain your reasoning.

Carbon monoxide, CO, is an important ligand in coordination chemistry. When CO is reacted with nickel metal, the product is \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right],\) which is a toxic, pale yellow liquid. (a) What is the oxidation number for nickel in this compound? (b) Given that \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is a diamagnetic molecule with a tetrahedral geometry, what is the electron configuration of nickel in this compound? (c) Write the name for \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) using the nomenclature rules for coordination compounds.

Draw the structure for $\mathrm{Pt}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}$ and use it to answer the following questions: (a) What is the coordination number for platinum in this complex? (b) What is the coordination geometry? (c) What is the oxidation state of the platinum? (d) How many unpaired electrons are there? [Sections 23.2 and 23.6\(]\)

The value of \(\Delta\) for the \(\left[\mathrm{MoI}_{6}\right]^{3-}\) complex is \(198.58 \mathrm{~kJ} / \mathrm{mol}\). Calculate the expected wavelength of the absorption corresponding to promotion of an electron from the lower energy to the higher-energy \(d\) -orbital set in this complex. Should the complex absorb in the visible range?

For each of the following compounds, determine the electron configuration of the transition-metal ion. (a) CuO, (b) \(\mathrm{Cu}_{2} \mathrm{O}\) (c) \(\mathrm{V}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{MnO}\).
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free