Skip to main content
Ch.21 - Transition Elements and Coordination Chemistry
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.21 - Transition Elements and Coordination ChemistryProblem 21.114
Chapter 21, Problem 21.114

Which of the following complexes are paramagnetic?
(a) [Mn(CN)6]3-
(b) [Zn(NH3)4]2+ (tetrahedral)
(c) [Fe(CN)6]4-
(d) [FeF6]4-

Verified step by step guidance
1
Identify the oxidation state of the metal in each complex.
Determine the electron configuration of the metal ion in each complex.
Assess the ligand field strength: CN^- is a strong field ligand, NH_3 is a moderate field ligand, and F^- is a weak field ligand.
Apply crystal field theory to determine the electron distribution in the d-orbitals for each complex.
Identify if there are unpaired electrons in the d-orbitals, which would indicate paramagnetism.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Paramagnetism

Paramagnetism is a property of materials that have unpaired electrons, which causes them to be attracted to magnetic fields. In transition metal complexes, the presence of unpaired electrons in d-orbitals is a key factor in determining whether a complex is paramagnetic. The number of unpaired electrons can be influenced by the metal's oxidation state and the nature of the ligands surrounding it.

Crystal Field Theory

Crystal Field Theory (CFT) explains how the arrangement of ligands around a central metal ion affects its electronic structure and properties. According to CFT, the interaction between the metal ion and the ligands leads to the splitting of d-orbitals into different energy levels. The extent of this splitting, influenced by the ligand's strength (strong field vs. weak field), determines the number of unpaired electrons and thus the magnetic properties of the complex.

Oxidation States of Transition Metals

The oxidation state of a transition metal in a complex is crucial for determining its electronic configuration and magnetic properties. Different oxidation states can lead to varying numbers of d-electrons, which directly affect the number of unpaired electrons. Understanding the oxidation states of the metals in the given complexes is essential for predicting whether they will exhibit paramagnetism or not.
Recommended video:
Guided course
03:12
Transition Metals
Related Practice
Textbook Question

What is the highest oxidation state for each of the elements from Sc to Zn?

101
views
Textbook Question

What is a racemic mixture? Does it affect plane-polarized light? Explain.

87
views
Textbook Question

The oxalate ion is a bidentate ligand as indicated in Figure 21.8. Would you expect the carbonate ion to be a monodentate or bidentate ligand? Explain your reasoning.

108
views
Textbook Question

Look at the colors of the isomeric complexes in Figure 21.12, and predict which is the stronger field ligand, nitro (-NO2) of nitrito (-ONO). Explain. 

89
views
Textbook Question

Based on the wavelength of maximum absorption of the cobalt complexes, arrange the following ligands in a spectrochemical series from weakest-field to strongest-field ligand. 

(a) Cl- < NCS- < H2O < NH3 

(b) Cl- < NCS- < H2O < NH3 

(c) H2O < Cl- < NH3 < NCS-

(d) Cl- < H2O < NCS- < NH3

105
views
Textbook Question

What hybrid orbitals are used by the metal ion and how many unpaired electrons are present the complex ion [VCl4]- with tetrahedral geometry?

(a) sp3; 2 unpaired electrons

(b) sp3; 3 unpaired electrons

(c) sp3d2; 3 unpaired electrons

(d) sp3d2; 4 unpaired electrons

88
views