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Chapter 20: Problem 45

Which one has the highest paramagnetism among the following ions? (a) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (b) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (c) \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) (d) \(\left[\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\)

Short Answer

Expert verified
(b) \\(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) has the highest paramagnetism with 4 unpaired electrons.

Step by step solution

01

Determine the Electronic Configuration

Identify the electronic configuration for the central metal ions in each complex. - (a) \([ ext{Cr}^{3+}] : [Ar] 3d^{3}\)- (b) \([ ext{Fe}^{2+}] : [Ar] 3d^{6}\)- (c) \([ ext{Cu}^{2+}] : [Ar] 3d^{9}\)- (d) \([ ext{Zn}^{2+}] : [Ar] 3d^{10}\)
02

Count the Unpaired Electrons

Determine the number of unpaired electrons in the 3d orbitals for each metal ion. - (a) \([ ext{Cr}^{3+}] ext{ has } 3 ext{ unpaired electrons}\) - (b) \([ ext{Fe}^{2+}] ext{ has } 4 ext{ unpaired electrons}\) - (c) \([ ext{Cu}^{2+}] ext{ has } 1 ext{ unpaired electron}\) - (d) \([ ext{Zn}^{2+}] ext{ has } 0 ext{ unpaired electrons}\)
03

Analyze Paramagnetism

Paramagnetism is determined by the presence of unpaired electrons. The more unpaired electrons, the greater the paramagnetism. Therefore, compare the number of unpaired electrons in each complex.
04

Determine the Highest Paramagnetism

Since (b) \([ ext{Fe}^{2+}] ext{ has the most unpaired electrons (4), it is the most paramagnetic among the options.}\)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Unpaired Electrons
Unpaired electrons are electrons in an orbital that do not have a corresponding electron with opposite spin. When we discuss paramagnetism, the concept of unpaired electrons becomes pivotal. This is because unpaired electrons create a magnetic moment.
In a magnetic field, substances with unpaired electrons may become attracted due to this magnetic moment, thus exhibiting paramagnetism.
Transition metal ions often have unpaired electrons due to their partially filled d orbitals. Here's how you can assess the number of unpaired electrons in a transition metal complex:
  • Identify the electronic configuration of the metal ion.
  • Count the electrons present in d orbitals.
  • Determine which electrons are unpaired.
Electronic Configuration
The electronic configuration describes how an atom's or ion's electrons are arranged in its orbitals, and this arrangement dictates many of its chemical properties, including magnetism.
In coordination compounds, we often look at the transition metals' electronic configuration to understand their magnetic properties. Transition metals are unique as their d orbitals are filled in a specific way, impacting the number of unpaired electrons.
For instance, the electronic configurations for the complexes in our example are like this:
  • For \(\text{Cr}^{3+}\) (option a), it has an electronic configuration of [Ar] 3d\(^{3}\), leaving us with 3 unpaired electrons.
  • For \(\text{Fe}^{2+}\) (option b), it follows [Ar] 3d\(^{6}\), resulting in 4 unpaired electrons.
  • For \(\text{Cu}^{2+}\) (option c), it has [Ar] 3d\(^{9}\), leaving only 1 unpaired electron.
  • For \(\text{Zn}^{2+}\) (option d), it is [Ar] 3d\(^{10}\), with 0 unpaired electrons.
These configurations influence their paramagnetic or diamagnetic nature.
Transition Metal Complexes
Transition metal complexes are formed when transition metal ions coordinate with ligands, which are atoms, ions, or molecules that donate pairs of electrons.
These complexes have intriguing electronic properties due to the arrangement of electrons in their d orbitals, significantly influencing their magnetic properties.
  • A complex is paramagnetic if it has unpaired electrons, as in the case of \(\left[\text{Fe}\left(\text{H}_2\text{O}\right)_6\right]^{2+}\) with 4 unpaired electrons.
  • While, a complex with all paired electrons, such as \(\text{Zn}^{2+}\), is diamagnetic.
These characteristics make transition metal complexes highly dynamic, with a range of applications in various fields like catalysis and materials science.

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Most popular questions from this chapter

The main draw back of valence bond theory is/are (a) It cannot explain magnetic properties of co-ordination compounds (b) It cannot distinguish between high spin and low spin complex (c) It does not provide an answer to the origin of characteristic colours of complex ions (d) It is a qualitative approach

The number of ions produced from one molecule of [Pt \(\left.\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Br}\right] \mathrm{Br}_{3}\) in the aqueous solution will be (a) 4 (b) 5 (c) 6 (d) 7

In photography, hypo is used in the reduction of (a) \(\mathrm{Ag}\) from \(\mathrm{AgBr}\) (b) \(\mathrm{AgBr}\) into \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) (c) AgBr into soluble thiosulphate complex (d) both (b) and (c)

Which of the following are diamagnetic? (1) \(\mathrm{K}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (2) \(\mathrm{K}_{3}\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]\) (3) \(\mathrm{K}_{3}\left[\mathrm{Co}(\mathrm{CN})_{6}\right]\) (4) \(\mathrm{K}_{2}\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]\) Select the correct answer using the codes given below: (a) \(\mathrm{l}\) and 2 (b) 2,3 and 4 (c) 1,3 and 4 (d) 2 and 4

Which one of the following is true? (a) The charge on the complex ion in \(\mathrm{K}_{2}\left[\mathrm{PtCl}_{4}\right]\) is \(+2\) (b) The coordination number of \(\mathrm{Hg}\) in \(\left[\mathrm{Hg}(\mathrm{en})_{2}\right]^{2+}\) is 4 (here en is ethylenediamine) (c) The oxidation number of iron in \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4}\) is \(+6\). (d) In transition metal complexes, ligands act as lewis acid
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