Ch.21 - Transition Elements and Coordination Chemistry

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.21 - Transition Elements and Coordination Chemistry

Problem 21.112

Chapter 21, Problem 21.112

Draw a crystal field energy-level diagram for a square planar complex, and explain why square planar geometry is especially common for d⁸ complexes.

Verified step by step guidance

Identify the metal ion and its oxidation state in the square planar complex. This will help determine the electron configuration and the number of d electrons present.

Understand that in a square planar complex, the ligands are positioned at the corners of a square in the xy-plane, leading to a specific splitting pattern of the d orbitals.

Recognize that the d orbitals split into different energy levels due to the ligand field. For a square planar complex, the order of increasing energy is typically: d_z², d_xy, d_yz = d_xz, and d_x²-y².

Place the d electrons into the energy levels according to Hund's rule and the Pauli exclusion principle, starting from the lowest energy level. For a d⁸ complex, fill the lower energy orbitals first.

Explain that square planar geometry is common for d⁸ complexes because it allows for a stable electron configuration with lower energy, minimizing electron repulsion and maximizing ligand field stabilization energy.

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Key Concepts

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

Crystal Field Theory

Crystal Field Theory (CFT) explains how the arrangement of ligands around a central metal ion affects the energy levels of the d-orbitals. In a square planar geometry, the ligands are positioned in a way that causes specific splitting of the d-orbitals, leading to distinct energy levels. This theory helps predict the electronic structure and color of coordination complexes.

d8 Electron Configuration

The d8 electron configuration refers to transition metal complexes that have eight electrons in their d-orbitals. This configuration is particularly stable in square planar complexes, as it allows for optimal pairing of electrons and minimizes electron-electron repulsion. Common examples include complexes of metals like nickel(II) and platinum(II).

Ligand Field Stabilization Energy (LFSE)

Ligand Field Stabilization Energy (LFSE) is the energy difference between the actual electronic configuration of a complex and the hypothetical configuration where all d-electrons are in the highest energy level. In square planar complexes, d8 configurations can achieve a high LFSE due to effective pairing and lower energy arrangements, making this geometry energetically favorable.

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Guided course

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Strong-Field Ligands result in a large Δ and Weak-Field Ligands result in a small Δ.

Related Practice

Textbook Question

For each of the following complexes, draw a crystal field energy-level diagram, assign the electrons to orbitals, and predict the number of unpaired electrons.

(d) [Cu(en)2]2+ (square planar)

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Textbook Question

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

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Textbook Question

What is the general trend in standard potentials for the oxidation of first-series transition metals from Sc to Zn? What is the reason for the trend?

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Textbook Question

Predict the crystal field energy-level diagram for a square pyramidal ML₅ complex that has two ligands along the axes but only one ligand along the z axis. Your diagram should be intermediate between those for an octahedral ML₆complex and a square planar ML₄ complex.

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Textbook Question

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

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Textbook Question

Which of the following complexes are diamagnetic?

(a) [Ni(H₂O)₆]²⁺

(b) [Co(CN)₆]^3-

(d) [Cu(NH₃)₄]²⁺ (square planar)

122

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