/*! 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 33 Explain why the compounds of mos... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 23: Problem 33

Explain why the compounds of most of the first-row transition metals are colored.

Short Answer

Expert verified
Answer: The compounds of most first-row transition metals are colored due to the d-d transitions that occur as a result of crystal field splitting in their complexes. When these metals form complexes with ligands, their d orbitals split into two sets of energy levels, allowing electrons to absorb visible light and promote to higher energy levels. The color observed in these complexes is the complementary color of the absorbed light.

Step by step solution

01

Understanding electronic configuration of transition metals

The first-row transition metals are the elements with atomic numbers from 21 (Scandium) to 29 (Copper). These metals have partially filled d orbitals in their electronic configurations. The general electronic configuration for these elements can be written as [Ar] 4s^2 3d^n, where n varies from 1 to 10.
02

Understanding the effect of ligands on d-orbitals

When transition metal elements form complexes with ligands, the d orbitals of these metals interact with the ligands' electron pairs. This interaction results in splitting the energy levels of the d orbitals into two sets: t2g orbitals (dxy, dyz, dxz) and eg orbitals (dx^2-y^2 and dz^2). This process is known as crystal field splitting.
03

Understanding d-d transitions

When the transition metal complexes absorb light in the visible range, electrons can be excited from the lower energy t2g orbitals to higher energy eg orbitals resulting in a phenomenon called d-d transition. The energy required for this transition corresponds to the energy of the absorbed light. Consequently, the complementary color is observed as the color of the complex.
04

Explaining the color of the transition metal compounds

Most of the first-row transition metal compounds are colored because they exhibit d-d transitions. In other words, their d orbitals split into two sets of energy levels when they form complexes with ligands, allowing electrons to absorb visible light and promote to higher energy levels. The color observed in these complexes is the complementary color of the absorbed light. If no d-d transition is possible (like in the case of Zn^2+ complexes), the complex is colorless. Therefore, the color observed in most of the first-row transition metal compounds is due to the d-d transitions that occur as a result of crystal field splitting in their complexes.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

Which of the following cations can, have either a high-spin or a low-spin electron configuration in a tetrahedral field? \(\mathrm{Co}^{2+}, \mathrm{Cr}^{3+}, \mathrm{Ni}^{2+},\) and \(\mathrm{Zn}^{2+}\)

Many transition metal complexes are brightly colored. Why is the titanium(IV) compound budotitane be colorless?

Does the complex \(\mathrm{Co}(\mathrm{en})\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}\) have stereoisomers?

What do the prefixes cis-and trans-mean in the context of an octahedral complex ion?

Sketch the stereoisomers of the complex ion \(\mathrm{Ni}(\mathrm{en}) \mathrm{Cl}_{2}(\mathrm{CN})_{2}^{2-} .\) Are any of these isomers chiral?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Inorganic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

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.