/*! 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 3 Discuss the salient features of ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 23: Problem 3

Discuss the salient features of valence bond theory. What are all its applications?

Short Answer

Expert verified
Valence Bond Theory is a fundamental theory that describes covalent bond formation via atomic orbital overlap, differentiating between sigma and pi bonds. It helps understand bond energies, lengths, and angles in molecules. Its main applications include predicting bond strengths and lengths, understanding hybridization, and anticipating molecule shapes.

Step by step solution

01

Understanding Valence Bond Theory

The first step is understanding the Valence Bond Theory. It is a fundamental theory that reveals the electronic structure of molecules. It postulates that a covalent bond is formed between two atoms by the overlap of half-filled valence electronic orbitals, one from each atom. The two electrons (one from each atom) which go into making the bond must have opposite spins. The overlapping of atomic orbitals can be sigma (蟽) or pi (蟺). Sigma bonds are stronger and are formed by head on overlapping, while pi bonds are weaker and result from lateral overlap.
02

Features of Valence Bond Theory

The second step is defining the main features of the theory. The first key point is the type of bonds: valence bond theory helps explain how they are created through orbital overlap. Secondly, the theory also sheds light on bond energies and bond lengths: higher overlap leads to stronger bonds with more energy and shorter lengths. Thirdly, the theory also highlights bond angles which vary depending on the molecules.
03

Applications of Valence Bond Theory

The third step is summarising its applications. The valence bond theory offers several applications such as predicting the strengths and lengths of bonds, clarifying the concept of hybridization, understanding the electronic structure of molecules, foreseeing the geometric shape of molecules, and mapping the characteristic properties of molecules.

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

Discuss the main points of Werner theory. What is the significance?

Discuss in brief the crystal field theory and represent the splitting of ' \(d\) ' orbitals in octahedral and tetrahedral fields.

How does ligand field theory describe the origin of charge transfer spectra in coordination complexes.

Discuss Sidgwick's concept of effective atomic number with the help of suitable example.

Explain the following: (a) \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) is paramagnetic and coloured. (b) \(\left(\mathrm{Ni}(\mathrm{CN})_{4}\right)^{2-}\) is square planar, but \(\left[\mathrm{Ni}(\mathrm{Cl})_{4}\right]^{2-}\) is tetrahedral. (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}\) is more stable than \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\), while \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\) is more stable than \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}\) (d) Octahedral complexes are less stable than the square planar complexes. (e) \(\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3-}\) is a low-spin complex, but \(\left[\mathrm{CoF}_{6}\right]^{3-}\) is high-spin complex.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Nuclear Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Inorganic 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.