Last edited by Molrajas
Monday, May 4, 2020 | History

7 edition of Orbitals in Chemistry found in the catalog.

Orbitals in Chemistry

A Modern Guide for Students

by Victor M. S. Gil

  • 193 Want to read
  • 27 Currently reading

Published by Cambridge University Press .
Written in English

    Subjects:
  • PHYSICS,
  • Quantum & theoretical chemistry,
  • Molecular Chemistry,
  • Science,
  • Science/Mathematics,
  • Chemistry - Industrial & Technical,
  • Chemistry - Physical & Theoretical,
  • Science / Chemistry / General,
  • Molecular orbitals

  • The Physical Object
    FormatHardcover
    Number of Pages326
    ID Numbers
    Open LibraryOL7750744M
    ISBN 100521661676
    ISBN 109780521661676

    This text presents a unified and up-to-date discussion of the role of atomic and molecular orbitals in chemistry, from the quantum mechanical foundations to recent developments and applications. Abundantly illustrated, the volume critically establishes the relationships between the more formal Price: $ Get this from a library! Orbitals in chemistry: modern guide for students. [Victor M S Gil] -- This text presents a unified and up-to-date discussion of the role of atomic and molecular orbitals in chemistry, from the quantum mechanical foundations to the recent developments and applications.

    In chemistry, orbital hybridisation (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond orbitals are very useful in the explanation of molecular geometry and atomic bonding properties and are. We use the 3s orbital, the three 3p orbitals, and one of the 3d orbitals to form the set of five sp 3 d hybrid orbitals (Figure ) that are involved in the P–Cl bonds. Other atoms that exhibit sp 3 d hybridization include the sulfur atom in SF 4 and the chlorine atoms in ClF 3 and in ClF 4 +.

    Summary Summary: Orbitals This SparkNote presents two approaches to describing orbitals in molecules: the Valence Bond (VB) model and the Molecular Orbital (MO) model. The VB model, which is an extension of Lewis structures, assumes that covalent bonds are the overlap of individual atomic orbitals. Check our section of free e-books and guides on Molecular Chemistry now! This page contains list of freely available E-books, Online Textbooks and Tutorials in Molecular Chemistry Molecular Chemistry Books. Trigonal Bipyramidal arrangment, Polarity, Overlap and Bonding, Hybrid Orbitals, Valence Bond Theory, Single Bonds, Multiple Bonds.


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Orbitals in Chemistry by Victor M. S. Gil Download PDF EPUB FB2

"Orbitals in Chemistry" is invaluable in explaining the concepts behind the complex derivations and cryptic explanations found in Levine's "Physical Chemistry".

Nothing can make physical chemistry easy. This book included. But it is a book definitely written for by: 3. This volume is a result of our attempt to establish a theory of chemistry in terms of orbitals ― A Chemical Orbital Theory.

The amplitude of orbitals represents a spatial extension of orbitals. An orbital strongly interacts with others at the position and in the direction of great : Hardcover.

This book describes atomic orbitals at a level suitable for undergraduates in chemistry. The mathematical treatment is brought to life by many illustrations rendered from mathematical functions (no artists' impressions), including three-dimensional plots of angular functions, showing orbital phase, and contour plots of the wavefunctions that result from orbital hybridisation.5/5(1).

This book describes atomic orbitals at a level suitable for undergraduates in chemistry. The mathematical treatment is brought to life by many illustrations rendered from mathematical functions (no artists' impressions), including three-dimensional plots of angular functions, showing orbital phase, and contour plots of the wavefunctions that result from orbital cturer: ICP.

System Upgrade on Tue, May 19th, at 2am (ET) During this period, E-commerce and registration of new users may not be available for up to 12 hours. The amplitude of orbitals represents a spatial extension of orbitals. An orbital strongly interacts with others at the position and in the direction of great extension.

Orbital amplitude controls the reactivities and selectivities of chemical reactions. Shapes of Orbitals of an Atom What is orbital. In chemistry, an orbital is a mathematical function which portrays the wave-like Orbitals in Chemistry book of an electron pair, electron or nucleons in Quantum Mechanics and Chemistry.

Orbitals are also referred to as electron or Orbitals in Chemistry book orbitals. Atomic orbitals are the three- dimensional regions of space around the [ ]. Orbital Interactions in Chemistry begins by developing models and reviewing molecular orbital theory.

Next, the book explores orbitals in the organic-main group as well as in solids. Next, the book explores orbitals in the organic-main group as well as in by: Molecular orbital theory describes the distribution of electrons in molecules in much the same way that the distribution of electrons in atoms is described using atomic orbitals.

Using quantum mechanics, the behavior of an electron in a molecule is still described by a wave function, Ψ. The four basic types of orbitals are designated as s, p, d, and f. An atomic orbital is the probability description of where an electron can be found.

Atomic Structure - Orbitals - Chemistry LibreTexts. This concise, highly regarded text on the nature of orbitals, terms, and states offers a fine introduction to quantum chemistry.

The treatment is especially suitable for students with a limited mathematical background. Topics include atomic and molecular spectroscopy, quantum mechanics, and /5(2).

These prop- ties are well represented by orbitals, which contain the amplitude and phase ch- acteristics of waves. This volume is a result of our attempt to establish a theory of chemistry in terms of orbitals — A Chemical Orbital Theory.

The amplitude of orbitals represents a spatial extension of orbitals. The Organic Chemist's Book of Orbitals focuses on the mechanisms, stereochemistry, and reactivity of molecular orbitals.

Composed of four chapters, the book outlines how molecular orbitals are created by delocalization. Concerns include CC and CH single-bond orbitals; bond orbitals and group orbitals; and the localized orbitals of CH2 and CH3.

The 1s orbital on the Oxygen atom is clearly a nonbonding core orbital. The Oxygen 2s orbital and its three 2p orbitals are of valence type, as are the two Hydrogen 1s orbitals. In the absence of symmetry, these six valence orbitals would give rise to a 6x6 secular problem.

Orbital, in chemistry and physics, a mathematical expression, called a wave function, that describes properties characteristic of no more than two electrons in the vicinity of an atomic nucleus or of a system of nuclei as in a molecule. An orbital often is depicted as a three-dimensional region.

The linear combination of atomic orbitals always gives back the same number of molecular orbitals. So if we start with two atomic orbitals (e.g., an s and a p z orbital as shown in Fig.

\(\PageIndex{1}\)), we end up with two molecular orbitals. When atomic orbitals add in phase, we get constructive interference and a lower energy orbital. In chemistry and quantum mechanics, an orbital is a mathematical function that describes the wave-like behavior of an electron, electron pair, or (less commonly) nucleons.

An orbital may also be called an atomic orbital or electron orbital. Although most people think of an "orbit" regarding a circle, the probability density regions that may contain an electron may be spherical, dumbbell-shaped. The orbitals are described completely by specifying three quantum numbers, but only two are used in this book.

The principal quantum number (symbolized n) is a whole number, 1 or greater, that identifies the main energy shell of the orbital, with 1 being closest to the nucleus and each subsequent level farther from the second quantum number, known as the azimuthal quantum number.

Molecular orbital theory holds, as its name suggests, that electrons reside in molecular orbitals that are distributed over the entire molecule. Quantum mechanics specifies that we can get molecular orbitals through a linear combination of atomic orbitals; that is, by adding and subtracting them.

Source: Purcell + Kotz, Inorganic Chemistry, These are determined by quantum numbers l and m l. Resulting orbital shapes: Note that the orbitals are 3D waves.

All atomic orbitals of a given atom must be orthogonal to one another. The surface is typically the 75% probability boundary. This volume is a result of our attempt to establish a theory of chemistry in terms of orbitals - A Chemical Orbital Theory.

The amplitude of orbitals represents a spatial extension of orbitals. An orbital strongly interacts with others at the position and in the direction of great : Satoshi Inagaki.Molecular Orbitals and Organic Chemical Reactions is both a simplified account of molecular orbital theory and a review of its applications in organic chemistry; it provides a basic introduction to the subject and a wealth of illustrative examples.

In this book molecular orbital theory is presented in a much simplified, and entirely non.In excess of problems with full worked answers at all levels are provided and will certainly become a major teaching resource.” Richard G Compton Tutor in Chemistry St John's College Oxford University, UK This book describes atomic orbitals at a level suitable for undergraduates in chemistry.5/5(1).