Organic Chemistry
Organic Chemistry
8th Edition
ISBN: 9781305580350
Author: William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote
Publisher: Cengage Learning
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Chapter 1, Problem 1.78AP
Interpretation Introduction

Interpretation:

The bonding of PCl5 is to be described without using d-orbitals.

Concept introduction:

Hybridization is the process of combinations of atomic orbitals forms hybrid orbitals.

sp3 Hybrid orbital:

The combination of one s atomic orbital and three p atomic orbitals forms sp3 hybrid orbital.

sp2 Hybrid orbital:

The combination of one s atomic orbital and two p atomic orbitals forms sp2 hybrid orbital.

sp Hybrid orbital:

The combination of one s atomic orbital and one p atomic orbitals forms sp hybrid orbital.

According to VSPER theory the bond angle is depends on the valence electron of an atom. Valence electrons may be involved in the formation of single, double, or triple bonds or they may be unshared (lone pair) electrons.

According to VSPER theory,

  1. (1) Regions of electron density around the central atom are four, the geometry of the molecule may be tetrahedral and the bond angle is 109.5o.
  2. (2) Regions of electron density around the central atom is three, the geometry of the molecule may be trigonal planar and the bond angle is 120o.
  3. (3) Regions of electron density around the central atom are two, the geometry of the molecule may be linear and the bond angle is 180o.
Groups bonded to carbonOrbital hybridizationBond angleTypes of bond
4sp3109.5oFour σ bonds
3sp2120 oThree σ bonds and one π bond
2sp180 oTwo σ bonds and two π bond

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Chapter 1 Solutions

Organic Chemistry

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