study guide ch 1 pt 3 - Professor M. J. Krische Chemistry...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Chemistry 318M, Fall 2008 Chapter 1-Study Guide (Part 3 ) I. The Electronic Structure of Organic Molecules (Chapters 1) i. Historical Perspective ii. Lewis Structures iii. Molecular Shape (VSEPR) iv. Resonance Structures v. Atomic Orbitals vi. Molecular Orbitals vii. Hybrid Atomic Orbitals viii. Functional Groups vii. Hybrid Atomic Orbitals We know from VSEPR that methane (CH 4 ) has a tetrahedral geometry. If we try to construct methane (CH 4 ) using the atomic orbitals of carbon (2s 2 p x 1 p y 1 or 2s 1 p x 1 p y 1 p z 1 ) and hydrogen, we obtain an H-C-H bond angle of 90 o . This is inconsistent with the observed bond angle of methane of 109.5 o . How can this be? Atomic orbitals on the same atom can "mix" to give hybrid orbitals that are simply the sum and difference of the two orbitals. Again, the total number of orbitals is conserved. For example, an s-orbital and a p-orbital may combine to give two “sp-hybrid” orbitals that possess 50% s- and 50% p-orbital character. Similarly, an s-orbital and 2 p-orbitals may combine to give two “sp
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 02/09/2009 for the course CH 318M taught by Professor Bocknack during the Fall '08 term at University of Texas at Austin.

Page1 / 4

study guide ch 1 pt 3 - Professor M. J. Krische Chemistry...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online