Carbon’s valence electrons?. Hybrid Orbitals  Mixing of valence shell orbitals to form new similar orbitals for bonding electrons.

Slides:



Advertisements
Similar presentations
Covalent Bonding: Orbitals
Advertisements

Chapter 9 Molecular Geometry and Bonding Theories
1 Covalent Bonding: Molecular Geometry Hybridization of Atomic Orbitals Molecular Orbitals.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.
Molecular Geometry & Bonding Theories
1 Covalent Bonding: Orbitals Chapter The four bonds around C are of equal length and Energy.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Covalent Bonding: Orbitals Chapter 09.
Chapter 9 Molecular Geometry and Bonding Theories.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Daniel L. Reger Scott R. Goode David W. Ball Chapter 10 Molecular Structure and Bonding Theories.
Chemistry 100 Chapter 9 Molecular Geometry and Bonding Theories.
Molecular Geometry and Bonding Theories 9.1 Molecular Shapes The size and shape of a molecule of a particular substance play an important part in determining.
PowerPoint Lecture Presentation by J
Chapter 10 Chemical Bonding II. Lewis Structure  Molecular Structure Structure determines chemical properties.
Base Pairing in DNA. Red = O Grey = C White = H Purple = K Ionic Radii Li + = 0.68 Å Na + = 0.97 Å K + = 1.33 Å Rb + = 1.47 Å Cavity Size (O-O Dist.)
AP Chemistry Chapters 9. Vocab (Ch 9) VSEPR- Valence Shell e- Pair Repulsion bonding pair non bonding pair – lone pair of electrons electron domain –
Chapter 10: Covalent Bond Theories
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.
Chapter 9 Molecular Shapes -shape of molecule is based on bond angles Valence Shell Electron Pair Repulsion (VSEPR) -based on the idea that electron groups.
AP CHEMISTRY CHAPTER 9 BONDING. Hybridization When drawing Lewis structures to explain bonding, we have been using the Localized Electron Model of bonding.
Chapter 9 Covalent Bonding: Orbitals. Chapter 9 Table of Contents 2 Return to TOC Copyright © Cengage Learning. All rights reserved 9.1 Hybridization.
Chapter 9 Covalent Bonding: Orbitals. Copyright © Cengage Learning. All rights reserved 2 Draw the Lewis structure for methane, CH 4. –What is the shape.
AP CHEMISTRY CHAPTER 9 BONDING 1. Hybridization 2.
COVALENT BONDING Chapter 16 AND THE SUBJECTS ARE… THE NAME IS BOND, COVALENT BOND SINGLES, DOUBLES & TRIPPPLES COORDINATE COVALENT BONDS RESONATE THIS!
MOLECULAR STRUCTURE CHAPTER 14 Experiments show O 2 is paramagnetic.
Covalent Bonding Orbitals Adapted from bobcatchemistry.
By: Maggie Dang. 9.1 Molecular Shapes  The overall shape of a molecule is determined by its bond angles, the angles made by the lines joining the nuclei.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.
Molecular Geometry and Bonding Theories. Physical and chemical properties of a molecule are determined by: size and shape strength and polarity of bonds.
1 Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Bonding II: Molecular Geometry and Hybridization.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Molecular Geometry & Bonding Theories Chapter 9. Molecular Shapes  Lewis Structures that we learned do not tell us about shapes, they only tell us how.
Dipole Moments and Polar Molecules 10.2 H F electron rich region electron poor region    = Q x r Q is the charge r is the distance between charges.
Molecular Geometries and Bonding Chapter Bonding Theory Valence Bond Theory Molecular Orbital Theory Complete Ch 9 problems # 29, 36, 38, 39, 42,
Ch. 9 Molecular Geometry & Bonding Theories
Covalent Bonding: Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Molecular Geometry and Bonding Theories
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.
AP CHEMISTRY CHAPTER 9 BONDING. Hybridization When drawing Lewis structures to explain bonding, we have been using the Localized Electron Model of bonding.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc. Permission required.
1 Molecular Geometry and Hybridization of Atomic Orbitals.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Chapter 9 Notes AP CHEMISTRY Galster.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Unit 2.3: Chemical Bonding
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Rules for Predicting Molecular Geometry   1.  Sketch the Lewis structure of the molecule or ion 2.  Count the electron pairs and arrange them in.
Molecular Orbital Theory
Let’s Focus on Valence Bond Theory
Sigma (s) and Pi Bonds (p)
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Covalent bonds are formed by:
Valence Shell Electron Pair Repulsion Theory
Chapter 9 – Molecular Geometry and Bond Theory
Covalent Bonding: Orbitals
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Ch. 9 Molecular Geometry & Bonding Theories
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 10.
The Central Themes of VB Theory
DEPARTMENT OF CHEMISTRY
Presentation transcript:

Carbon’s valence electrons?

Hybrid Orbitals  Mixing of valence shell orbitals to form new similar orbitals for bonding electrons.

Formation of sp 3 Hybrid Orbitals

Formation of sp 2 Hybrid Orbitals

Formation of sp Hybrid Orbitals

sp hybrid orbital – from an s and a p orbital sp 2 hybrid orbital – from 1 s and 2 p orbitals sp 3 hybrid orbital – from 1 s and 3 p orbitals...

# of Lone Pairs + # of Bonded Atoms HybridizationExamples sp sp 2 sp 3 sp 3 d sp 3 d BeCl 2 BF 3 NH 3, H 2 O PCl 5 SF 6

Sigma (  ) Bond Electron pair shared in an area between the atoms. Pi (  ) Bond Forms double and triple bonds by sharing electron pair(s) in the space above and below the σ bond. Uses the unhybridized p orbitals.

The Orbitals for CO 2

Sigma (  ) and Pi Bonds (  ) Single bond 1 sigma bond Double bond 1 sigma bond and 1 pi bond Triple bond 1 sigma bond and 2 pi bonds How many  and  bonds are in the acetic acid molecule CH 3 COOH? C H H CH O OH  bonds = = 7  bonds = 1

Bonding Order (non-MO method) Number of bonding electron pairs between two bonded atoms The larger the bond order, the stronger the bond Bond order = total number of bonding pairs number of bonding locations Single bonds: bond order = 1 Double bonds: = 2 Triple bonds: = 3 Resonance: an average of the resonance structures

 For a molecule to be polar, at least one bond must be polar.

 If there is no dipole, the molecule is nonpolar  If there is a dipole (usually asymmetrical), the molecule is polar

.. :H:.. │.. :Cl−C −Cl: ˙ ˙ │ ˙ ˙ :H: ˙˙ Polar or nonpolar?

 Bond polarity: electronegativity difference  Molecule polarity: 1) must have a polar bond 2) asymmetrical shape

Which of the following molecules have a dipole moment? H 2 O, CO 2, SO 2, and CH 4 O H H dipole moment polar molecule S O O CO O no dipole moment nonpolar molecule dipole moment polar molecule C H H HH no dipole moment nonpolar molecule

Polarity of Molecules Dipole Moments of Polyatomic Molecules Example: CO 2 : There is no C-O dipole because of the molecule’s shape. H 2 O: there is an overall dipole (separation of central positions of partial positive and negative charges) because the molecule is bent.

Polarity of Molecules Dipole Moments of Polyatomic Molecules

Optional: Energy levels of bonding and antibonding molecular orbitals in hydrogen (H 2 ). A bonding molecular orbital has lower energy and greater stability than the atomic orbitals from which it was formed. An antibonding molecular orbital has higher energy and lower stability than the atomic orbitals from which it was formed.

1.The number of molecular orbitals (MOs) formed is always equal to the number of atomic orbitals combined. 2.The more stable the bonding MO, the less stable the corresponding antibonding MO. 3.The filling of MOs proceeds from low to high energies. 4.Each MO can accommodate up to two electrons. 5.Use Hund’s rule when adding electrons to MOs of the same energy. 6.The number of electrons in the MOs is equal to the sum of all the electrons on the bonding atoms. Optional: Molecular Orbital (MO) Configurations

bond order = 1 2 Number of electrons in bonding MOs Number of electrons in antibonding MOs ( - ) bond order ½10½ Optional

Molecular orbital theory – bonds are formed from interaction of atomic orbitals to form molecular orbitals. O O No unpaired e - Should be diamagnetic Experiments show O 2 is paramagnetic

Delocalized molecular orbitals are not confined between two adjacent bonding atoms, but actually extend over three or more atoms.