Hybridization A Blending of Orbitals Methane CH 4 CH 4 Sometimes called “natural gas, ” methane is used to heat homes. Sometimes called “natural gas,

Slides:

Advertisements

Similar presentations

Orbitals and Covalent Bond

Advertisements

Molecular Shape Sect 9.4. VSEPR Model Valence Shell Electron Pair Repulsion Valence Shell Electron Pair Repulsion Electron pairs will position themselves.

Covalent Bonding Sec. 8.4: Molecular shape.

Covalent Bonding Sec. 8.4: Molecular shape. Objectives n Discuss the VSEPR bonding theory n Predict the shape of and the bond angles in a molecule n Define.

+ Wave Mechanics and Covalent Bond Formation Ch 9.

Hybrid Orbitals: Bonding in Complex Molecules 1-8 Mixing of atomic orbitals from the same atom results in new atomic orbitals of different energy and directionality.

Chapter 9 Chemical Bonding Theories Valence Bond Theory: Uses Lewis Structures Bonds form using shared electrons between overlapping orbitals on adjacent.

Chapter 9 Chemical Bonding Theories Valence Bond Theory: Uses Lewis Structures Bonds form using shared electrons between overlapping orbitals on adjacent.

Hybridisation of s and p orbitals in alkanes, alkenes and alkynes Unit 3.

Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.

Geometry of Molecules VSEPR Theory. Valence Shell Electron Pair Repulsion Theory (VSEPR) The geometry of the molecule at any given central atom is determined.

Medical Chemistry (1) 1433 – 1434 H. Carbon Compounds.

© Prentice Hall 2001Chapter 11 Atomic Orbitals We cannot know the exact course of electrons as they orbit the nucleus - Heisenberg uncertainty principle.

Hybridization of Orbitals Sections 9.1 and 9.5

Molecular Shape Section 9.4

Chapter 9 Chemical Bonding Theories

Orbitalsand Covalent Bonds. Atomic Orbitals Don’t Work n to explain molecular geometry. n In methane, CH 4, the shape s tetrahedral. n The valence electrons.

Hybridization of Atomic Orbitals Some Material Copyright PGCC CHM 101 Sinex Some Graphics from Nelson Chemistry 12 Textbook.

Bonding theory Two methods of approximation are used to describe bonding between atoms. Valence bond method Bonds are assumed to be formed by overlap of.

Covalent bonding in Methane: CH 4 Carbon: 1S 2 2S 2 2P 2 Energy is released as carbon forms covalent bonds and the more energy released the more stable.

Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.

14.2 HYBRIDIZATION. ESSENTIAL IDEA Hybridization results from the mixing of atomic orbitals to form the same number of new equivalent hybrid orbitals.

Hybridization and Other Good Stuff. Introduction A hybrid results from combining two of the same type of objects, and it has characteristics of both Atomic.

Orbital Hybridisation & VSEPR Learning Goals Students will be able to predict the hybridization in a variety of compounds using Lewis Structures & energy.

Chapter 9 Chemical Bonding Theories

Sections 9.1 – 9.3 Valence Bond Theory Hybrid Orbitals Sigma and Pi Bonding.

Bonding Theories Part 2: VSEPR Theory. Objectives Describe how VSEPR theory helps predict the shapes of molecules Describe how VSEPR theory helps predict.

To offer more in-depth explanations of chemical bonding more sophisticated concepts and theories are required 14.1 and 14.2 Hybridization 1.

1 s orbital 2 Bonding between two s orbitals This is called a sigma (  ) bond.

VSEPR & HYBRIDIZATION. Two Theories Which Reinforce Each Other VSEPR is essentially the theory which helps to explain molecular geometry (shape, and bond.

Lecture 43 Molecular Shapes Ozgur Unal 1.  Using the formula or the lewis structure of the following molecule, can you determine its three-dimensional.

COVALENT BONDING: ORBITALS Chapter 9. Hybridization The mixing of atomic orbitals to form special molecular orbitals for bonding. The atoms are responding.

4.6 Quantum Mechanics and Bonding: Hybridization.

Hybridization Carbon configuration Carbon in excited state can form 4 bonds.

To be viewed with PowerPoint. Animation doesn’t work otherwise.

H C Valence Shell Electron Pair Repulsion Theory 2p 2s 1s Ken Rogers

Hybrid Orbitals © Evan P. Silberstein, 2010.

SUPA Chemistry Sigma and Pi Bonds.

Ch 9 – Covalent Bonding: Orbitals

Chapter 2: Structure and Properties of Organic Molecules

Honors Chemistry Mrs. Coyle

Ch.14 Covalent Bonding Hybridization.

CHEMISTRY Matter and Change

Molecular Geometry and VESPR Theory (3.5)

TOPIC 14 CHEMICAL BONDING AND STRUCTURE

Orbitals and Covalent Bond

Structure & Properties of Matter

Molecular Geometry & Bonding Theories

The Nature of the Chemical Covalent Bond

Bonding Theories Part 2: VSEPR Theory.

Molecular Shapes and Hybrid Orbitals

Honors Chemistry Mrs. Coyle

Ch 9 – Covalent Bonding: Orbitals

Section 8.4 – Molecular Shapes

Qantum Mechanics and Bonding Hybridization

8.3 Molecular Orbitals When two atoms combine, the molecular orbital model assumes that their atomic orbitals overlap to produce molecular orbitals,

Chapter 1B Carbon Compounds and Chemical Bonds

Chemical formula and Lewis Structures Constitutional Isomers

Molecular Geometry and VESPR Theory (3.5)

Molecular Geometry and VESPR Theory (3.5)

Objectives To understand molecular structure and bond angles

Qantum Mechanics and Bonding Hybridization

Chapter 10 Chemical Bonding II: Sections

Orbital Bonding Theory

Hybridization -often, molecular geometry is based on hybrid orbitals

Hybridization and Molecular Orbitals

Hybridization College Chemistry.

Molecular Shapes VSEPR Model

Presentation transcript:

Hybridization A Blending of Orbitals

Methane CH 4 CH 4 Sometimes called “natural gas, ” methane is used to heat homes. Sometimes called “natural gas, ” methane is used to heat homes.

Shape of Methane Tetrahedral geometry Tetrahedral geometry o angle between bonds o angle between bonds

Carbon’s atomic orbitals 4 valence electrons 4 valence electrons Outermost orbitals: 2s, 2p x, 2p y, 2p z Outermost orbitals: 2s, 2p x, 2p y, 2p z

How can this happen?

2 possibilities Maybe our quantum mechanical model of atomic orbitals is totally wrong. Maybe our quantum mechanical model of atomic orbitals is totally wrong.OR Maybe carbon is doing something else with its orbitals to form this compound. Maybe carbon is doing something else with its orbitals to form this compound.

Hybridization occurs A mathematical blending of orbitals A mathematical blending of orbitals Number of atomic orbitals blended = number of hybrid orbitals produced Number of atomic orbitals blended = number of hybrid orbitals produced Result: Identical orbitals Result: Identical orbitals –New shape –New orientation in space

sp 3 hybridization s + p x + P y + p z = 4 sp 3 orbitals s + p x + P y + p z = 4 sp 3 orbitals

Sp 3 hybridization on carbon 4 identical sp 3 orbitals o between orbitals Tetrahedral orientation

Bonds form when orbitals overlap Sigma bonds: end to end overlap of orbitals Sigma bonds: end to end overlap of orbitals

What happens in ethene? C2H4C2H4C2H4C2H4 Properties Properties Double bond between carbons Double bond between carbons Trigonal planar geometry around C Trigonal planar geometry around C 120 o bond angles 120 o bond angles

Sp 2 hybridization occurs S + p x + p y = 3 sp 2 orbitals S + p x + p y = 3 sp 2 orbitals 1 unused p orbital left over 1 unused p orbital left over

Bonding in ethene Sigma bond: end to end overlap Sigma bond: end to end overlap Pi bond: side to side overlap Pi bond: side to side overlap

Putting ethene together Carbon-carbon double bond = 1 sigma bond and 1 Pi bond Carbon-carbon double bond = 1 sigma bond and 1 Pi bond 4 C-H sigma bonds 4 C-H sigma bonds Trigonal planar Trigonal planar geometry results geometry results

What happens in ethyne? C 2 H 2 C 2 H 2 Linear geometry Linear geometry What type of hybridization is involved? What type of hybridization is involved? What hybrid and atomic orbitals can it use? What hybrid and atomic orbitals can it use? What types and numbers of bonds are present in the molecule? What types and numbers of bonds are present in the molecule?