1.6 Atomic Orbitals General Chemistry review

Slides:



Advertisements
Similar presentations
1)Use your white board to draw the Lewis structure for ozone, O 3. 2)What does the word hybridization mean? Use your own words. While you are doing warm.
Advertisements

Word Splash – Write a few sentences about how the following terms are related.
Structure and Bonding in Organic Chemistry Electron Configurations Lewis Dot Structures Hybridization Orbital depictions.
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.
1 Compounds Containing Double Bonds Ethene or ethylene, C 2 H 4, is the simplest organic compound containing a double bond. Lewis dot formula N = 2(8)
1 1.5The Nature of Chemical Bonds: Valence Bond Theory Covalent bond forms when two atoms approach each other closely so that a singly occupied orbital.
Francis A. Carey, Organic Chemistry, Fourth Edition. Copyright © 2000 The McGraw-Hill Companies, Inc. All rights reserved. Plot of potential energy versus.
Hybridisation of s and p orbitals in alkanes, alkenes and alkynes Unit 3.
Orbital Hybridization Edward A. Mottel Department of Chemistry Rose-Hulman Institute of Technology.
Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.
Organic Chemistry Second Edition Chapter 1 David Klein
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.
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.
Molecular Orbital Theory Electrons in atoms exist in atomic orbitals Electrons in molecules exist in molecular orbitals (MOs) Using Schrödinger equation,
Covalent Bonding: orbitals. Hybridization - The Blending of Orbitals = = + +s orbitalp orbital sp orbital.
1 Organic Chemistry Instructor Data Professor Lev R. RyzhkovSM 553/551 Phone FAX Web: pages.towson.edu/ryzhkov
AP CHEMISTRY CHAPTER 9 BONDING 1. Hybridization 2.
Delocalization of Electrons Section Introduction Delocalization allows the pi electrons to spread over more than two nuclei This spreading out of.
General Chemistry Review
1.15 Bonding in Methane and Orbital Hybridization.
Hybridization A Blending of Orbitals Methane CH 4 CH 4 Sometimes called “natural gas, ” methane is used to heat homes. Sometimes called “natural gas,
Chapter 1: Structure and Bonding mcmurry. Coverage: 1. Electron Configurations. 2. Lewis Structures 3. Covalent and Ionic bonds 4. Atomic and Molecular.
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.
Lecture 2 Chemical Bonds: Atomic Orbital Theory and Molecular Orbital Theory Dr. A.K.M. Shafiqul Islam
HL Bonding Hybridisation. Hybridization is a model which is used to explain the behavior of atomic orbitals during the formation of covalent bonds. When.
Hybridization Section Introduction A hybrid results from combining 2 of the same type of object and it has characteristics of both Atomic orbitals.
1 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Organic Chemistry Second Edition Chapter 1 A Review of General Chemistry: Electrons, Bonds, and Molecular Properties David Klein Copyright © 2015 John.
14.2 HYBRIDIZATION. ESSENTIAL IDEA Hybridization results from the mixing of atomic orbitals to form the same number of new equivalent hybrid orbitals.
Hybridization: Localized Electron Model
Orbital Hybridisation & VSEPR Learning Goals Students will be able to predict the hybridization in a variety of compounds using Lewis Structures & energy.
Hybridization Combination of atomic orbitals to form hybrid orbitals OR Hybridization is also way to explain molecular shapes that can't be explained easily.
AP CHEMISTRY CHAPTER 9 BONDING. Hybridization When drawing Lewis structures to explain bonding, we have been using the Localized Electron Model of bonding.
Hybridization.
Bonding in methane The simplest alkane, methane, has the molecular formula CH 4. Justify that formula. Write the electronic configuration of carbon and.
4.6 Quantum Mechanics and Bonding: Hybridization.
Hybridization Carbon configuration Carbon in excited state can form 4 bonds.
Organic Chemistry Third Edition Chapter 1 David Klein
1.1 Organic Chemistry The study of carbon-containing molecules and their reactions What happens to a molecule during a reaction? A collision Bonds break/form.
What is Organic Chemistry?
Lecture 2 Chemical Bonds: Atomic Orbital Theory and Molecular Orbital Theory Dr. A.K.M. Shafiqul Islam
1.9 Hybridized Atomic Orbitals
18.2 Bonding in Methane and Orbital Hybridization
Hybrid Orbitals © Evan P. Silberstein, 2010.
Principals of Organic Chemistry مبادئ الكيمياء العضوية
Structure and Bonding in Organic Chemistry
Chapter 2: Structure and Properties of Organic Molecules
Honors Chemistry Mrs. Coyle
TOPIC 14 CHEMICAL BONDING AND STRUCTURE
Structure and Bonding in Organic Chemistry
11/23/15 ll ork 2: What do like charges do?
Chemical Bonding II: Molecular Geometry and Hybridization of Atomic Orbitals Chapter 9 Copyright © The McGraw-Hill Companies, Inc.  Permission required.
Sigma () and Pi () Bonds
HYBRIDIZATION SIGMA AND PI BONDS
Honors Chemistry Mrs. Coyle
18.2 Valence bond theory: hybridized orbitals and polyatomic molecules
Qantum Mechanics and Bonding Hybridization
Chapter 1B Carbon Compounds and Chemical Bonds
Sigma () and Pi () Bonds
Organic Chemistry Second Edition Chapter 1 David Klein
Qantum Mechanics and Bonding Hybridization
Orbital Bonding Theory
Hybridization -often, molecular geometry is based on hybrid orbitals
Figure 1. 1: The position of carbon in the periodic table
Hybridization College Chemistry.
Hybridized Atomic Orbitals
Factors Affecting CB Stability: IO
Bonding Theory Overview
Covalent Bonding and Shapes of Molecules
Presentation transcript:

1.6 Atomic Orbitals General Chemistry review The type or orbital be identified by its shape An orbital is a region where there is a calculated 90% probability of finding an electron. The remaining 10% probability tapers off as you move away from the nucleus Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.6 Atomic Orbitals Because they are generated mathematically from wavefunctions, orbital regions can also be (–), (+), or ZERO The sign of the wave function has nothing to do with electrical charge. In this p-orbital, there is a nodal plane. The sign of the wavefunction will be important when we look at orbital overlapping in bonds. Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.6 Atomic Orbitals Electrons are most stable (lowest in energy) if they are in the 1s orbital The 1s orbital is full once there are two electrons in it. Why can’t it fit more? The 2s orbital is filled next. The 2s orbital has a node. WHERE? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.6 Atomic Orbitals Once the 2s is full, electrons fill into the three degenerate 2p orbitals Where are the nodes in each of the 2p orbitals? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals Given the electron configuration for C and H, imagine how their atomic orbitals might overlap Would such orbital overlap yield methane? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals To make methane, the C atom must have 4 atomic orbitals available for overlapping If an electron is excited from the 2s to the 2p, will that make it suitable for making methane? If four H atoms were to come in and overlap with the 2s and 2p orbitals, what geometry would the resulting methane have? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals The carbon must undergo hybridization to form 4 equal atomic orbitals The atomic orbitals must be equal in energy to form four equal-energy symmetrical C-H bonds Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals Should the shape of an sp3 orbital look more like an s or more like p orbital? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals To make CH4, the 1s atomic orbitals of four H atoms will overlap with the four sp3 hybrid atomic orbitals of C Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals Consider ethene (ethylene). Each carbon in ethene must bond to three other atoms, so only three hybridized atomic orbitals are needed Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals An sp2 hybridized carbon will have three equal-energy sp2 orbitals and one unhybridized p orbital Which is lower in energy, the sp2 or the p? Why? Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals The sp2 atomic orbitals overlap to form sigma (σ) bonds Sigma bonds provide maximum HEAD-ON overlap Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals The unhybridized p orbitals in ethene form pi (π) bonds, SIDE-BY-SIDE overlap Practice with conceptual checkpoint 1.20 Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals Consider ethyne (acetylene). Each carbon in ethyne must bond to two other atoms, so only two hybridized atomic orbitals are needed Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.9 Hybridized Atomic Orbitals The sp atomic orbitals overlap HEAD-ON to form sigma (σ) bonds while the unhybridized p orbitals overlap SIDE-BY-SIDE to form pi bonds Practice with SkillBuilder 1.7 Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e

1.10 Geometry Summary Practice with SkillBuilder 1.8 Copyright © 2015 John Wiley & Sons, Inc. All rights reserved. Klein, Organic Chemistry 2e