MOLECULAR STRUCTURE. The general molecular Schrödinger equation, apart from electron spin effects, is. nn ee en
|
|
- Noreen Alberta Jennings
- 5 years ago
- Views:
Transcription
1 MOLECULAR STRUCTURE The Born-Oppenheimer Approximation The general molecular Schrödinger equation, apart from electron spin effects, is ( ) + + V + V + V =E nn ee en T T ψ ψ n e where the operators in the Hamiltonian are the kinetic energy operators of the nuclei and the electrons, and then the potential energy operators between the nuclei, between the electrons, and between the nuclei and electrons.
2 Coordinates are defined below for a three nucleus, three electron molecule. Definition of distances in a molecule
3 In general, the explicit forms of these operators are as follows nuclei = n M α α α T T e electrons = m i=1 e i V nn nuclei α β = α β> α Z Z e R αβ V ee e = i=1 j>i r electrons ij V en nuclei electrons = α i There is a repulsive interaction among the nuclear charges and a repulsive charge-charge interaction among the electrons. However, the interaction potential between electrons and nuclei is attractive, since the particles have opposite charges. This particular interaction couples the motions of the electrons and the motions of the nuclei. Z e α r i α
4 T n = α α M α nuclei T e = electrons m i=1 e i V nn = nuclei α β> α ZZe α β Rαβ V ee = electrons e r i=1 j>i ij V en = nuclei electrons α i Zα e riα
5 Born-Oppenheimer Approximation The wavefunctions that satisfy this Hamiltonian must be functions of both the electron position coordinates and the nuclear position coordinates, and this differential equation is not separable. In principle, true solutions could be found, but this is a formidable differential equation to work with. An alternative is an approximate (but generally a very good approximation) separation of the differential equation based upon the very large difference between the mass of an electron and the masses of the nuclei. The difference suggests that the nuclei will be sluggish in their motions relative to the electron motions. Over a brief period of time, the electrons will "see" " the nuclei as if fixed in space; the nuclear motions will be relatively slight. The nuclei, on the other hand,,will "see" the electrons as something of a blur, given their fast motions. We can thus solve for electronic properties with fixed nuclei.
6 ( T + T + V + V + V ) Ψ( R, r, ) =E Ψ( R, r, ) nn ee en 1 1 n e So when the Born-Oppenheimer approximation is invoked, Ψ( Rr,,...) = c φψ φ Rψ r,... ( ) R ( ) 1 ij i j i j 1 i j Electronic: [T e + V ee + V (R) en] ψ (R) (r,r,...) = E (R) (R) 1 ψ (r 1,r,...) Nuclear: [T n +(V nn + E (R) ) E] φ = 0 R represents nuclear coordinates r i represents electron coordinates
7 It is the Born-Oppenheimer approximation that leads to the concept of potential ti energy surfaces!
8 Potential Energy Surfaces A potential energy surface is a representation of a function of all the internal coordinates of a molecular system. For even a simple molecule such as ammonia, the potential ti is a function of six coordinates, making is difficult to display or to visualize. We may, however, make a graphical representation of a slice through the multidimensional surface. The slice is the potential function with all but one or two of the coordinates fixed at certain chosen values. If all but one are fixed, the slice is a function of only that one coordinate and its representation is a potential curve. If all but two are fixed, the slice is a function of two coordinates. As an example, look at linear HCN Contour Plot of HCN Ground State
9 Functions of two coordinates are easily represented by contour diagrams. This is a very common method to present potential energy surface slices, as shown in the previous picture. The curves that we see in this figure connect equipotential points on the potential energy surface. Cutting across one of these curves means going "uphill" or "downhill" in energy. Usually, we may identify a lowest energy point on a slice though a potential energy surface (i.e., a two-dimensional contour plot), and as above, that point lies near the middle of the diagram. The contour plot can only show us that the potential is uphill in two directions away from this point. In the other directions, the ones that were fixed to create the slice, the surface might be sloping upward or downward. Should it be that the surface slopes upward in every direction, i then the point is a minimum energy point or minimum on the surface. For complicated surfaces, s it is possible for there to be several minima, and the one of lowest energy is called the global minimum. The global minimum is a point on the surface that corresponds to the equilibrium structure of the species.
10 A slice of a hypothetical potential energy surface of a hypothetical linear triatomic molecule ABC is shown below. One can envision several possible chemical processes taking place in this collinear configuration. This diagram extends to the regions where the molecule is dissociated into the diatomic AB and atom C and where it is dissociated into the diatomic BC and atom A. The minimum is near the lower left. Stretching either bond, which means increasing either coordinate, is an uphill process. However, there is a unique point in the A-B stretching where the potential will start to be downhill. This point, called a saddle point, is where the potential surface is uphill in each direction except one, and in that one direction, the potential is downhill, either forward or backward. Fig. Contour Plot of a Slice of a Representative Molecule ABC.
11 If we follow the contour plot of Fig to the right of the saddle point, we encounter a trough. This is simply a region where the potential is slowly changing, either upward or downward, along one direction. Eventually, this trough will have a flat bottom and walls that do not change with the A-B separation as the point is reached where the A atom is completely removed from the BC diatomic and there is no interaction. At this limit (far right of Fig. ), a cut through this two-dimensional surface for any A-B distance is a potential curve; it is the potential energy as a function of the B-C separation, which is just the stretching potential of the BC diatomic. Likewise, a horizontal cut across the top left of the surface in Fig. must be the stretching potential for the AB diatomic molecule. l
12 The bottom of a trough that connects limiting regions such as these with minima or with saddle points is called a minimum energy path. That is a good term, especially if we consider the potential surface as if it were a physical surface with real hills and valleys. If we were at the bottom of the trough on the far right of the surface in Fig. and wished to "hike" to the equilibrium structure on the lower left, the minimum climb would take us right through h the saddle point and then down the valley where the potential minimum is found. That is the minimum energy path. Notice that it does not follow any one coordinate direction. At the outset, it follows the direction of the coordinate of the horizontal axis. Then it twists a bit, and if we follow it further, it will follow the direction of the coordinate of the vertical axis.
13 Linear ABC and the Reaction Path Concept The bottom of a trough that connects limiting regions such as these with minima or with saddle points is called the minimum energy path.
14 Energetic profiles for reactions, interconversions, and isomerizations are often given as simple curves of potential energy (vertical axis) versus a reaction coordinate (horizontal axis). This is not as abstract a notion as it may seem, because the minimum energy path provides a perfectly acceptable reaction coordinate. That is, each step along a reaction coordinate is a step along the minimum i energy path. In this sense, energy profiles are simply special slices through potential energy surfaces. Again, the Born- Oppenheimer approximation has provided the basis for an important chemical concept, and it provides the context for discussing details of reaction energetics.
15 The H + ION We have seen how the Born-Oppenheimer Approximation allows us to separate nuclear motion from electronic motion and leads to the concept of molecular potential energy surfaces. This concept is at the heart of all of our understanding of chemical processes. With this approximation made, we then attempt to solve the one-electron molecule, H +. As with the H atom, these wave functions will become our building blocks to construct larger systems. Unlike the H-atom, where our answer was exact, we will resort to approximations for the one electron molecule. With the Born-Oppenheimer approximation, the H + Hamiltonian becomes ˆ = e e e + + H me r A r B R AB H
16 This Hamiltonian is separable in the confocal cylindrical i l coordinate system shown below, but we will not pursue the detailed solution in that system. Note however that we have the SAME symmetry y about the z-axis that we had in the H atom problem.
17 This means that we will obtain a Φ equation just like the one we saw for H, d Φ m = Φ d φ ( φ ) which h will have quantized solutions Φ(φ) = e imφ, with m = 0, ±1, ±,... As before, these values of m must reflect the quantized component of angular momentum along the z- axis. (Think about the H atom in an external electric field directed along z.) The m quantum number is given a Greek letter designation m Orbital 0 σ ±1 π ± δ Why are the values of m that are greater than 0 are doubly degenerate??
18 In complete analogy with the use of one electron ion orbitals to build up many electron atoms, these one electron molecular orbitals are our building blocks for many electron molecules. The many electron molecular wave functions are built up as products of one electron orbitals, and we then antisymmetrize the product function. We obtain Hartree-Fock limiting forms and add take correlation effects into account as for atoms. As for atoms, we must be concerned with TOTAL spin and angular momentum. The molecular cases become more complex as a result of the non-spherical molecular symmetry. Whil t t l t m l l m st b th While our prototype one electron molecule must be the general heteronuclear diatomic AB n+, we will first look at H +, and extend the treatment to H and other homonuclear diatomics. We then look at bonding in the heteronuclear diatomics.
QUANTUM MECHANICS AND MOLECULAR STRUCTURE
6 QUANTUM MECHANICS AND MOLECULAR STRUCTURE 6.1 Quantum Picture of the Chemical Bond 6.2 Exact Molecular Orbital for the Simplest Molecule: H + 2 6.3 Molecular Orbital Theory and the Linear Combination
More informationChemistry 2000 Lecture 1: Introduction to the molecular orbital theory
Chemistry 2000 Lecture 1: Introduction to the molecular orbital theory Marc R. Roussel January 5, 2018 Marc R. Roussel Introduction to molecular orbitals January 5, 2018 1 / 24 Review: quantum mechanics
More informationLecture 10. Born-Oppenheimer approximation LCAO-MO application to H + The potential energy surface MOs for diatomic molecules. NC State University
Chemistry 431 Lecture 10 Diatomic molecules Born-Oppenheimer approximation LCAO-MO application to H + 2 The potential energy surface MOs for diatomic molecules NC State University Born-Oppenheimer approximation
More informationElectron States of Diatomic Molecules
IISER Pune March 2018 Hamiltonian for a Diatomic Molecule The hamiltonian for a diatomic molecule can be considered to be made up of three terms Ĥ = ˆT N + ˆT el + ˆV where ˆT N is the kinetic energy operator
More informationLecture 9: Molecular Orbital theory for hydrogen molecule ion
Lecture 9: Molecular Orbital theory for hydrogen molecule ion Molecular Orbital Theory for Hydrogen Molecule Ion We have seen that the Schrödinger equation cannot be solved for many electron systems. The
More information3: Many electrons. Orbital symmetries. l =2 1. m l
3: Many electrons Orbital symmetries Atomic orbitals are labelled according to the principal quantum number, n, and the orbital angular momentum quantum number, l. Electrons in a diatomic molecule experience
More informationCHEM-UA 127: Advanced General Chemistry I
1 CHEM-UA 127: Advanced General Chemistry I I. OVERVIEW OF MOLECULAR QUANTUM MECHANICS Using quantum mechanics to predict the chemical bonding patterns, optimal geometries, and physical and chemical properties
More informationChemistry 334 Part 2: Computational Quantum Chemistry
Chemistry 334 Part 2: Computational Quantum Chemistry 1. Definition Louis Scudiero, Ben Shepler and Kirk Peterson Washington State University January 2006 Computational chemistry is an area of theoretical
More information(1/2) M α 2 α, ˆTe = i. 1 r i r j, ˆV NN = α>β
Chemistry 26 Spectroscopy Week # The Born-Oppenheimer Approximation, H + 2. Born-Oppenheimer approximation As for atoms, all information about a molecule is contained in the wave function Ψ, which is the
More informationCHEM3023: Spins, Atoms and Molecules
CHEM3023: Spins, Atoms and Molecules Lecture 3 The Born-Oppenheimer approximation C.-K. Skylaris Learning outcomes Separate molecular Hamiltonians to electronic and nuclear parts according to the Born-Oppenheimer
More informationCHAPTER 11 MOLECULAR ORBITAL THEORY
CHAPTER 11 MOLECULAR ORBITAL THEORY Molecular orbital theory is a conceptual extension of the orbital model, which was so successfully applied to atomic structure. As was once playfuly remarked, a molecue
More informationVALENCE Hilary Term 2018
VALENCE Hilary Term 2018 8 Lectures Prof M. Brouard Valence is the theory of the chemical bond Outline plan 1. The Born-Oppenheimer approximation 2. Bonding in H + 2 the LCAO approximation 3. Many electron
More informationExp. 4. Quantum Chemical calculation: The potential energy curves and the orbitals of H2 +
Exp. 4. Quantum Chemical calculation: The potential energy curves and the orbitals of H2 + 1. Objectives Quantum chemical solvers are used to obtain the energy and the orbitals of the simplest molecules
More informationwbt Λ = 0, 1, 2, 3, Eq. (7.63)
7.2.2 Classification of Electronic States For all diatomic molecules the coupling approximation which best describes electronic states is analogous to the Russell- Saunders approximation in atoms The orbital
More informationMolecular energy levels
Molecular energy levels Hierarchy of motions and energies in molecules The different types of motion in a molecule (electronic, vibrational, rotational,: : :) take place on different time scales and are
More informationThe Potential Energy Surface (PES) Preamble to the Basic Force Field Chem 4021/8021 Video II.i
The Potential Energy Surface (PES) Preamble to the Basic Force Field Chem 4021/8021 Video II.i The Potential Energy Surface Captures the idea that each structure that is, geometry has associated with it
More informationCh120 - Study Guide 10
Ch120 - Study Guide 10 Adam Griffith October 17, 2005 In this guide: Symmetry; Diatomic Term Symbols; Molecular Term Symbols Last updated October 27, 2005. 1 The Origin of m l States and Symmetry We are
More informationChapter 9. Molecular Geometry and Bonding Theories
Chapter 9. Molecular Geometry and Bonding Theories 9.1 Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. The shape of a molecule
More informationStructure of diatomic molecules
Structure of diatomic molecules January 8, 00 1 Nature of molecules; energies of molecular motions Molecules are of course atoms that are held together by shared valence electrons. That is, most of each
More informationMolecular Term Symbols
Molecular Term Symbols A molecular configuration is a specification of the occupied molecular orbitals in a molecule. For example, N : σ gσ uπ 4 uσ g A given configuration may have several different states
More informationNPTEL/IITM. Molecular Spectroscopy Lectures 1 & 2. Prof.K. Mangala Sunder Page 1 of 15. Topics. Part I : Introductory concepts Topics
Molecular Spectroscopy Lectures 1 & 2 Part I : Introductory concepts Topics Why spectroscopy? Introduction to electromagnetic radiation Interaction of radiation with matter What are spectra? Beer-Lambert
More informationChem 442 Review for Exam 2. Exact separation of the Hamiltonian of a hydrogenic atom into center-of-mass (3D) and relative (3D) components.
Chem 44 Review for Exam Hydrogenic atoms: The Coulomb energy between two point charges Ze and e: V r Ze r Exact separation of the Hamiltonian of a hydrogenic atom into center-of-mass (3D) and relative
More informationChapter 9. Molecular Geometry and Bonding Theories
Chapter 9. Molecular Geometry and Bonding Theories PART I Molecular Shapes Lewis structures give atomic connectivity: they tell us which atoms are physically connected to which atoms. The shape of a molecule
More informationMO Calculation for a Diatomic Molecule. /4 0 ) i=1 j>i (1/r ij )
MO Calculation for a Diatomic Molecule Introduction The properties of any molecular system can in principle be found by looking at the solutions to the corresponding time independent Schrodinger equation
More informationExperiment 15: Atomic Orbitals, Bond Length, and Molecular Orbitals
Experiment 15: Atomic Orbitals, Bond Length, and Molecular Orbitals Introduction Molecular orbitals result from the mixing of atomic orbitals that overlap during the bonding process allowing the delocalization
More informationσ u * 1s g - gerade u - ungerade * - antibonding σ g 1s
One of these two states is a repulsive (dissociative) state. Other excited states can be constructed using linear combinations of other orbitals. Some will be binding and others will be repulsive. Thus
More informationLecture 9 Electronic Spectroscopy
Lecture 9 Electronic Spectroscopy Molecular Orbital Theory: A Review - LCAO approximaton & AO overlap - Variation Principle & Secular Determinant - Homonuclear Diatomic MOs - Energy Levels, Bond Order
More informationChemistry 483 Lecture Topics Fall 2009
Chemistry 483 Lecture Topics Fall 2009 Text PHYSICAL CHEMISTRY A Molecular Approach McQuarrie and Simon A. Background (M&S,Chapter 1) Blackbody Radiation Photoelectric effect DeBroglie Wavelength Atomic
More informationGeneral Physical Chemistry II
General Physical Chemistry II Lecture 10 Aleksey Kocherzhenko October 7, 2014" Last time " promotion" Promotion and hybridization" [He] 2s 2 2p x 1 2p y 1 2p z0 " 2 unpaired electrons" [He] 2s 1 2p x 1
More informationCHAPTER 13 Molecular Spectroscopy 2: Electronic Transitions
CHAPTER 13 Molecular Spectroscopy 2: Electronic Transitions I. General Features of Electronic spectroscopy. A. Visible and ultraviolet photons excite electronic state transitions. ε photon = 120 to 1200
More informationChemistry 881 Lecture Topics Fall 2001
Chemistry 881 Lecture Topics Fall 2001 Texts PHYSICAL CHEMISTRY A Molecular Approach McQuarrie and Simon MATHEMATICS for PHYSICAL CHEMISTRY, Mortimer i. Mathematics Review (M, Chapters 1,2,3 & 4; M&S,
More informationIntermission: Let s review the essentials of the Helium Atom
PHYS3022 Applied Quantum Mechanics Problem Set 4 Due Date: 6 March 2018 (Tuesday) T+2 = 8 March 2018 All problem sets should be handed in not later than 5pm on the due date. Drop your assignments in the
More informationCHEM3023: Spins, Atoms and Molecules
CHEM3023: Spins, Atoms and Molecules Lecture 4 Molecular orbitals C.-K. Skylaris Learning outcomes Be able to manipulate expressions involving spin orbitals and molecular orbitals Be able to write down
More informationChemistry 2. Lecture 1 Quantum Mechanics in Chemistry
Chemistry 2 Lecture 1 Quantum Mechanics in Chemistry Your lecturers 8am Assoc. Prof Timothy Schmidt Room 315 timothy.schmidt@sydney.edu.au 93512781 12pm Assoc. Prof. Adam J Bridgeman Room 222 adam.bridgeman@sydney.edu.au
More informationMolecular Physics. Attraction between the ions causes the chemical bond.
Molecular Physics A molecule is a stable configuration of electron(s) and more than one nucleus. Two types of bonds: covalent and ionic (two extremes of same process) Covalent Bond Electron is in a molecular
More informationConical Intersections. Spiridoula Matsika
Conical Intersections Spiridoula Matsika The Born-Oppenheimer approximation Energy TS Nuclear coordinate R ν The study of chemical systems is based on the separation of nuclear and electronic motion The
More informationQuantum mechanics can be used to calculate any property of a molecule. The energy E of a wavefunction Ψ evaluated for the Hamiltonian H is,
Chapter : Molecules Quantum mechanics can be used to calculate any property of a molecule The energy E of a wavefunction Ψ evaluated for the Hamiltonian H is, E = Ψ H Ψ Ψ Ψ 1) At first this seems like
More informationCHEMISTRY Topic #1: Bonding What Holds Atoms Together? Spring 2012 Dr. Susan Lait
CHEMISTRY 2000 Topic #1: Bonding What Holds Atoms Together? Spring 2012 Dr. Susan Lait Why Do Bonds Form? An energy diagram shows that a bond forms between two atoms if the overall energy of the system
More informationMolecular-Orbital Theory
Prof. Dr. I. Nasser atomic and molecular physics -551 (T-11) April 18, 01 Molecular-Orbital Theory You have to explain the following statements: 1- Helium is monatomic gas. - Oxygen molecule has a permanent
More informationIntroduction to Hartree-Fock Molecular Orbital Theory
Introduction to Hartree-Fock Molecular Orbital Theory C. David Sherrill School of Chemistry and Biochemistry Georgia Institute of Technology Origins of Mathematical Modeling in Chemistry Plato (ca. 428-347
More informationMolecular Orbitals. Based on Inorganic Chemistry, Miessler and Tarr, 4 th edition, 2011, Pearson Prentice Hall
Molecular Orbitals Based on Inorganic Chemistry, Miessler and Tarr, 4 th edition, 2011, Pearson Prentice Hall Images from Miessler and Tarr Inorganic Chemistry 2011 obtained from Pearson Education, Inc.
More information221B Lecture Notes Many-Body Problems II Molecular Physics
1 Molecules 221B Lecture Notes Many-Body Problems II Molecular Physics In this lecture note, we discuss molecules. I cannot go into much details given I myself am not familiar enough with chemistry. But
More informationChapter IV: Electronic Spectroscopy of diatomic molecules
Chapter IV: Electronic Spectroscopy of diatomic molecules IV.2.1 Molecular orbitals IV.2.1.1. Homonuclear diatomic molecules The molecular orbital (MO) approach to the electronic structure of diatomic
More informationCHEM6085: Density Functional Theory Lecture 10
CHEM6085: Density Functional Theory Lecture 10 1) Spin-polarised calculations 2) Geometry optimisation C.-K. Skylaris 1 Unpaired electrons So far we have developed Kohn-Sham DFT for the case of paired
More informationOrbital approximation
Orbital approximation Assign the electrons to an atomic orbital and a spin Construct an antisymmetrized wave function using a Slater determinant evaluate the energy with the Hamiltonian that includes the
More informationYingwei Wang Computational Quantum Chemistry 1 Hartree energy 2. 2 Many-body system 2. 3 Born-Oppenheimer approximation 2
Purdue University CHM 67300 Computational Quantum Chemistry REVIEW Yingwei Wang October 10, 2013 Review: Prof Slipchenko s class, Fall 2013 Contents 1 Hartree energy 2 2 Many-body system 2 3 Born-Oppenheimer
More informationOn the Uniqueness of Molecular Orbitals and limitations of the MO-model.
On the Uniqueness of Molecular Orbitals and limitations of the MO-model. The purpose of these notes is to make clear that molecular orbitals are a particular way to represent many-electron wave functions.
More informationMolecular Bonding. Molecular Schrödinger equation. r - nuclei s - electrons. M j = mass of j th nucleus m 0 = mass of electron
Molecular onding Molecular Schrödinger equation r - nuclei s - electrons 1 1 W V r s j i j1 M j m i1 M j = mass of j th nucleus m = mass of electron j i Laplace operator for nuclei Laplace operator for
More informationMolecular orbitals, potential energy surfaces and symmetry
Molecular orbitals, potential energy surfaces and symmetry mathematical presentation of molecular symmetry group theory spectroscopy valence theory molecular orbitals Wave functions Hamiltonian: electronic,
More informationThe Potential Energy Surface
The Potential Energy Surface In this section we will explore the information that can be obtained by solving the Schrödinger equation for a molecule, or series of molecules. Of course, the accuracy of
More informationChemistry, Physics and the Born- Oppenheimer Approximation
Chemistry, Physics and the Born- Oppenheimer Approximation Hendrik J. Monkhorst Quantum Theory Project University of Florida Gainesville, FL 32611-8435 Outline 1. Structure of Matter 2. Shell Models 3.
More informationPHYSICAL CHEMISTRY I. Chemical Bonds
PHYSICAL CHEMISTRY I Chemical Bonds Review The QM description of bonds is quite good Capable of correctly calculating bond energies and reaction enthalpies However it is quite complicated and sometime
More informationwe have to deal simultaneously with the motion of the two heavy particles, the nuclei
157 Lecture 6 We now turn to the structure of molecules. Our first cases will be the e- quantum mechanics of the two simplest molecules, the hydrogen molecular ion, H +, a r A r B one electron molecule,
More information26 Group Theory Basics
26 Group Theory Basics 1. Reference: Group Theory and Quantum Mechanics by Michael Tinkham. 2. We said earlier that we will go looking for the set of operators that commute with the molecular Hamiltonian.
More informationElectronic structure considerations for C 2 and O 2
1 Electronic structure considerations for and O Millard H. Alexander This version dated January 3, 017 ONTENTS I. Preface 1 II. Electronic Hamiltonian III. Molecular Orbitals: 4 IV. Electronic States:
More informationElectronic structure theory: Fundamentals to frontiers. 1. Hartree-Fock theory
Electronic structure theory: Fundamentals to frontiers. 1. Hartree-Fock theory MARTIN HEAD-GORDON, Department of Chemistry, University of California, and Chemical Sciences Division, Lawrence Berkeley National
More informationTheoretical Chemistry - Level II - Practical Class Molecular Orbitals in Diatomics
Theoretical Chemistry - Level II - Practical Class Molecular Orbitals in Diatomics Problem 1 Draw molecular orbital diagrams for O 2 and O 2 +. E / ev dioxygen molecule, O 2 dioxygenyl cation, O 2 + 25
More informationMolecular Structure & Spectroscopy Friday, February 4, 2010
Molecular Structure & Spectroscopy Friday, February 4, 2010 CONTENTS: 1. Introduction 2. Diatomic Molecules A. Electronic structure B. Rotation C. Vibration D. Nuclear spin 3. Radiation from Diatomic Molecules
More informationChapter 9: Multi- Electron Atoms Ground States and X- ray Excitation
Chapter 9: Multi- Electron Atoms Ground States and X- ray Excitation Up to now we have considered one-electron atoms. Almost all atoms are multiple-electron atoms and their description is more complicated
More information(a) What are the probabilities associated with finding the different allowed values of the z-component of the spin after time T?
1. Quantum Mechanics (Fall 2002) A Stern-Gerlach apparatus is adjusted so that the z-component of the spin of an electron (spin-1/2) transmitted through it is /2. A uniform magnetic field in the x-direction
More informationIntroduction to Computational Chemistry
Introduction to Computational Chemistry Vesa Hänninen Laboratory of Physical Chemistry room B430, Chemicum 4th floor vesa.hanninen@helsinki.fi September 3, 2013 Introduction and theoretical backround September
More informationThe general solution of Schrödinger equation in three dimensions (if V does not depend on time) are solutions of time-independent Schrödinger equation
Lecture 27st Page 1 Lecture 27 L27.P1 Review Schrödinger equation The general solution of Schrödinger equation in three dimensions (if V does not depend on time) is where functions are solutions of time-independent
More informationThe Hydrogen Molecule-Ion
Sign In Forgot Password Register ashwenchan username password Sign In If you like us, please share us on social media. The latest UCD Hyperlibrary newsletter is now complete, check it out. ChemWiki BioWiki
More informationLecture 19: Building Atoms and Molecules
Lecture 19: Building Atoms and Molecules +e r n = 3 n = 2 n = 1 +e +e r y even Lecture 19, p 1 Today Nuclear Magnetic Resonance Using RF photons to drive transitions between nuclear spin orientations in
More information2 Electronic structure theory
Electronic structure theory. Generalities.. Born-Oppenheimer approximation revisited In Sec..3 (lecture 3) the Born-Oppenheimer approximation was introduced (see also, for instance, [Tannor.]). We are
More informationVibrations and Rotations of Diatomic Molecules
Chapter 6 Vibrations and Rotations of Diatomic Molecules With the electronic part of the problem treated in the previous chapter, the nuclear motion shall occupy our attention in this one. In many ways
More informationChem 467 Supplement to Lecture 19 Hydrogen Atom, Atomic Orbitals
Chem 467 Supplement to Lecture 19 Hydrogen Atom, Atomic Orbitals Pre-Quantum Atomic Structure The existence of atoms and molecules had long been theorized, but never rigorously proven until the late 19
More informationLecture 08 Born Oppenheimer Approximation
Chemistry II: Introduction to Molecular Spectroscopy Prof. Mangala Sunder Department of Chemistry and Biochemistry Indian Institute of Technology, Madras Lecture 08 Born Oppenheimer Approximation Welcome
More informationLecture 5: Harmonic oscillator, Morse Oscillator, 1D Rigid Rotor
Lecture 5: Harmonic oscillator, Morse Oscillator, 1D Rigid Rotor It turns out that the boundary condition of the wavefunction going to zero at infinity is sufficient to quantize the value of energy that
More informationQUANTUM MECHANICS AND ATOMIC STRUCTURE
5 CHAPTER QUANTUM MECHANICS AND ATOMIC STRUCTURE 5.1 The Hydrogen Atom 5.2 Shell Model for Many-Electron Atoms 5.3 Aufbau Principle and Electron Configurations 5.4 Shells and the Periodic Table: Photoelectron
More informationIntroduction to Electronic Structure Theory
Introduction to Electronic Structure Theory C. David Sherrill School of Chemistry and Biochemistry Georgia Institute of Technology June 2002 Last Revised: June 2003 1 Introduction The purpose of these
More informationRethinking Hybridization
Rethinking Hybridization For more than 60 years, one of the most used concepts to come out of the valence bond model developed by Pauling was that of hybrid orbitals. The ideas of hybridization seemed
More information2m 2 Ze2. , where δ. ) 2 l,n is the quantum defect (of order one but larger
PHYS 402, Atomic and Molecular Physics Spring 2017, final exam, solutions 1. Hydrogenic atom energies: Consider a hydrogenic atom or ion with nuclear charge Z and the usual quantum states φ nlm. (a) (2
More informationPRACTICE PROBLEMS Give the electronic configurations and term symbols of the first excited electronic states of the atoms up to Z = 10.
PRACTICE PROBLEMS 2 1. Based on your knowledge of the first few hydrogenic eigenfunctions, deduce general formulas, in terms of n and l, for (i) the number of radial nodes in an atomic orbital (ii) the
More informationA few principles of classical and quantum mechanics
A few principles of classical and quantum mechanics The classical approach: In classical mechanics, we usually (but not exclusively) solve Newton s nd law of motion relating the acceleration a of the system
More informationMolecular Structure Both atoms and molecules are quantum systems
Molecular Structure Both atoms and molecules are quantum systems We need a method of describing molecules in a quantum mechanical way so that we can predict structure and properties The method we use is
More informationAN INTRODUCTION TO QUANTUM CHEMISTRY. Mark S. Gordon Iowa State University
AN INTRODUCTION TO QUANTUM CHEMISTRY Mark S. Gordon Iowa State University 1 OUTLINE Theoretical Background in Quantum Chemistry Overview of GAMESS Program Applications 2 QUANTUM CHEMISTRY In principle,
More informationAn Introduction to Quantum Chemistry and Potential Energy Surfaces. Benjamin G. Levine
An Introduction to Quantum Chemistry and Potential Energy Surfaces Benjamin G. Levine This Week s Lecture Potential energy surfaces What are they? What are they good for? How do we use them to solve chemical
More information4πε. me 1,2,3,... 1 n. H atom 4. in a.u. atomic units. energy: 1 a.u. = ev distance 1 a.u. = Å
H atom 4 E a me =, n=,,3,... 8ε 0 0 π me e e 0 hn ε h = = 0.59Å E = me (4 πε ) 4 e 0 n n in a.u. atomic units E = r = Z n nao Z = e = me = 4πε = 0 energy: a.u. = 7. ev distance a.u. = 0.59 Å General results
More informationLecture 19: Building Atoms and Molecules
Lecture 19: Building Atoms and Molecules +e r n = 3 n = 2 n = 1 +e +e r ψ even Lecture 19, p 1 Today Nuclear Magnetic Resonance Using RF photons to drive transitions between nuclear spin orientations in
More informationCHEM3023: Spins, Atoms and Molecules
CHEM3023: Spins, Atoms and Molecules Lecture 5 The Hartree-Fock method C.-K. Skylaris Learning outcomes Be able to use the variational principle in quantum calculations Be able to construct Fock operators
More informationLUMO + 1 LUMO. Tómas Arnar Guðmundsson Report 2 Reikniefnafræði G
Q1: Display all the MOs for N2 in your report and classify each one of them as bonding, antibonding or non-bonding, and say whether the symmetry of the orbital is σ or π. Sketch a molecular orbital diagram
More informationAtomic Structure and Atomic Spectra
Atomic Structure and Atomic Spectra Atomic Structure: Hydrogenic Atom Reading: Atkins, Ch. 10 (7 판 Ch. 13) The principles of quantum mechanics internal structure of atoms 1. Hydrogenic atom: one electron
More informationonly two orbitals, and therefore only two combinations to worry about, but things get
131 Lecture 1 It is fairly easy to write down an antisymmetric wavefunction for helium since there are only two orbitals, and therefore only two combinations to worry about, but things get complicated
More informationChemistry 3502/4502. Final Exam Part I. May 14, 2005
Chemistry 3502/4502 Final Exam Part I May 14, 2005 1. For which of the below systems is = where H is the Hamiltonian operator and T is the kinetic-energy operator? (a) The free particle (e) The
More informationBe H. Delocalized Bonding. Localized Bonding. σ 2. σ 1. Two (sp-1s) Be-H σ bonds. The two σ bonding MO s in BeH 2. MO diagram for BeH 2
The Delocalized Approach to Bonding: The localized models for bonding we have examined (Lewis and VBT) assume that all electrons are restricted to specific bonds between atoms or in lone pairs. In contrast,
More informationChemistry 3502/4502. Final Exam Part I. May 14, 2005
Advocacy chit Chemistry 350/450 Final Exam Part I May 4, 005. For which of the below systems is = where H is the Hamiltonian operator and T is the kinetic-energy operator? (a) The free particle
More informationeigenvalues eigenfunctions
Born-Oppenheimer Approximation Atoms and molecules consist of heavy nuclei and light electrons. Consider (for simplicity) a diatomic molecule (e.g. HCl). Clamp/freeze the nuclei in space, a distance r
More informationPrinciples of Molecular Spectroscopy
Principles of Molecular Spectroscopy What variables do we need to characterize a molecule? Nuclear and electronic configurations: What is the structure of the molecule? What are the bond lengths? How strong
More information( ( ; R H = 109,677 cm -1
CHAPTER 9 Atomic Structure and Spectra I. The Hydrogenic Atoms (one electron species). H, He +1, Li 2+, A. Clues from Line Spectra. Reminder: fundamental equations of spectroscopy: ε Photon = hν relation
More informationExam 4 Review. Exam Review: A exam review sheet for exam 4 will be posted on the course webpage. Additionally, a practice exam will also be posted.
Chem 4502 Quantum Mechanics & Spectroscopy (Jason Goodpaster) Exam 4 Review Exam Review: A exam review sheet for exam 4 will be posted on the course webpage. Additionally, a practice exam will also be
More informationPAPER :8, PHYSICAL SPECTROSCOPY MODULE: 29, MOLECULAR TERM SYMBOLS AND SELECTION RULES FOR DIATOMIC MOLECULES
Subject Chemistry Paper No and Title Module No and Title Module Tag 8: Physical Spectroscopy 29: Molecular Term Symbols and Selection Rules for Diatomic Molecules. CHE_P8_M29 TLE OF CONTENTS 1. Learning
More informationECE440 Nanoelectronics. Lecture 07 Atomic Orbitals
ECE44 Nanoelectronics Lecture 7 Atomic Orbitals Atoms and atomic orbitals It is instructive to compare the simple model of a spherically symmetrical potential for r R V ( r) for r R and the simplest hydrogen
More informationThe Simple Harmonic Oscillator
The Simple Harmonic Oscillator Michael Fowler, University of Virginia Einstein s Solution of the Specific Heat Puzzle The simple harmonic oscillator, a nonrelativistic particle in a potential ½C, is a
More informationChemistry 3502/4502. Exam III. All Hallows Eve/Samhain, ) This is a multiple choice exam. Circle the correct answer.
B Chemistry 3502/4502 Exam III All Hallows Eve/Samhain, 2003 1) This is a multiple choice exam. Circle the correct answer. 2) There is one correct answer to every problem. There is no partial credit. 3)
More informationCHEM-UA 127: Advanced General Chemistry I
CHEM-UA 7: Advanced General Chemistry I I. LINEAR COMBINATION OF ATOMIC ORBITALS Linear combination of atomic orbitals (LCAO) is a simple method of quantum chemistry that yields a qualitative picture of
More informationMagentic Energy Diagram for A Single Electron Spin and Two Coupled Electron Spins. Zero Field.
7. Examples of Magnetic Energy Diagrams. There are several very important cases of electron spin magnetic energy diagrams to examine in detail, because they appear repeatedly in many photochemical systems.
More informationMO theory is better for spectroscopy (Exited State Properties; Ionization)
CHEM 2060 Lecture 25: MO Theory L25-1 Molecular Orbital Theory (MO theory) VB theory treats bonds as electron pairs. o There is a real emphasis on this point (over-emphasis actually). VB theory is very
More informationLecture 8: Introduction to Density Functional Theory
Lecture 8: Introduction to Density Functional Theory Marie Curie Tutorial Series: Modeling Biomolecules December 6-11, 2004 Mark Tuckerman Dept. of Chemistry and Courant Institute of Mathematical Science
More information