To calculate the energy of a single electron atom with quantum numbers L, S, and J: E L,S,J = ½ hc [J(J+1) - L(L+1) – S(S+1)] where  is the spin-orbit.

Slides:

Advertisements

Similar presentations

Emission of Light from Gases

Advertisements

Lecture 6 ATOMIC SPECTROSCOPY

Atomic Spectroscopy: Atomic Emission Spectroscopy

Atomic Emission Spectra. The Electromagnetic Spectrum High frequency Short wavelength High energy lower frequency longer wavelength lower energy.

Physics and the Quantum Mechanical Model

Pisgah High School Chemistry Mike Jones The Hydrogen Spectrum Rev Canton, NC.

Chapter 30 Light Emission

Energy and Electrons. Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the.

AAS and FES (Ch 10, 7th e, WMDS)

Atomic Emission Spectroscopy. Chem Introduction Atomic absorption is the absorption of light by free atoms. An atomic absorption spectrophotometer.

Atomic Emission Spectroscopy

Atomic Spectroscopy: Atomic Emission Spectroscopy

Atomic Emission - AES M* → M + hn Thermal excitation M → M*

Atomic spectra are a result of energy level diagrams - quantum theory.

Infrared Spectroscopy Near Infrared: 770 to 2500 nm Near Infrared: 770 to 2500 nm 12,900 to 4000 cm -1 Mid Infrared: 2500 to 50,000 nm (2.5 to 50  m)

Rotational Spectra Simplest Case: Diatomic or Linear Polyatomic molecule Rigid Rotor Model: Two nuclei joined by a weightless rod J = Rotational quantum.

Lecture 2110/24/05. Light Emission vs. Absorption Black body.

Solid State Chemistry Chapter 3 Atomic Structure and Spectra.

Vibrational Transitions

Allowed and Forbidden Transitions Only a fraction of all possible transitions are observed. Allowed transitions -high probability, high intensity, electric.

Electromagnetic Spectrum The energy of the photon determines the type of transition or interaction that occurs. Table 1-1 – Ingle and Crouch, Spectrochemical.

Atomic Spectroscopy: Atomic Emission Spectroscopy Atomic Absorption Spectroscopy Atomic Fluorescence Spectroscopy * Elemental Analysis * Sample is atomized.

Allowed and Forbidden Transitions Only a fraction of all possible transitions are observed. Allowed transitions -high probability, high intensity, electric.

Lecture 22 Spin-orbit coupling

Particle Properties of Light. Objectives To discuss the particle nature of light.

Hans Zinnecker Deutsches SOFIA Institut NASA-Ames and Univ. Stuttgart

Auger Electron Spectroscopy (AES) 1. Brief History Auger Effect discovered in 1920’s Meitner published first journal Auger transitions considered noise.

Atomic Spectra. Much of what we know about atomic structure comes from analysis of light either being emitted or absorbed by substances. Elements can.

Figure 6-4. Figure 6-8 Figure 6-11 W lamp W filament vacuum valence electrons in solid are excited by heat, relax to GS, and give off light.

Chapter 10 Atomic Structure and Atomic Spectra. Spectra of complex atoms Energy levels not solely given by energies of orbitals Electrons interact and.

ELECTROMAGNETIC SPECTRUM. OUTER (VALENCE) ELECTRONS AND ATOMIC STRUCTURE U.V. and VISIBLEOuter Valence Electrons in Atoms & Molecules Give Rise to Atomic.

Chapter 8 An Introduction to Optical Atomic Spectrometry 1

ARRANGEMENT of ELECTRONS in ATOMS CHAPTER 4. DESCRIBING THE ELECTRON Questions to be answered: How does it move? How much energy does it have? Where could.

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

Electromagnetic radiation – transmission of energy through space in the form of oscillating waves wavelength, – distance between identical points on successive.

Chapter 7: Quantum theory of the atom Chemistry 1061: Principles of Chemistry I Andy Aspaas, Instructor.

1 Atomic Emission Spectroscopy Molecular Absorption Spectroscopy Lecture 21.

Elemental Analysis using Atomic Absorption and Emission Spectroscopy Bodhisatwa Das.

Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.

Lecture 22 Spin-orbit coupling. Spin-orbit coupling Spin makes an electron act like a small magnet. An electron orbiting around the nucleus also makes.

H spectra 656 nm 486 nm 434 nm 410 nm. Ne spectra 540.1green 585.2yellow 588.2yellow 603.0orange 607.4orange 616.4orange 621.7red-orange 626.6red-orange.

 Waves & Energy H Ch 5&6. Waves  Vibrating disturbance by which energy is transmitted Amplitude (Wavelength) u = λν.

Introduction to Optical Atomic spectrometry

Atomic Structure and Atomic Spectra

Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing.

CHAPTER 2 ATOMIC STRUCTURE 2.1 Bohr's atomic model 2.2 Electronic configuration.

Schrödinger Equation – Model Systems: We have carefully considered the development of the Schrödinger equation for important model systems – the one, two.

Electrons and the Electromagnetic Spectrum. Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties.

5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.

Electrons in Atoms Chapter 4.

Bohr’s Model of the Atom

,..,_ -, =.. t :: ;... t---aM 0 d -...c " ss ''- !j!j ! )

Atomic emissions and absorption

Why Light, why now?.

Physics and the Quantum Mechanical Model

Effective Nuclear Charge

Wave-Particle Duality

Atomic Absorption Process

Energy and Electrons energy

- I, n i i. JJ- l__!l__!

Bound Systems and Spectra

The ELECTRON: Wave – Particle Duality

Light and Quantized Energy

Atomic emission spectrum

Bohr, Emissions, and Spectra

Unit 3: Light and Electrons

Quantum Numbers.

Electrons and Light!.

Unit 3: Light and Electrons

Presentation transcript:

To calculate the energy of a single electron atom with quantum numbers L, S, and J: E L,S,J = ½ hc [J(J+1) - L(L+1) – S(S+1)] where  is the spin-orbit coupling constant Calculating Energies for Transitions

Atomic emission spectra show a doublet in the Na spectrum due to spin-orbit coupling of the 2 P state. Given that = 11.4 cm -1, find the energy spacing (in cm -1 ) between the atomic emission lines from 2 P 3/2 and 2 P 1/2 to 2 S 1/2. Are you getting the concept?

Example AE Spectra H2H2H2H2 Hg He

Arcs and Sparks Arc = An electrical discharge between two or more conducting electrodes (1-30 A)Arc = An electrical discharge between two or more conducting electrodes (1-30 A) Spark = An intermittent high-voltage discharge (few  sec)Spark = An intermittent high-voltage discharge (few  sec) Limited to qualitative and semi-quantitative use (arc flicker)Limited to qualitative and semi-quantitative use (arc flicker) Particularly useful for solid samples (pressed into electrode)Particularly useful for solid samples (pressed into electrode) The burn takes > 20 sec (need multichannel detector)The burn takes > 20 sec (need multichannel detector) Ingle and Crouch