Quantum Mechanics Theory

Slides:



Advertisements
Similar presentations
…the study of how light and matter interact
Advertisements

Chemistry Daily 10’s Week 5.
Waves. Characteristics of Waves Frequency Amplitude.
Honors Chemistry Section 4.1
What do you see? Old woman? Or young girl?  Is turning a light on and off a chemical or physical change? ◦ Physical change  What creates light?
ENERGY & LIGHT THE QUANTUM MECHANICAL MODEL. Atomic Models What was Rutherford’s model of the atom like? What is the significance of the proton? What.
Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.
Electrons and Light How does the arrangement of electrons in the atom determine the color of light that it emits?
Classical vs Quantum Mechanics Rutherford’s model of the atom: electrons orbiting around a dense, massive positive nucleus Expected to be able to use classical.
The Bohr Model: Orbits and Line Spectra. Understand the historical development of the Quantum Mechanical Model of the atom. Describe how a produced line.
Quantum Mechanics.  Write what’s in white on the back of the Week 10 Concept Review  Then, answer the questions on the front Your Job.
Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.
Electromagnetic Spectra Review Game. When do electrons emit light? Moving from higher to lower energy levels.
Electromagnetic Radiation and Light
Introduction to Excited Elements Lab
Aim: How are an atom’s electrons configured? Electromagnetic SpectrumElectromagnetic Spectrum -the total range of light including gamma rays, x-rays, ultraviolet,
Electron Behavior Electron absorb energy and jump to higher energy level (Excited State). Immediately fall back to original level (Ground State) emitting.
Electronic Structure. Bohr Bohr proposed that the __________ atom has only certain allowable energy states.
Electromagnetic Spectrum
Wave-Particle Duality: The Beginnings of Quantum Mechanics.
Electrons in Atoms Chapter 5. Duality of Light Einstein proved that matter and energy are related E = mc 2 Einstein proved that matter and energy are.
December 1 The wave-mechanical model of the atom Homework Finish worksheet.
Atomic spectra 10/2/14. The Dual Nature of Light: The Particle and The Wave Ancient Greeks people thought of light as a stream of tiny particles -like.
Slide 1 of 38 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 38 Physics and the Quantum Mechanical Model Neon advertising signs are formed from.
Evidence of Energy Levels. e-e- e-e- Ground state Excited state Electrons can only be at specific energy levels, NOT between levels.
Development of a New Atomic Model Properties of Light.
Emission Spectra and Bohr-Rydberg
Quantum Theory and the Atom In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame. Analysis of the emitted.
Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.
Chemistry – Chapter 4. Rutherford’s Atomic Model.
Lesson 3 : The Bohr Model. Bohr Model of an Atom  Electrons orbit the nucleus in fixed energy ranges called orbits (energy levels)  An electron can.
CHAPTER 2 ATOMIC STRUCTURE 2.1 Bohr's atomic model 2.2 Electronic configuration.
Chemistry Physics and the Quantum Mechanical Model.
Chapter 11 Modern Atomic Theory. Rutherford’s Atom What are the electrons doing? How are the electrons arranged How do they move?
The Bohr Model of the Atom
Atomic Emission Spectra and Quantum mechanical Model
Chapter 6 Electronic Structure of Atoms
Chapter 11. Modern Atomic Theory
The Bohr Model & Bright-Line Spectra
Radiant Energy Objectives:
Atomic Structure: The Quantum Mechanical Model
Physics and the Quantum Mechanical Model
Electromagnetic Radiation
Physics and the Quantum Mechanical Model
Quantum Theory.
The Atom Lesson 3 : The Bohr Model.
Electrons and Light Chapter 13.3.
Aim: What happens when electrons get excited?
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
Please write an electron configuration for Br-
The end of classical physics: photons, electrons, atoms
Matter is a Wave Does not apply to large objects
Energy and Electrons energy
Electromagnetic radiation
I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )
Orbits and Line Spectra
ATOMIC STRUCTURE.
Light and electrons.
The fingerprints of elements
Quantum Theory.
Electrons and Light!.
The Atom Lesson 3 : The Bohr Model.
Quantum Mechanics.
Electron Configurations
Development of Quantum Mechanics Bohr’s Contribution
4.6 NOTES Atomic Emission Spectra
Ch. 5 - Electrons in Atoms Waves & Particles.
Atomic Spectra As atoms gain energy their electrons can be excited and absorb energy in discrete amounts called quanta and produce absorption spectrums.
Excited State vs. Ground State
Light and EM Spectrum Light is all thanks to electrons…well… photons…but whatever. What do you REALLY know about light?
Presentation transcript:

Quantum Mechanics Theory Quantum means packet or bundle Quanta are discrete steps

Quantum replaces classical Classical (Newtonian) Mechanics is still valid at speeds, sizes and distances which you encounter on a daily basis. Miles 55 mph Loaf of bread On the atomic level, classical mechanics fails

Quanta and the Spectrum We use the visible light spectra from stars to determine all the information we have about them The vertical lines of light we see on an emission spectra are produced when an electron falls to a lower energy level and a photon is released.

Quanta and the Spectrum The electron goes to a higher energy shell (makes a quantum leap) when it is struck by a photon of just the right energy.