Simultaneous measurement of p,x impossible

Slides:

Advertisements

Similar presentations

Electrons as Waves Sarah Allison Claire.

Advertisements

How many wavelengths are represented in each figure below?

Wave Particle Duality – Light and Subatomic Particles

Wave Particle Duality & the Heisenberg Uncertainty Principle By: Nick Day, Edward Moore, Sarah Russell.

Electron Configuration Mapping the electrons. Electron Configuration The way electrons are arranged around the nucleus.

CHAPTER 2 Introduction to Quantum Mechanics

1 Recap Heisenberg uncertainty relations  The product of the uncertainty in momentum (energy) and in position (time) is at least as large as Planck’s.

P2-13: ELECTRON DIFFRACTION P3-51: BALMER SERIES P2-15: WAVE PACKETS – OSCILLATORS P2-12: X-RAY DIFFRACTION MODEL P2-11: INTERFERENCE OF PHOTONS Lecture.

Lecture 2210/26/05. Moving between energy levels.

Heisenburg’s Uncertainty Principle Electrons have wave-particle duality, but it is impossible to show an electron behaving as a wave and a particle at.

Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave.

Electrons in Atoms The Quantum Model of the Atom.

Physical Chemistry 2nd Edition

Periodicity and Atomic Structure

Particles (matter) behave as waves and the Schrödinger Equation 1. Comments on quiz 9.11 and Topics in particles behave as waves:  The (most.

Wave Mechanics and Orbitals. The quantum theory provided many improvements in the understanding of different electron energy states within an atom. HOWEVER,

Chapter 5 Section 5.3 & 5.4 The Quantum Model. Problems with the Bohr Model 1. Worked well for predicting hydrogen spectrum, but not for elements with.

1 Introduction to quantum mechanics (Chap.2) Quantum theory for semiconductors (Chap. 3) Allowed and forbidden energy bands (Chap. 3.1) What Is An Energy.

The Quantum Model of the Atom. Proposed that the photoelectric effect could be explained by the concept of quanta, or packets of energy that only occur.

Arrangement of Electrons In Atoms

CHEMISTRY T HIRD E DITION Gilbert | Kirss | Foster | Davies © 2012 by W. W. Norton & Company CHAPTER 7-B Quantum Numbers.

Section 2 The Quantum Model of the Atom Lesson Starter Write down your address using the format of street name, house/apartment number, and ZIP Code. These.

Quantum Atom. Louis deBroglie Suggested if energy has particle nature then particles should have a wave nature Particle wavelength given by λ = h/ mv.

Electromagnetic Spectrum Light as a Wave - Recap Light exhibits several wavelike properties including Refraction Refraction: Light bends upon passing.

CHEMISTRY 161 Chapter 7 Quantum Theory and Electronic Structure of the Atom

Modern Chemistry Chapter 4 Arrangement of Electrons in Atoms

Chapter 6 Electronic Structure of Atoms. The Wave Nature of Light The light that we can see with our eyes, visible light, is an example of electromagnetic.

Aufbau Principle An electron occupies the lowest energy orbital that can receive it.

Classical mechanics: how energy and forces affect the motion of macroscopic objects Ex: As the driver inputs more energy into the car, the kinetic energy.

Electrons as waves Scientists accepted the fact that light has a dual wave- particle nature. De Broglie pointed out that in many ways the behavior of the.

Electrons in the Atom. Heisenberg Uncertainty Principle This is the theory that states that it is impossible to determine simultaneously both the position.

Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave. 

Chapter 7: Quantum Mechanical Model of Atom CHE 123: General Chemistry I Dr. Jerome Williams, Ph.D. Saint Leo University.

Electrons in Atoms Chapter 5. Chapter 5: Electrons in Atoms 5.1 Light and Quantized Energy Wave nature of light.

Electromagnetic Spectrum Section 1 The Development of a New Atomic Model Chapter 4.

Last hour: The PIB Hamiltonian: Eigenfunctions of the PIB Energy eigenvalues of the PIB E scales with n 2, 1/m, 1/a 2 Eigenfunctions are alternating between.

The Quantum Mechanical Model of the Atom = model in which e- are treated as having wave characteristics.

Quantum Mechanical Model of Atom. Name This Element.

The Quantum Mechanical Model Chemistry Honors. The Bohr model was inadequate.

Electron Configuration

Last hour: Generalized angular momentum EV’s: j·(j+1)·ħ2 for ; m·ħ for ; -j ≤ m ≤ j in steps of 1 The quantum numbers j can be.

Wave packet: Superposition principle

Uncertainty Principle

The Bohr Model, Wave Model, and Quantum Model

Quiz_14 Previous material – Compton scattering, pair production New material – Wave-Particle duality, probability, Uncertainty Principle Physics 274 9/30/2016.

the quantum model of the atom

PHYS274 Atomic Structure I

Quantum Model of the Atom

WHAT THE HECK DO I NEED TO BE ABLE TO DO?

Quantum Theory Light Theory Part 4.

The Heisenberg Uncertainty Principle states that it is impossible to know with high levels of certainty both the location and the velocity of an electron.

Quantum Theory and Electronic Structure of the Atom

Chapter 7: Atomic Structure

Atomic Models Main Concept:

Arrangement of electrons

Electron Orbitals Heisenberg 1. The ____________ ______________ principle states that it is impossible to determine simultaneously both the position and.

Wave packets: The solution to the particle-wave dilemma

Do all the reading assignments.

Chapter 4 Electrons as Waves

Lesson 12: Bohr to Heisenberg

Electron Configuration

Last hour: Orbit magnetism

III. Quantum Model of the Atom (p )

Last hour: Raising & Lowering Operators

Chapter 4:Arrangement of Electrons in atoms

Quantum Mechanics College Chemistry.

Do Now (3B/4B) Take-out: Be ready to review p. 12 at the bell! Paper

Last hour: Variation Theorem in QM: If a system has the ground state energy E0 and the Hamiltonian ,then for any normalizeable WF  we have We can.

Last hour: Particles at step functions

Presentation transcript:

Simultaneous measurement of p,x impossible d < picture from Ira Levine “Quantum Chemistry” 5th ed. >

Learning Goals for Chapter 2 – Heisenberg’s Uncertainty Principle After this chapter, the related homework problems, and reading the relevant parts of the textbook, you should be able to: construct a simple wave packet from plane waves and explain the result verbally and graphically formulate HUP mathematically for several pairs of variables explain the consequences of HUP using examples use HUP to estimate orders of magnitude of uncertainties of position, momentum, energy, etc.