Physics 6C Heisenberg Uncertainty Principle Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.

Slides:



Advertisements
Similar presentations
Physics and the Quantum Mechanical Model Section 13.3
Advertisements

e-e- E n eV n = 1 ground state n = 3 0 n = ∞ n = n = 4 ionisation N.B. All energies are NEGATIVE. REASON: The maximum energy.
Electromagnetic Waves Physics 6C Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Physics 6C The Photoelectric Effect Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
The Modern Atomic Model After Thomson: Bohr, Placnk, Einstein, Heisenberg, and Schrödinger.
Physics 6C Photons Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Electrons. Wave model – scientist say that light travels in the form of a wave.
Physics 6C De Broglie Wavelength Uncertainty Principle Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Physics 6C De Broglie Wavelength Uncertainty Principle Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Announcements First project is due in two weeks. In addition to a short (~10 minute) presentation you must turn in a written report on your project Homework.
Electromagnetic Radiation
Physics 6C Energy Levels Bohr Model of the Atom Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Physics 6B Electric Potential and Electric Potential Energy Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic Radiation.
Differential Equations Verification Examples Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Niels Bohr’s Energy Levels
Physics and the Quantum Model
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.
Chapter 4 Arrangement of Electrons in Atoms
Chapter 4 Arrangement of Electrons in Atoms
Chemistry Chapter 4 Arrangement of Electrons in Atoms
Electronic Structure. Bohr Bohr proposed that the __________ atom has only certain allowable energy states.
Decibels and Doppler Effect
In an experiment to demonstrate the photoelectric effect, you shine a beam of monochromatic blue light on a metal plate. As a result, electrons are emitted.
Development of Modern Atomic theory. Modern Model of Atom When energy is added to an atom : Low NRG State (ground state)  High energy state (excited.
Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model
Electrons Negative charge e- Located in the electron cloud far from the nucleus Have mass, but it is negligible Also have wave-like properties.
The Development of a New Atomic Model  The Rutherford model of the atom was an improvement over previous models of the atom.  But, there was one major.
Explain why different colors of light result
Bohr Model and Quantum Theory
Section 4-1 Continued.  Ground State – the lowest energy state of an atom  Excited State – a state in which an atom has a higher energy than in its.
atomic excitation and ionisation
Electromagnetic Spectrum Section 1 The Development of a New Atomic Model Chapter 4.
Inner Product, Length and Orthogonality Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Physics 102: Lecture 24, Slide 1 Bohr vs. Correct Model of Atom Physics 102: Lecture 24 Today’s Lecture will cover Ch , 28.6.
Orthogonal Projections Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB.
Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s.
Each energy level is like a step on a stair. Electrons move up or down energy levels like going up or down stairs.
Chem-To-Go Lesson 7 Unit 2 ENERGY OF ELECTRONS. ENERGY BASICS All energy travels in the form of a wave. Scientists measure the wavelength of a wave to.
Models, Waves, and Light Models of the Atom Many different models: – Dalton-billiard ball model (1803) – Thompson – plum-pudding model (1897) – Rutherford.
CHAPTER 11 NOTES MODERN ATOMIC THEORY RUTHERFORD’S MODEL COULD NOT EXPLAIN THE CHEMICAL PROPERTIES OF ELEMENTS.
Wavelength, Frequency, and Planck’s Constant. Formulas 1)E = hf E = energy (Joules J) h = Planck’s constant = 6.63 x J x s f = frequency (Hz) 2)
Light Light is a kind of electromagnetic radiation, which is a from of energy that exhibits wavelike behavior as it travels through space. Other forms.
Electromagnetic Radiation. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance.
Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.
5.3 Physics and the Quantum Mechanical Model. Light By 1900 enough experimental evidence to convince scientists that light consists of waves.
Physics and the Quantum
7.4 The Wave Nature of Matter – 7.5 Quantum Mechanics and the Atom
Still have a few registered iclickers (3 or 4
The Bohr Model, Wave Model, and Quantum Model
Light and Quantized Energy
Aim: How Do We Describe an Atoms Energy Levels?
Chapter 6: Electromagnetic Radiation
Physics and the Quantum Mechanical Model
Electromagnetic Radiation
5.3 Physics and the Quantum Mechanical Model
4.8 – NOTES Intro to Electron Configurations
Please write an electron configuration for Br-
The Bohr Model (1913) revolve sun energy
Heisenberg Uncertainty Principle
Light and Quantized Energy
5.3 Physics and the Quantum Mechanical Model
Electromagnetic Radiation
Chemistry “Electrons in Atoms”
Chapter 4 Arrangement of Electrons in Atoms
Electron Configurations
Chapter 6: Electromagnetic Radiation
5.3 Physics and the Quantum Mechanical Model
Light and EM Spectrum Light is all thanks to electrons…well… photons…but whatever. What do you REALLY know about light?
Presentation transcript:

Physics 6C Heisenberg Uncertainty Principle Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Heisenberg Uncertainty Principle Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB Basic Idea – you can’t get exact measurements 2 Versions:

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Example: For the electrons in the previous example, their wavelength was 0.123nm. Take this to be the uncertainty in their position, and find the corresponding uncertainty in their speed. Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB Compare this to the velocity we found in the previous problem. That value was 5.9x10 6. So the uncertainty is almost as much as the actual velocity!

Example A certain atom has an energy level 3.50eV above the ground state. When excited to this state, it remains 4.0µs, on average, before emitting a photon and returning to the ground state. a) What is the energy of the photon? What is the wavelength of the photon? b) What is the smallest possible uncertainty in the energy of the photon? Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB

Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB The photon has energy 3.50 eV. Its wavelength is calculated in the usual way: Example A certain atom has an energy level 3.50eV above the ground state. When excited to this state, it remains 4.0µs, on average, before emitting a photon and returning to the ground state. a) What is the energy of the photon? What is the wavelength of the photon? b) What is the smallest possible uncertainty in the energy of the photon?

Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB The photon has energy 3.50 eV. Its wavelength is calculated in the usual way: Example A certain atom has an energy level 3.50eV above the ground state. When excited to this state, it remains 4.0µs, on average, before emitting a photon and returning to the ground state. a) What is the energy of the photon? What is the wavelength of the photon? b) What is the smallest possible uncertainty in the energy of the photon?

Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB The photon has energy 3.50 eV. Its wavelength is calculated in the usual way: Use Heisenberg’s formula to find the minimum uncertainty in the energy: Example A certain atom has an energy level 3.50eV above the ground state. When excited to this state, it remains 4.0µs, on average, before emitting a photon and returning to the ground state. a) What is the energy of the photon? What is the wavelength of the photon? b) What is the smallest possible uncertainty in the energy of the photon?

Prepared by Vince Zaccone For Campus Learning Assistance Services at UCSB The photon has energy 3.50 eV. Its wavelength is calculated in the usual way: Use Heisenberg’s formula to find the minimum uncertainty in the energy: Note that this is much smaller than the energy of the photon, so the uncertainty is negligible. Example A certain atom has an energy level 3.50eV above the ground state. When excited to this state, it remains 4.0µs, on average, before emitting a photon and returning to the ground state. a) What is the energy of the photon? What is the wavelength of the photon? b) What is the smallest possible uncertainty in the energy of the photon?