PARTICLE NATURE OF LIGHT. A Black Object Appears black because it absorbs all frequencies of light A black block of iron does this.

Slides:

Advertisements

Similar presentations

Physics and the Quantum Mechanical Model Section 13.3

Advertisements

Niels Bohr in 1913 proposed a quantum model for the hydrogen atom which correctly predicted the frequencies of the lines (colors) in hydrogen’s atomic.

The Photoelectric Effect Waves as particles? What, are you crazy??

Waves. Characteristics of Waves Frequency Amplitude.

Bellwork: Friday October 12th Envision the way the water molecules on a lake’s surface behave as a water wave travels across the lake. What does it look.

The Rutherford model of the atom was an improvement over previous models, but it was incomplete. J. J. Thomson’s “plum pudding” model, in which electrons.

Creating a foldable for the electrons in atoms notes

Electromagnetic Radiation. Definitions Electromagnetic Radiation is energy with wavelike characteristics Moves at a speed of 3.0 x 10 8 m/s.

Chapter 5 Electrons In Atoms.

Rutherford’s model -Shows where protons & neutrons are -Not good at showing the location of electrons.

Entry Task: October 12 th Friday Question: What makes up the colors in a rainbow? What other types of waves exist? You have 5 minutes!

The dual nature of light l wave theory of light explains most phenomena involving light: propagation in straight line reflection refraction superposition,

November 22, Name of the Game: ENERGY And also: NOBEL PRIZES FOR PHYSICS.

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.

Chapter 7. Light as a wave  carries energy but doesn’t actually move  Think of a cork on water and surfer. The above diagram is a typical way to visualize.

Index Unit 03 Electron Configuration Module 02: Light as a Particle Based on the PowerPoints By Mr. Kevin Boudreaux, Angelo State Univerisity U03Mod01.

Particle Nature of Light page 49 of Notebook VISIBLE LIGHT ELECTRONS.

Light and Electrons October 27, 2014.

Ch. 6 Electronic Structure and the Periodic Table Part 1: Light, Photon Energies, and Emission Spectra.

Particle Nature of Light

Many scientists found Rutherford’s Model to be incomplete  He did not explain how the electrons are arranged  He did not explain how the electrons were.

I II III  Suggested Reading Pages  Section 4-1 Radiant Energy.

Light and the Electromagnetic Spectrum. Light Phenomenon Isaac Newton ( ) believed light consisted of particles. By 1900, most scientists believed.

Energy. Radiant Energy Radiant: think light…. How does light carry energy through space???

Electromagnetic Spectrum

Arrangement of Electrons in Atoms The Development of a New Atomic Model.

Electrons in Atoms Chapter 5.

Thompson’s experiment (discovery of electron) + - V + - Physics at the end of XIX Century and Major Discoveries of XX Century.

I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms yC. JOHANNESSON.

Light and the Atom. Light Much of what we know about the atom has been learned through experiments with light; thus, you need to know some fundamental.

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.

Chapter 5: Electrons in Atoms

Bellwork Envision the way the water molecules on a lake’s surface behave as a water wave travels across the lake. What does it look like? What happens.

Modern Chemistry Chapter 4 Arrangement of Electrons in Atoms Sections 1-3 The Development of a New Atomic Model The Quantum Model of the Atom Electron.

Electrons and Light. Light’s relationship to matter Atoms can absorb energy, but they must eventually release it When atoms emit energy, it is released.

Development of a New Atomic Model Properties of Light.

Electron As a Particle and Wave Electrons get excited when energy is absorbed by using heat or electrical energy Electrons get excited when energy is absorbed.

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

THE PHOTOELECTRIC EFFECT. When red light is incident on a clean metal surface: no electrons are released, however long light is shone onto it, however.

LIGHT and QUANTIZED ENERGY. Much of our understanding of the electronic structure of atoms has come from studying how substances absorb or emit light.

Vocabulary Review New radiation electromagnetic radiation wavelength

Light: Wave or Particle Chapter 4, Section 1 notes.

1 Part 02 Quantum Theory. 2 Beginning of 20 th century - wave model of light universally accepted - questions still existed that could not be answered.

Electrons in Atoms. Wave Behavior of Light Day 1.

1. Page 124: 5, Q + 5 A from today’s class.

C. Johannesson I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms.

Section 2.2 and Chapter 7 Electron Configurations and Waves.

4-2 Quantum Theory. Planck’s Theory Max Planck predicted accurately how the spectrum of radiation emitted by an object changes with temperature.

Wave-Particle Nature of Light

Atomic Structure.

Quantized Energy and Photons

Electrons in Atoms Chapter 4.

Quantum Energy and Photoelectric Effect

Chapter 5 Electrons in Atoms

Chemistry 1 Chapter 5 Part I Light and Quantized Energy

I. Light and Quantized Energy (Cont.)

Atomic Emission Spectrum

Chemistry 1 Notes # 8 Light and Quantized Energy

THE PHOTOELECTRIC EFFECT

Physics and the Quantum Mechanical Model

Section 5.1 Light and Quantized Energy

I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )

UNIT 3 ELECTRON CONFIGURATION AND MODERN ATOMIC THEORY

Waves and particles Ch. 4.

Light and Quantized Energy

Chemistry 1 Chapter 5 Part I Light and Quantized Energy

Light and Energy Electromagnetic Radiation is a form of energy that is created through the interaction of electrical and magnetic fields. It displays wave-like.

5.1 – ELECTRONS IN ATOMS.

Ch. 5 - Electrons in Atoms Waves & Particles.

Quantized Energy and Photons

Presentation transcript:

PARTICLE NATURE OF LIGHT

A Black Object Appears black because it absorbs all frequencies of light A black block of iron does this

WHEN IRON IS HEATED Might expect the energy it has absorbed would radiate back out, exhibiting all the frequencies it had absorbed THIS IS NOT WHAT HAPPENS! Specific colors come out depending on the temperature of the metal Red Yellow White Blue-White HOTTER

Max Planck – Germany, 1900 “Matter can only gain or lose energy in small, specific amounts called QUANTA E quantum = h h = Planck’s Constant = x J.s

EXAMPLE PROBLEMS 1. A metal is heated until it is red hot with a shade of red corresponding to a frequency of 4.42 x Hz. What is the wavelength of this radiation? What is its energy in Joules?

EXAMPLE PROBLEMS 2. Tiny water drops in the air disperse the white light of the sun into a rainbow. What is the energy of the violet light that has a frequency of 7.23 x Hz?

The Photoelectric Effect When light of a particular frequency shines on the surface of a particular metal, electrons are emitted. “photoelectrons”

The Photoelectric Effect Light of lower frequency produces no photoelectrons regardless of intensity or brightness. However, dim light of sufficient frequency produces“photoelectrons” Wave Theory fails to explain this!

Albert Einstein 1905 Expanded on Planck’s theory that EMR has a Dual Nature – Wave and Particle E photon = h  PHOTON – light particle or energy particle 

Planck & Einstein’s results reveal an important PARTICLE MODEL FOR LIGHT Example: It is found that light with a wavelength of 486 nm is necessary to produce photoelectrons from a photoelectric cell. What is the energy of this photon?

Planck & Einstein’s results reveal an important PARTICLE MODEL FOR LIGHT Example: It is found that light with a wavelength of 486 nm is necessary to produce photoelectrons from a photoelectric cell. What is the energy of this photon? ans 4.10 x J