Section 4.6—Light. Light is Electromagnetic Radiation Electromagnetic energy is energy that has electric and magnetic fields There are many types of Electromagnetic.

Slides:



Advertisements
Similar presentations
Physics and the Quantum Mechanical Model
Advertisements

Physics and the Quantum Mechanical Model l OBJECTIVES: - Calculate the wavelength, frequency, or energy of light, given two of these values.
Light, Photon Energies, and Atomic Spectra
Chapter 4 The Electromagnetic Spectrum Part 1. Demonstration Gas spectral tubes: NeonArgon.
Creating a foldable for the electrons in atoms notes
Electromagnetic Spectrum
Electrons as Waves.
4-1 Radiant Energy. Waves  Light travels in Waves similar to ocean waves  Light waves are electromagnetic and consist of an electric and magnetic fields.
Radiant Energy  .
Properties of Light Is Light a Wave or a Particle?
ELECTROMAGNETIC RADIATION
Introduction to Physical Science Monday, Wednesday, Thursday Tom Burbine
Wave Nature of Light and Quantum Theory
Light. Light Terminology Which is not a measure we use to identify a type of light? A. Wavelength B. Speed C. Frequency D. Energy.
Index Unit 03 Electron Configuration Module 01: Light as a Wave Based on the PowerPoints By Mr. Kevin Boudreaux, Angelo State Univerisity U03Mod01 Light.
Light as a Wave OBJECTIVES:
Lecture 11 Electromagnetic Waves Chapter 21.8  Outline Discovery and Studies of Electromagnetic Waves Properties of Electromagnetic Waves The Spectrum.
Electromagnetic Spectra Review Game. When do electrons emit light? Moving from higher to lower energy levels.
12.6 Light and Atomic Spectra
Section 5.3 Physics and the Quantum Mechanical Model
Electron Behavior Electron absorb energy and jump to higher energy level (Excited State). Immediately fall back to original level (Ground State) emitting.
Facts about photons PHOTONS n Smallest quantity of electromagnetic radiation n bundle of energy (AKA quantum) n travels at 186,400 miles per second n.
Light and Energy Chemistry I. Classical description of light Light is an electromagnetic wave. Light consists of elementary particles called photons.
Chapter 6 Electronic Structure of Atoms Light The study of light led to the development of the quantum mechanical model. Light is a kind of electromagnetic.
Unit 6: Electrons in Atoms part 1: properties of waves.
Energy Levels & Photons Atomic & Nuclear Lesson 2.
Physics and the Quantum Mechanical Model
Atomic Emission Spectra
Chapter 13 Section 3 -Quantum mechanical model grew out of the study of light -light consists of electromagnetic radiation -includes radio and UV waves,
Electrons in Atoms Chapter 5 General Chemistry. Objectives Understand that matter has properties of both particles and waves. Describe the electromagnetic.
Bellwork What is the majority of the volume of an atom?
Section 5.3.  Neon advertising signs are formed from glass tubes bent in various shapes. An electric current passing through the gas in each glass tube.
1 CHAPTER 13: Electrons in the Atom. 2 Quantum Mechanical Model of the Atom and Ernest Schrodinger The model of the atom was developed based on the study.
The Bohr Model for Nitrogen 1. Bohr Model of H Atoms 2.
Light and Electrons! Ch 11. Light & Atomic Spectra A Brief Bit of History (development of the quantum mechanical model of the atom) Grew out of the study.
5.1 Electromagnetic Radiation. Wave motion The transfer of energy without matter is called wave motion Two Types.
The Bohr Model of the Atom: Bohr’s major idea was that the energy of the atom was quantized, and that the amount of energy in the atom was related to the.
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.
Electromagnetic Spectrum and Quantized Energy Why the electron is what it is.
ELECTROMAGNETIC RADIATION subatomic particles (electron, photon, etc) have both PARTICLE and WAVE properties Light is electromagnetic radiation - crossed.
LIGHT and QUANTIZED ENERGY. Much of our understanding of the electronic structure of atoms has come from studying how substances absorb or emit light.
Do Now: 1.If you could solve one problem using science, what would it be? 2.What branch of science do you think you would need to use to solve the problem?
Models, Waves, and Light Models of the Atom Many different models: – Dalton-billiard ball model (1803) – Thompson – plum-pudding model (1897) – Rutherford.
Chemistry Physics and the Quantum Mechanical Model.
Light and Quantized Energy Light and Quantized Energy Essential Question: What are the quantitative and qualitative properties across the range of the.
EM SPECTRUM Chapter 4 EM Spectrum with Frequency and Wavelength.
Electrons in Atoms Chapter 4.
Physics and the Quantum Mechanical Model
The Electromagnetic Spectrum Part 1
Electromagnetic Radiation
Light Ken Rogers Miami Killian.
Light: Electromagnetic Spectrum
Light and the Atomic Spectra
Atomic Theory Notes.
25.1 The Electromagnetic Spectrum
EM SPECTRUM Chapter 4 EM Spectrum with Frequency and Wavelength.
Waves and Electromagnetic Radiation
Section 4.6—Light.
FLAME TEST.
e–’s absorb (+) energy, move to outer levels
Atomic Theory Notes.
5.2 Properties of Light Our goals for learning What is light?
2.3 Light Objectives 3 and 5:b
Quantum Theory.
c =  f E = ℏf Where : ℏ = 6.63 x J٠s velocity -
Warm-up Example 3 from Practice Atomic Mass notes on pg 31!
Quantum Physics – Photons Mr Nesbo
AP Chemistry Chapter 7 Introduction Presentation
Presentation transcript:

Section 4.6—Light

Light is Electromagnetic Radiation Electromagnetic energy is energy that has electric and magnetic fields There are many types of Electromagnetic Radiation…visible is just one type! Electromagnetic energy travels in waves at the speed of light “c” (3.0 × 10 8 m/s)

Wavelengths (cm) Cosmic Rays Gamma Rays X- Rays Ultraviolet Rays Infrared Rays MicrowavesRadio wavesElectric Power Visible light 400 nm700 nm Types of Electromagnetic Radiation

Wave Properties—Frequency Frequency (  ) is the number of times a wave completes a cycle in one second (cycles per second is “Hertz” or “Hz”) Lower frequency Higher frequency

Wave Properties—Wavelength Wavelength ( ) is the distance from trough to trough of a wave (measured in meters “m”) wavelength

Relationship between wave properties The shorter the wavelength, the higher the frequency The higher the frequency, the higher the energy The speed of light is equal to wavelength (in meters) times frequency (in sec -1 or s -1 or Hz)  c = 

Visible Range Visible light 400 nm700 nm Wavelength increases Frequency decreases Energy decreases White light is made of all the colors…a prism can separate white light into a rainbow!

Light is Quantized Light is quantized, which means it comes in packets—you can only have certain amounts of it The “packets” are called “photons” The Energy of a photon (in Joules, “J”) is equal to Planck’s constant “h” times frequency)  E = h  where h = 6.63 × Js