The Wave Nature of Light Section 6.1. Objectives Study light (radiant energy or electromagnetic radiation) as having wavelike properties. Identify the.

Slides:

Advertisements

Similar presentations

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.

Advertisements

Physics and the Quantum Mechanical Model

Light, Photon Energies, and Atomic Spectra

Light and Quantized Energy

Creating a foldable for the electrons in atoms notes

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

Light and the Electromagnetic Spectrum

Index Unit 03 Electron Configuration Module 01: Light as a Wave Based on the PowerPoints By Mr. Kevin Boudreaux, Angelo State Univerisity U03Mod01 Light.

Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.

Lecture 11 Electromagnetic Waves Chapter 21.8  Outline Discovery and Studies of Electromagnetic Waves Properties of Electromagnetic Waves The Spectrum.

Electronic Structure. Wavelength ____________ (λ) - the shortest distance between equal points wave.

Warm Up 10/21 Where can electrons be found in an atom? What is their electric charge?

12.6 Light and Atomic Spectra

Chapter 5 in your textbook pp Wave Nature of Light  In the early 1900s scientists observed that certain elements emitted visible light when.

Light and the Electro- magnetic Spectrum. Light and the Electromagnetic Spectrum Almost all of our information on the heavens is derived from the light.

Electron Behavior Electron absorb energy and jump to higher energy level (Excited State). Immediately fall back to original level (Ground State) emitting.

Unit 6: Electrons in Atoms part 1: properties of waves.

The Electromagnetic Spectrum

Electronic Structure. Bohr Bohr proposed that the __________ atom has only certain allowable energy states.

Light and Quantized Energy Chapter 5 Section 1. Wave Nature of Light Electromagnetic radiation is a form of energy that exhibits wavelike behavior as.

Section 11.1 Atoms and Energy 1.To review Rutherford’s model of the atom 2.To explore the nature of electromagnetic radiation 3.To see how atoms emit light.

Physics and the Quantum Mechanical Model

Lesson: Electcromagnetic Spectrum (EMS)

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 and the Electromagnetic Spectrum Table Team Review — DEFINE in your own words ‘Electromagnetic radiation’. LIST three examples.

Physics and the Quantum Mechanical Model Notes. Light and the Atomic Spectrum Light is composed of waves at different wavelengths The wave is composed.

 Peak  Trough  Amplitude  Wavelength ( ) (in meters)  Frequency measured in Hertz: (Hz): cycles per second.

Waves carry energy from one place to another WAVES: SOUND & LIGHT.

Electromagnetic Radiation Definition: Characteristics of Waves Wavelength (λ): Frequency (v): Amplitude: Draw and Label the parts of a wave: Other relevant.

Bellwork What is the majority of the volume of an atom?

Electromagnetic Spectrum. Copyright McGraw-Hill The Nature of Light The electromagnetic spectrum includes many different types of radiation. Visible.

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.

“Physics and the Quantum Mechanical Model” Read pg. 138 p. 1

The Bohr Model for Nitrogen 1. Bohr Model of H Atoms 2.

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.

Light l The study of light led to the development of the quantum mechanical model. l Light is a kind of electromagnetic radiation. l Electromagnetic radiation.

Warm Up  Write the correct answers for the following:  1) 2.00 x m = __________m  2) 1.23 x m = __________nm.

Section 1 chapter 4. Electromagnetic Radiation (EMR) - a form of energy that travels in waves which includes radio waves, T.V. waves, microwaves, visible.

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.

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.

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.

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

LIGHT and QUANTIZED ENERGY.

Section 5.1 Light and Quantized Energy. Objectives Compare the wave and particle models of light Compare the wave and particle models of light Define.

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 the EM Spectrum The terms light, radiation, and electromagnetic wave can all be used to explain the same concept Light comes in many forms and.

Light and Quantized Energy Light and Quantized Energy Essential Question: What are the quantitative and qualitative properties across the range of the.

Wave Basics. Wave Definition  Any traveling disturbance that transfers energy. WAVES DON’T MOVE MATTER!!!

LIGHT and QUANTIZED ENERGY.

Electrons in Atoms Chapter 4.

Electromagnetic Spectrum

WAVES AND THE ELECTROMAGNETIC SPECTRUM

Light and the Atomic Spectra

Electrons in Atoms Section 2.2.

Waves and Electromagnetic Radiation

Electromagnetic radiation

UNIT 3 ELECTRON CONFIGURATION AND MODERN ATOMIC THEORY

Light and Quantized Energy

Electronic Structure.

Different Colored Fireworks

2.3 Light Objectives 3 and 5:b

Warm-up Example 3 from Practice Atomic Mass notes on pg 31!

The Wave Nature of Light

Presentation transcript:

The Wave Nature of Light Section 6.1

Objectives Study light (radiant energy or electromagnetic radiation) as having wavelike properties. Identify the characteristics of wavelength, frequency, and speed

Key Terms Electromagnetic radiation Wavelength Frequency Speed

Why Study Light? Our understanding of the electronic structure of atoms came from the analysis of light either emitted or absorbed

Visible Light Light we can see with our eyes An example of electromagnetic radiation

Electromagnetic Radiation Carries energy through space a.k.a radiant energy Many types of ER Visible light Radio waves Infrared radiation X rays

The different forms of ER share certain fundamental characteristics They all move through a vacuum as the speed of light: 3.00 x 10 8 m/s Radio AND X rays??

Wavelike Characteristics All ER types also behave like water waves Up and down motion Pattern of peaks and troughs repeated at regular intervals

Wavelength, Shortest distance between equivalent points on a continuous wave Between 2 adjacent peaks or troughs Measure in meters or nm

Frequency, Number of complete wavelengths or cycles that pass a given point per second. Measured in Hz (Hertz)

Amplitude Wave’s height from the origin to a peak, or from the origin to a trough Relates to the intensity of the radiation

Characteristics of Waves

What makes water waves travel at various speeds?

ER versus Water Waves ER move at the same speed Wavelength and frequency are always related

Why Your Radio Won’t Take an X ray ER types have different properties as a result of their varying wavelengths, expressed in units of length

Electromagnetic Spectrum

A VERY Large Spectrum Gamma rays = Radio waves =

Don’t Forget… ROY G BIV Order of colors (L  S) on the visible spectrum

Practice Problem The yellow light given off by a sodium vapor lamp used for public lighting has a wavelength of 589 nm. What is the frequency of this radiation?

Solution