Light and the Electromagnetic Spectrum. Light Phenomenon Light can behave like a wave or like a particle A “particle” of light is called a photon.

Slides:

Advertisements

Similar presentations

Physics and the Quantum Mechanical Model Section 13.3

Advertisements

Light and the Electromagnetic Spectrum

Physics and the Quantum Mechanical Model

Light and the Electromagnetic Spectrum

What do you see? Old woman? Or young girl?  Is turning a light on and off a chemical or physical change? ◦ Physical change  What creates light?

Electromagnetic Radiation

ENERGY & LIGHT THE QUANTUM MECHANICAL MODEL. Atomic Models What was Rutherford’s model of the atom like? What is the significance of the proton? What.

Properties of Light Is Light a Wave or a Particle?

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

Light and the Electromagnetic Spectrum

Warm Up Draw the Bohr Model for Aluminum and Neon.

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

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

Light and the Quantum Mechanical Model of the Atom

Waves & Particles Ch. 4 - Electrons in Atoms.

12.6 Light and Atomic Spectra

Section 5.3 Physics and the Quantum Mechanical Model

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

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

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

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.

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

Chapter 5 Section 5.1 Electromagnetic Radiation

Chapter 13 Section 3 -Quantum mechanical model grew out of the study of light -light consists of electromagnetic radiation -includes radio and UV waves,

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

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

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

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

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.

Light Waves and Particle Characteristics. Parts of a Wave = wavelength (lambda) =frequency(nu)

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

Objectives I can calculate wavelength, frequency or energy of light. I can explain the emission spectrum of an element.

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

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.

Electrons in Atoms Light is a kind of electromagnetic radiation. All forms of electromagnetic radiation move at 3.00 x 10 8 m/s. The origin is the baseline.

Electrons in Atoms. Wave Behavior of Light Day 1.

Models, Waves, and Light Models of the Atom Many different models: – Dalton-billiard ball model (1803) – Thompson – plum-pudding model (1897) – Rutherford.

Electromagnetic Waves & the Electromagnetic Spectrum electromagnetic spectrum power point.

Waves & Particles Electrons in Atoms. Electrons Electrons which are negatively charged, travel around the nucleus (the center of the atom).

Observing Atomic Spectra Wave simulation Bohr’s Model of the Atom.

Light and the Electromagnetic Spectrum

Electrons in Atoms Chapter 4.

Light and the Electromagnetic Spectrum

Light and the Electromagnetic Spectrum

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Arrangement of electrons in atoms

Light and the Electromagnetic Spectrum

The Electromagnetic Spectrum

Chapter 5 Electrons in Atoms.

EM SPECTRUM Chapter 4 EM Spectrum with Frequency and Wavelength.

Light and the Electromagnetic Spectrum

Waves and Electromagnetic Radiation

11/10/16 Today I will define the characteristics of a wave and compare the major regions of the electromagnetic spectrum. Warm Up – What are the three.

Section 5.1 Light and Quantized Energy

Light and the Electromagnetic Spectrum

Waves and particles Ch. 4.

Light and the Electromagnetic Spectrum

Light and Quantized Energy

Light and the Electromagnetic Spectrum

5.1 – ELECTRONS IN ATOMS.

Light and the Electromagnetic Spectrum

Electron Configurations

Electromagnetic Spectrum

Light and the Electromagnetic Spectrum

Light and the Electromagnetic Spectrum

Light and the Electromagnetic Spectrum

Light and the Electromagnetic Spectrum

Presentation transcript:

Light and the Electromagnetic Spectrum

Light Phenomenon Light can behave like a wave or like a particle A “particle” of light is called a photon

The Electromagnetic Spectrum The electromagnetic spectrum represents the range of energy from low energy, low frequency radio waves with long wavelengths up to high energy, high frequency gamma waves with small wavelengths.

Frequency Ranges The shorter the wavelength, the higher the frequency. The longer the wavelength, the lower the frequency. Close your eyes for a moment……..

Frequency and Wavelength The frequency (f) of a wave is the number of waves to cross a point in 1 second (units are Hertz – cycles/sec or sec -1 ) the wavelength (λ) - the distance from crest to crest on a wave. measured in meters (m), centimeters (cm), and nanometers (nm).

The product of wavelength and frequency always equals the speed of light. c = λf Why does this make sense? NOTE: c is a constant value= 3.00 x 10 8 m/s

Calculate the wavelength of yellow light emitted from a sodium lamp if the frequency is 5.10 x Hz (5.10 x s -1 ) List the known infoList the unknown c = 3.00 x 10 8 cm/swavelength (λ) = ? cm Frequency (f) = 5.10 x s -1 C = λf λ = c f λ = 3.00 x 10 8 cm/s = 5.88 x cm 5.10 x s -1 PROBLEMS

YOUR TURN

The photoelectric effect – When light shines on metals, electrons (photoelectrons) are ejected (or released) from their surface. Planck discovered the relationship between a quantum of energy and the frequency of radiation. Einstein called the particles that carried a quantum of energy photons. Red light will not cause electrons to eject!

Energy of light

The photoelectric effect has practical applications in photoelectrical cells used for solar powered cars, and solar powered calculators.

Below is a picture of the spectral lines given off by hydrogen. Note there are 3 different frequencies. Hydrogen-Atom Line-Emission Spectrum

Current is passed through a glass tube containing Hydrogen. This current excites the electrons into an excited state. The excited electrons fall back down to its ground state and gives off energy in the form of colored light Each element has its own unique line-emission spectrum

The emission spectra makes it possible to identify inaccessible substances. Most of our knowledge of the universe comes from studying the emission spectra of stars. Below is the spectra of a few more elements. Helium

Neon Argon