Wavelength and Frequency E = h c =  c = speed of light (3 x 10 8 m/s) = frequency (s -1 )  = wavelength (m) E = energy (Joules or J) h  = Planck’s constant.

Slides:

Advertisements

Similar presentations

Frequency and Wavelength

Advertisements

Chapter 4 The Electromagnetic Spectrum Part 1. Demonstration Gas spectral tubes: NeonArgon.

Wavelength, Frequency, and Energy Practice Problems

Spectroscopy. LEQs: What is the relationship between the types of energy in the electromagnetic spectrum and their frequency and wavelength? How does.

Wave Nature of Light and Quantum Theory

SPECTRUMSPECTRUMSPECTRUMSPECTRUM  Electromagnetic Spectrum.

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

Electromagnetic Radiation The speed of electromagnetic radiation (speed of light) is constant at x 10 m/s – We’ll express it as 3x10 m/s – The symbol.

Section 5.3 Physics and the Quantum Mechanical Model

T HINK F IRST Follow the directions on the document being sent to you on the TI-nspire. There are 6 questions. Do not submit your answers. I will retrieve.

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.

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

Waves & Electromagnetic Spectrum

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

Part II. Waves & Particles Ch. 5 - Electrons in Atoms.

BIG topics... Light (electromagnetic radiation)  particle/wave dual nature of light  c, λ, ט, E & h Quantum theory (wave mechanical model)  Bohr model.

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.

Things to remember… Calculating wavelength and frequency: C = λν where c = 3.00 x 10 8 m/s Energy per photon: E = hν where h = x J ∙s photon.

The Electromagnetic Spectrum, Planck, and Bohr Honors Coordinated Science II Wheatley-Heckman.

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.

Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model

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.

Chapter 5: Electrons in Atoms

Einstein’s photon theory Photons = corpuscular theory E = hf E = Photon energy (Joules) h = Planck’s constant = x Js f = frequency of oscillations.

BIG topics... Light (electromagnetic radiation)  particle/wave dual nature of light  c, λ, ט & E Quantum theory (wave mechanical model)  Bohr model.

ELECTROMAGNETIC RADIATION subatomic particles (electron, photon, etc) have both PARTICLE and WAVE properties Light is electromagnetic radiation - crossed.

Electromagnetic Spectrum Basics Pg

Chemistry – Chapter 4. Rutherford’s Atomic Model.

Electrons in Atoms. Wave Behavior of Light Day 1.

Electrons and the Electromagnetic Spectrum. Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties.

Electromagnetic Spectrum Chemistry 6(B). Lesson Objectives Explore the electromagnetic spectrum Understand the mathematical relationships between energy,

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

A. Waves  Wavelength ( ) - length of one complete wave  Frequency ( ) - # of waves that pass a point during a certain time period hertz (Hz) = 1/s 

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)

The Atom Electrons outside the nucleus are attracted to the protons in the nucleus (positive and negative charge attract!) When charged particles move.

Using Planck’s Constant…. Picture credit: He was a German physicist and is considered as the founder.

Remember that all types of EM waves move at the speed of light (3.0 x 10 8 m/s).

Electrons in Atoms Chapter 4.

The Electromagnetic Spectrum Part 1

Electromagnetic Radiation

WARM UP 1. Write the chemical symbol for a nitrogen isotope that has 11 neutrons. 2. What is the average atomic mass of magnesium if you determine the.

Why Light, why now?.

كيمياء الثاني الثانوي الفصل الثاني الوحدة السادسة

Quantum Theory and the Atom

Kennesaw State University Physics 2212

BIG topics... Light (electromagnetic radiation)

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

Waves and particles Ch. 4.

650 nm = red, 580 nm = yellow, 450 nm = blue

Electromagnetic Waves

e–’s absorb (+) energy, move to outer levels

Electromagnetic Radiation

5.2 Properties of Light Our goals for learning What is light?

Quantum Theory.

Unit 3: Light and Electrons

Sample Problem c =    c  =  3.00  108 m/s  = 6.0  /s

Wavelength and Frequency

5.1 – ELECTRONS IN ATOMS.

c =  f E = ℏf Where : ℏ = 6.63 x J٠s velocity -

The speed of light in air is essentially c. (c = 3.00x108 m/s).

Quantum Physics – Photons Mr Nesbo

Electromagnetic Spectrum

Ch. 5 - Electrons in Atoms Waves & Particles.

Unit 3: Light and Electrons

BIG topics... Light (electromagnetic radiation)

BIG topics... Light (electromagnetic radiation)

Presentation transcript:

Wavelength and Frequency E = h c =  c = speed of light (3 x 10 8 m/s) = frequency (s -1 )  = wavelength (m) E = energy (Joules or J) h  = Planck’s constant (6.6 x J/s) = frequency (s -1 ) f f f f “nu” “lambda”

Electromagnetic Spectrum Frequency & wavelength are inversely proportional c = c:speed of light (3.00  10 8 m/s) :wavelength (m, nm, etc.) :frequency (Hz) Courtesy Christy Johannesson

Electromagnetic Spectrum GIVEN: f = ? = 434 nm = 4.34  m c = 3.00  10 8 m/s WORK: f = 3.00  10 8 m/s 4.34  m f = 6.91  Hz EX: Find the frequency of a photon with a wavelength of 434 nm. Courtesy Christy Johannesson 1 x 10 9 nm 1 m