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.

Slides:



Advertisements
Similar presentations
RADIO WAVES, MICROWAVES, INFRARED, VISIBLE, ULTRAVIOLET, X-RAYS, GAMMA RAYS HIGH< wavelength LOW.
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.
Waves. Characteristics of Waves Frequency Amplitude.
Physics and the Quantum Mechanical Model l OBJECTIVES: - Calculate the wavelength, frequency, or energy of light, given two of these values.
Chapter 4 The Electromagnetic Spectrum Part 1. Demonstration Gas spectral tubes: NeonArgon.
Creating a foldable for the electrons in atoms notes
Rutherford’s model -Shows where protons & neutrons are -Not good at showing the location of electrons.
Properties of Light Is Light a Wave or a Particle?
Light, Photon Energies, and Atomic Spectra
Wavelength – λ – distance between successive points on a wave (crest to crest)
ELECTROMAGNETIC RADIATION AND THE NEW ATOMIC MODEL.
Wave Nature of Light and Quantum Theory
Light and Electrons October 27, 2014.
Light, Photon Energies, and Atomic Spectra
SPECTRUMSPECTRUMSPECTRUMSPECTRUM  Electromagnetic Spectrum.
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
Section 1: Light and Quantized Energy
Waves, Particles, and the Spectrum Quantum Theory.
Chapter 13 Section 3 -Quantum mechanical model grew out of the study of light -light consists of electromagnetic radiation -includes radio and UV waves,
I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms yC. JOHANNESSON.
Bellwork What is the majority of the volume of an atom?
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 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.
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.
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.
Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model
Electronic Behavior of Atoms. LO Describe how light is created. Explain how wavelengths of light relate to energy levels in the atom. SC View the spectrum.
Chapter 5: Electrons in Atoms
CONTENT OBJECTIVE understand the electromagnetic spectrum and the mathematical relationships between energy, frequency, and wavelength of light. WHAT.
ELECTROMAGNETIC RADIATION subatomic particles (electron, photon, etc) have both PARTICLE and WAVE properties Light is electromagnetic radiation - crossed.
Calculating Wave Speed
Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.
LIGHT and QUANTIZED ENERGY. Much of our understanding of the electronic structure of atoms has come from studying how substances absorb or emit light.
Electromagnetic Spectrum Basics Pg
Vocabulary Review New radiation electromagnetic radiation wavelength
Chemistry – Chapter 4. Rutherford’s Atomic Model.
Electrons in Atoms. Wave Behavior of Light Day 1.
Electromagnetic Spectrum Chemistry 6(B). Lesson Objectives Explore the electromagnetic spectrum Understand the mathematical relationships between energy,
Do Now 1. How can a flame test be used to identify an unknown element? 2. Why did each element in this experiment produce a different color flame? 3. What.
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 
Light and Quantized Energy Light and Quantized Energy Essential Question: What are the quantitative and qualitative properties across the range of the.
The Bohr ModelNiels Bohr Violet: nm Indigo: nm Blue: nm Green: nm Yellow: nm Orange:
Electromagnetic Radiation. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance.
Chapter 5 Light Energy and Electron Configurations.
Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.
Using Planck’s Constant…. Picture credit: He was a German physicist and is considered as the founder.
Electromagnetic Spectrum
Chapter 11. Modern Atomic Theory
Light and Quantized Energy
Electromagnetic Radiation
Chemistry 1 Notes # 8 Light and Quantized Energy
Light, Photon Energies, and Atomic Spectra
AP Chemistry Unit 2 – Atoms, Molecules, and, Ions
Section 5.1 Light and Quantized Energy
I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )
FLAME TEST.
Waves and particles Ch. 4.
Light and Quantized Energy
Chemistry 1 Chapter 5 Part I Light and Quantized Energy
Unit 3: Light and Electrons
Wavelength and Frequency
5.1 – ELECTRONS IN ATOMS.
Electromagnetic Spectrum
Chemistry Unit 3 Chapter 4 and 5 – Atomic Structure
Ch. 5 - Electrons in Atoms Waves & Particles.
Unit 3: Light and Electrons
Presentation transcript:

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 your answers at ________. Get your calculator and log in

T ODAY ’ S L EARNING T ARGET I/We can make distinctions between light as a wave and light as a particle Vocabulary to know and use: frequency= ν (nu), wave length= λ (lambda), speed of light= c, quantum, Photon, Photoelectric effect, Planck’s constant, emission spectrum, electromagnetic spectrum

E LECTROMAGNETIC S PECTRUM mology-and-astronomy/v/introduction-to- light Light as a wave and light as a particle

c =λν Speed of light = c = 3.00 x 10 8 m/s Also written as 3.00 x 10 8 m s -1 Wavelength = λ = lambda = measurement from crest to crest = measured in nm or m (1 nm = m) Frequency = ν = nu = one wave per second =1 Hz = 1/s = s -1 Write this in your composition book.

H OW TO SOLVE A PROBLEM : E X. W HAT IS THE WAVELENGTH OF LIGHT THAT HAS A FREQUENCY OF 5.77 X H Z ? What is the problem asking you to solve? Ex. wavelength Write down what the problem gives to you (numerical values) and what they represent (units). Ex x Hz which is the frequency Write the formula(s) needed to solve the problem. Ex. c=λν Input the numerical values in the formula. Ex x 10 8 ms -1 = λ x s -1 Do the math and put a box around your answer. Include units x 10 8 ms -1 /5.77 x s -1 = λ x m = λ 5.20 x m = λ (Copy this in your composition book)

Energy of a photon E quantum = hv E quantum = energy of a photon h = Planck’s constant = x J. s v = frequency J = joule = unit for energy s = second Write this in your composition book.

C ALCULATING THE ENERGY OF A PHOTON What is the energy of a photon of red light with a frequency of 4.30 x s -1 ?

F IVE A CTIVITIES 1. Do the following five activities: a. Flame tests pg. 142; follow directions in book. There is one change: use an inoculating loop rather than a cotton swab. Answer all of the Analyze and Conclude questions. b. Emission spectrum drawing: Choose a gas and draw it’s emission spectrum. Follow directions at this station. c. Read pp in the chemistry text and complete practice problems 15 and 116 on pg. 141 d. Read pp in the chemistry text and complete practice problems on pg. 144 e. Create a Frayer Model in your composition book of light as a particle and light as a wave (see example on white board). 2. When you are done with all five show me your work to receive 25 lab points for your learning. 3. Complete as much as you can by the end of the period. Focus on the flame test 4. If you finish early, read pp in the chemistry text. Your homework is to finish any of the problems in c and d above and the Frayer Model.