Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Slides:



Advertisements
Similar presentations
Physics and the Quantum Mechanical Model Section 13.3
Advertisements

Physics and the Quantum Mechanical Model
Waves. Characteristics of Waves Frequency Amplitude.
5.3 Atomic Emission Spectra
Electromagnetic Radiation. Definitions Electromagnetic Radiation is energy with wavelike characteristics Moves at a speed of 3.0 x 10 8 m/s.
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.
Wavelength – λ – distance between successive points on a wave (crest to crest)
Chemistry Chapter 5 Ch5 Notes #1.
Wave Nature of Light and Quantum Theory
What gives gas-filled lights their colors?
Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.
12.6 Light and Atomic Spectra
Many scientists found Rutherford’s Model to be incomplete  He did not explain how the electrons are arranged  He did not explain how the electrons were.
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.
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.
Arrangement of Electrons in Atoms The Development of a New Atomic Model.
Physics and the Quantum Mechanical Model
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?
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.
5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.
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.
5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.
Chapter 5 – Electrons in Atoms text pages
Objectives I can calculate wavelength, frequency or energy of light. I can explain the emission spectrum of an element.
Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.
 Waves & Energy H Ch 5&6. Waves  Vibrating disturbance by which energy is transmitted Amplitude (Wavelength) u = λν.
Physics and the Quantum Mechanical Model.  Light consists of waves  A wave cycle begins at zero, increases to its highest value (crest), returns to.
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?
Electrons and the Electromagnetic Spectrum. Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties.
C. Johannesson I. Waves & Particles (p ) Ch. 5 - Electrons in Atoms.
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.
5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.
5.3 Physics and the Quantum Mechanical Model. Light By 1900 enough experimental evidence to convince scientists that light consists of waves.
Waves and the EM Spectra
Electrons in Atoms Chapter 4.
Wave-Particle Nature of Light
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
Electrons in Atoms Chapter 4.
Physics and the Quantum Mechanical Model
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
Chapter 6 Electronic Structure of Atoms
5.3 Atomic Emission Spectra
Light and the Atomic Spectra
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
Physics and the Quantum Mechanical Model
CHAPTER 5:Electrons in Atoms Light and Quantized Energy
5.3 Physics and the Quantum Mechanical Model
Electrons and Light Chapter 13.3.
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
Physics and the Quantum Mechanical Model
I. Waves & Particles (p ) Ch. 4 - Electrons in Atoms I. Waves & Particles (p )
FLAME TEST.
UNIT 3 ELECTRON CONFIGURATION AND MODERN ATOMIC THEORY
Waves and particles Ch. 4.
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
e–’s absorb (+) energy, move to outer levels
2.3 Light Objectives 3 and 5:b
Physics and the Quantum Model
Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra
5.1 – ELECTRONS IN ATOMS.
Electron Configurations
Chemistry Unit 3 Chapter 4 and 5 – Atomic Structure
Electromagnetic Spectrum
Ch. 5 - Electrons in Atoms Waves & Particles.
5.3 Physics and the Quantum Mechanical Model
Presentation transcript:

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra 5.1 Revising the Atomic Model 5.2 Electron Arrangement in Atoms 5.3 Atomic Emission Spectra and the Quantum Mechanical Model Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

The Quantum Mechanical Model Do Now Get a Chrome Book and log into Google Classroom. Complete Do Now. Get a spectroscope and begin the worksheet. https://www.youtube.com/watch?v=cfXzwh3KadE https://www.youtube.com/watch?v=jjy-eqWM38g Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Light and Atomic Emission Spectra Light consists of electromagnetic waves. Amplitude - wave’s height from zero to the crest. Wavelength () - distance between the crests. Frequency () - number of wave cycles to pass a given point per unit of time. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Light and Atomic Emission Spectra Low energy ( = 700 nm) High energy ( = 380 nm) Frequency  (s-1) 3 x 106 3 x 1012 3 x 1022 102 10-8 10-14 Wavelength  (m) Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Light and Atomic Emission Spectra Speed of Light = wavelength x frequency c = 2.998  108 m/s. c = ln Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Light and Atomic Emission Spectra Frequency () and wavelength () are inversely proportional. As wavelength increases, frequency decreases. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Calculating the Wavelength of Light Sample Problem 5.2 Calculating the Wavelength of Light Calculate the wavelength of the yellow light emitted by a sodium lamp if the frequency of the radiation is 5.09 × 1014 Hz (5.09 × 1014/s). Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Sample Problem 5.2 c = ln Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What is the frequency of a red laser that has a wavelength of 676 nm What is the frequency of a red laser that has a wavelength of 676 nm? Note: 1 m = 109 nm Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What is the frequency of a red laser that has a wavelength of 676 nm? c = ln c   =  = = = 4.43  1014 Hz c 2.998  108 m/s  6.76  10–7 m Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

The Quantum Concept and Photons The Quantization of Energy The energy (E) of a single quantum absorbed or emitted by a body is proportional to the frequency of radiation (n). h = Plank’s Constant = 6.626 x 10-34 J·s E = hn Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

The Quantum Concept and Photons Photoelectric effect: electrons are ejected when light of sufficient frequency shines on a metal. Light quanta are called photons Energy of a photon = E = h x ⋎ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Calculating the Energy of a Photon Sample Problem 5.3 Calculating the Energy of a Photon What is the energy of a photon of microwave radiation with a frequency of 3.20 × 1011/s? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

E = h  = (6.626  10–34 J·s)  (3.20  1011/s) = 2.12  10–22 J Sample Problem 5.3 E = h  = (6.626  10–34 J·s)  (3.20  1011/s) = 2.12  10–22 J Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What is the frequency of a photon whose energy is 1.166  10–17 J? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What is the frequency of a photon whose energy is 1.166  10–17 J? E = h n n = h E  = = = 1.760  1016 Hz 6.626  10–34 J 1.166  10–17 J·s E h Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

END OF 5. 3 EM Waves https://www. youtube. com/watch END OF 5.3 EM Waves https://www.youtube.com/watch?v=cfXzwh3KadE Fireworks https://www.youtube.com/watch?v=nPHegSulI_M Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.