Chemistry Physics and the Quantum Mechanical Model.

Slides:



Advertisements
Similar presentations
Chapter Two …continued
Advertisements

Unit 3 Light, Electrons & The Periodic Table.
Light.
Physics and the Quantum Mechanical Model
Chemistry.
Physics and the Quantum Mechanical Model l OBJECTIVES: - Calculate the wavelength, frequency, or energy of light, given two of these values.
The Electromagnetic Spectrum & Electromagnetic Radiation
Electromagnetic Spectrum
Electrons and Light How does the arrangement of electrons in the atom determine the color of light that it emits?
Physics and the Quantum Model
Light, Photon Energies, and Atomic Spectra
Quantum Mechanics.  Write what’s in white on the back of the Week 10 Concept Review  Then, answer the questions on the front Your Job.
Index Unit 03 Electron Configuration Module 01: Light as a Wave Based on the PowerPoints By Mr. Kevin Boudreaux, Angelo State Univerisity U03Mod01 Light.
Light and the Quantum Mechanical Model of the Atom
Waves & Particles Ch. 4 - Electrons in Atoms.
Electromagnetic Radiation and Light
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.
Section 5.3 Physics and the Quantum Mechanical Model
Electron Behavior Electron absorb energy and jump to higher energy level (Excited State). Immediately fall back to original level (Ground State) emitting.
Light and Energy Chemistry I. Classical description of light Light is an electromagnetic wave. Light consists of elementary particles called photons.
Unit 6: Electrons in Atoms part 1: properties of waves.
Chapter 5 Electrons in Atoms.
Physics and the Quantum Mechanical Model
Electronic Configurations of Atoms
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.
Electromagnetic Radiation & Light. 2 What are the atom models we know of? 2.
Bellwork What is the majority of the volume of an atom?
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.
“Physics and the Quantum Mechanical Model” Read pg. 138 p. 1
The Bohr Model for Nitrogen 1. Bohr Model of H Atoms 2.
Slide 1 of 38 chemistry. Slide 2 of 38 © Copyright Pearson Prentice Hall Physics and the Quantum Mechanical Model > Light The amplitude of a wave is the.
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.
Section 1 chapter 4. Electromagnetic Radiation (EMR) - a form of energy that travels in waves which includes radio waves, T.V. waves, microwaves, visible.
Objectives I can calculate wavelength, frequency or energy of light. I can explain the emission spectrum of an element.
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.
Drill Determine the electron configuration of the following: Determine the electron configuration of the following: H He He.
Physics and the Quantum Mechanical Model.  Light consists of waves  A wave cycle begins at zero, increases to its highest value (crest), returns to.
Chapter 5 “Electrons in Atoms”. Section 5.3 Physics and the Quantum Mechanical Model l OBJECTIVES: Describe the relationship between the wavelength and.
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.
5.3 Physics and the Quantum Mechanical Model. Light By 1900 enough experimental evidence to convince scientists that light consists of waves.
Slide 1 of 38 chemistry. © Copyright Pearson Prentice Hall Slide 2 of 38 Physics and the Quantum Mechanical Model Neon advertising signs are formed from.
Chapter 5: Electrons in Atoms Revising the Atomic Model Atomic Emission Spectra and the Quantum Mechanical Model.
Physics and the Quantum
Wave-Particle Nature of Light
Physics and the Quantum Mechanical Model
Chemistry.
Light and the Atomic Spectra
Physics and the Quantum Mechanical Model
Chapter 5 Notes Electrons.
Physics and the Quantum Mechanical Model
5.3 Physics and the Quantum Mechanical Model
Chapter 11 “The Electromagnetic Spectrum”
Have you ever wondered how you get different colored fireworks?
Quantum Theory and the Atom
Electron Emission Spectra
Section 5.3 Physics and the Quantum Mechanical Model
Electromagnetic radiation
Light, Photon Energies, and Atomic Spectra
Light and electrons.
5.3 Physics and the Quantum Mechanical Model
2.3 Light Objectives 3 and 5:b
Quantum Mechanics.
Electron Configurations
Electromagnetic Spectrum
5.3 Physics and the Quantum Mechanical Model
Light and EM Spectrum Light is all thanks to electrons…well… photons…but whatever. What do you REALLY know about light?
2 Light & Electromagnetic Spectrum
Presentation transcript:

Chemistry Physics and the Quantum Mechanical Model

Section 3 Terms Amplitude Wavelength Frequency Hertz Electromagentic Radiation Spectrum Ground State Photons Heisenberg Uncertainty Principle

Star Light, Star Bright Light has dual personality, acting as a particle and a wave Characteristics of waves include: – AMPLITUDE – WAVELENGTH – FREQUENCY

AMPLITUDE: Distance from zero to waves highest or lowest point – Highest point is the crest, lowest point is the trough – Amplitude affects brightness, or the intensity of light

WAVELENGTH: The distance between crests or troughs – Represented by the Greek letter lambda ( λ ) – This affects the type of light Wavelength

FREQUENCY: The # of wave cycles to pass a given point per unit time – Represented by Greek letter nu ( ν ) – SI unit is cycles per second, or Hertz (Hz)

Waves with different frequencies look different A wave with a frequency of 4 Hz has two times more cycles per unit time than one with a frequency of 2 Hz

Practice Problems Draw six waves in two seconds with an amplitude of 3 Draw 3 waves in two seconds with an amplitude of 2 Draw a wave with a frequency of 4 Hz, an amplitude of 1 over two seconds

The relationship between wavelength, and frequency is: – c = λ ν, where c is always a constant, the speed of light Speed of light is 3.0 x 10 8 m/s (in a vacuum) – Wavelength and frequency are INVERSELY PROPORTIONAL to each other One goes up, the other goes down

Practice Problems Practice Problem – A radio wave has a wavelength of 700 m. If traveling in a vacuum, what is the waves frequency? – An x-ray with a wavelength of 4.5 x m is traveling through a vacuum. What is its frequency? – Red light has a wavelength of 480 nm. What is its frequency in a vacuum? – The frequency of a wave traveling through a vacuum is Hz (5 MHz). What is the wave’s wavelength?

ELECROMAGNETIC RADIATION: Energy waves that travel in a vacuum at 3.0 x 10 8 m/s – Includes radio, microwave, infrared, visible, ultraviolet, x-ray, and gamma rays – EM SPECTRUM: the range of different wavelengths of light – You must be able to reproduce this exact picture!!!

Atomic Spectra Electrons can absorb certain amounts of energy, such as the energy in electricity Electrons will then move into higher energy sublevels – Electrons now in an “excited” state Electrons will immediately release that energy and move back to their GROUND STATE – The lowest possible energy of the electron Released energy is in the form of a specific color of light When ordinary light is passed through a prism, it produces all visible colors

ATOMIC EMISSION SPECTRA: The unique color fingerprint of an element when its light is passed through a prism – Combination is unique to that element

Light behaves like a wave as well as a particle – PHOTON: A bundle of EM energy that interacts with matter similarly to a particle

Chapter 5 Review Pg – Problems 23, 26-29, 32-37, 41 – Question 73, calculate only the frequency of the waves; they give you the wavelengths in cm, you cannot use cm