Niels Bohr’s Energy Levels

Slides:



Advertisements
Similar presentations
Ch. 13 Electrons in Atoms Ch Models of the Atom
Advertisements

Arrangement of Electrons in Atoms
Electron Configuration and New Atomic Model Chapter 4.
The Modern Atomic Model After Thomson: Bohr, Placnk, Einstein, Heisenberg, and Schrödinger.
The Arrangement of Electrons in Atoms
CH 4 NOTES HOW ELECTRONS ARE ARRANGED. ELECTROMAGNETIC SPECTRUM Includes : –Gamma rays –Xrays –Ultraviolet –Visible –Infrared –Microwaves –Radio waves.
Electromagnetic Radiation
Pre-IB/Pre-AP CHEMISTRY
Properties of Light Is Light a Wave or a Particle?
Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.
Arrangement of Electrons in Atoms Part One Learning Objectives Read Pages Asgn #16: 103/1-6 1.
Physics and the Quantum Model
Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.
Chapter 4 Arrangement of Electrons in Atoms. Starter Look at the colors on a computer screen. What do you notice? Close inspection reveals that they are.
Chapter 4 Arrangement of Electrons in Atoms
Where are the electrons ? Rutherford found the nucleus to be in the center. He determined that the atom was mostly empty space. So, how are the electrons.
Chapter 4 Arrangement of Electrons in Atoms
Chemistry Chapter 4 Arrangement of Electrons in Atoms
Chemistry UNIT 3. Name: Date: Chemistry Unit 3 Atomic Theory and structure of an Atom.
I II III  Suggested Reading Pages  Section 4-1 Radiant Energy.
Chapter 5 Section 5.1 Electromagnetic Radiation
Electrons in Atoms By: Ms. Buroker. Okay … We now know that an element’s identity lies in its number of protons … but there is another particle which.
Mullis Chemistry Holt Ch.41 Atomic Structure Summary of Contributions Max Planck –A hot object emits energy in small, specific amounts called quanta. Albert.
 Unit 4 The Arrangement of Electrons Ch. 4. Exam 4 Analysis  Averages  The Atom+/25(%)  Measurement+/15(%) up from %  Phases/KMT+/10(82%) down from.
Chapter 4 Arrangement of Electrons in Atoms 4.1 The Development of a New Atomic Model.
Modern Chemistry Chapter 4 Arrangement of Electrons in Atoms
Arrangement of Electrons in Atoms The Development of a New Atomic Model.
Chapter 5 : Electrons in Atoms. Problems with Rutherford’s Model Chlorine # 17 Reactive Potassium # 19 Very reactive Argon # 18 Not reactive.
Electrons in Atoms Chapter 5. Duality of Light Einstein proved that matter and energy are related E = mc 2 Einstein proved that matter and energy are.
Development of Atomic Models
Quantum Theory and the Electronic Structure of Atoms Chapter 7 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Electrons Negative charge e- Located in the electron cloud far from the nucleus Have mass, but it is negligible Also have wave-like properties.
Electrons in Atoms The Development of a New Atomic Model.
The Development of a New Atomic Model  The Rutherford model of the atom was an improvement over previous models of the atom.  But, there was one major.
Mullis Chemistry Holt Ch.41 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location.
Modern Chemistry Chapter 4 Arrangement of Electrons in Atoms Sections 1-3 The Development of a New Atomic Model The Quantum Model of the Atom Electron.
Mullis Chemistry Holt Ch.41 Arrangement of Electrons in Atoms Principles of electromagnetic radiation led to Bohr’s model of the atom. Electron location.
Development of a New Atomic Model Properties of Light.
The Dilemma  Particles have mass and a specific position in space (matter)  Waves have NO mass and NO specific position in space (light and energy)
4.1 Refinements of the Atomic Model
Section 4-1 Continued.  Ground State – the lowest energy state of an atom  Excited State – a state in which an atom has a higher energy than in its.
Electromagnetic Spectrum Section 1 The Development of a New Atomic Model Chapter 4.
Enriched Chemistry Chapter 4 – Arrangement of Electrons in Atoms
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 Review. Wave Nature of Light Wavelength- Wavelength- The distance between two consecutive peaks or troughs. Frequency- Frequency- The number.
Unit 4 Energy and the Quantum Theory. I.Radiant Energy Light – electrons are understood by comparing to light 1. radiant energy 2. travels through space.
CHAPTER 11 NOTES MODERN ATOMIC THEORY RUTHERFORD’S MODEL COULD NOT EXPLAIN THE CHEMICAL PROPERTIES OF ELEMENTS.
Chemistry I Chapter 4 Arrangement of Electrons. Electromagnetic Radiation Energy that exhibits wavelike behavior and travels through space Moves at the.
Chapter 11 Modern Atomic Theory. Rutherford’s Atom What are the electrons doing? How are the electrons arranged How do they move?
Section 1 The Development of a New Atomic Model Objectives Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic.
Chapter 5.  Energy transmitted from one place to another by light in the form of waves  3 properties of a wave;  Wavelength  Frequency  Speed.
Light Light is a kind of electromagnetic radiation, which is a from of energy that exhibits wavelike behavior as it travels through space. Other forms.
Electromagnetic Radiation. Waves To understand the electronic structure of atoms, one must understand the nature of electromagnetic radiation. The distance.
CHAPTER 4 CHEMISTRY. PROPERTIES OF LIGHT (P91-93) Originally thought to be a wave It is one type of ELECTROMAGNETIC RADIATION (exhibits wavelike behavior.
Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.
Electrons in Atoms Chapter 4.
Chapter 6 Electronic Structure of Atoms
Arrangement of electrons in atoms
Physics and the Quantum Mechanical Model
Physics and the Quantum Mechanical Model
Chapter 4 The Wave Description of Light
Please write an electron configuration for Br-
Arrangement of electrons
Electrons.
Electromagnetic Spectrum
Light and electrons.
Arrangement of Electrons in Atoms
Arrangement of Electrons in Atoms
Chapter 4 Arrangement of Electrons in Atoms
Quantum Mechanical Model
Presentation transcript:

Niels Bohr’s Energy Levels Electrons in certain energy levels Orbits with certain amounts of energy Low energy levels: closer to nucleus High energy levels: farther from nucleus Ground state Electrons in lowest energy level possible Aufbau principle Electrons will occupy the lowest available energy level Episode 303

Excited Atom Atom has absorbed energy Excited state is unstable Quanta – Energy required to excite an electron Excited state is unstable Atom soon emits same amount of absorbed energy Energy seen as visible light Photon – particle with no mass containing a quanta of energy COLOR Episode 303

Wave Description of Light Wavelength (λ) Distance between corresponding points on adjacent waves Frequency(f or γ) The number of waves passing a given point in a given time Hertz C = λf C = 3.0 x 108 m/s : speed of light Episode 303

Electromagnetic Spectrum http://education.jlab.org/frost/speed_of_light.html What is the frequency of light if the wavelength is 6.0 x 10-7 m? C = λf C = 3.0 x 108 m/s : speed of light 3.0 x 108 m/s = (6.0 x10-7 m) f 3.0 x 108 m/s = f 6.0 x10-7 m 5.0 x 1014/s = f Episode 303

Electromagnetic Spectrum What is the wavelength of light if its frequency is 5.0 x 1014 Hertz? C = λf C = 3.0 x 108 m/s : speed of light 3.0 x 108 m/s = λ(5.0 x 1014/s) 3.0 x 108 m/s = λ 5.0 x 1014/s 6.0 x 10-7 m = λ Episode 303

Particle Description of Light Energy exists as particles called quanta Photoelectric Effect Metal emits electrons when light strikes the metal E =hf h is Plank’s Constant 6.626 x 10-34 Js Episode 303

Electromagnetic Spectrum How much energy does light contain if its frequency is 5.0 x 1014 Hertz? E = hf h = 6.626 x 10-34 Js : Plank’s Constant E= (6.626 x 10-34Js)(5.0 x 1014/s) E = 3.3 x 10-19 J Episode 303

The Modern View of Light Light has a dual nature Light may behave as a wave Light may behave as a stream of particles called quanta or photons Episode 303

Spectroscopy Spectral lines represent energy released as electrons return to lower energy levels Spectral lines identify an element Called the Bright Line Spectrum of an Element Episode 303

Orbital Region of space where an electron is likely to be found http://www.youtube.com/watch?v=rNM21emkMJo&feature=related Region of space where an electron is likely to be found Heisenberg Uncertainty Principle Impossible to determine location and velocity of a particle Episode 303

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2024 SlidePlayer.com Inc. All rights reserved.