1.6.  A spectroscope separates light into its component wavelengths, revealing a line spectrum that is unique to each element.

Slides:



Advertisements
Similar presentations
Wave-Particle Duality 1: The Beginnings of Quantum Mechanics.
Advertisements

Objectives To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy To learn about Bohr’s model of the hydrogen.
Anyone who is not shocked by quantum mechanics has not understood it. —Neils Bohr (1885–1962)
Electron Configuration and Energy Levels: Ground state: All the electrons in an atom have the lowest possible energies Most stable electron configuration.
Emission and Absorption of Electromagnetic Energy
Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.
Electrons and Light How does the arrangement of electrons in the atom determine the color of light that it emits?
The Bohr Model: Orbits and Line Spectra. Understand the historical development of the Quantum Mechanical Model of the atom. Describe how a produced line.
Electrons Arrangement in the Atom Key words: Energy, wavelength, frequency, photon Use these terms in a sentence (s) which makes sense.
Electromagnetic Radiation and Light
Emission Spectra Bohr Model of the Atom.
Atomic Theory Part 2 The Bohr Model of the Atom. Problems with Rutherford’s Model Two pieces of evidence could not be explained: 1.The Stability of the.
Quantization of Energy. When the atom gets excited… To help visualize the atom think of it like a ladder. The bottom of the ladder is called GROUND STATE.
Chapter 4 The Bohr Model of the Atom Part 1. Visible Light.
Bohr-ing! Toward a Modern Atomic Theory LG: I can explain Bohr’s model of the atom and the experimental evidence to support this.
Electron Energy and Radiation Quantum Mechanics and Electron Movement.
Light and Energy How the structure of electrons relates to the function of emitting energy as light.
New Way Chemistry for Hong Kong A-Level Book 11 Chapter 4 The Electronic Structure of Atoms.
Wave-Particle Duality: The Beginnings of Quantum Mechanics.
Wave-Particle Duality: The Beginnings of Quantum Mechanics.
December 1 The wave-mechanical model of the atom Homework Finish worksheet.
Development of Modern Atomic theory. Modern Model of Atom When energy is added to an atom : Low NRG State (ground state)  High energy state (excited.
THE ELECTROMAGNETIC SPECTRUM
Niels Bohr (1913) Bright-Line Spectrum Energy Levels Planetary Model
The Bohr Model of the Atom. The behavior of electrons in atoms is revealed by the light given off when the electrons are “excited” (made to absorb energy).
Electrons Negative charge e- Located in the electron cloud far from the nucleus Have mass, but it is negligible Also have wave-like properties.
Electromagnetic radiation – transmission of energy through space in the form of oscillating waves wavelength, – distance between identical points on successive.
Unit 2: Atoms and Bonding 2.62 Unit 2: Atoms and Bonding 2.62 Photons and Energy Textbook ch 6.2 and ch 6.3.
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.
Topic: Electrons in Atoms Ground/Excited States Do Now: List the charge, number of protons, and number of electrons for: 1.Ca +2 2.Fe +3 3.F -1 4.P -3.
The Bohr Model: Atoms with Orbits pg LO: I can explain what line spectra represent.
Electromagnetic Spectrum Section 1 The Development of a New Atomic Model Chapter 4.
Quantum Theory and the Atom In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame. Analysis of the emitted.
AtomsSection 3 Modern Models of the Atom 〉 What is the modern model of the atom? 〉 In the modern atomic model, electrons can be found only in certain energy.
Section 11.2 The Hydrogen Atom 1.To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy 2.To learn about Bohr’s.
Wave-Particle Duality JJ Thomson won the Nobel prize for describing the electron as a particle. His son, George Thomson won the Nobel prize for describing.
Electromagnetic Spectrum and the Atom. Electromagnetic energy Commonly known as light energy Charged particles move in waves.
Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.
Interpretation of Hydrogen Emission Spectra
Bohr Model Of Atom.
Bohr Model Of Atom.
Quantum Theory & the Atom
Interpretation of Hydrogen Emission Spectra
Waves.
Quantum Theory.
5.1 Light & Energy F. Electrons & Light
0:56 0:55 0:54 0:53 0:57 0:58 1:02 1:01 1:00 0:59 0:52 0:51 0:44 0:43 0:42 0:41 0:45 0:46 0:50 0:49 0:48 0:47 1:03 1:04 1:19 1:18 1:17 1:16 1:20 1:21 1:25.
Wave-Particle Duality
The Bohr Model (1913) revolve sun energy
Neils Bohr.
Bohr’s Model Why don’t the electrons fall into the nucleus?
Electromagnetic Spectrum and the Atom
Bohr's Model of the Atom.
Energy and Electrons energy
WHAT THE HECK DO I NEED TO BE ABLE TO DO?
Light and Quantized Energy
Light, Photon Energies, and Atomic Spectra
Flame Tests.
M. Billings North Surry High School
Section 3: Modern Atomic Theory
Light and electrons.
The fingerprints of elements
Bohr, Emissions, and Spectra
Atomic Theory – Bohr & Chadwick
Interpretation of Hydrogen Emission Spectra
Section 3: Modern Atomic Theory
Flame tests.
Development of Quantum Mechanics Bohr’s Contribution
Excited State vs. Ground State
Aim: How are an atom’s electrons configured?
Presentation transcript:

1.6

 A spectroscope separates light into its component wavelengths, revealing a line spectrum that is unique to each element.

 Bohr explained this phenomena by suggesting that electrons revolve around the atom’s nucleus in orbits of fixed energy

 The electrons are restricted to certain energy levels, and the energy is quantized  Quantized means the electrons have a specific amount of energy at each energy level

 If an electron absorbs energy, it becomes excited and can jump to a higher energy level  In order for the electron to return to its original energy level, it must release the same amount of energy  The lines that are produced in a line spectrum are a result of the electron falling back to its original position

 Electrons can exist at different levels around the nucleus of an atom  These levels, correspond to the quantum numbers

Quantum mechanics

Page 22 #1-7