Notes #3: History of the Atom (Part 3)

Slides:

Advertisements

Similar presentations

Electron Configuration and Energy Levels: Ground state: All the electrons in an atom have the lowest possible energies Most stable electron configuration.

Advertisements

Emission and Absorption of Electromagnetic Energy

Electrons Arrangement in the Atom Key words: Energy, wavelength, frequency, photon Use these terms in a sentence (s) which makes sense.

Emission Spectra Bohr Model of the Atom.

December 1 The wave-mechanical model of the atom Homework Finish worksheet.

Chapter 4 Electrons. ELECTRON BEHAVIOR Who made this model of the atom?

Chem Saver Pg 18 Electrons absorb energy and jump to excited state Electrons release energy as a photon and fall back to ground state.

Electrons Negative charge e- Located in the electron cloud far from the nucleus Have mass, but it is negligible Also have wave-like properties.

Student will learn: Relationship between light & electrons What produces color Electromagnetic Spectrum Readings Neils Bohr Model of Hydrogen Readings.

Atomic History Part 2. Bohr Model Each element gave off different colors of light when they absorbed energy from some source and then released it. These.

Bohr Diagrams Electron Energy States. Bohr Model Bohr - electrons in an atom can have only specific amounts of energy NEW idea! quantum number (n) assigned.

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.

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.

Models of the Atom Chapter 4 Chm and

Interpretation of Hydrogen Emission Spectra

The Bohr Model of the Atom

Bohr Model Of Atom.

Models of the Atom SCH3U.

Quantum Theory & the Atom

Noble-ity Page 175.

II. Bohr Model of the Atom (p )

Bohr Model of the Atom (p ) Read the text

Bohr Model of the Atom & Light

The Nuclear Atomic Model

Bohr's Model of the Atom.

Interpretation of Hydrogen Emission Spectra

Bohr & Schrödinger.

Models of the Atom SCH4C September 2017.

II. Bohr Model of the Atom (p )

Electrons in Atoms Chapter 5.

Bohr and Introduction To Electron Structure Part I.

Aim: What happens when electrons get excited?

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.

Electrons orbit the nucleus only within allowed energy levels.

The Bohr Model (1913) revolve sun energy

Bohr’s Model Why don’t the electrons fall into the nucleus?

Bohr's Model of the Atom.

HYDROGEN EMISSION SPECTRUM

EXCITING OF ELECTRONS.

Ch. 4/5 Notes Day 5 2/2/16.

Energy and Electrons energy

WHAT THE HECK DO I NEED TO BE ABLE TO DO?

Bohr's Model of the Atom.

The Bohr Model of the Hydrogen Atom

Bohr's Model of the Atom.

“Spanish Steps”, Francesco de Sanctis, 1726, Rome, Italy

II. Bohr Model of the Atom (p )

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.

Bohr's Model of the Atom.

M. Billings North Surry High School

Flame Test Recap WCHS Chemistry.

Niels Bohr The Bohr Model.

The fingerprints of elements

Bohr, Emissions, and Spectra

Atomic Theory – Bohr & Chadwick

Niels Bohr The Bohr Model.

Interpretation of Hydrogen Emission Spectra

The Nuclear Atomic Model

Give the symbol and number of protons in one atom of:

Atomic Spectra and Flame Test

Electron Configurations

Bohr Model Starter: What do you picture when you think of an atom?

Excited State vs. Ground State

Electrons in Atoms Chapter 5.

The Nature of Electrons

Presentation transcript:

Notes #3: History of the Atom (Part 3) WCHS Chemistry

RUTHERFORD

WRONG! Correct :) NEILS BOHR (1919) Bohr Model of the Atom Electrons orbit around the nucleus like planets around the sun Each orbit is a different energy level: Farther from nucleus → greater energy Highest Energy WRONG! 4 3 2 1 Nucleus Correct :)

PROBLEMS!!! NEILS BOHR (1919) Bohr Model of the Atom Bohr’s model incorrectly said: E- are in specific places We can predict where orbits are

Discovered the neutron Must have a neutral “buffer” JAMES CHADWICK (1932) Discovered the neutron Must have a neutral “buffer”

BOHR’S MODEL VS. FLAME TESTS There are 2 states for an electron to be in: Ground State vs. Excited State Low energy e- picture ADD ENERGY e- gain energy to jump up to higher energy levels e- as close to nucleus as possible e- e- e- e- e- e- e- e-

BOHR’S MODEL VS. FLAME TESTS Then, they fall back down to their original orbit, releasing that energy as a photon of light. See light!! Photon We see photons of light. Different amounts of energy are different colors! Bohr’s model could predict these colors, but it only worked well for hydrogen -- why? B/c Hydrogen is so simple! → only 1 electron!

WHITE LIGHT Lowest Energy Highest Energy We see different colors of light due to different amounts of energy!

HYDROGEN EMISSION SPECTRUM You will see a “bar code” Every “bar” on the code is an electron releasing a photon when it falls back down from an excited state to ground state.

HELIUM EMISSION SPECTRUM

NITROGEN EMISSION SPECTRUM

NEON EMISSION SPECRUM