Which kind of electromagnetic radiation has the least amount of energy? RADIO WAVES.

Slides:

Advertisements

Similar presentations

Chemistry Daily 10’s Week 5.

Advertisements

1. To describe Rutherford’s model of the atom 2. To explore the nature of electromagnetic radiation 3. To see how atoms emit light 11.1 Objectives.

Light and Quantized Energy

The Modern Atom Figure: 05-00CO Caption:

A) The wavelength and frequency of a light wave

Electrons And Light. Electromagnetic Radiation Energy that travels as a wave through space Wavelength –λ – distance between corresponding points on adjacent.

Chapter 11 Review Presentation Presenter in class using clickers.

Wave Nature of Light and Quantum Theory

Unit 2 Practice Review Ch. 3,4,5 no periodic trends

Electromagnetic Spectrum

Electromagnetic Radiation and Light Waves. Let’s Review Rutherford’s Atom The atom has a small dense nucleus which – Contains most of the mass of the.

Which scientist studied glowing metals and discovered that only certain wavelengths of light are emitted at each specific temperature & represented a.

Zumdahl • Zumdahl • DeCoste

General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc.1 Chapter 3 Atoms and Elements 3.6 Electron Energy Levels.

Nature of Light chapter s – 1900s Is Light a wave or a stream of particles.

Unit 2 Extra Practice October 15 (ODD) October 16 (EVEN)

© Copyright Pearson Prentice Hall Slide 1 of 26 Light and Atoms. 5.1.

Electron Configuration And a Brief Introduction to the Quantum Model of the Atom.

5.2 QUANTUM THEORY AND THE ATOM PART THREE Quantum numbers and orbitals.

CHEMISTRY World of Zumdahl Zumdahl DeCoste. Copyright© by Houghton Mifflin Company. All rights reserved. Chapter 11 Modern Atomic Theory.

Chapter 4 Electron Configurations. Early thoughts Much understanding of electron behavior comes from studies of how light interacts with matter. Early.

Section 11.1 Atoms and Energy 1.To describe Rutherford’s model of the atom 2.To explore the nature of electromagnetic radiation 3.To see how atoms emit.

Unit #4 CP Chemistry.  Bohr  Quantum Numbers  Quantum Mechanical Model.

Electromagnetic Spectrum. Matter Review All matter is made of A______ Matter exists in different forms or phases. They are.

Chapter 5 #1) Why did Rutherford’s atomic model need to be replaced?

Ernest Rutherford’s Model l Discovered dense positive piece at the center of the atom- “nucleus” l Electrons would surround and move around it, like planets.

Modern Atomic Theory: How are an atom’s electrons configured?

Chapter 7. Electromagnetic Radiation  aka. Radiant energy or light  A form of energy having both wave and particle characteristics  Moves through a.

The distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals an energy is associated with each electron.

Electrons in Atoms Chapter 5. Chapter 5: Electrons in Atoms 5.1 Light and Quantized Energy Wave nature of light.

Class Notes-Bohr & New Atomic Model (Chapter 4, Section 1)

Chapter 5 Review. Vocabulary Discrete bundle of energy Energy needed to move an electron from one energy level to another Separation of light into different.

Electron Configuration Quantum Mechanics (Ohh scary)

Models of the Atom.  An atomic orbital is a region of space where an electron can be found  There are energy levels existing outside the nucleus ◦ These.

Chapter 5 UEQ Electrons in Atoms What does an atom really look like?

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.

Mrs Schultz Chemistry & Integrated Science Week beginning Mon. Nov. 17, 2014.

Chemistry Jeopardy Chemistry Jeopardy Chapter 4 Catch the Wave Step into the Light Orbit an Orbital Electron Fun Figure or Configure Me Bohr Me Famous.

Chapter 4 and 5 Test Review Bounceback Game. Rules of Bounceback – Students are in two groups, A and B. – Pick a number starting with 1 until everyone.

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.

Chapter 11 Modern Atomic Theory. EXIT Copyright © by McDougal Littell. All rights reserved.2 Figure 11.1: The Rutherford atom.

Electromagnetic Spectrum and the Atom. Electromagnetic energy Commonly known as light energy Charged particles move in waves.

Chapter 5: Electrons in Atoms Revising the Atomic Model Atomic Emission Spectra and the Quantum Mechanical Model.

Newton studies the Sun’s spectrum

Rutherford Model Know where the protons and neutrons are, but where are the electrons? If opposite charges attract, why do the electrons not fall into.

Lesson 1: The Nature of Electromagnetic Waves

Chapter 3 Atoms and Elements

Atomic Structure: The Quantum Mechanical Model

Zumdahl Zumdahl DeCoste

II. Bohr Model of the Atom (p )

Quantum Theory.

Wave Nature of Matter.

Electromagnetic Spectrum and the Atom

Unit 3 – Electron Configurations Part B: Bohr’s Model of Hydrogen

Energy and Electrons energy

ELECTRONS IN ATOMS.

The ELECTRON: Wave – Particle Duality

Light, Photon Energies, and Atomic Spectra

Electrons in Atoms Bohr Model

Electromagnetic Spectrum

Electromagnetic Radiation

Chapter 5 Electrons in Atoms

Which kind of electromagnetic radiation has the least amount of energy? RADIO WAVES.

Quantum Theory.

Which kind of electromagnetic radiation has the least amount of energy? RADIO WAVES.

Electrons and Light!.

Quantum Mechanical Model

The E.M.S. S1 Physics Energy.

Aim: How are an atom’s electrons configured?

Chapter 5 Review Questions

Presentation transcript:

Which kind of electromagnetic radiation has the least amount of energy? RADIO WAVES

TRUE OR FALSE Light is considered to be quantized because it comes in waves. FALSE Light is considered to be quantized because it can be considered to be a stream of photons!

What sublevel is pictured below? p sublevel

How many orbitals are pictured below?

How many total electrons can fit into the sublevel pictured below?

How many total electrons can fit the third principal energy level? 3s = 2 e- 3p = 6 e- 3d = 10 e- 18 electrons

What element am I? 1s22s22p63s23p64s23d104p65s24d105p4