Electrons and the Electromagnetic Spectrum. Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties.

Slides:

Advertisements

Similar presentations

Wavelength, Frequency, and Energy Practice Problems

Advertisements

Electromagnetic Spectrum

The Development of a New Atomic Model  Problem with Rutherford model – no explanation of where e-s are  New info about light led to new model.

Properties of Light Is Light a Wave or a Particle?

Wavelength – λ – distance between successive points on a wave (crest to crest)

ELECTROMAGNETIC RADIATION AND THE NEW ATOMIC MODEL.

Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.

NCCS & Properties of Light The Wave Description of Light Electromagnetic radiation is a form of energy that exhibits wavelike behavior.

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.

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

Chapter 5 Section 5.1 Electromagnetic Radiation

Arrangement of Electrons in Atoms The Development of a New Atomic Model.

Electrons and the Electromagnetic Spectrum Table Team Review — DEFINE in your own words ‘Electromagnetic radiation’. LIST three examples.

Physics and the Quantum Mechanical Model Notes. Light and the Atomic Spectrum Light is composed of waves at different wavelengths The wave is composed.

Bellwork What is the majority of the volume of an atom?

Electromagnetic Spectrum. Copyright McGraw-Hill The Nature of Light The electromagnetic spectrum includes many different types of radiation. Visible.

1 CHAPTER 13: Electrons in the Atom. 2 Quantum Mechanical Model of the Atom and Ernest Schrodinger The model of the atom was developed based on the study.

Light and the Atom. Light Much of what we know about the atom has been learned through experiments with light; thus, you need to know some fundamental.

Electrons in Atoms The Development of a New Atomic Model.

Chapter 5: Electrons in Atoms

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.

Electrons and Light. Light’s relationship to matter Atoms can absorb energy, but they must eventually release it When atoms emit energy, it is released.

Development of a New Atomic Model Properties of Light.

CONTENT OBJECTIVE understand the electromagnetic spectrum and the mathematical relationships between energy, frequency, and wavelength of light. WHAT.

Chemistry – Chapter 4. Rutherford’s Atomic Model.

Section 5.1 Light and Quantized Energy. Objectives Compare the wave and particle models of light Compare the wave and particle models of light Define.

Electromagnetic Spectrum Chemistry 6(B). Lesson Objectives Explore the electromagnetic spectrum Understand the mathematical relationships between energy,

Section 1 The Development of a New Atomic Model Objectives Explain the mathematical relationship among the speed, wavelength, and frequency of electromagnetic.

Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.

Electrons in Atoms The Development of a New Atomic Model.

5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.

Electrons in Atoms Chapter 4.

I. Waves and Particles De Broglie’s Hypothesis

Electrons in Atoms Chapter 4.

Electromagnetic Spectrum

Light, Electromagnetic Spectrum, & Atomic Spectra

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.

Atomic Structure & Periodicity

Light’s Wave Nature.

Arrangement of electrons in atoms

Light and Quantized Energy

Section 5.1 Light and Quantized Energy

Light: Electromagnetic Spectrum

WAVES AND THE ELECTROMAGNETIC SPECTRUM

Light and the Atomic Spectra

Electromagnetic Radiation

Chapter 4 The Wave Description of Light

Chemistry 1 Chapter 5 Part I Light and Quantized Energy

Chemistry 1 Notes # 8 Light and Quantized Energy

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

Waves and Electromagnetic Radiation

Electromagnetic radiation

Light and the electron Quest continues to discover the structure of atom and how electrons are arranged within atoms.

Arrangement of Electrons in Atoms

Chemistry 1 Chapter 5 Part I Light and Quantized Energy

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

Electromagnetic Radiation

Arrangement of Electrons in Atoms

Light’s Wave Nature.

Quantum Theory.

Chapter 5 Electrons In Atoms 5.3 Atomic Emission Spectra

5.1 – ELECTRONS IN ATOMS.

Warm-up Example 3 from Practice Atomic Mass notes on pg 31!

Electromagnetic Spectrum

Chapter 4 Arrangement of Electrons in Atoms

Ch. 5 - Electrons in Atoms Waves & Particles.

Arrangement of Electrons

Presentation transcript:

Electrons and the Electromagnetic Spectrum

Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties of Light

**remember, all of these waves travel at the same speed…the speed of light!

Continuous and Line Spectra light Na H Ca Hg nm Visible spectrum  (nm)

Atoms emit energy on the EMR spectrum when their electrons relax to a ground state. We can calculate this energy, wavelength and frequency!!!! Atoms and EMR

Wavelength ( λ ) is the distance between wave peaks Frequency ( ν ) is the number of waves that pass in a second Frequency and wavelength are inversely proportional Properties of light, con’t

Wavelength and Frequency

Frequency and wavelength are mathematically related to each other: c = λν c = is the speed of light = 3.0 x 10 8 m/s λ = is the wavelength (in m) ν= is the frequency (in s −1 ).

**Remember c is a constant = 3.0 x 10 8 m/s 1. A wave has a frequency of 2 x Hz. What is the wavelength? Practice using the equation c = λν

2. A certain microwave has a wavelength of meters. Calculate the frequency of this microwave. Practice

A Quantum of energy is the minimum energy that can be lost or gained by an atom. E= h v E = energy in Joules h= planks constant, x J s v= frenquency Quantum Energy!

1.Determine the energy of a photon whose frequency is 3.55 x Hz. Practice

1. Determine the energy of a photon who’s frequency is 6.7 x 10 3 Hz 2. A radio wave has a frequency of 250,000 Hz. What is the wavelength of this radiowave? Mixed practice, determining which equation to use..