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Wavelength, Frequency, and Energy Practice Problems
1. A certain violet light has a wavelength of 413 nm. What is the frequency of this light?
2. What is the wavelength of radiation whose frequency is 1.50 x 10 13 Hz?
3. How much energy is associated with a photon in the microwave region of the spectrum with a frequency of 6.6 x 10 12 Hz?
4. A hydrogen lamp emits several lines in the visible region of the spectrum. One of these lines has a wavelength of 6.56 x 10 -5 cm. What is the energy of this radiation?
5. A very bright line in the bright-line spectrum of sodium has a wavelength of 590 nm. What is the speed of this wave?
Things to remember… Calculating wavelength and frequency: C = λν where c = 3.00 x 10 8 m/s Energy per photon: E = hν where h = x J ∙s photon.
Electrons and the Electromagnetic Spectrum. Electromagnetic Radiation: energy that exhibits wavelike behavior and travels at the same speed Properties.
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5.3 Atomic Emission Spectra and the Quantum Mechanical Model 1 > Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 5.
12.6 Light and Atomic Spectra The quantum mechanical model of the atom grew out of the study of light. The quantum mechanical model of the atom grew out.
ELECTROMAGNETIC SPECTRA. c = λν E = hν E = mc 2 c = 3.00 x 10 8 m / sec h = x J sec Hz = 1 / sec HELPFUL EQUATIONS.
Light and the Electromagnetic Spectrum. Light Phenomenon Isaac Newton ( ) believed light consisted of particles. By 1900, most scientists believed.
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.
Electromagnetic Radiation The speed of electromagnetic radiation (speed of light) is constant at x 10 m/s – We’ll express it as 3x10 m/s – The symbol.
Chemistry Notes: Electromagnetic Radiation. Electromagnetic Radiation: is a form of energy that exhibits wavelike behavior as it travels through space.
Radiant Energy particles or waves of energy emitted Electromagnetic radiation – energy released from all objects Nuclear radiation – energy released.
Chapter 4 The Electromagnetic Spectrum Part 1. Demonstration Gas spectral tubes: NeonArgon.
Electromagnetic Spectrum The emission of light is fundamentally related to the behavior of electrons.
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4-1 Radiant Energy. Waves Light travels in Waves similar to ocean waves Light waves are electromagnetic and consist of an electric and magnetic fields.
Light, Photon Energies, and Atomic Spectra. Questions this answers… Why does FM sound better than AM radio waves? Why am I able to tune in to AM radio.
Wavelength, Frequency, and Planck’s Constant. Formulas 1)E = hf E = energy (Joules J) h = Planck’s constant = 6.63 x J x s f = frequency (Hz) 2)
Chemistry 5.3 “Physics and the Quantum Mechanical Model” Read pg. 138 p. 1.
Light, Photon Energies, and Atomic Spectra. Electrons and Waves Louis deBroglie proposed the dual nature of matter, which means that matter has matter-like.
Problems with Rutherford’s Model Why do elements produce spectral lines instead of a continuous spectrum? And Why aren’t the negative electrons pulled.
Modern Atomic Theory Ms. Hoang ACP Chemistry. Summary Visible light is a small section of the EM spectrum Light exhibits wave-like and particle-like.
Physics and the Quantum Mechanical Model Light and Atomic Spectra.
Waves & Particles Ch. 4 - Electrons in Atoms. Properties of Light Different types of electromagnetic radiation (x-rays, radio waves, microwaves, etc…)
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Chem-To-Go Lesson 7 Unit 2 ENERGY OF ELECTRONS. ENERGY BASICS All energy travels in the form of a wave. Scientists measure the wavelength of a wave to.
T HE QUANTUM MECHANICAL MODEL OF THE ATOM WAS DEVELOPED THROUGH THE STUDY OF LIGHT. I SAAC N EWTON ( )-L IGHT CONSISTS OF PARTICLES LIGHT.
ENERGY & LIGHT THE QUANTUM MECHANICAL MODEL. Atomic Models What was Rutherford’s model of the atom like? What is the significance of the proton? What.
Energy Levels & Photons Atomic & Nuclear Lesson 2.
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.
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.
The Wave Nature of Light Section 6.1. Objectives Study light (radiant energy or electromagnetic radiation) as having wavelike properties. Identify the.
Which of the following describes the dual nature of light? 1. Light has a frequency and a wavelength. 2. Light behaves as particle and as wave. 3. Light.
Electromagnetic Spectrum. Matter Review All matter is made of A______ Matter exists in different forms or phases. They are.
SPECTRUMSPECTRUMSPECTRUMSPECTRUM Electromagnetic Spectrum.
5.3 Physics and the Quantum Mechanical Model. Light By 1900 enough experimental evidence to convince scientists that light consists of waves.
Warm Up Write the correct answers for the following: 1) 2.00 x m = __________m 2) 1.23 x m = __________nm.
EMS (ELECTRO MAGNETIC SPECTRUM). WHAT TYPES OF RADIATION (WAVES) ARE NOT VISIBLE? CAN YOU RANK THEM IN ORDER OF ENERGY? (WHICH ARE MORE ENERGETIC)?
Peak Trough Amplitude Wavelength ( ) (in meters) Frequency measured in Hertz: (Hz): cycles per second.
Chemical Ideas 6.1 Light and the electron.. Sometimes we use the wave model for light … λ (lambda)= wavelength.
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Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11.
c = 13.A mercury vapor lamp emits radiation with a wavelength of 4.36 x m. a.Use the wave equation to determine the frequency. = c Knowns and unknown.
The Electromagnetic Spectrum A continuous range of oscillating electric and magnetic waves. The energy in an electromagnetic wave increases as the frequency.
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