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Light Emission vs. Absorption Black body
Dual Nature of Light Wave Refraction Diffraction Particle Photoelectric effect
Line Emission Spectrum “Excited” atoms emit light
Line Emission Spectrum
Balmer series Rydberg equation Balmer Series
Atomic Spectra and Bohr 1. 1.Any orbit should be possible and so is any energy. 2.But a charged particle moving in an electric field should emit energy. Electron would eventually run out of energy
Bohr New theory : Quantum or Wave Mechanics e- can only exist in certain discrete orbits Stationary states e- is restricted to QUANTIZED energy states.
n= principal quantum number n is an integer n with the lowest possible energy is said to be in the ground state Electrons with higher energy than ground state are said to be in an excited state
Calculate the energies of n=1, n=2, and n=3 states of the hydrogen atom in J/atom. R = 1.097 x 10 7 m -1 h = 6.626 x 10 -34 J-s c = 2.998 x 10 8 m/s
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Aim: How can we explain energy transitions in an atom? Do Now: What were the limitations of the Rutherford model of the atom and how did the Bohr model.
The photoelectric effect and the photon theory of light
1 Light as a Particle The photoelectric effect. In 1888, Heinrich Hertz discovered that electrons could be ejected from a sample by shining light on it.
Honors Chemistry Section 4.1
Light as a Wave Waves are traveling disturbances that carry energy from one place to another The speed of a wave is calculated by using the equation: V.
1 Atomic Structure chapter 6 written by JoAnne L. Swanson University of Central Florida.
Objectives To understand how the emission spectrum of hydrogen demonstrates the quantized nature of energy To learn about Bohr’s model of the hydrogen.
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.
1 Light as a Particle In 1888, Heinrich Hertz discovered that electrons could be ejected from a sample by shining light on it. This is known as the photoelectric.
Quantum Model of the Atom l Bohr l de Broglie l Heisenberg l Schrödinger.
Lecture 15: Bohr Model of the Atom
Spectra of Atoms When an atom is excited, it emits light. But not in the continuous spectrum as blackbody radiation! The light is emitted at discrete wavelengths.
Quantum Physics. Black Body Radiation Intensity of blackbody radiation Classical Rayleigh-Jeans law for radiation emission Planck’s expression h =
THE BOHR MODEL OF THE ATOM October 23, The Bohr Model of Hydrogen Atom Light absorbed or emitted is from electrons moving between energy levels.
Quantum Mechanical Model
Lecture 2010/19/05. wavelength Amplitude Node Electromagnetic Radiation (Light as waves) Moving Waves.
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.
Wave-Particle Duality 1: The Beginnings of Quantum Mechanics.
Learning Target: Explain the electromagnetic spectrum. Learning Outcome: Be able to describe a wave in terms of frequency, wavelength, speed, and amplitude.
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