Light and Quantized Energy

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Section 1: Light and Quantized Energy
Section 1: Light and Quantized Energy
Presentation transcript:

Light and Quantized Energy

Electromagnetic Radiation Electromagnetic radiation: A form of energy that exhibits wavelike behavior as it travels through space Light: a form of electromagnetic radiation

What are some examples of electromagnetic radiation? What else?

Electromagnetic Radiation Waves have a frequency Use the Greek letter “nu”, , for frequency, and units are “cycles per sec”  stand for wavelength – it’s the shortest distance between equivalent points on a continuous wave All radiation: c =  •  where c = velocity of light = 3.00 x 108 m/sec

Electromagnetic Radiation wavelength Visible light Ultaviolet radiation Amplitude Node Crest

Electromagnetic Spectrum In increasing energy, ROY G BIV

Electromagnetic Spectrum Long wavelength --> small frequency Short wavelength --> high frequency increasing frequency increasing wavelength

Practice Problems What is the frequency of green light, which has a wavelength of 4.90 x 10-7m? What is the speed of an electromagnetic wave that has a frequency of 7.8 x 106 Hz?

Quantum Concept 1900 German physicist Max Planck started to search for WHY light emitted from heated objects. Found that QUANTUM is the minimum amount of energy that can be gained or lost by an atom Matter can gain or lose energy in small specific amounts called quanta

Quantum Concept Planck showed mathematically that the energy of a quantum is related to the frequency of the emitted radiation. Equantum = hn E = energy h = Planck’s constant = 6.626 x 10-34 J·s n = frequency

Photoelectric Concept Photoelectric effect: photons are emitted from a metal’s surface when light of a certain frequency shines on a surface Albert Einstein proposed that electromagnetic radiation has both wavelike and particlelike natures. He calculated that the photon energy was: Ephoton = hn

Electromagnetic radiation.

“Ground State” – lowest energy state “Excited State” – Electrons jump to higher energy levels due to an input of energy Absorption – amount of E absorbed to “boost” e- to higher E level (excited state) Emission – e- releasing E when “falling” back to lower E level (ground state)

Bohr model Studying H atom emission spectrum lead to Bohr’s model – electrons are restricted to certain orbits corresponding to E levels Rutherford never explained how e- fill space surrounding the nucleus

Practice Problems What is the energy for each of the following types of radiation? a. 6.32 x 1020 s-1 b. 9.50 x 1013 Hz c. 1.05 x 1016 s-1

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