Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave...
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Transcript of Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave...
![Page 1: Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave zFrequency ( ) - # of waves that pass a point during a certain.](https://reader033.fdocuments.us/reader033/viewer/2022051516/56649f135503460f94c28026/html5/thumbnails/1.jpg)
Waves & Particles
Electrons in Atoms
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A. Waves
Wavelength () - length of one complete wave
Frequency () - # of waves that pass a point during a certain time period hertz (Hz) = 1/s
Amplitude (A) - distance from the origin to the trough or crest
![Page 3: Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave zFrequency ( ) - # of waves that pass a point during a certain.](https://reader033.fdocuments.us/reader033/viewer/2022051516/56649f135503460f94c28026/html5/thumbnails/3.jpg)
A. Waves
Agreater
amplitude(intensity)
greater frequency
(color)
crest
origin
trough
A
![Page 5: Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave zFrequency ( ) - # of waves that pass a point during a certain.](https://reader033.fdocuments.us/reader033/viewer/2022051516/56649f135503460f94c28026/html5/thumbnails/5.jpg)
B. EM Spectrum
LOW
ENERGY
HIGH
ENERGY
![Page 6: Waves & Particles Electrons in Atoms. A. Waves zWavelength ( ) - length of one complete wave zFrequency ( ) - # of waves that pass a point during a certain.](https://reader033.fdocuments.us/reader033/viewer/2022051516/56649f135503460f94c28026/html5/thumbnails/6.jpg)
B. EM Spectrum
LOW
ENERGY
HIGH
ENERGY
R O Y G. B I V
red orange yellow green blue indigo violet
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B. EM Spectrum
Frequency & wavelength are inversely proportional
c = c: speed of light (3.00 108 m/s): wavelength (m, nm, etc.): frequency (Hz)
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B. EM Spectrum
GIVEN:
= ? = 434 nm = 4.34 10-7 mc = 3.00 108 m/s
WORK: = c
= 3.00 108 m/s 4.34 10-7 m
= 6.91 1014 Hz
EX: Find the frequency of a photon with a wavelength of 434 nm.
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C. Quantum Theory
Planck (1900)
Observed - emission of light from hot objects
Concluded - energy is emitted in small, specific amounts (quanta)
Quantum - minimum amount of energy change
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C. Quantum Theory
Planck (1900)
vs.
Classical Theory Quantum Theory
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C. Quantum Theory
Einstein (1905)
Observed - photoelectric effect
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C. Quantum Theory
Einstein (1905)
Concluded - light has properties of both waves and particles
“wave-particle duality”
Photon - particle of light that carries a quantum of energy
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C. Quantum Theory
E: energy (J, joules)h: Planck’s constant (6.6262 10-34 J·s): frequency (Hz)
E = h
The energy of a photon is proportional to its frequency.
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C. Quantum Theory
GIVEN:
E = ? = 4.57 1014 Hzh = 6.6262 10-34 J·s
WORK:E = h
E = (6.6262 10-34 J·s)(4.57
1014 Hz)
E = 3.03 10-19 J
EX: Find the energy of a red photon with a frequency of 4.57 1014 Hz.