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Formation of Light
Nucleus
e e
e
Lithium Atom
+
Ground State
e e e e e e
e
Excited State
e
Electron Returns to Ground State
Light is given offe
Ion is formedLi e + Li1+
hv
n = 1
n = 2
n = 3
n = 4
n = 5
n = 6
n = 7
Nucleus Nucleus Nucleus
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
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
f
The Electromagnetic Spectrum
AM radio
Short waveradio
Television channels
FM radio
RadarMicrowave
Radio Waves Gamma Rays
X- Raysinfrared
Increasing photon energy
Increasing frequency
Decreasing wavelength
Red Orange Yellow Green Blue Indigo Violet
UV Rays
Visible
Light
R O Y G B I V
HIGH
ENERGY
LOW
ENERGY
Frequency
O’Connor, Davis, MacNab, McClellan, CHEMISTRY Experiments and Principles 1982, page 166
1 second
Frequency
4 cycles/second = 4 hertz
12 cycles/second = 12 hertz
36 cycles/second = 36 hertz
AM & FM WavesCarrier frequency
Sound pattern
Amplitude Modulated carrier
Frequency Modulated carrier
AM - FM Radio
Electromagnetic Spectrum
LOW
ENERGY
HIGH
ENERGY
g rays X-rays Ultraviolet Infrared Microwave
Radar
Radio waves
TVFM
ShortWave
LongWave
Visible spectrum
10-2nm 10-1nm 100nm 101nm 102nm 10-3cm 10-2cm 10-1cm 100cm 101cm 1cm 101m 102m 103m 104m
1019Hz 1018Hz 1017Hz 1016Hz 1014Hz 1013Hz 1012Hz 1011Hz 1010Hz 109Hz 100 MHz 10 MHz 1 MHz 100 KHz
RedOrangeYellowViolet Blue Green
700 nm600 nm500 nm400 nm
Wavelength, l
Frequency, n
103nm
1015Hz
Electromagnetic spectrum
WhiteLight
Davis, Frey, Sarquis, Sarquis, Modern Chemistry 2006, page 98
Waves
Low frequency
High frequency
Amplitude
Amplitude
long wavelength l
short wavelength l
Waves
Low frequency
High frequency
Amplitude
Amplitude
long wavelength l
short wavelength l
60 photons
162 photons
low energy
high energy
Electromagnetic Radiation
Light as a wave
Light as a stream of energy
(packets of photons)Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 325
Wavelength and Frequency
E = h n
c = n l c = speed of light (3 x 108 m/s)n = frequency (s-1) l = wavelength (m)
E = energy (Joules or J)h = Planck’s constant (6.6 x10-34 J/s)n = frequency (s-1)
f f
ff
ch
E
“nu” “lambda”
c f
Electromagnetic Spectrum
GIVEN:
f = ?
= 434 nm
= 4.34 10-7 m
c = 3.00 108 m/s
WORK:
f = 3.00 108 m/s 4.34 10-7 m
f = 6.91 1014 Hz
• EX: Find the frequency of a photon with a wavelength of 434 nm.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
f c
1 x 109 nm
1 m
Coins are Quantified
Do we have a coin for 37cents?
Light is also quantified and only comes in certain bundles called photons.
Bohr Model of Hydrogen
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 331
Nucleus
Possible electron orbits
e
e
Continuous vs. Quantized Energy
Ene
rgy
A BZumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 330
continuous quantized
Continuous vs. Quantized
A BZumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 330
Wavelength and Frequency
E = h n
c = n l c = speed of light (3 x 108 m/s)n = frequency (s-1) l = wavelength (m)
E = energy (Joules or J)h = Planck’s constant (6.6 x10-34 J/s)n = frequency (s-1)
f f
ff
ch
E
“nu” “lambda”
Photoelectric Effect
No electrons are emitted Electrons are emitted
Metal plate Metal plate
Bright red light
infrared rays
or
Dimblue light
ultraviolet rays
or
Intensity of Radiation
1x 2x 3x
¼ light 1/9 light
Light intensity = 1/(distance)2
The Photoelectric Effect
When light strikes a metal surface,electrons are ejected.
If the threshold frequency has beenreached, increasing the intensity onlyincreases the number of electrons ejected.
If the frequency is increased, theEjected electrons will travel faster.
A B C
Light
Electron
MetalNucleus
More Light
Electron
MetalNucleus
Electron
HigherfrequencylightFaster
electron
MetalNucleus
Photoelectric Effect
Some key results
For low frequency light (low energy, below threshold) - electrons are not ejected regardless of the light’s intensity (number of light waves)
For high frequency light (high energy, above threshold) - same number of electrons are ejected regardless of the frequency (energy of light waves)
- Increasing the light’s intensity increases the number of electrons ejected (increases the current)
Einstein considered light as mass-less, energetic particles (photons)to help explain this effect – energy follows Planck’s equation.
Photoelectric Generator
Solar Calculator
The Photoelectric effect and the frequency of light
IR, infraredRedOrangeYellowGreenBlueVioletUV, ultraviolet
UV v b g y o r IR
Lens
Slit
Quartz prism
Light source
Hill, Petrucci, General Chemistry An Integrated Approach 1999, page 292
Potassium
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.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
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
• Example: Find the energy of a red photon with a frequency of 4.57 1014 Hz.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Color = Energy of Photons
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 329
Energy Level
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 329
A
B
C
D
Ground state
En
erg
y
Fourexcitedstates
An Excited Lithium Atom
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 326
Photon ofred lightemitted
Li atom inlower energy state
Excited Li atom
Ene
rgy
Frequency A
Frequency B
Frequency C
n = 2
n = 1
n = 3
A
B
C
A + B = C
Bohr’s Experiment
Kelter, Carr, Scott, Chemistry A Wolrd of Choices 1999, page 76 Animation by Raymond Chang – All rights reserved.
Hydrogen Spectral Lines
Lyman series(ultraviolet)
Balmer series(visible)
Paschen series(infrared)
Frequency(hertz)
1016 1015 1014
7 6 5 4 3 2 1 n =
Hydrogen Spectral Lines
A B C D E F
Lyman series (UV)
A B C D E
Balmer (Visible)
A B C D
Paschen (IR)
E1
E2
E3
E4
E5
E6
En
erg
y
Bohr’s model of the atom accounted mathematically for the energy of each of the transitions shown.
IRregion
UVregion
656 nm
486 nm
434 nm
410 nm
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 97
ionization
Continuous and Line Spectra
4000 Ao
5000 6000 7000
light
Na
H
Ca
Hg
400 450 500 550 600 650 700 750 nm
Visiblespectrum
l (nm)
Flame Emission Spectra
Photographs of flame tests of burning wooden splints soaked in different salts.
Include link to web page
http://www.unit5.org/christjs/flame%20tests.htm
methane gas wooden splint strontium ioncopper ionsodium ion calcium ion
The Electromagnetic Spectrum
AM radio
Short waveradio
Television channels
FM radio
RadarMicrowave
Radio Waves Gamma Rays
X- Raysinfrared
Increasing photon energy
Increasing frequency
Decreasing wavelength
Red Orange Yellow Green Blue Indigo Violet
UV Rays
R O Y G B I V
Visible
Light
1.5
1.2
0.9
0.6
0.3
0.0300 400 500 600 700 800
Wavelength (nm)
Abs
orb
ance
Absorbance of Chlorophyll
1026 1024 1022 1020 1018 1016 1014 1010 108 106 104 102 1
10-8 10-6 10-4 10-2 1 102 104 106 108 1010 1012 1014 1016
Frequency (Hz)
Wavelength (nm)
cosmicrays
gammarays
x-rays ultra-violet
infra-red
radio(microwave)
radar tele-vision
radio powertransmission
Violet Blue Green Yellow Orange RedUV
NearInfrared
400 nm 500 nm 600 nm 700 nm
Wave Interference
Wave Interference
Bright
Bright
Bright
Bright
Bright
Bright
Bright
A
B
C
D
Waves
crest
trough
wavelength
amplitude
E F G Hreflection refraction total internal reflection diffraction
crest
wavelength
amplitude
troughreflection
refractiondiffraction
total internal reflection(Match the terms…)
Polarizing Filter
Vertical polarizing filter
Horizontal polarizing filter
Vertical wavepasses through
Horizontal waveis blocked
side view
Vertical wave is blocked
by horizontal polarizing filter