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Transcript of Wavelength Visible light wavelength Ultraviolet radiation Amplitude Node Chapter 6: Electromagnetic...
wavelength Visible light
wavelength
Ultraviolet radiation
Amplitude
Node
Chapter 6: Electromagnetic Radiation
Figure 7.1Figure 7.1
Long wavelength --> small frequency
low energy
Short wavelength --> high frequency
high energy
Which has the longest wavelength?
1 2 3 4
25% 25%25%25%1. Infrared
2. Ultraviolet
3. X-rays
4. Radio waves
Rank the following in order of increasing frequency:
microwaves
radiowaves
X-rays
blue light
red light
UV light
IR light
• Waves have a frequency• Use the Greek letter “nu”, , for frequency,
and units are “cycles per sec”• All radiation: • = c • c = velocity of light = 3.00 x 108 m/sec• Long wavelength --> small frequency• Short wavelength --> high frequency
What is the wavelength of WONY?
What is the wavelength of cell phone radiation? Frequency = 850 MHz
What is the wavelength of a microwave oven? Frequency = 2.45 GHz
Energy of radiation is proportional to frequencyEnergy of radiation is proportional to frequency
h = Planck’s constant = 6.6262 x 10h = Planck’s constant = 6.6262 x 10-34-34 J•s J•s
Light acts as if it consists of particles called PHOTONS, with discrete energy.
E = h •
Quantization of Energy
Relationships:
E = h •
Short wavelength light has:
1 2 3 4
25% 25%25%25%1. High frequency and low energy
2. High frequency and high energy
3. Low frequency and low energy
4. Low frequency and high energy
Rank the following in order of increasing photon energy:
microwavesradiowavesX-raysblue lightred lightUV lightIR light
E = h •
What is the energy of a WONY photon?What is the energy of a WONY photon?
Energy of RadiationWhat is the frequency of UV light with a What is the frequency of UV light with a
wavelength of 230 nm?wavelength of 230 nm?
What is the energy of 1 photon of UV light What is the energy of 1 photon of UV light with wavelength = 230 nm?with wavelength = 230 nm?
What is the energy of a photon of 525 nm light?
1 2 3 4
25% 25%25%25%1. 3.79 x 10-19 J
2. 4.83 x 10-22 J
3. 3.67 x 1020 J
4. 8.43 x 1023 J
What is the energy of a mole of 230 nm photons?What is the energy of a mole of 230 nm photons?
Can this light break C-C bonds with an energy Can this light break C-C bonds with an energy of 346 kJ/mol?of 346 kJ/mol?
Does 1200 nm light have enough energy to Does 1200 nm light have enough energy to break C-C bonds?break C-C bonds?
Where does light come from?
• Excited solids emit a continuous spectrum of light
• Excited gas-phase atoms emit only specific wavelengths of light (“lines”)
Light emitted by solids
Light emitted by hydrogen gas
The Bohr Model of Hydrogen Atom
• Light absorbed or emitted is from electrons moving between energy levels
• Only certain energies are observed• Therefore, only certain energy levels exist
– This is the Quanitization of energy levels
• Excited atoms emit light of only certain wavelengths
• The wavelengths of emitted light depend on the element.
Emission spectra of gaseous atoms
Line spectra of atoms
Energy Absorption and Emissionsim
For H, the energy levels correspond to:
18
n 2
2.18 x 10 JE =
n
Energy level diagram:
Each line corresponds to a transition:
Example: n=3 n = 2
Balmer seriesBalmer series
Explanation of line spectra
Longest wavelength emission?
A. 1
B. 2
C. 3
D. 4
E. 5
1 2 3 4 5
20% 20% 20%20%20%
Longest wavelength absorption?
A. 1
B. 2
C. 3
D. 4
E. 5
1 2 3 4 5
20% 20% 20%20%20%
Lowest energy emission?
A. 1
B. 2
C. 3
D. 4
E. 5
1 2 3 4 5
20% 20% 20%20%20%
Lowest energy absorption?
A. 1
B. 2
C. 3
D. 4
E. 5
1 2 3 4 5
20% 20% 20%20%20%
Ionization?
A. 1
B. 2
C. 3
D. 4
E. 5
1 2 3 4 5
20% 20% 20%20%20%
Matter Waves
• All matter acts as particles and as waves.• Macroscopic objects have tiny waves- not
observed.• For electrons in atoms, wave properties are
important.
• deBroglie Equation: h
mv
Can see matter waves in experiments
Matter waves
Macroscopic object: 200 g rock travelling at 20 m/s has a wavelength:
Electron inside an atom, moving at 40% of the speed of light:
Heisenberg Uncertainty Principle
• Can’t know both the exact location and energy of a particle
• So, for electrons, we DO know the energy well, so we don’t know the location well
Schrodinger’s Model of H
• Electrons act as standing waves• Certain wave functions are “allowed”• Wave behavior is described by wave
functions: 2 describes the probability of finding the
electron in a certain spot– Also described as electron density
Hydrogen Wave Functions
Example Wavefunction
Equation slightly simplified:
o-r/a2 2 = x e g
Where is this function zero or near zero?
1 2 3
33% 33%33%1. When x = 0
2. When r = 0
3. When r is large
o-r/a2 2 = x e
It’s all about orbitals
• Each wavefunction describes a shape the electron can take, called an ORBITAL
• Allowed orbitals are organized by shells and subshells– Shells define size and energy (n = 1, 2, 3, …)– Subshells define shape (s, p, d, f, …)
• Number of orbitals is different for each subshell: s = 1 orbital
p = 3 orbitals d = 5 orbitals f = 7 orbitals
NODES
Spherical Nodes
Quantum Numbers and Numbers of Orbitals