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Summary
Visible light is a small section of the EM spectrum
Light exhibits wave-like and particle-like properties
To characterize wave, scientists use wavelength, frequency, speed (and amplitude)
Short wavelength = (high/low) frequency = (high/low) energy
Long wavelength = (high/low) frequency = (high/low) energy
Wavelength determines color of light
White light is light of all wavelengths
Objects around us absorb visible light of different wavelengths and emit light of different wavelengths. That is why objects appear to have colors.
Concept Check-in
What color is a banana under white light?
Yellow
What color is a banana under green light?
Black
Objectives
Use light and wave formulae to calculate wavelength and frequency of light
Contrast continuous spectra with line spectra
Explain why the emission spectra of elements are line spectra rather than continuous spectra
Example
A photon has an energy of 4.00 x 10-19J.
Find the frequency of the radiation
Find the wavelength of the radiation
Find the color of the photon if possible
E = 4.00 x 10-19J = (6.626 x 10-34J.s)(ν)
ν = E/h =
cሺm sΤሻ= λሺmሻ× ν(s−1)
4.96×10− 7𝑚=496×10−9𝑚=496𝑛𝑚→𝐵𝐿𝑈𝐸
𝐸=h ν
Your turn
A photon has an energy of 3.00 x 10-19J.
Find the frequency of the radiation
Find the wavelength of the radiation
Find the color of the photon if possible
Your turn
A bright line spectrum contains a line with a wavelength of 518 nm.
The color of the line is:
A. Violet
B. Green
C. Yellow
E. Red
The energy is:
A. 5.12 x 10-23 J
B. 3.84 x 1019 J
C. 5.12 x 1023 J
D. 3.84 x 10-19 J
Types of spectra
_______ light = contains light of all wavelengths __________
Light from an excited element (electrical current) = contains light of _______ wavelengths _____________
Question: Why do atoms emit line spectra?
Bohr Model of the Atom
Electrons go in orbits around the nucleus like the solar system
Each orbit is a discrete
Only works for Hydrogen atom