Light

# Light - Wavelength Frequency Wavelength Frequency lambda...

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avelength & Frequency Wavelength & Frequency lambda λ distance between waves ll i t 1 t 10 usually in nanometers 1meter = 10 9 nm ν nu number of waves per second p λ * ν = c (speed of light = 3.0 x 10 8 m/s) 1

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lectromagnetic Spectrum Electromagnetic Spectrum rays 0 -14 γ rays 10 m X-rays 10 -10 m V 0 UV 10 -8 m Visible 4x10 -7 to 7 x 10 -7 m IR 10 -4 m Microwaves 10 -2 m Radio waves 10 2 to 10 8 m 2
Energy E = h ν or E = h c/ λ h = Plank’s constant = 6.626 x 10 -34 J*s Visible Light E = (6.626 x 10 -34 J*s)(3.0 x 10 8 m/s) 5 x 10 -7 m =4x10 -19 4 x 10 J 3

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Energy Gamma Ray = .626x10 -34 *s)(3.0 x 10 8 /s) E (6.626 x 10 J s)(3.0 x 10 m/s) 10 -16 m 2 x 10 - =2 x 10 9 J Radio Wave E = (6.626 x 10 -34 J*s)(3.0 x 10 8 m/s) 10 2 m =2 x 10 -27 J 4
hompson Model of the Atom Thompson Model of the Atom hompson had the “plum- udding model” for Thompson had the plum pudding model for atoms Electrons (plums) are in a pudding of positive charge. Rutherford’s experiment showed that the electron could not be a pudding. 5

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ohr Model of the Atom Bohr Model of the Atom hy do the atoms emit light only at specific Why do the atoms emit light only at specific wavelengths? Bohr came up with Quantum Mechanics & Nbl P i f h i i d won a Nobel Prize for his idea. Hydrogen- central proton with a single electron in orbit 6
Quantized Energy Bohr proposed that the electron could only ave certain definite energies have certain, definite energies, n n = 1,2,3,4 … ro nd state n 1 lo est energ state

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