WWU -- Chemistry Chemistry 354 Organic Chemistry Laboratory I.
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Transcript of Chemistry
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Top of the wave to the origin lineCarries the energy – does not impact either frequency or wavelength
Chapter 6.1 - 6.4 Review
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Distance between 2 successive peaks of 2 waves Represented by the Greek letter (lambda)
Chapter 6.1 - 6.4 Review
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Number of complete waves passing a fixed point in a given time Represented by the Greek letter (nu)
Chapter 6.1 - 6.4 Review
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Radiant energy emitted across a wide variety of wavelengths
Chapter 6.1 - 6.4 Review
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3 x 108 m/s
Chapter 6.1 - 6.4 Review
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c = x
So c = wavelength times frequency
Chapter 6.1 - 6.4 Review
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Inverse relationship – As one variable increases, the other variable decreases
Chapter 6.1 - 6.4 Review
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Red at 750 nm
Chapter 6.1 - 6.4 Review
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Violet at 400 nm
Chapter 6.1 - 6.4 Review
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Gamma Rays
Chapter 6.1 - 6.4 Review
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Radio waves (specifically, AM radio)
Chapter 6.1 - 6.4 Review
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Gamma Rays – X Rays – Ultraviolet (UV) – Visible Light – Infrared (IR) –Microwaves – Radio Waves
Chapter 6.1 - 6.4 Review
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Gamma Rays – X Rays – Ultraviolet (UV) – Visible Light – Infrared (IR) –Microwaves – Radio Waves
Chapter 6.1 - 6.4 Review
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ROYGBIVRed – Orange – Yellow – Green – Blue – Indigo - Violet
Chapter 6.1 - 6.4 Review
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“Chunk” or fixed minimum amount of energy absorbed or emitted
Chapter 6.1 - 6.4 Review
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Chapter 6.1 - 6.4 Review
hchE
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Chapter 6.1 - 6.4 Review – Period 7
h = 6.6262 x 10-34 J∙s
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Light consist of quanta called photons that carries energy equal to h
Chapter 6.1 - 6.4 Review
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Sunlight striking a sheet of metal will knock off and move electrons, thereby causing an electric current
Chapter 6.1 - 6.4 Review
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Both electrons and photons sometimes act as if they are particles (mass) and sometimes act like they are waves (energy) – Dual wave/particle nature
Chapter 6.1 - 6.4 Review
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Radiation composed of only one wavelength
Chapter 6.1 - 6.4 Review
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A spectrum
Chapter 6.1 - 6.4 Review
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A spectrum of only certain wavelengths – not all of them
Chapter 6.1 - 6.4 Review
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Specific energy levels that electrons existed in
Chapter 6.1 - 6.4 Review
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When electrons are excited (added energy), jump into higher energy levels. When they moved back into lower energy levels - gave off light.
Chapter 6.1 - 6.4 Review
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No. They absorb and emit only a quantum (fixed amount) of energy.
Chapter 6.1 - 6.4 Review
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Chapter 6.1 - 6.4 Review
hEEE if
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Chapter 6.1 - 6.4 Review
2218 11
J 1018.2
if nn
hchE
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Absorbed
Chapter 6.1 - 6.4 Review
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Emitted
Chapter 6.1 - 6.4 Review
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Principal quantum number
Denotes energy level
Chapter 6.1 - 6.4 Review
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Ground State
Chapter 6.1 - 6.4 Review
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Excited State
Chapter 6.1 - 6.4 Review
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Chapter 6.1 - 6.4 Review
mv
hWhere v = velocity
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It is impossible to know the position, direction, and speed of an electron at any one point in time – can know two variables, but not the third
Chapter 6.1 - 6.4 Review