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Electrons & Light

TermDefinition
wavelength decreases left to right, distance between 2 crests
energy increases left to right
frequency increases left to right, the number of waves that pass a particular point in an amount of time
frequency increases --> wavelength decreases
excited electrons emit light when they fall from higher energy levels to lower energy levels
ground state the lowest energy level possible for an electron
visible light can be seen by the eye
shortest wavelength violet light, x-rays, gamma rays
longest wavelength red light, AM radio waves
wavelength gets shorter--> frequency gets higher (inverse relationship)
the speed of light is the same for all colors of light
there are many... different shades of each color
most energy violet light
least energy red light
wavelength decreases --> energy increases (inverse relationship)
hydrogen emission spectra 4 colors - red, blue-green, blue-violet, violet, cannot produce more than one color at once since it only has one electron
boron emission spectra 5 colors - red, orange, blue-green, 2 blues, 3 violets
boron has different electrons than hydrogen, so different shades are created
smallest wavelength--> most energy
spectral lines are different for each element and identify what the element is, much like fingerprints
electrons and protons attract each other
as an electron gets closer to the nucleus, the attraction gets stronger
when an electron moves from an energy level close to the nucleus to one far from it the electron loses/absorbs energy & light
when an electron moves from an energy level far from the nucleus to one close to it the electron gains/releases energy & light
excited states higher energy levels
straight arrow in Bohr model represents amount of energy put in
hydrogen electron transition with the UV range (10-400 nm) 400 is smaller than violet 410 (smallest in hydrogen spectra), so smaller waves need to be produced which involves more energy, n=6-->n=1 (bigger arrow, more energy, shorter wavelength)
Created by: ts2819
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