NOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!)

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NOTES: 5.3 Light and Atomic Spectra (more Quantum Mechanics!)

Light WAVE or PARTICLE?

Electromagnetic Radiation Electromagnetic radiation includes: -radio waves -microwaves -infrared waves -visible light -ultraviolet waves -x-rays -gamma rays

Electromagnetic Radiation according to the wave model, light consists of electromagnetic waves all EM waves travel in a vacuum at a speed of 3.0 x 10 8 m/s

Electromagnetic Radiation Electromagnetic radiation (radiant energy) is characterized by its: -WAVELENGTH (color): λ (Greek letter lambda) -FREQUENCY (energy): ν (Greek letter nu)

WAVES Wavelength = distance between successive crests measured in units of length (m, nm) Frequency = the # of crests passing a given point per second measured in # per sec, or s -1, or Hertz

NOTICE: as wavelength decreases, frequency (& therefore ENERGY) increases!

VISIBLE LIGHT: When sunlight or white light is passed through a prism, it gives the continuous spectrum observed in a rainbow. each color blends into the next in the order: red, orange, yellow, green, blue, indigo, violet RED LIGHT: longest wavelength, lowest freq. VIOLET LIGHT: shortest wavelength, highest freq.

Light and Electrons each element emits light when it is excited by an electric current passing through its gas or vapor the atoms first absorb energy, then lose the energy as they emit light passing light emission through a prism gives a unique atomic emission spectrum

Light and Electrons recall: white light gives a continuous spectrum atomic emission spectra: relatively few lines **this suggests the emission of very specific, exact frequencies of energy/light! each line corresponds to a specific amt. of energy being emitted!!

Bright Line Emission Spectrum The light emitted by an element when its electrons return to a lower energy state can be viewed as a bright line emission spectrum.

Light and Electrons the emission spectrum of each element is unique to that element emission spectra can be used to identify the components of an unknown compound **we can even discover the composition of far away stars by studying their emission spectra!! (stars are hot, glowing bodies of gases!) Wow Science is cool!

The Quantum Concept: according to classical physics, there is no limit to how small the energy gained or lost by an object can be so classical physics cannot explain emission spectra which only allows SOME amounts of energy, but not others enter: Max Planck! (1858-1947) he wondered, what if light energy consists of little packets of energy called QUANTA?

The Quantum Concept: Einstein added the proposal we can describe light as composed of particles, or PHOTONS. each photon of light has a particular amount or packet of energy (a quantum). the amt. of energy (frequency) possessed by a photon depends on the color (wavelength) of the light.

The Quantum Concept & the Photoelectric Effect: Photons light quanta or packets of energy Photons can be observed indirectly through photoelectric effect PHOTOELECTRIC EFFECT - metals eject electrons called photoelectrons when light shines on them

The Quantum Concept & the Photoelectric Effect: HOWEVER, not all colors / frequencies of light will work on all metals! (because only specific frequencies, quanta, may be absorbed) in what ways do we use the energy of light to generate electricity??? -cars with photoelectric cells; solar-powered calculators; etc.

What does this have to do with electron arrangement in atoms? When all electrons are in the lowest possible energy levels, an atom is said to be in its GROUND STATE. When an atom absorbs energy so that its electrons are boosted to higher energy levels, the atom is said to be in an EXCITED STATE.

Electron States Ground state lowest energy level or n = 1 Excited state energy level of n = 2, 3, 4. energy levels are quantized (only certain values of electron energy are possible). QUANTA of energy are absorbed and then released when electrons drop from an excited state to a lower energy state Only electrons in transition from high to low energy levels emit energy in the form of light

Bright Line Emission Spectrum The light emitted by an element when its electrons return to a lower energy state can be viewed as a bright line emission spectrum.

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