electron configuration radiant energy waves light travels as both waves and packets of energy. light...
TRANSCRIPT
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Electron Configuration
Radiant Energy
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Waves
• Light travels as both Waves and Packets of energy.
• Light is a form of Electromagnetic Radiation.– EM Radiation has
waves in the electric and magnetic fields
• All waves (Water or Electromagnetic) have 4 key characteristics:– Amplitude
– Wavelength
– Frequency
– Speed
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Wave Characteristics
• Amplitude.– Height of a wave from
origin to a peak/crest.
– Affects brightness and intensity.
• Wavelength.– Distance from crest to crest.
Distance for one full cycle.
– Visible light: 400-750nm.
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Wave Characteristics
• Frequency.– How fast a wave oscillates
(moves up and down).
– Units: s-1, 1/s or Hz.
• Speed.– Speed of light a constant:
3.00 X 108 m/s.
• Frequency and Wavelength related by the equation: = c /
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Try this…
If the frequency of a wave is 93.1 x 106 s-1, what is the wavelength?
Answer: 3.22 m
If the wavelength of a wave is 1.54 mm, what is it’s frequency?
Answer: 1.95 x 1011 Hz (s-1)
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Have a Problem?
Rearranging the equation:
• First, multiply by (frequency): = (c/)
• Now, divide by (wavelength):() / = c /
• Leaving: = c/Moving on….
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Electromagnetic Spectrum
• Many parts including:– Gamma Rays (10-11 m)
– X-Rays (10-9 m)
– Ultra-violet (10-8 m)
– Visible (10-7 m)
– Infared (10-6 m)
– Microwave (10-2 m)
– TV/Radio (10-1 m)
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Electromagnetic Spectrum
• Visible Spectrum:ROY G BIV
– Red
– Orange
– Yellow
– Green
– Blue
– Indigo
– Violet
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Electromagnetic Spectrum (once more)
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Electron Configuration
Quantum Theory
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Early Puzzlements
• Wave model for light was originally accepted by scientific community.
• This couldn’t explain why metals heating first emitted invisible radiation and then visible radiation.
• Other questions included why elements only emitted certain characteristic colors of light.
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Plank’s Theory
• Every object can only absorb or emit a fundamental amount of energy.
• This amount is called a quantum.
• The amount is like moving up or down steps.
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Plank’s Theory
• Plank’s Theory is based on the relationship between frequency and the energy of the particle.
• E = h• Plank’s Constant:
– h = 6.6262 X 10-34 J-s
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Quick Practice
If a wave has a frequency of 9.33x106 Hz, what is it’s energy?
6.18x10-27 J
What is the frequency of a wave if its energy is 4.32x10-31 J?
652 Hz
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Photoelectric Effect
• Einstein used Plank’s equation to explain a puzzling phenomenon, the Photoelectric Effect.– Electrons ejected from metal when light shines on it.
– Metal need’s certain frequency of light to release electrons. In Sodium, red light is no good, violet releases them off easily.
– Photons: Tiny particles of light providing energy to “knock off” electrons.
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Dual Nature of Radiant Energy
• Proven in 1923 by Arthur Compton– Showed photon could
collide with an electron like tiny balls.
• Summary:– Light behaves as a
wave ( = c/)– Light behaves as a
particle (E = h)
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Electron Configuration
Another Look at the Atom
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Line Spectra
• Def: A spectrum that contains only certain colors/wavelengths.
• AKA: The Atomic Emission Spectrum
• Each element has it’s own “fingerprint” emission spectrum.
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The Bohr Model
• Bohr drew the connection between Rutherford's model of the atom and Planks idea of quantization.
• Energy levels labeled with Quantum Numbers (n)
• Ground state, or lowest energy level – n=1
• Excited State – level of higher energy
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Matter Waves
• If energy has dual nature, why not matter?• De Broglie thought so.
– Matter Waves – the wavelike behavior of waves.
– Didn’t stand without experimental proof
• Davison and Germer proved this with experiments in 1927.
• Why don’t we see these matter waves? Mass must be very small to observe wavelength.
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Heisenberg Uncertainty
• Uncertainty Principle– The position and momentum of a moving
object cannot simultaneously be measured and known exactly.
• Translation:– Cannot know exactly where and how fast an
electron is moving at the same time.
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Electron Configurations
A New Approach to the Atom
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Quantum-mechanics Model
• Includes all the ideas of the atom we have covered:– Energy of electrons is quantized– Electrons exhibit wavelike behavior– Electrons position and momentum cannot be
simultaneously known– Model does describe the probable location of
electrons around the nucleus
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Probability and Orbitals
• Electron Density:– The density of an
electron cloud.
• Atomic Orbitals:– A region around the
nucleus of an atom where an electron with a given energy is likely to be found.
• Kinds of orbitals:– Each kind has own
different basic shape.– Given letter
designations of s, p, d and f.
– s-orbitals are spherical– p-orbitals are dumbbell– d- and f-orbitals more
complex.
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Orbitlas and Energy
• Principle energy levels (n) can be divided into sublevels.
• Number of sublevels is equal to the number of the principle energy level.
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Orbitals and Energy
• Each sublevel has one or more orbitals– s – one
– P – three
– d – five
– f – seven
• Summary provided in figure 4-28 (pg 145)
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Electron Spin
• Electrons have two spins:– Up or clockwise– Down or counterclockwise
• Only two electrons (one of each spin) can occupy an orbital. These electrons are said to be “paired”.
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Electron Configurations
Electron Configurations