Atomic Structure and Periodicity Electromagnetic Radiation The Nature of Matter The Atomic Spectrum...
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Atomic Structure and Periodicity
Electromagnetic RadiationThe Nature of Matter
The Atomic Spectrum of HydrogenThe Bohr Model
The Quantum Mechanical ModelQuantum Numbers
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Electromagnetic Electromagnetic SpectrumSpectrum
10-12 10-10 10-8
4x10-7 5x10-7 6x10-7 7x10-7
10-4 10-2 1021 104
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Electromagnetic Electromagnetic RadiationRadiation
Gamma
X rays
Ultraviolet
Visible (400-700nm)
Infrared
Microwaves
Radio waves
Power waves
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Electromagnetic Electromagnetic RadiationRadiation
Three primary characteristics Wavelength (…lambda) Frequency (…nu) Speed (c)
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WavelengthWavelength Distance between two consecutive crests
or troughs of a wave
Measured in m or nm, typically
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FrequencyFrequency
Number of wave cycles per second that pass a given point in space
Cycle is understood in SI language
Measured in 1/s or s-1, also known as a hertz (Hz)
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SpeedSpeed Constant, known as the speed of light
2.9979 x 108m/s
Since the speed of a wave is constant, then frequency and wavelength must vary inversely
c =
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Problem #1Problem #1
A wave is known to have a frequency of 5.09 x 1014Hz. What is its wavelength and what type of electromagnetic radiation is it?
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Electromagnetic Electromagnetic SpectrumSpectrum
10-12 10-10 10-8
4x10-7 5x10-7 6x10-7 7x10-7
10-4 10-2 1021 104
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Problem #1Problem #1
5.89 x 10-7 mVisibleYellow-orange
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The Nature of MatterThe Nature of Matter
Matter and energy (in the form of light) were thought to be distinct until 1900 Matter was made of particles that had
mass, took up space, and could absorb or emit any quantity of energy
Light was made of waves that were massless and of unknown location (delocalized)
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Max Planck (1858-1947)Max Planck (1858-1947) German physicist
Observed that heated solid bodies emitted energy only in specific whole-number multiples
They were multiples of the quantity “h”
h is known as Planck’s constant and has a value of 6.626 x 10-34J•s
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Max Planck (1858-1947)Max Planck (1858-1947) Thus, the change in
internal energy of a system is represented by E = h
“h” came to be known as a quantum
Proved that energy is indeed quantized not continuous
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Problem #2Problem #2
Cuprous ions will emit 4.41 x 10-19J when heated to approximately 1200C. What is the wavelength of the light emitted and what color is it?
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Electromagnetic Electromagnetic SpectrumSpectrum
10-12 10-10 10-8
4x10-7 5x10-7 6x10-7 7x10-7
10-4 10-2 1021 104
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Problem #2Problem #2
4.50 x 10-7 mblue-green
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Albert EinsteinAlbert Einstein Proposed the
electromagnetic radiation may be viewed as a stream of particles, known as “photons”
Said that the energy of a photon equaled the change in internal energy that a system experienced
Ephoton= h = hc/
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Albert EinsteinAlbert Einstein In 1905, he proposed that
energy has mass and put forth the famed equation
E = mc2 or m = E/c2
Thus,
m = E = hc/ = h c2 c2 c
Established the phrase “dual nature of light”
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Prince Louis-Victor Pierre Prince Louis-Victor Pierre Raymond de BroglieRaymond de Broglie
Proved that the opposite of the dual nature of light was true
Showed that particles also exhibited wave properties
de Broglie’s equation replaces the speed of light with the speed of the particle
m = h or = h v mv
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Problem #3Problem #3 Compare the wavelength of an electron
with a mass of 9.11 x 10-31 kg traveling at a speed of1.00 x 107 m/s with that of a tennis ball with amass of 0.0089kg traveling at 42.5 m/s.
Electron—7.27 x 10-11 mTennis ball—1.75 x10-33 m
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DiffractionDiffraction Scattering of light from a regular array of
points or lines..make a diffraction pattern
Proves the wave properties of particulate matter
Pattern results from constructive interference Light spots
And destructive interference Dark spots
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MatterMatter Exhibits particulate and wave properties
Big bits have tiny wavelengths and have more particulate properties
Itty-bitty bits have larger wavelengths and behave more like waves than particles
Medium bits have fairly equal representation of particles and waves
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Atomic Spectrum of Atomic Spectrum of HydrogenHydrogen
When H atoms are excited, they emit the excess energy according to the electromagnetic spectrum
This is known as an emission spectrum
It is not continuous as white light through a prism is
Rather, it is known as a line spectrum
Verifies quantization of energy emission
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Line Spectrum of Line Spectrum of HydrogenHydrogen
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The Bohr ModelThe Bohr Model developed in 1913 by Danish
physicist, Niels Bohr
Proposed that the electron in H moves in particular circular orbits
Agreed with the emission spectrum of hydrogen assuming the angular momentum of the electron occurred in specific increments
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The Bohr ModelThe Bohr Model provides the equation that
gives the energy levels available in hydrogen
E = -2.178 x 10-18 J(Z2/n2) n represents the integer
indicating the distance from the nucleus (will eventually be shown to be the energy level)
Z represents the nuclear charge which is +1 for hydrogen
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The Bohr ModelThe Bohr Model If a hydrogen electron is
excited to a higher energy level and then falls back down to the 1st energy level (the ground state), then the associated energy change can be determined.
E = Ef – Ei
E = -2.178 x 10-18 J(1/nf2 – 1/ni
2)
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Problem #4Problem #4 Determine the wavelength of light emitted
when a hydrogen electron falls from the 6th energy level to the 1st energy level. What type of electromagnetic radiation is this?
9.38 x 10-8 multraviolet
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The Quantum Mechanical The Quantum Mechanical ModelModel
Begun by de Broglie
Remember the dual nature of light and the idea that all matter traveled in waves and as particles?
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The Quantum Mechanical The Quantum Mechanical ModelModel
Erwin Schrödinger (1887-1961)
Austrian physicist
Treated electron pathways as standing waves
Designated wave functions (functions of x, y, and z coordinates) that we peons tend to call orbitals
Proved orbitals are not circular
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Werner Heisenberg (1901-1976)
German physicist
“We cannot always assign to an electron a position in space at a given time, nor follow it in its orbit, so that we cannot assume that the planetary orbits postulated by Niels Bohr actually exist. Mechanical quantities,
The Quantum Mechanical The Quantum Mechanical ModelModel
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such as position, velocity, etc. should be represented, not by ordinary numbers, but by abstract mathematical structures called matrices.“
Proposed the above postulate at the age of 23!!
Later came up with his famed Uncertainty Theory
The Quantum Mechanical The Quantum Mechanical ModelModel
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Heisenberg’s Uncertainty Heisenberg’s Uncertainty PrinciplePrinciple
There is a fundamental limitation to just how precisely we can know both the position and momentum of a particle at a given time.
x • (mv) > h/4 x is the uncertainty in position (mv) is the uncertainty in
momentum h is Planck’s constant
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ProbabilityProbability
Shown is that of the hydrogen 1s orbital
Distribution graph shows adarker image where an electron tends to be found morefrequently
Approximately 90% of the time, the electron may be found in this sphere
Also called an electron density map
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Electron Electron ConfigurationsConfigurations
Energy level
Sublevel
s
p
d
f
# electrons
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Electron Electron ConfigurationsConfigurations
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Electron Electron ConfigurationsConfigurations
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Electron Electron ConfigurationsConfigurations
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Orbital DiagramsOrbital Diagrams
E
1s
2s
2px 2py 2pz
3px 3py 3pz
3s
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Orbital DiagramsOrbital Diagrams
E
1s
2s
2px 2py 2pz
3px 3py 3pz
3s
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Orbital DiagramsOrbital Diagrams
E
1s
2s
2px 2py 2pz
3px 3py 3pz
3s
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