the electron: wave – particle duality
DESCRIPTION
“No familiar conceptions can be woven around the electron. Something unknown is doing we don’t know what.” -Sir Arthur Eddington The Nature of the Physical World (1934). The ELECTRON: Wave – Particle Duality. The Dilemma of the Atom. - PowerPoint PPT PresentationTRANSCRIPT
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“No familiar conceptions can be woven around the electron. Something unknown is doing we don’t know what.”
-Sir Arthur EddingtonThe Nature of the Physical World (1934)
The ELECTRON:Wave – Particle
Duality
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The Dilemma of the Atom
• Electrons outside the nucleus are attracted to the protons in the nucleus
• Charged particles moving in curved paths lose energy
• What keeps the atom from collapsing?
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Wave-Particle DualityJJ Thomson won the Nobel prize for describing the electron as a particle.
His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.
The electron
is a particle!
The electron is an energy
wave!
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The Wave-like Electron
Louis deBroglie
The electron propagates through space as an
energy wave. To understand the atom, one must understand
the behavior of electromagnetic waves.
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c = fc = speed of light, a constant (3.00 x 108 m/s)
f = frequency, in units of hertz (hz, sec-1) = wavelength, in meters
Electromagnetic radiation propagates through space as a wave moving at the speed of light.
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E = hf
E = Energy, in units of Joules (kg·m2/s2)
h = Planck’s constant (6.626 x 10-34 J·s)
f = frequency, in units of hertz (hz, sec-1)
The energy (E ) of electromagnetic radiation is directly proportional to the frequency () of the radiation.
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Long Wavelength
=Low Frequency
=Low ENERGY
Short Wavelength
=High
Frequency=
High ENERGY
Wavelength Table
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Answering the Dilemma of the Atom
• Treat electrons as waves• As the electron moves toward the
nucleus, the wavelength shortens• Shorter wavelength = higher
energy• Higher energy = greater distance
from the nucleus
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The Electromagnetic Spectrum
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This produces bandsof light with definite wavelengths.
Electron transitionsinvolve jumps of
definite amounts ofenergy.
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…produces a “bright line” spectrum
Spectroscopic analysis of the hydrogen spectrum…
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Flame Tests
strontium sodium lithium potassium copper
Many elements give off characteristic light which can be used to help identify them.
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Electron Orbitals
Cartoon courtesy of lab-initio.com
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The Bohr Model of the Atom
Neils Bohr
I pictured electrons orbiting the nucleus much like planets orbiting the sun.
But I was wrong! They’re more like bees around a hive.
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Quantum MechanicalModel of the Atom
Mathematical laws can identify the regions outside of the nucleus where electrons are most likely to be found.
These laws are beyond the scope of this class…
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Heisenberg Uncertainty Principle
You can find out where the electron is, but not where it is going.
OR…
You can find out where the electron is going, but not where it is!
“One cannot simultaneously determine both the position and momentum of an electron.”
WernerHeisenberg
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Electron Energy Level (Shell)
Generally symbolized by n, it denotes the probable distance of the electron from the nucleus. “n” is also known as the Principle Quantum numberNumber of electrons that can fit in a shell:2n2
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Orbital shapes are defined as the surface that contains 90% of the total electron probability.
An orbital is a region within an energy level where there is a probability of finding an electron.
Electron Orbitals
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The s orbital has a spherical shape centered aroundthe origin of the three axes in space.
s Orbital shape
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Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”…and a “dumbell with a donut”!
d orbital shapes
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There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.
p orbital shape
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Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”…and a “dumbell with a donut”!
d orbital shapes
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Shape of f orbitals
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Energy
Level (n)
Orbital type in the
energy level (types = n)
Number oforbitals
Number ofElectrons
Number ofelectrons
perEnergy
level (2n2)
1 s 1 2 2
2 sp
13
26
8
3 spd
135
26
10
18
4 spdf
1357
26
1014
32
Energy Levels, Orbitals, Electrons
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Orbital filling table
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Electron SpinElectron spin describes the behavior (direction of spin) of an electron within a magnetic field.
Possibilities for electron spin:
1
2
1
2
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Electron SpinElectron spin describes the behavior (direction of spin) of an electron within a magnetic field.
Possibilities for electron spin:
1
2
1
2
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Pauli Exclusion Principle
Two electrons occupying the same orbital must have opposite spins
Wolfgang Pauli
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Electron configuration of the elements of the first three
series
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Element Configuration notation
Orbital notation Noble gas notation
Lithium 1s22s1 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s1
Beryllium 1s22s2 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2
Boron 1s22s22p1 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2p1
Carbon 1s22s22p2 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2p2
Nitrogen 1s22s22p3 ____ ____ ____ ____ ____
1s 2s 2p
[He]2s2p3
Oxygen 1s22s22p4 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2p4
Fluorine 1s22s22p5 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2p5
Neon 1s22s22p6 ____ ____ ____ ____ ____ 1s 2s 2p
[He]2s2p6
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