Transcript Quantum Theory

Quantum Theory
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Schroedinger’s Cat
Place a cat in a box
Also place a radioactive
isotope and a vial of poison
The isotope decays once per
hour
If the particle triggers a
Geiger counter, the cat dies
If the Geiger counter is not
triggered, the cat lives
Seal the box and wait an hour
What happened to the cat?
Electromagnetic Spectrum
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The speed of light©
is 3.00 x 108 m/s
Photoelectric Effect
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The emission of _________
from a metal when
______________ on the
metal
Light had to be a certain
______________ ____for
electrons to be emitted
Wave theory of light said that
_____________ of light
should have worked
This led to the concept of
light as a ___________
Light as a particle
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Max Planck (1900)
Hot objects emit light and
other forms of
electromagnetic radiation,
but not continuously, as
expected
Instead, it is emitted in small,
specific amounts called
quanta.
E=hv
H=6.626 x 10 -34 J*s
This number is called
Planck’s constant
Dual Nature of Light
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Albert Einstein (1905)
Light behaves as a ________ when
it travels through space
Light behaves as a _________
when interacting with matter
Even though it isn’t quite right to
do so, you can think of light as a
__________________ that travels
as a wave
A _________ is a massless bundle
of light
E photon=hv
Some metals hold electrons more
tightly than others and require
____________________ to move
electrons
Emission Spectra
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Ground State
___________ energy state of an
electron
Excited State
___________ energy state
Energy is absorbed to move from
___________ ___________ states and
is released as ___________
___________ when returning to the
ground state
___________ ___________ of light
are emitted for any given element
___________ spectrum___________ range of em
light(rainbow)
(Bright) Line emission spectrum-Only
___________ ___________ of light
are seen
The Bohr Model
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Niels Bohr (1913)
Allowed for electrons to have
___________
Electrons have ___________ energies
Lower energy- ___________ to
nucleus
Higher energy- ___________ from
nucleus
Electrons can ___________ energy to
raise to the next energy level and
___________ the same energy when
falling to the ground state
This model works well for
___________ but not for other
elements
Electrons as Waves
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Louis de Broglie (1924)
Suggested that electrons
could be considered as
___________ confined
to the space around a
nucleus
___________ - bending
of light around edges
Wave Interference- when
waves ___________
Quantum Theory
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Werner Heisenberg
(1927)
The Uncertainty
Principle
One cannot
simultaneously know
the ___________ and
___________ of an
electron
Quantum Theory
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Erwin Schroedinger (1926)
Wave Equation- The
quantization of an
electron’s energies is an
outcome
Quantum Theorymathematically describes
wave properties of
___________ and other
___________ ___________
Atomic Orbitals and Quantum
Numbers
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Quantum Numbersproperties of
___________
___________ and
properties of
___________ in
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orbitals
Like the address of an
electron or a seat in a
stadium or theater
Principal Quantum Number
(n) ___________
___________
1,2,3
K,L,M
This would be like the
section on a ticket for
a stadium seat
Angular Momentum Quantum
Number
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___________ of an
orbital
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0,1,2,3
s,p,d,f
Like the row in a stadium
or theater
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Magnetic Quantum Number
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m
___________ of an
orbital around the
nucleus
+1 to -1
Like finding your seat in
a stadium or theater
Spin Quantum Number
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Ms
Fundamental ___________
of an electron
+1/2 or -1/2
A single orbital can hold up to a
maximum of ___________
of ___________ spin
This would be which direction
you are facing in a theater or
stadium seat
Some Quantum Theory Rules
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Pauli Exclusion Principle- No two electrons
have the same set of
______________________ .
Or An orbital within a sublevel can contain up
to ___________ of opposite spin
Hund’s Rule- Each orbital within a
___________ receives an electron of
___________ spin before any can receive an
electron of ___________ spin