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Quantum Chemistry 0
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In quantum mechanics, the Schrödinger
equation is used to solve Newton's equations
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This course consists
of 120 videos that are organized into 10 chapters
and a course playlist, as well as various chapter
playlists
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On the
other hand, in quantum mechanics, the behavior
is probabilistic
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However, atoms and electrons behave
differently from these objects
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1 Introduction
2
Quantum Chemistry 0
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1 Blackbody Radiation
This discussion will focus on blackbody radiation and
the origins of early quantum theory
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The theory predicts that as the frequency of light
increases, the amount of radiation also increases with
the square of the frequency
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Planck proposed that the energy levels inside the black
box cannot have any possible level, as classical theory
suggests, but rather there exists a quantized set of
values
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Here are a few examples of this formula:
At a frequency of 1 Hz and temperature of 1000 K,
the density of radiation is 0
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At a frequency of 10 14 Hz and temperature of 300 K,
the density of radiation is 2
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Quantum Chemistry 1
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1 Blackbody Radiation
Quantum Chemistry 1
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This effect was solved by a quantum
hypothesis, providing an example of a quantum
solution to a classical physics problem
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Changing the frequency of
the light from red to green to blue would not change
the electrons that are ejected from the surface
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This means
that changing the intensity of the UV light will not
change the speed of the ejected electrons
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2 Photoelectric Effect
Quantum Chemistry 1
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3 Rydberg Formula
Rydberg Formula
In this article, we will discuss the Rydberg formula
and an example of when a quantization hypothesis
solved a problem that classical physics couldn't seem
to solve
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This radiation
occurs when transitioning from one energy level to
another
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6 inverse centimeters so wave numbers or ν
is equal to the frequency of the light divided by the
speed of light
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This number, 109
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Quantum Chemistry 1
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4 - Bohr Hydrogen Model
1: Radius
we will explore the Bohr model for the hydrogen
atom and calculate the radius of a hydrogen atom in
certain conditions
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General Physics Review
In physics, we have mass and the resistance to
acceleration is the moment of inertia
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This presents a situation
with two unknowns: v and r
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Niels Bohr had a hypothesis in 1911:
The Bohr radius is the radius at which n equals 1, and
then the radius goes up quadratically with n
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1 nanometers (nanometer being 10^-9
or 1 billionth of a meter)
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Quantum Chemistry 1
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We will start by using the
equation derived from Bohr's hypothesis:
r = (n^2 * h^2)/(4*pi^2 * me * k * e^2)
Where:
r = radius of the hydrogen atom
n = principal quantum number (for hydrogen, n
= 1)
h = Planck's constant (6
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109 x 10^-31 kg)
k = Coulomb's constant (8
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602 x 10^-19 C)
Plugging in the values, we get:
r = (1^2 * (6
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109 x 10^31 * 8
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602 x 10^-19)^2)
Simplifying and converting to nanometers, we get:
r = 0
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053 nanometers
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4 - Bohr Hydrogen Model
1: Radius
Quantum Chemistry 1
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To determine the radius of the ground state of the atom, we looked at a
rotating reference frame and concluded that the Coulomb force attracting the electron
to the nucleus must be balanced by the centrifugal force keeping it rotating constantly
around the proton
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So, it starts at low energy and continuously goes up
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Jumps Between Two Energy Levels
We calculate the energy difference between two energy levels as delta E
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The
value of the Rydberg constant (Rh), or what we might refer to as R infinity, is
expressed analytically and is accurate to within 0
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Note that the
proton has finite mass, and the electron does not weigh infinitely more than the proton
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Assumption: angular momentum of the electron is quantized
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Quantum Chemistry 1
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7 - Uncertainty Principle
in Measurement
Einstein, in 1906, described light as both a particle and a
wave with the photoelectric effect
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He suggested that matter is something that can have
a wavelength, which can be defined as the wavelength
equals Planck's constant divided by momentum of the
particle