EVIDENCE #1:
Integrating an
Understanding of Coulomb's Law
Into
the Intermolecular Force UNIT
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THE CONTENT
Dr. Robert's Coulomb's Law POGIL (from Chem501): (click
for larger view)
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Through my coursework in Chem501,
Chem503,
and the integration of the concept of Coulomb's law (shown in the above
POGIL), I have gotten a deeper appreciation for how integral and
understanding of this law is to chemical phenomena.
COULOMB'S LAW
states the relationship between potential energy or electrostatic force
(of attraction or repulsion, depending upon the sign of the charged
particles involved) and charge magnitude and distance. As charge
magnitude increases, the magnitude of the electrostatic force
increases; as the distance increase, the magnitude of the electrostatic
force decreases.
Coulomb's law has been mentioned and can be applied to various chemical
concepts. For example, the concept of shielding electrons can be
explained by the competing electrostatic forces acting upon a valence
electron. Furthermore, Coulomb's law is also integral to an
understanding of intermolecular forces and how polarity and the ability
of molecules to pack closely together impacts properties such as
tensile strength, boiling point, and viscosity.
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Baseline evidence:
- Old worksheets on
intermolecular forces (IMFs)
JANUARY 2007
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Later
evidence:
- Excerpts from content-integration
project report in Chem503
JANUARY 2008
- Reading assignment
used in conjunction with intermolecular forces lecture and lab
JANUARY 2009
- Coulomb's
Law and Intermolecular Forces POGIL
(made for future use)
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I
had NOT taught Coulomb's Law as the basis for intermolecular
attractions or periodic properties related to shielding before taking Chem507.
Old worksheets on intermolecular forces
(click
on image to see larger view of highlighted view)
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Intermolecular Force Reading Assignment
p. 2, Questions #6-12
(click here for full
.pdf)
(click on
image to see larger view of selection section)
Coulomb's Law POGIL &
HW
(click on image for
full .pdf)
Intermolecular Forces POGIL
(click on image for
full .pdf)
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REFLECTION ON GROWTH
Comparison of the
baseline and later evidence shows a shift from having students learn
only what an intermolecular force is and the properties it is related
with toward having students also connect this understanding to
Coulomb's law of electrostatic attraction (a law of physics). I
would not have integrated these concepts and pushed my students toward
a deeper understanding (one based on physical laws) had I not
encountered Dr. Robert's Coulomb's Law POGIL in Chem501. Future
growth (in the coming years) will consist of trying to integrate this
law into other units where it applies (e.g. shielding in the periodic
properties unit).
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EVIDENCE #2:
Integrating Lessons
on Color Perception and Fluorescence
Into
the Quantum Theory UNIT
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THE CONTENT
My molecular spectroscopy project on fluorescent brightening
agents (from Chem507):
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Through my regular
coursework and my molecular
spectroscopy project on fluorescent brightening agents (FBAs) in Chem507, I have a newly
acquired understanding of color perception, fluorescence, and its
applicability to real life (e.g. lightbulbs, paper dyes, laundry
detergent additives). I wanted to integrate
these interesting
concepts into my quantum theory unit to make the concepts more tangible
and relevant to my students..
Color Perception
White light
can be broken down into a range of wavelengths with characteristic
colors shown in the first image--the
color wheel. When various colored lights are emitted
simultaneously or overlap, the human eye cannot differentiate between
the disparate wavelength lights, but rather perceives a different hue
which is a mix of the two (e.g. instead of seeing both red and green
simultaneously, a person would see the color yellow). This "additive" mixing is shown by the
second image. The perception of color as a property of an object
occurs when that object absorbs certain wavelengths and reflects
others. The third diagram shows an example of this absorption and reflection that makes an
object appear colored. In this example, the object would
appear yellow because it would absorb blue light, but reflect red and
green light. In the simplest case, when a particular wavelength
light is strongly absorbed, its complementary color (located on the
opposite side of the color wheel) is observed.
Fluorescence
When
substances fluoresce,
1. An electron is excited from the ground electronic energy state to an
excited electronic energy state by the absorption of energy, typically
ultraviolet light. During this transition, the vibrational state
also changes according to the Frank-Condon principle (which states that
the internuclear distance cannot change).
2. The electron relaxes to a lower vibrational energy level in the
excited state via a radiationless transfer (i.e. collision) or by the
release of an infrared photon. This transition is fast.
3. The electron relaxes from the excited state to the ground state,
emitting a photon. This transition is slow and typically in the visible range, yielding
fluorescence.
(A similar mechanism occurs for phosphorescence, but the second step is
slower as a result of a forbidden transition, allowing for a prolonged
lag between initial excitation and visible light emission)
Fluorescent
Brightening Agents (FBAs)
FBAs
are essentially fluorescent dyes that act similarly to the quinine
in tonic water, which emits blue light under blacklight. FBAs
contribute to the perception of brighter and whiter whites and colors
by absorbing UV light and emitting blue light. This disguises the
natural yellowing that often occurs as white linens and clothes yellow
with age and contributes to a brighter product.
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Baseline evidence:
OLD
LESSON PLAN:
(Electromagnetic radiation and quantum theory)
2008-2009 school year
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Later evidence:
NEW
LESSON PLAN:
(Color vision and fluorescence)
planned for
2009-2010 school year
JANUARY 2010
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I
had NOT taught color perception or fluorescence in concert with my
electromagnetic radiation and quantum theory before taking Chem507.
Day 1-2:
Electromagnetic radiation/ intro to quantum theory with atomic emission
spectra lesson
Note sheet
(click on image for
full .pdf)
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Click here
for the full original lesson plan from the molecular spectroscopy
project.
Previous Days:
-electromagnetic radiation lesson
-intro to quantum theory with atomic emission spectra lesson
Day 1:
POGIL PhET applet
activity on color vision
(click on image for
full .pdf)
The color
applet activity that describes how various wavelength (i.e.
color) lights produce a particular perception of color (e.g. a
combination of green and red light creates the perception of yellow
colored light) would help students understand how the different bands
of light in an element's emission spectrum produce the perception of a
particular color (e.g. the pinkish glow of an argon spectral tube even
though its emission spectrum shows blue, green, and red bands).
Furthermore, I thought it would be an interesting foundation concept to
learn, especially for students interested in stage lighting and
photography.
Day 2:
-discussion/ review of POGIL PhET applet activity
-small QUIZ on electromagnetic radiation/ color perception
-(some lecture/ old lessons on quantum theory)
Day 3-6:
-continue old lessons on quantum theory (electron
configurations, atomic orbital diagrams)
-do flame test lab
-small QUIZ on quantum theory
-some lecture on fluorescence
Day 7:
Fluorescence worksheet
(click on
image for
full .pdf)
Day 8-9:
Fluorescent brightening agents in laundry
detergent LAB
(click on image for
full .pdf)
Day 10: TEST
Beyond
the use of fluorescent light bulbs, most students
are unaware of how pervasive fluorescence-based applications are.
The ability to absorb higher energy, invisible UV light and emit lower
energy visible light has allowed for the creation of "brighter"
pigments and colors that can also appear "whiter" if the proper
wavelength light is emitted (going back to the first, color perception
lesson). I thought this lesson would connect quantum theory with
something more tangible in the everyday routine of an average student.
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