Transcript Extending this to Hydrogen

EMISSION/ABSORPTION SPECTRA
EXTENDING THIS TO HYDROGEN
• Results from solving the Shrodinger
equation for the hydrogen atom
• Z is the atomic number
• me is the mass of an electron
• e is the charge of an electron or proton
• h is Planks constant
• r is atomic radius
• e0 is the permittivity of free space
• Agrees with experimental results
• Constants combined= Rydberg constant
RYDBERG EQUATION: DERIVATION
• IF THE ENERGY OF A GIVEN ENERGY LEVEL IS DEFINED AS EN=-RH(1/N2).
WE CAN FIND THE DIFFERENCE IN ENERGY SHELLS BY ENF-ENI
Change= Final-initial
Either of these are often shown
in text books. Use whichever
you prefer but be sure not to
mix them up. One has a
negative one does not.
RYDBERG EXAMPLE
• I’ll do:
• The energy levels of hydrogen-like one-electrons of atomic number Z differ from
those of hydrogen by a factor of Z2. Predict the wavelength of the transition from
n=2 to n=1 in He+. (1.17)
RYDBERG EXAMPLE
A violet line is observed at 434 nm in the spectrum of atomic hydrogen.
Determine the values of n for the beginning and ending energy levels of the
electron during the emission of energy that leads to this spectral line (1.16).
Hints:
We are observing a line, therefore is a photon being absorbed or emitted?
Based on the answer to the above: is the final higher or lower than the initial? What does that
mean about DE
The Balmer series is the hydrogen emission series that is in the visible region what does this
mean about nf? (homework you could look up, on an exam I’d tell you).
Please type your answer into your iclicker
EXTENDING TO OTHER ATOMS:
• If we have all one type of atom, and we excite all of them to a particular energy
level, what will be true of the emitted light?
A) The photons will all have the same wavelength
B) The photons have different wavelengths
C) No photons will be emitted
D) The photons will have different energies
E) I do not know
Reflected vs. Emitted
• Emitted light comes from a particular source.
• Examples?
• Reflected light “bounces” off other objects
• Examples?
• Each time we think about light think about which it belongs
too.
LASERS
• Light Amplification by Stimulated Emission of Radiation.
Why can’t we see the laser light until it hits the wall?
http://www.infoplease.com/images/ESCI112LASERS003.gif
TRANSITIONAL EXAMPLE PROBLEM
• If a bag of potato chips has 1000 calories and 100 chips, how many calories are
there per chip?
• How did you did you do that?
• Now if a laser pulse has 1 J Total and 1000 Photons how many joules per photon?
• Make an Equation using these two questions relating total energy to energy of a
photon.
EXAMPLE PROBLEM:
A monochromatic beam of light with a total energy of 2.5J contains 8.56x10-4 mols
of photons. What is the wavelength of the beam?
WHAT DO WE USE EMISSION SPECTRA FOR?
Hydrogen Emission Spectra
Fe Emission Spectra
Given the above, and furthermore, that elements have specific emission spectra,
what could we use spectroscopy of elements for?
WHAT DO WE USE EMISSION SPECTRA FOR?
Hydrogen Emission Spectra
Fe Emission Spectra
• Emission Spectra is unique to individual elements
Flame test
• Spectra can be collected and matched to known
emission spectra to determine the element
present.
• Flame tests
EMISSION SPECTRA: APPLICATIONS IN
ASTRONOMY
•Spectra is collected
•Compared to known ions
•Temperatures known
TIME TO REGRESS TO OUR 5 YR OLD SELVES
• WHY IS THE GRASS
GREEN?
THE GRASS IS GREEN BECAUSE…
chlorophyll absorbs red light and
reflects green light
eyes see reflected green light
What happens if you shine green light
on the plants?
What happens if you shine red light on
the plants?
TIME TO REGRESS TO OUR 5 YR OLD SELVES
• Why is the sky blue?
WHY IS THE SKY BLUE?
TIME TO REGRESS TO OUR 5 YR OLD SELVES
• Why is the Sun
Yellow/Orange?
• (hint: is it really?)
WHY IS THE SUN YELLOW/ORANGE
SPECTROSCOPY
microscopyU
**don’t memorize this
GREEN FLUORESCENT PROTEIN (GFP)
Tsien
Anthony Chan, Emory University