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IB PHYSICS
Name: __________________________________
Period: ________ Date: ___________________
DEVIL PHYSICS
BADDEST CLASS ON CAMPUS
TSOKOS READING ACTIVITY
Section 6-5 (5 Points)
1. IB Assessment Statements for Topic 13.1, Quantum Physics:
Atomic Spectra and Atomic Energy States
13.1.8.
Outline a laboratory procedure for producing and observing atomic spectra.
13.1.9.
Explain how atomic spectra provide evidence for the quantization of energy in atoms.
13.1.10.
Calculate wavelengths of spectral lines from energy level differences and vice versa.
13.1.11.
Explain the origin of atomic energy levels in terms of the “electron in a box” model.
13.1.12.
Outline the Schrödinger model of the hydrogen atom.
13.1.13.
energy.
Outline the Heisenberg uncertainty principle with regard to position-momentum and time-
2. Objectives for Tsokos Lesson 6-5, Quantum Theory and The Uncertainty Principle
a. Describe emission and absorption spectra and understand their significance for atomic structure
b. Explain the origin of atomic energy levels in terms of the ‘electron in a box’ model
c. Describe the hydrogen atom according to Schrödinger
d. Do calculations involving wavelengths of spectral lines and energy level differences
e. Outline the Heisenberg Uncertainty Principle in terms of position-momentum and time-energy
3. Read section 6-5, Quantum Theory and the Uncertainty Principle (wait a minute . . . is that right? . . . no .
. . yeah, that’s right . . . I think) in your textbook.
4. Answer the following questions:
a. What is a spectrometer?
b. What is the emission spectrum of an element?
c. How do emission lines differ between elements?
d. What does the quality in c. above allow you to do?
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e. What happens when white light (consisting of all wavelengths in the visible spectrum) is transmitted
through a gas and then through a spectrometer?
f. What is this pattern of black lines called?
g. What is the Balmer formula for the wavelengths in the hydrogen spectra?
h. What is a reasonable assumption you can make about the energy of an atom during light emission?
i. If the emitted energy is in the form of light, and light consists of photons, what is the equation for the
emitted energy?
j. The above discussion points to what important fact about the energy of an atom?
k. What was the purpose of the ‘Electron In A Box’ mind experiment?
l. Explain Schrödinger’s quantum model for the behaviour of electrons in atoms.
m. How did Max Born clarify the meaning of 𝜓(𝑥, 𝑡)?
n. The application of Schrödinger’s theory to a hydrogen atom yields what equation for energy?
o. Bonus: Is Schrödinger’s cat alive or dead? How do you know?
p. In view of the above, what is meant by the term energy levels?
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q. When will an electron change energy levels and what happens when it does?
r. What can we calculate if we know the number of levels the electron transitions and what equations
will we use ?
s. Schrödinger’s theory doesn’t give us the exact position of an electron, but it does give us the next
best thing. What is that?
t. What is the Heisenberg Uncertainty Principle as applied to position and momentum?
u. Are you sure of your answer to t. above?
ℎ
v. Using the equation Δ𝑥Δ𝑝 ≥ 4𝜋 , explain why an increase in accuracy of position or momentum makes
the accuracy of the other decrease?
w. The Heisenberg Uncertainty Principle can also be applied to what two other concepts?
x. Does this discussion motivate you to want to tackle Option J?
5. Answers may be typed or neatly printed. Drawings may be freehand, but try to make use of the ‘Shapes’
or ‘Insert Clipart” functions of MS Word. If you submit this assignment electronically, the filename
must be in the following format, “LastnameFirstinitialPerXReadActX-X”.
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