Download Exam 1 Review Items

Name:
Electrons Review
This review is not all-inclusive.
I. Vocabulary – Be sure that you can describe the following items and explain their significance
to the unit to someone else.
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Amplitude
Wavelength
Frequency
Hertz
Electromagnetic radiation
Electromagnetic spectrum
Atomic emission spectrum
Ground state
Excited state
Quantum
Photons
Heisenberg uncertainty principle
Electron configuration
Energy level / shell
Sublevel
Orbital
II. Concepts – Discuss the following items with a classmate to ensure that you have a thorough
knowledge of each.
1. Describe energy. What is it? Units?
2. Explain the work / contributions of each of the following scientists:
 Rutherford
 Planck
Can you make connections between
 Bohr
each scientist’s ideas related to electron
behavior? How did each further the
 Einstein
work of those before him?
 de Broglie
 Heisenberg
 Schrödinger
3. Use a labeled diagram of a Bohr atom to explain how emission spectra are used to study
electrons.
4. Compare and contrast the Bohr model with the quantum mechanic model of the atom.
5. Describe each of the following rules governing electron configurations:
 Aufbau principle
Can you illustrate each rule with an
 Pauli exclusion principle
orbital drawing? Can you draw an orbital
 Hund’s rule
that violates each rule?
 Cr / Cu exception
6. Create a list of steps for properly labeling and numbering a periodic table so that it can be
used as a shortcut for writing electron configurations. Have a classmate check your steps
by following them as written.
7. Answer each of the following in terms of “n”:
Maximum # of electrons in a shell
Maximum # of subshells in a shell
Maximum # of orbitals in a shell
_______
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What does “n” tell you? Are you
familiar with the terms used in this
section?
8. Draw sketches of the orbitals in the following sublevels: s, p, d
III. Gizmos
u: haydenchem
p: chemistry
1. Revisit the ExploreLearning Gizmos completed in class.
2. Can you explain the fundamental concepts involved? Can you complete the assessment
questions at the end?
IV. Wave Relationships
1. Draw a graph showing the relationship between each pair of terms.
1. Energy / Frequency
2. Energy / Wavelength
3. Frequency / Wavelength
Which relationships are directly proportional?
What equation is associate with each
relationship?
V. Practice Problems – Answers must include the appropriate unit.
1. The yellow light given off by a sodium vapor lamp used for public lighting has a
wavelength of 589 nm. What is the frequency of this radiation?
2. A laser used in eye surgery to fuse detached retinas produces radiation with a frequency
of 4.69 x 1014 Hz. What is the wavelength of this radiation in nanometers?
3. Calculate the smallest increment of energy, that is, the quantum energy, that an object can
absorb from yellow light whose wavelength is 589 nm.
4. A laser emits light with a frequency of 4.69 x 1014 s-1. What is the energy of one
quantum of this energy? The laser emits its energy in pulses of short duration. If the
laser emits 1.3 x 10-2 J of energy during a pulse, how many quanta of energy are emitted
during the pulse?
5. What wavelength of radiation has photons with energy of 5.44 x 10-18 J? In what portion
of the electromagnetic spectrum would this radiation be found?
6. Excited mercury atoms emit light strongly at a wavelength of 436 nm. What is the
frequency of this radiation?
7. Calculate and compare the energy of a photon of wavelength 3.3 μm with that of
wavelength 0.154 nm.
VI. Electron Configurations – For each of the following atoms, provide:
a. Orbital notation
b. Electron configuration
c. Noble gas shorthand
1.
2.
3.
4.
5.
6.
7.
B
Ga
Sr
No
Mn
Bi
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