Download LT1: Electron.NOTES - Simpson County Schools

UNIT 3-LT1: Electron Arrangement (Ch.5)
http://www.youtube.com/watch?v=-YYBCNQnYNM
http://www.youtube.com/watch?v=sMt5Dcex0kg
I.
Light and Quantized Energy (136-145)
a.
Rutherford’s Model
Contribution to Atomic Structure
Problems with his model
Nucleus:
Electron Arrangement:
b.
Electromagnetic Radiation (EM) is
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c.
Characteristics of waves
Wavelength
Frequency
Amplitude
d.
EM radiation (Draw the spectrum indicating how wavelength and frequency change as you move across the
types.)
e.
f.
Why did the wave model of light need a revision?
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g.
h.
i.
j.
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What was Planck’s idea of QUANTUM? How did it relate to an atom?
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Is Light a wave or a particle?
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Why do we see colors emitted by atoms like in neon signs?
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What is Atomic Emission Spectrum?
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II.
Quantum Theory of the Atom (page 146-155)
a.
Bohr’s Model
Contributions to Atomic Structure
Problems with his model
Energy Levels (states):
Quantum number:
b.
What is the quantum mechanical model of the atom and how is it different from the Bohr model?
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c.
De Broglie and Schrodinger: Quantum mechanical model
Contributions to Atomic Structure
Wave-like motion of electrons:
Atomic Orbitals:
Principal Quantum Number:
Principal energy level:
Energy sublevels:
Type of sublevel
Shape
# of orbitals (configurations)
Max # of
electrons
s
p
d
f
Energy level or
Sublevels
Max # of
Principal Quantum
electrons
Number
1
2
3
4
5
6
7
d. What is the Heisenberg Uncertainty Principle and how does it relate to electrons and atomic structure?
III.
Electron Configuration (156-162)
Main Idea: A set of three rules can be used to determine electron arrangement in an atom.
Aufbau
principle
Pauli Exclusion
Principle
Hund’s Rule
a.
Electron Configurations
b.
Orbital Notation
c.
Noble Gas Configuration
d.
Exceptions to the Rules: