•
Objective
– Today I will be able to:
• Explain the behavior of electrons based on Pauli’s exclusion
Principle and Hund’s Rule
• Illustrate the location of an electron by drawing an orbital
diagram
• Determine the number of unpaired electrons in an atom
• Identify the location of valance electrons in an atom
• Calculate the wavelength, energy and frequency of light
emitted from an atom
•
Evaluation/ Assessment
– Informal assessment – student responses when
reviewing electron configuration problems, orbital
diagrams and valence electrons. Listening to group
interactions on practice sheets
– Formal Assessment – collecting and analyzing responses
to electron configuration worksheet 2 and the where is
the electron lab. Reviewing responses to the exit ticket
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Warm – Up

Explain: principles, rules
and diagrams of electron
configurations
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Elaborate: Students
complete orbital diagrams
worksheet
Evaluate: Students will draw
orbital diagrams on the
board and explain their
answers (informal
assessment)
Explain: Valance Electrons
Notes
Elaborate: Students
complete a valance
electrons worksheet
Evaluate: Students will
share responses to the
worksheet
Explain: Spectra Calculation
Notes
Elaborate: Spectra
Calculations
Exit Ticket
Write the electron configuration
for the following elements:
•
Magnesium
•
Iron
•
Arsenic
What is the abbreviated configuration for
Sulfur?

Today I will be able to:
◦ Explain the behavior of electrons based on Pauli’s
exclusion Principle and Hund’s Rule
◦ Illustrate the location of an electron by drawing an
orbital diagram
◦ Determine the number of unpaired electrons in an
atom
◦ Identify the location of valance electrons in an atom
◦ Calculate the wavelength, energy and frequency of
light emitted from an atom
◦

Electrons Exam
◦ B-Day Tuesday, November 5
◦ A-Day Wednesday, November 6
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Warm – Up
Collect Flame Test Lab
Notes Pauli Exclusion Principle, Hund’s Rule,
Orbital Diagrams
Orbital Diagram Practice
Review Practice as a class
Valence Electron Notes
Valance Electron Practice
Spectra Calculation Notes
Spectra Calculation Practice
Exit Ticket

Electrons fill in lower energy levels before
filling in higher energy levels
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An orbital can hold a max of 2 eTo occupy the same orbital, they must spin
in opposite directions
If 2 e- occupy an orbital, they are said to be
“paired”
If only 1 e- is present in an orbital, it is
“unpaired”


e- occupy orbitals so that a max
number of unpaired e- result
More stable arrangement
 Shows
the electrons in their
sublevels
 Represented with arrows
1s
2s
2px
2py 2pz
H
↑
He
↑↓
C
↑↓
↑↓
↑
↑
Ne
↑↓
↑↓
↑↓
↑↓
↑↓

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
Electrons in the outermost
energy level
Determines the number of
electrons an atom gains, loses,
or shares
These are the electrons that are
involved in bonding
 Write
the electron configuration
for oxygen
 1s2 2s2 2p4
 Oxygen has six valence electrons
(2s2 and 2p4)
 Write
the electron configuration
for potassium
 1s2 2s2 2p6 3s2 3p6 4s1
 Potassium has 1 valence electron
(4s1)
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Exceptions are the d and f sublevels! Use
the number of electrons in the last s
sublevel (and the p sublevel, if available)
Write the electron configuration for Bromine
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Bromine has seven valence electron (4s2 and
4p5)
 Most
atoms want 8 electrons in
their outermost level OR full s
and/or p sublevels
 Atoms will form bonds to achieve
the desired amount of electrons
 Atoms are most stable when they
have a full outer shell
c = λν
◦ C= 3.0 x 108 m/s (speed of light)
◦ λ = wavelength (meters)
◦ ν = frequency (Hertz or 1/seconds)

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
Planck came up with the equation
E= hν
E = Energy (Joules)
h = Planck’s Constant
◦ 6.626 x 10-34 J*s

ν = frequency (Hertz or 1/seconds)
Complete the practice at your desk. Ask Ms.
Ose for help if you have questions.

For the element Chlorine:
◦ Write the electron configuration
◦ Write the abbreviated electron configuration
◦ Draw an orbital diagram
 Explain why you drew the electrons in the location of
the orbital's that you did
◦ Determine the number of valence electrons