Electron Configuration, Electron
Lab
• Objective
– Today I will be able to:
• Calculate the electron configuration for elements on the
periodic table
• Construct a model of where electrons in the 1s orbital are
located.
• Evaluation/ Assessment
– Informal assessment – student responses when
reviewing electron configuration problems. Listening
to group interactions on practice sheets and lab
– Formal Assessment – collecting and analyzing
responses to electron configuration worksheet 2 and
the where is the electron lab?
Lesson Sequence
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Warm – Up
Elaborate: write electron
configurations with a partner for
questions 1-18
Evaluate: review the questions as a
class (informal assessment)
Explain: electron configurations using
3d orbitals.
Elaborate: Students will complete 1936 on electron configuration WS with
a partner
Evaluate: review the questions as a
class (informal assessment)
Explain: abbreviated electron
configurations
Elaborate: Students will add a column
to the WS and repeat write the
abbreviated configuration
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•
Evaluate: Abbreviated configurations
will be reviewed as a class (informal
assessment)
Explore: Students will be sorted into
groups and will complete the where
is the 1s electron lab located
– I will be assessing students progress
during the lab as I monitor group
discussions
•
•
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Evaluate: Students will complete an
electron configuration WS
(assessment)
Explain: principles, rules and
diagrams of electron configurations
Exit Ticket
Warm - Up
• How many electrons can each orbital hold?
–
–
–
–
s=
p=
d=
f=
• Write the electron configuration for the following
elements
– Helium
– Nitrogen
– Silicon
Objective
• Today I will be able to:
– Calculate the electron configuration for elements
on the periodic table
– Construct a model of where electrons in the 1s
orbital are located.
Homework
• Electron Configuration Practice
Agenda
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Warm – Up
Electron Configuration Practice
Electron Configuration Notes
Electron Configuration Practice
Where’s the electron Lab
Exit Ticket
Electron Configuration Practice
Complete numbers 1-18
Electron Configuration
Electron Configuration
n
1
2
3
4
5
6
7
p-block
s-block
d-block
n-1
f-block
n-2
Electron Configurations
• We can write the electron configurations for
each element (assuming the atom has a
neutral charge) representing the location of
the elements electrons in the energy levels
Examples
• Sodium (Na)
– Has 11 electrons (when neutral)
– Electron Configuration:
• 1s22s22p63s1
• Cobalt (Co)
– Has 27 electrons (when neutral)
– Electron Configuration
• 1s22s22p63s23p64s23d7
Why does 4s come before 3d?
• 3d is of slightly higher energy than 4s, but 4s is
further from the nucleus
• It takes less energy for a 3d electron to form pairs
then a 4s electron
Aufbau Diagram
• Instead of using the periodic table as a road
map, you can use the aufbau diagram to
determine the order that the electrons occupy
the different energy levels
• Electrons fill the lowest energy orbitals first
Aufbau Diagram
Complete Electron Configuration
Practice Worksheet 19 - 36
Abreviated Electron Configuration
• Scientists are lazy ;)
• We need a shorthand way to represent
electron configuration
• It would take a long time to write the
configuration for elements with a lot of
electrons
• How do we do this?
• Noble Gas Configuration
Noble Gas Configuration
• The last column on the periodic table is
referred to as the noble gases
• To write in abbreviated configuration:
– Find the last noble gas within the configuration
– Write the symbol
– Write the remaining configuration
• Example
• Ca - 1s2 2s2 2p6 3s2 3p6 4s2
• Noble Gas Configuration = [Ar] 4s2
Noble Gas Configuration
• Writing Noble Gas Configurations for ions is a
little bit different
• Must account for an electron being gained or
lost
– Chlorine Ion = Cl-1
• [Ne] 3s2 3p6
– Sodium Ion = Na+1
• [He] 2s2 2p6
Electron Configuration Practice
Go back and write the Abbreviated
(Noble Gas) configuration for the
elements on the worksheet on the right
hand margin
Where is the electron lab?
Electron Configuration Practice 2
More Electron Configuration
Rules and Principles
Pauli Exclusion Principle
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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”
Pauli Exclusion Principle
Hund’s Rule
• e- occupy orbitals so that a max number
of unpaired e- result
• More stable arrangement
Orbital Diagram
• Shows the electrons in their sublevels
• Represented with arrows
Orbital Diagram
1s
2s
2px
2py 2pz
H
↑
He
↑↓
C
↑↓
↑↓
↑
↑
Ne
↑↓
↑↓
↑↓
↑↓
↑↓
Exit Ticket
• Draw an orbital diagram representing the
arrangement of the electrons in sulfer