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Chapter 5 Electron ConfigurationEnergy Levels, sublevels and orbital
Notes
Tamara Lookabaugh
Moore High School
Chemistry 2017
DAY ONE: October 3Where are the electrons?• How do you know how many electrons are in an element and WHERE
are they?
• LOOK at your periodic table
• How many electrons for a CARBON atom?
• How do you know?
How do you read this? Write this on your periodic table
Atomic Number = # protons
# of p always = # e
Symbol for Element
Name for the Element
Atomic mass unitAverage of all the
Isotope masses x their percent abundance
Electron Energy Level Notes
• Electrons do not travel around the nucleus of an atom in orbits
• They are found in energy levels at different distances away from the nucleus. (kind of like shells or layers).
Electron Energy Level Notes• There are 7 energy levels write these on your periodic
table.(they correspond to the horizontal rows known as periods.)
• There are at least 4 possible types of sublevels—given labels: s, p, d, or f
Periodic Table write the levels 1-7 on your periodic table
1
2
3
4
5
6
7
Energy levels and number of electrons maximum that can be found in that shell or ring. PLEASE DRAW this in your notes
s,p,d,f blocks—Periodic Tablemark these on your table using the next slide
Mark the s,p,d,f blocks on your chart like this
1
2
3
4
5
6
7
Electron Energy Level 1
• In each energy level, electrons fill sublevels in a certain order
Level 1:
a) only has one s sublevel (a spherical shape)
b) 2 electrons may fit in this sublevel--each has an opposite “spin”,
*Pauli exclusion principle—no more than 2 electrons may be found in the same orbital
S Orbitals
Electron Energy Level 2
• Level 2 has two sublevels: s and p
a)2 electrons in s
b)3 different p orbitals —2 electrons in each
c)8 electrons overall in Level 2
Electron Energy Level 3
• Level 3:
a)has 3 sublevels: s, p, and d
b)2 electrons in s
c)6 electrons in p
d)5 different d orbitals, and 2
electrons can fit in each—total of 10.
a)total of 18 electrons in level 3
Each energy sublevel relates to orbitals
of different shape.
Electron Energy Level 4
• Level 4:
a)has 4 sublevels: s, p, d , and f
b)2 electrons in s
c)6 electrons in p
d)10 electrons in d
e)14 electrons in f (7 different orbitals for f)
f)total of 32
Day one assignment: Receive a Periodic Table Worksheet and draw Bohr Diagrams for the six elements listed on back of your worksheet DUE tomorrow
• Aluminum
• Nitrogen
• Neon
• Chlorine
• Calcium
• Zinc
Electron Energy Level NotesDay 2 October 4• The order that electrons fill up orbitals does not follow the logical
order of all 1’s, then all 2’s, then all 3’s, etc.
• Just like in a hotel, guests don’t always fill up all rooms and floors the same way.
• They follow the order found on pg. 156.
Order in which subshells are filled with electrons follows the pattern below
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
3d
4d
5d
6d
4f
5f
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d …2 2 6 2 6 2 10 6 2 10
Ground-State Electron Configuration
The arrangement of electrons in the atom is
called the electron configuration.
The aufbau principle states that each
electron occupies the lowest energy
orbital available. This is an AUFBAU
diagram
Order of Orbitals—Periodic Table
For the d block n-1
For the f block n-2
Hotel analogy video
s
s
s
s
p
d
d
p
p
f
These are 4 levels each
Showing the possible
Sublevels available to be
Filled with electrons
Electron Energy Level Notes
• An easy way to remember this is to use the periodic table--it is arranged to show how these orbitals are filled.
How do you write Electron Configurations?
• Watch this video to see how to write the
correct ORDER of how the shells fill from
level, sublevel and orbital.
NOW it is YOUR TURN to PRACTICE:
Receive handout on Electron configuration to complete and turn in tomorrow.
