![Page 1: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/1.jpg)
![Page 2: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/2.jpg)
• Erwin Schrodinger proved
the idea of the “Planetary
Atom” wrong
• He said the e- does not move
around in fixed orbits
• He proved that the e- moves
in 3D areas around the
nucleus
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• He made a complicated
math equation describing
the area of an e-
• BUT…its just a probability of
where an e- may be in the
atom
• We do not know exactly
where an e- is in an atom
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• e- have different energy
levels called principal
quantum numbers (n)
• Within the energy levels
are sublevels that have their
own significant shape
• 3D non-circular areas where
e- can be
• Inside sublevels there are
orbitals, where e- are
arranged
![Page 5: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/5.jpg)
• s is the first and
simplest sublevel
• Has only 1 orbital that
holds 2 electrons
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• p is the second sublevel
• 3 orbitals
each holds 2 electrons
• A total of 6 electrons
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• d is the third sublevel
• 5 orbitals
each holds 2 electrons
• A total of 10 electrons
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• f is the last sublevel
• 7 orbitals
each holds 2 electrons
• A total of 14 electrons
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Sublevel Orbitals Electrons
s 1 2
p 3 6
d 5 10
f 7 14
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All electrons follow three
rules when filling energy
levels and sublevels. They
are:
• Aufbau Principle
• Pauli Exclusion Principle
• Hund’s Rule
![Page 11: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/11.jpg)
• Each electron occupies
the lowest energy
orbital available
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Here’s how to remember…
• Principal quantum numbers are like floors of a hotel
• e- enters the lowest level first
The Hotel Californium
1st floor
2nd floor
5th floor
n = 1
n =2
n = 5
= electron
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• A maximum of two
electrons may occupy a
single orbital, but only
if the electrons have
opposite spins
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Here’s how to remember…
Spin one index finger away
from your
Spin the other index finger
toward you
![Page 15: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/15.jpg)
• Single electrons with
the same spin must
occupy each equal-
energy orbital before
additional electrons
with opposite spins can
occupy the same
orbital.
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Here’s how to remember…
“Strangers on a bus”
• Do you sit next to a stranger or pick an empty seat?
• Pick an empty seat…unless there isn’t one, then you sit with the stranger
![Page 17: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/17.jpg)
• Includes a box for each
of the atom’s orbitals
• Boxes are filled with
arrows representing
electrons
Up and down facing
arrows to show opposite
spins
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Orbital Diagrams
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f • Start from bottom of
Aufbau diagram.
• Remember orbital table
for the sublevels
1s2s2p3s3p4s3d
Incr
easi
ng e
ner
gy
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• Remember the rules
electrons follow when
filling energy levels,
sublevels and orbitals
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule
• Let’s determine the
orbital diagram for
Phosphorus
15 electrons
![Page 20: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/20.jpg)
Filling in Orbital Diagrams:
• The first 2 e- go into 1s
orbital (line )
• only 13 more to go...
• Next e- go into 2s orbital
• only 11 more…
• Next e- go into 2p orbital
• only 5 more…
• Next e- go into 3s orbital
• only 3 more…
• Last e- go into 3p orbital
• e- by themselves before
being paired
• 3 unpaired e-
1s2s2p3s3p4s3d
Notice the opposite
spins (one ↑, one ↓)
![Page 21: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/21.jpg)
• Determine the orbital
diagram for the
following:
Cobalt (Co)
Germanium (Ge)
![Page 22: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/22.jpg)
1s2s2p3s3p4s3d
Cobalt – 27 e- Germanium – 32 e-
1s2s2p3s3p4s3d
4p
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Electron
Configurations• 1s2 2e-
• 1s22s2 4e-
• 1s22s22p63s2 12e-
• 1s22s22p63s23p64s2 20e-
• 1s22s22p63s23p64s23d10
4p65s2 38e-
• 1s22s22p63s23p64s23d10
4p65s24d105p66s2 56e-1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f
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Example: Oxygen
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
7s 7p 7d 7f• 1s2
• 2 electrons
• 4 electrons
• Total 8 electrons
• Stop once the # e- = the
atomic number
• Last sublevel doesn’t have
to be completely filled
8
16O
8 electrons2s2 2p4
![Page 25: Erwin Schrodinger proved - Ms. Phornvoranunt Chemistrydhsmsp.weebly.com/uploads/1/3/7/3/13735507/electrons_-_oribital... · 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s](https://reader030.vdocuments.net/reader030/viewer/2022040519/5e770c084ad7412de83ccd32/html5/thumbnails/25.jpg)
• Use your periodic
tables to find the
atomic numbers and
the electron
configurations of the
following elements:
Silicon
Uranium
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• Silicon
1s22s22p63s23p2
• Uranium
1s22s22p63s23p64s23d10
4p65s24d105p66s24f14
5d106p67s25f4