the quantum mechanical model
DESCRIPTION
The Quantum Mechanical Model. The nucleus is found inside a blurry “electron cloud” A area where there is a high probability of finding an electron. Electron Configuration. Principal Quantum Number (n) = the energy level of the electron. (max # e- = 2n 2 ) - PowerPoint PPT PresentationTRANSCRIPT
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The Quantum Mechanical ModelThe nucleus is
found inside a blurry “electron cloud”
A area where there is a high probability of finding an electron.
![Page 2: The Quantum Mechanical Model](https://reader035.vdocuments.site/reader035/viewer/2022082203/56812cfa550346895d91cb0e/html5/thumbnails/2.jpg)
Principal Quantum Number (n) = the energy level of the electron. (max # e- = 2n2 )
Sublevels- like theater seats arranged in sections (s,p,d,f) (# of sublevels = n )
Within each energy level, the complex math of Schrodinger’s equation describes several shapes.
These are called atomic orbitals - regions where there is a high probability of finding an electron
*No more than 2 electrons in each orbital*
Electron Configuration
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Summary
s
p
d
f
# of orbitals
Max electrons
Starts at energy level
1 2 1
3 6 2
5 10 3
7 14 4
sublevel
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Electron Configurations
Three main “guiding” principles:
The way electrons are arranged in atoms.
Aufbau principle- electrons enter the lowest energy first.
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Electron ConfigurationsPauli Exclusion Principle- at most 2 electrons per orbital
Why only 2 electrons per orbital?like charges repel each other, but…
electrons spin on axis,
clockwise or counterclockwise,
creating magnetic polarization ( ↑↓ )
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Hund’s Rule- When electrons occupy orbitals of equal energy (same sublevel ) they don’t pair up until they have to.
- one electron enters each orbital until all orbitals contain one electron with spins parallel.
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Writing Electron Configurations(Letter - number designation)
H 1s1
Principle Energy Level
Sublevel
# of e-
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Orbital Diagrams
Show each orbital as a circle, box, or line.
Show each electron as an arrow, ↑ or ↓ spin.
Label electron configuration (letter –number).
N 1s 2s 2p
7↑↑ ↑↑ ↑↓ ↓
2 2 3
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Incr
easi
ng e
nerg
y
1s
2s
3s
4s
5s6s
7s
2p
3p
4p
5p
6p
3d
4d
5d
7p 6d
4f
5f
Orbital (Aufbau) diagram
![Page 13: The Quantum Mechanical Model](https://reader035.vdocuments.site/reader035/viewer/2022082203/56812cfa550346895d91cb0e/html5/thumbnails/13.jpg)
ExampleLet’s determine the electron configuration & orbital diagram for Phosphorus
Need to account for 15 electrons
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Incr
easi
ng e
nerg
y
1s
2s
3s
4s
5s6s
7s
2p
3p
4p
5p
6p
3d
4d
5d
7p 6d
4f
5f
1s22s22p6 3s23p3
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Remember…When we write electron
configurations, we are writing the lowest energy (ground state) configuration.
Do Problems 21-24 pg 160
*** # 21 draw orbital diagrams,
not just e- configurations