electron configuration
DESCRIPTION
Electron Configuration. Quantum Number. Number that specifies the properties of the atomic orbitals Tells us the distance from the nucleus and the shape of the orbital. Principal Quantum Number. Main level or shell These are the Bohr energy levels n = 1, n = 2, n = 3 - PowerPoint PPT PresentationTRANSCRIPT
![Page 1: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/1.jpg)
Number that specifies the properties of the atomic orbitals
Tells us the distance from the nucleus and the shape of the orbital
Quantum Number
![Page 2: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/2.jpg)
Electron Configuration
![Page 3: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/3.jpg)
Main level or shell These are the Bohr energy levels
n = 1, n = 2, n = 3 As n increases, the distance from the
nucleus increases
Principal Quantum Number
![Page 4: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/4.jpg)
Each main level is divided into sublevels Four types of sublevels
spdf
Sublevel
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Each sublevel is made of orbitals Every orbital can hold 2 electrons
Orbital
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s – 1 orbital – 2 electrons p – 3 orbitals – 6 electrons d – 5 orbitals – 10 electrons f – 7 orbitals – 14 electrons
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S orbital One spherical
shaped orbital
![Page 8: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/8.jpg)
P orbitals
Three dumbbell shaped One dumbbell in each axis
![Page 9: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/9.jpg)
P Orbitals
![Page 10: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/10.jpg)
D orbitals (5)
![Page 11: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/11.jpg)
F orbitals (7)
![Page 12: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/12.jpg)
![Page 13: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/13.jpg)
Main Level Sublevels Number of Sublevels
Electrons in sublevels
Total Electrons in Main Level
1 s 1 2 2
2 sp
13
26
8
3 spd
135
26
1018
4 spdf
1357
26
1014
32
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Arrangement of electrons in an atom Aufbau Principle – electrons fill into an atom
starting with the lowest energy levels
Electron Configuration
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Way which the electrons rotate on their axis Pauli Exclusion Principle – in order for two
electrons to occupy the same orbital, they must have opposite spin
Electron Spin
![Page 16: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/16.jpg)
Orbital Diagram
Hund’s Rule – electrons occupy orbitals singly first before doubling up
![Page 17: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/17.jpg)
Write the configuration for each of the below
CSBrNaClKr
Writing Configurations
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Valence Electrons Electrons in the last main energy level These are the electrons farthest out on the
atom These will interact with other atoms These are the electrons involved in
chemical reactions There are a maximum of 8 valence
electrons
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How to find valence e- Write configuration and count electrons in
last main energy level Examples: Find valence electrons for
CNaPFeAr
![Page 21: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/21.jpg)
Atoms will give up, accept, or share electrons in order to achieve a filled valence shell (8 valence electrons)
Octet Rule
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Metallic Character Metals become more reactive (more
metallic in character) as you go down a group
Most metallic elements bottom left corner of the periodic table
Least metallic, top right corner
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Ionization Energy Energy required to remove the most
loosely held electron from an atom The greater the ionization energy, the
more strongly the atom holds onto its electrons
M + energy → M+ + e Ionization energy increases as moving
across a period Ionization energy decreases as moving
down a group
![Page 26: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/26.jpg)
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Atomic Radius Half of the distance between two adjacent
nuclei Radius decreases across a period (atoms
hold the electrons tightly in) Radius increases down a group
![Page 28: Electron Configuration](https://reader035.vdocuments.us/reader035/viewer/2022062305/56816608550346895dd93edf/html5/thumbnails/28.jpg)