electron configuration - plainfield north high...
TRANSCRIPT
![Page 1: Electron Configuration - Plainfield North High Schoolpnhs.psd202.org/documents/lcasey/1536685651.pdf · 2018-09-11 · ELECTRON ARRANGEMENT • Two methods: • Orbital Diagrams •](https://reader033.vdocuments.us/reader033/viewer/2022042306/5ed203e56731c53a5734c253/html5/thumbnails/1.jpg)
ELECTRON CONFIGURATION
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HOTEL CHEMISTRY
• Welcome to the electron hotel ……what a lovely place!
• Imagine you are the owner of a hotel.
• Rooms are filled up in a certain order.
• You want to fill the rooms on the lower floors first.
• Each room can only hold a certain number of people.
• Each room can only hold 2 people!
• Some rooms fill faster than others.
• Each person in a hotel can be found using their floor, room, and bed number.
• THIS IS JUST LIKE THE ELECTRONS AND THEIR ORBITALS!
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ELECTRON HOTEL
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QUANTUM MECHANICAL MODEL• Describes electrons
behaving as waves.• The exact location of the
electron is determined by Schrödinger’s wave equation.
• Describes the probable location of the electrons as a location in an orbital.
• The electron can be described using four quantum numbers.
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ATOMIC ORBITAL• Principal quantum number (n)
• Principal energy level• n = 1-7
• Relative size and energy of atomic orbitals
• As n increases, the electron is further from nucleus, and atom’s energy level increases
• Angular quantum number (llll)• Describes the shape of the orbital
• (s, p, d, f)
• l = l = l = l = 0 to n-1
• Magnetic quantum number (mllll)
• x, y, z• m
llll= = = = ---- l l l l to + llll
• Electron spin quantum number (ms)• ↑ (up)
• ↓ (down)
• ms =+½ or -½
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ORBITAL SUBLEVELS
• s, p, d, f• s orbital can hold 2 electrons
• p orbitals (3) can hold a total of 6 electrons
• d orbitals (5) can hold a total of 10 electrons
• f orbitals (7) can hold a total of 14 electrons
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AUFBAU PRINCIPLE
• Aufbau Principle – Each electron occupies the lowest energy orbital available.
• Aufbau Diagram
• Each box represents an atomic orbital
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PAULI EXCLUSION PRINCIPLE
• Pauli Exclusion Principle –a maximum of two electrons can occupy a single atomic orbital, but only if the electrons have opposite spins.
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HUND’S RULE
• Hund’s Rule – single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals
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ELECTRON ARRANGEMENT
• Two methods:
• Orbital Diagrams
• Electron Configuration
• Orbital Diagrams
• Aufbau Diagrams
• Electron Configuration
• 1s1
1s1
Sub-level
# of electrons
(Orbital)
Energy level
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ELECTRON CONFIGURATION & ORBITAL DIAGRAM
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ELECTRON CONFIGURATION & ORBITAL DIAGRAM
• Energy level 1 = s orbital
• Energy level 2 = s, p orbital
• Energy level 3 = s, p, d orbital
• Energy level 4 = s, p, d, f orbital
• Energy level 5 = s, p, d, f orbital
• Energy level 6 = s, p, d orbital
• Energy level 7 = s, p orbital
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PRINCIPLE QUANTUM
NUMBER(row or distance from
nucleus)
Size and energy
SUBLEVEL# ORBITALS IN
SUBLEVELMAX # e-
1 s 1 2
2 s p 1 3 8
3 s p d 1 3 5 18
4 s p d f 1 3 5 7 32
5 s p d f 1 3 5 7 32
6 s p d 1 3 5 18
7 S p 1 3 8
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FILLING THE ORBITAL1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d
7s 7p