Applied Chapter 3.3 : Electron Configuration
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Transcript of Applied Chapter 3.3 : Electron Configuration
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Chapter 3.3
Electron Configuration
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Compare the Rutherford, Bohr, and Quantum models of the atom.Rutherford’s model of atom
Electrons orbit the nucleus just as planets orbit the sun
Bohr’s model of the atomElectrons travel around the nucleus in specific
energy level
Quantum – difference in energy between
two energy levels.
Objective 1:
Bohr Video
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Quantum model of the atomElectrons are found in orbitals around the
nucleus of atom.Orbital (electron cloud) – region of atom where
there is a high probability of finding electrons
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Particles Cathode ray tubePhotoelectric effect
WavesElectromagnetic spectrumLine-emission spectrum
Electrons – Act like particles and waves
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Electrons start in ground stateLowest possible energy level
Run electricity through gasElectrons absorb this energy
They move to excited stateElectron has more energy than normal
Quickly fall back to ground stateEnergy is emitted as light
Light has a specific wavelengthDetermines color (and line-emission
spectrum)
Light provides information about electrons Neon
Krypton
Argon
Objective 2:Explain how the wavelengths of light emitted by an atom provide information about energy levels.
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Emission Spectrums
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List the four quantum numbers, and describe their significance.
Quantum numbers:Number that specifies the properties of electrons
Tells where they are in the atom.
1. Principle quantum number ( n ) Main energy level n = 1,2,3,4,5 …….. Infinity
Distance from nucleus
2. Angular Momentum quantum number ( l ) indicates the shape of the orbital l = 0, 1, 2, 3 s p d f
Objective 3:
sp
d
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3. Magnetic (m) • orientation of orbital around
nucleus
m =-2,-1,0,+1,+2
m =-1,0,+1
m = 0
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4. Spin Quantum Number ( +1/2, -1/2) or ,
Indicates the two fundamental spin states of electron in an orbital
Single orbital can hold a maximum of 2 electrons
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Quantum Numbers of the 1st thirty atomic orbitalsn l m Orbital
nameNumbe
r of Orbital
s
Number of
Electrons
1 0 0 1s 1 2
2 0 0 2s 1 2
2 1 -1,0,1 2p 3 6
3 0 0 3s 1 2
3 1 -1,0,1 3p 3 6
3 2 -2,-1,0,1,2 3d 5 10
4 0 0 4s 1 2
4 1 -1,0,1 4p 3 6
4 2 -2,-1,0,1,2 4d 5 10
4 3 -3,-2,-1,0,1,2,3 4f 7 14
2
8
18
32
Total Electrons in
n
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Write the electron Configuration of an atom by using the Pauli Exclusion principle and the aufbau principle.
Objective 4
Electron ConfigurationThe arrangement of electrons in an atom
Lowest-energy arrangement – ground-state electron configuration
Rules Governing Electron Configuration1. Aufbau Principle – electron occupies the lowest-
energy orbital that can receive it. Pg. 105
2. Pauli exclusion Principle – no two electrons in the same atom can have the same set of four quantum numbers
3. Hund’s Rule – orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.
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4f 5f 6f 7f
3d 4d 5d 6d 7d
2p 3p 4p 5p 6p 7p
1s 2s 3s 4s 5s 6s 7s
Aufbau principle
** Gives the order of energy levels and orbitals
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Pauli Exclusion Principle
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Hund’s Rule
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Representing Electron Configurations
1. Orbital Notation
• Na __ __ __ __ __ __
1s 2s 2p 3s
2. Electron-Configuration Notation
• Na 1s22s22p63s1
3. Noble-Gas Notation
• Na [Ne] 3s1
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1. Write the electron configuration, orbital notation, and noble gas notation for an atom whose atomic number is:
a) 20b) 8c) 17
Writing Electron Configuration