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Quantum Mechanical Model of the Atom
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Progression of Atomic Theory
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Bohr Model
• Energy levels
• 1st energy level can hold 2
• 2nd energy level can hold 8
• 3rd energy level can hold 8
• Bohr Model Breaks down after 3rd energy level and no longer applies to Modern Quantum Mechanical Model of the Atom
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Bohr Model for Hydrogen• Energy level of an electron
• analogous to the rungs of a ladder
• The electron cannot exist between energy levels, just like you can’t stand between rungs on a ladder
• A quantum of energy is the amount of energy required to move an electron from one energy level to another
• The Bohr model explained the emission spectrum of the hydrogen atom but did not always explain those of other elements.
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The Quantum Mechanical Model• In 1926, Erwin Schrodinger
derived an equation with 4quantum numbers that described the energy and position of the electrons in an atom
• The 4 quantum numbers are used in the electron configuration which is a notation using energy levels and sublevels to show how the electrons are distributed within the atom.
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Quantum Numbers Chem Saver p 23
11 SS 11
Row # = Energy level or distance
from nucleus
Possibilities 1 –7
7 Rows
Subshell
Possibilities are
s, p, d, or f
4 subshells
# electrons occupying this
orbital
Possibilities are:
s: 1 or 2
p: 1-6
d: 1-10
f: 1-14
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Energy Levels and Sublevels• The first energy level has only one type of orbital
(sublevel)– S
• The second energy level has 2 types of orbitals– S and P
• The third energy level has three types of orbitals– S, P and D
• The fourth energy level has four types of orbitals– S, P, D and F
• Successive energy levels follow the same pattern. • Relative energy: s < p < d < f
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Principal Energy Level (n=?)
Orbital Types(sublevels available)
1 s
2
p
3
4
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Orbital Shapess orbital: (one possible orientation)
2s
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Orbital shapes• P orbital: ( three possible orientations)
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Orbital shapes• d: orbital: ( five possible orientations)
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Orbital shapes• f orbital: (seven possible orientations)
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The Quantum Atom
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Orbital Types(sublevels available)
# of orbital's per level
s 1
p 3
d 5
f 7
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Principal Energy Level (n=?)
Total # of orbitals per P.E.L. (n2)
1 1
2
3
4
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Orbital Types(sublevels available)
# of e’s per orbital type
s 2
p 6
d 10
f 14
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Principal Energy Level (n=?)
Total # of e’s per P.E.L. (2n2)
1 2
2
3
4
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Electron Configurations• Electrons fill the lowest energy levels first (H, Z=1)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s1
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Lewis Dot Structures• Lewis dot structures are shorthand to represent the
valence electrons of an atom. • The structures are written as the element symbol
surrounded by dots that represent the valence electrons.
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• Review Electron Configuration (H, Z=1)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s1
Lewis Dot Structures
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Pauli Exclusion Principle• no two e- in an atom can have the same four
quantum numbers.
• each electron needs its own space.
• Result – an orbital can hold a maximum of 2 electrons with opposite spin
Fourth Quantum number is the Spin
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Electron Configurations• Electrons fill the lowest energy levels first (He, Z=2)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s2
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Electron Configurations• Electrons fill the lowest energy levels first (Li, Z=3)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s1
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Electron Configurations• Electrons fill the lowest energy levels first (Be, Z=4)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s2
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Electron ConfigurationsElectrons fill the lowest energy levels first (B, Z=5)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p1
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Hund’s Rule• Don’t pair electrons in degenerate orbitals
until necessary.
• Unpaired electrons have the same spin.
• Applies to p, d, and f orbitals
2p
3d
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Electron Configurations• Electrons fill the lowest energy levels first
(C, Z=6)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p2
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Electron Configurations• Electrons fill the lowest energy levels first • (N, Z=7)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p3
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Electron Configurations• Electrons fill the lowest energy levels first • (O, Z=8)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p4
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Electron Configurations• Electrons fill the lowest energy levels first • (F, Z=9)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p5
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Electron Configurations• Electrons fill the lowest energy levels first • (Ne, Z=10)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p6
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Electron Configurations• Electrons fill the lowest energy levels first • (Na, Z=11)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p63s1
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Lewis Dot Structures Chem Saver p 24• Lewis dot structures are shorthand to represent the
valence electrons of an atom. • The structures are written as the element symbol
surrounded by dots that represent the valence electrons.
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Electron Configurations• Your Turn: Try Krypton (Kr, Z=36)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
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Electron Configurations• Electrons fill the lowest energy levels first (Ca, Z=20)
5s
4s
3s
2s
1s
2p
3p
4p
3d
4d
E E N N E E R R G G YY
• 1s22s22p63s23p64s2
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• An internet program about electron configurations is:
Electron Configurations
(Just click on the above link)
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Diagonal Rule for Writing Configurations and Practice Chem Saver p 23
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The relation between orbital filling and the periodic table
Chem Saver p 23ns1
np1
n-1d1
n-2f1
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In your composition notebook complete, Z=11 to 54 odd only. Be sure to show the electron configuration short hand notation
and the Lewis dot structure for each.
1 s 2 s 2 p 3 s 3 p 4 s 3 d
4 p 5 s 4 d 5p
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Electron Configuration on the Periodic Table
• The elements in the same family groups on the periodic table have similar physical and chemical properties
• The elements in the same family groups also tend to form similar types of compounds with other elements
• This is because the elements in the same family groups have the same number of electrons in the outer energy level
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Short Hand noble gas configurations
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