Download Quantum Numbers of Wavefuntions

Quantum Numbers of Wavefuntions
Quantum #
Symbol
Values
Description
Principal
n
1,2,3,4,…
Size & Energy of orbital
Angular
Momentum

0,1,2,…(n-1)
for each n
Shape of orbital
Magnetic
m
-…,0,…+ 
for each 
Relative orientation of orbitals within
same 
Spin
ms
+1/2 or –1/2
Spin up or Spin down
Angular Momentum Quantum # ()
Name of Orbital
0
s (sharp)
1
p (principal)
2
d (diffuse)
3
f (fundamental)
4
g
Quantum Mechanics and Atomic Orbitals
n
ℓ
Orbital Name
mℓ (“sub-orbitals)
Comment
Quantum Mechanics and Atomic Orbitals
Orbitals and Quantum Numbers
Representations of Orbitals
The s-Orbitals
Representations of Orbitals
The p-Orbitals
d-orbitals
Orbitals and Their Energies
Orbitals CD
Many-Electron Atoms
Many-Electron Atoms
Electron Spin and the Pauli Exclusion
Principle
Many-Electron Atoms
Electron Spin and the Pauli Exclusion
Principle
• Since electron spin is quantized, we define ms = spin
quantum number =  ½.
• Pauli’s Exclusions Principle: no two electrons can have
the same set of 4 quantum numbers.
•
Therefore, two electrons in the same orbital must have opposite spins.
Figure 6.27
Orbitals CD
Figure 6.27
Figure 6.28
Orbitals CD
Orbitals and Their Energies
Orbitals CD
Many-Electron Atoms
Electron Configurations
Species
Electron Configuration
Box Orbital
Comment
Electron Configurations
Species
Electron Configuration
Box Orbital
Comment
Metals, Nonmetals, and Metalloids
Metals
Figure 7.14
Periodic Trends
Two Major Factors:
•principal quantum number, n, and
•the effective nuclear charge, Zeff.
Figure 7.5:
Radius
video Clip
Figure 7.6
Figure 7.10
IE clip
Figure 7.9
Electron Affinities
• Electron affinity is the opposite of ionization energy.
• Electron affinity: the energy change when a gaseous atom
gains an electron to form a gaseous ion:
Cl(g) + e-  Cl-(g)
• Electron affinity can either be exothermic (as the above
example) or endothermic:
Ar(g) + e-  Ar-(g)
Figure 7.11: Electron Affinities
Group Trends for the Active Metals
Group 1A: The Alkali Metals
Group Trends for the Active Metals
Group 2A: The Alkaline Earth Metals
Group Trends for Selected Nonmetals
Group 6A: The Oxygen Group
Group Trends for Selected Nonmetals
Group 7A: The Halogens
Group Trends for the Active Metals
•
•
•
•
Group 1A: The Alkali Metals
Alkali metals are all soft.
Chemistry dominated by the loss of their single s
electron:
M  M+ + eReactivity increases as we move down the group.
Alkali metals react with water to form MOH and
hydrogen gas:
2M(s) + 2H2O(l)  2MOH(aq) + H2(g)
Group Trends for the Active Metals
Group 2A: The Alkaline Earth Metals
• Alkaline earth metals are harder and more dense than the
alkali metals.
• The chemistry is dominated by the loss of two s
electrons:
M  M2+ + 2e-.
Mg(s) + Cl2(g)  MgCl2(s)
2Mg(s) + O2(g)  2MgO(s)
• Be does not react with water. Mg will only react with
steam. Ca onwards:
Ca(s) + 2H2O(l)  Ca(OH)2(aq) + H2(g)
Atomic Structure
c   
Atomic H Spectrum
E
hc

( per photon)
Heisenberg Uncertainty
[ n ,  , m , ms ]
Wave/Particle Concept
Quantization
Bohr Model
Quantum Mechanics
Quantum Numbers
Applications
Energy Levels
Ei  f
1 1
 2.178 10 J   2  2 
 n f ni 
Electron Configuration
Electron Affinity
Ionization Energy
Electronegativity
Size
18