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Schrödinger’s Equation
Beginning of
Quantum Mechanics
(Wave Mechanics)
Wave Functions
are solutions to Schrödinger
equation
H
ψ
= E
ψ
describe the electron in an atom.
Square of a wave function
(
ψ
2
) provides information
about location of an electron in terms of
probability or
electron density, also called orbitals
.
For
hydrogen atom
the allowed energies
of the electron are
the same as those
predicted by the
Bohr model;
however, the Bohr
model assumed a
symmetrical circular
orbit.
Bohr model doesn’t
work for other atoms
Don’t confuse orbitals with orbits.
1
Electron density distribution for 1s orbital
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View Full Document Shapes of Orbitals
Determined by the
probability
(
Ψ
2
) of finding an
electron at a certain distance (r) from the nucleus
Example: s orbitals
•
2s is
than 1s
•
Size of s orbital
as n increases
•
Shape:
symmetry
2
p and d Orbitals
First p orbitals
n
= 2
l
= 1
m
l
= 1, 0, 1
Two “lobes” with
in between
p orbitals are
First d orbitals
:
n
= 3
l
= 2
m
l
=
3
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View Full Document Representation of p and d
Orbitals
4
n
2
= number of states
= number of orbitals in the n
th
shell.
Subshells
# of orbitals in shell?
1s
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This note was uploaded on 09/29/2008 for the course CHEM 110 taught by Professor Hofmann,brucerob during the Fall '08 term at Pennsylvania State University, University Park.
 Fall '08
 HOFMANN,BRUCEROB
 Electron

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