Beginning of Chapter 6: 3, 4, 7, 13,
18, 22, 25, 29, 35
End of Chapter 6: 39, 41, 45, 47, 49, 51, 56, 59,
65, 69
Beginning of Chapter 8: 8.2, 8.7, 8.9, 8.17, 8.23, 8.27, 8.32, 8.33, 8.34,
8.37
Uncertainty principle
Hydrogen atom (levels, shells, subshells and orbitals)
The Rydberg/Bohr energy formula, Ehydrogen = -RH/n2 (n = 1, 2, 3, . . .)
implies that there are discrete energy levels in this
atom (and in all atoms). The different values of n (n=1, n=2, n=3, etc)
correspond to the possible energies of excited levels of hydrogen.
Each energy level (value of n) has sublevels associated with it according to
the following rules:
1) Subshells are labelled by an integer (quantum number),
l which can have values from 0 to n-1. (l is script "el")
2) Each subshell is further divided into atomic orbitals which have a value of
ml specified from -l, -l+1,..., 0,...l-1,l.
Example: suppose n=3. This table shows the possible values of l and the
allowed values of ml for a total of 1+3+5 = 9 orbitals in the n=3 shell:
l=0 ; ml = 0
l=1 ; ml = -1, 0, +1
l=2 ; ml = -2, -1, 0, +1, +2
orbitals with l =0 are called s-orbitals or s-states
orbitals with l =1 are called p-orbitals or p-states
orbitals with l =2 are called d-orbitals or d-states
orbitals with l =3 are called f-orbitals or f-states
Electrons have spin. This means that they act like little magnets with a "north" and "south" pole.
The Pauli exclusion principle expresses the fact that no more than two electrons can exist in
any given atomic orbital (specified by allowable values of n, l , ml ).
One of the electrons must be spin up and the other spin down if they are in the same orbital.
ALLOWED: filled orbitals 
and 
;
half filled orbitals 
and 
unfilled orbitals ___
NOT ALLOWED: 
or 
(both electrons with same spin)
In the example above, where 9 orbitals are shown in the n=3 shell,
we can put a maximum of 18 electrons into the shell.
n= 4 shell: 1 + 3 + 5 + 7 = 16 orbitals : 2 + 6 + 10 + 14 = 32 electrons MAX
n= 3 shell: 1 + 3 + 5 = 9 orbitals : 2 + 6 + 10 = 18 electrons MAX
n= 2 shell: 1 + 3 = 4 orbitals : 2 + 6 = 8 electrons MAX
n= 1 shell: 1 = 1 orbitals : 2 = 2 electrons MAX
Click here for an energy level diagram for the H atom
In complex atoms with more than one electron, the same notation is used to describe the atomic
orbitals as is used for the ground state and excited states of the H atom. The actual energies of the
orbitals are shifted. The order of filling of orbitals for the ground state of any atom is given by
the following diagram (two electrons per orbital)
Click here for an energy level diagram for a complex atom