Transcript Quantum Numbers

Quantum Numbers
Ryan Morrison & Ally Gray
What are Quantum Numbers?
•
Specify the properties of an atomic orbital.
•
An orbital is where an atom keeps its electrons.
 orbitals
Each element on the periodic table has a different set of Quantum Numbers, like their own address.
The primary rule of quantum numbers is that no two elements can have the same set of numbers,
this principle is also known as the Pauli Exclusion Principle.
For example:
Nitrogen
n=2 l=1 m=1 s=+½
Oxygen
n=2 l=1 m=(-1) s=(- ½)
These two elements may have a very similar address but it is not the same.
n
n represents the number of the orbital.
•Whatever row the
element is in, is
the number you 
place for ‘n’.
•This number tells us
the energy level and
shell that the electron
is found in.
The higher a value for n,
means a higher amount
of energy and the further
away it is from the
nucleus.
•The principal quantum number (n)
cannot be zero. The allowed values of
n are therefore 1, 2, 3, 4, and so on.
l
l represents the subshell
There are 4 different sub shells, they are 0, 1, 2 or 3 & are all represented by letters.
s is the purple (considered as 0)
p is the green (considered as 1)
d is the yellow (considered as 2)
f is the blue
(considered as 3)
This quantum number characterizes the
electrons angular momentum and
determines the shape of the orbit.
Its possible values for an electron depend
on the value of that electron's principal
quantum numbers, ranging from 0 to n-1.
Because of these different possibilities,
shells (other than the first shell) include
subshells. These are designated as
s(where l=0), p (where l=1), d (where l=2),
and f (where l=3)
If n = 1, the only
possible value for
quantum number l
is 0 (s).
If n = 2, the only
possible values for
quantum number l
are 0 & 1 (s & p)
If n = 3+, the possible values
for quantum number l are
0,1,2,3, (s,p,d,f)
m
m represents magnetism.
The m orbital corresponds with the l orbital (subshells). If the subshell was d, it would
be equal to saying that m is: -2 ≤ m ≤ 2 or if the shell was p it would be -1 < m > 1. The
value of m indicates the orientation of the electron's orbit within the subshell.
m can range from 0 to a positive or negative number depending on the subshell.
For each column periodic table, the
magnetism that would be your number
for m is constant . If you find that your
number is bigger than 3 or smaller than
-3, you are incorrect because L only
ranges from -3<m<-3.
Example: if l = 2 then your m values will be:
-2, -1, 0, 1, 2,  repeated twice to fill the column.
s
s represents spin.
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Moves in a circular/spherical shape
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Contains either a positive or
negative charge.
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A positive spin means the electrons
spin clockwise. (+½)
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A negative spin means the electron
spins counter-clockwise. (- ½)
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The first half of each orbital is + ½
and the other half is – ½ .
Examples.
n=4
l=2
m = -2
s = +1/2
n=3
l=1
m=0
s = +1/2
n=4
m=0
l=0
s = +1/2