Quantum Quantum NumbersNumbers

Ryan Morrison & Ally GrayRyan Morrison & Ally Gray

• Specify the properties of an atomic orbital.Specify the properties of an atomic orbital.

• An orbital is where an atom keeps its electrons.An orbital is where an atom keeps its electrons.

Each element on the periodic table has a different set of Quantum Each element on the periodic table has a different set of Quantum Numbers, like their own address. The primary rule of quantum numbers is 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 that no two elements can have the same set of numbers, this principle is also known as the Pauli Exclusion Principle. also known as the Pauli Exclusion Principle.

For example: NitrogenFor example: Nitrogen OxygenOxygen

n=2 l=1 m=1 s=+n=2 l=1 m=1 s=+½½ n=2 l=1 n=2 l=1 m=(-1) s=(- ½)m=(-1) s=(- ½)

These two elements may have a very similar address but it is not the same.These two elements may have a very similar address but it is not the same.

What are Quantum Numbers?

orbitals

nnn represents the number of the n represents the number of the orbitalorbital..•Whatever row the

element is in, is the number you place for ‘n’.

•The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.

•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.

lll represents the subshell l represents the subshell

There are 4 different sub shells, they are 0, 1, 2 or 3 & are all There are 4 different sub shells, they are 0, 1, 2 or 3 & are all represented by letters.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.

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)

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)

mmm represents m represents magnetismmagnetism. .

The m orbital corresponds with the l orbital (subshells). If the The m orbital corresponds with the l orbital (subshells). If the subshell was d, it would be equal to saying that m is: -2 subshell was d, it would be equal to saying that m is: -2 ≤ m ≤ 2 ≤ m ≤ 2 or if the shell was p it would be -1 or if the shell was p it would be -1 < < m m >> 1. 1. The value of m The value of m indicates the orientation of the electron's orbit within the indicates the orientation of the electron's orbit within the subshellsubshell. .

m can range from 0 to a positive or negative number depending on m can range from 0 to a positive or negative number depending on the subshell. 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.

sss represents s represents spinspin..

• Moves in a circular/spherical Moves in a circular/spherical shape shape

• Contains either a positive or Contains either a positive or negative charge. negative charge.

• A positive spin means the A positive spin means the electrons spin clockwise. electrons spin clockwise. (+(+½)½)

• A negative spin means the A negative spin means the electron spins counter-electron spins counter-clockwise. (- clockwise. (- ½)½)

• The first half of each orbital is The first half of each orbital is + ½ and the other half is – ½ . + ½ and the other half is – ½ .

Examples.Examples.

n = 4

l = 2

m = -2

s = +1/2

n = 3

l = 1

m = 0

s = +1/2

n = 4

l = 0

m = 0

s = +1/2