How many orbitals are contained in the n=2 level? Give the l and ml values of each of them.
ell = 0,1,2,3 etc to max of n-1.
ml = -ell to + ell.
To find the number of orbitals in the n=2 level, we can use the formula:
Number of orbitals = n^2
So, for n=2:
Number of orbitals = 2^2 = 4
Therefore, there are 4 orbitals in the n=2 level.
Now, let's determine the quantum numbers (l and ml) for each orbital in the n=2 level.
The value of l can range from 0 to (n-1). In this case, since n=2, the possible values for l are 0 and 1.
For l=0, ml can only have one value, which is 0. This corresponds to the s orbital.
For l=1, ml can have three values: -1, 0, and 1. These correspond to the three p orbitals: px, py, and pz.
So, the l and ml values for each of the orbitals in the n=2 level are as follows:
s orbital: l=0, ml=0
px orbital: l=1, ml=-1
py orbital: l=1, ml=0
pz orbital: l=1, ml=1