The following combinations of quantam numbers are not allowerd
1. n=3 l=0 m=-1
2. n=4 l=4 m=0
Can someone explain to me why the second one is not allowed.
Also check my explaination for the first one.
If L=0 then m also has to also =0
The s subshell (ℓ = 0) contains only one orbital, and therefore the mℓ of an electron in an s subshell will always be 0.
The l (orbital angular momentum) quantum number cannot exceed n-1.
Your explanation for to the first "no" is correct.
And what about the second one, can you explain that to me?
To determine why the second combination of quantum numbers is not allowed (n=4, l=4, m=0), we need to understand the allowed values for each quantum number.
The principal quantum number (n) represents the energy level or shell of an electron and can have any positive integer value (1, 2, 3, etc.).
The azimuthal quantum number (l) represents the shape of the electron's orbital and can have values ranging from 0 to n-1. So, for n=4, the allowed values for l are 0, 1, 2, and 3.
The magnetic quantum number (m) represents the orientation of the orbital and can have values ranging from -l to l. Therefore, for each value of l, the allowed values for m are -l, -l+1, ..., 0, ..., l-1, l.
In the second combination, n=4 and l=4. This means that the maximum possible value for l is 3 (n-1). However, the combination states l=4, which is outside the allowed range. Hence, the second combination of quantum numbers is not allowed.
Regarding your explanation for the first combination (n=3, l=0, m=-1), it is partially correct. For l=0, the m value can only be 0 since there is only one orbital (s-subshell). However, in the given combination, the value for m is -1, which is not allowed. Hence, your explanation is correct in stating that if l=0, m must also be 0.