What is wrong with these sets? Fix what's wrong:
n=4, l=3, ml=4
n=2,l=-1, ml=1
I don't exactly even know what the question is asking!
You must know the rules Here they are.
n may be any whole number from 1 (that is, 1, 2, 3, 4, 5, etc)
l may take values of 0 and increase by increments of 1 but may not be larger than n-1. (Therefore, for n = 1, l may be zero only. For n = 2, l may be 0 or 1)
ml may have values from -l up to +1 with all values between in whole numbers, including 0.
Ms may have values of +/- 1/2.
The first one:
Starting with n = 4, we know l may be 0, 1, 2, or 3 so l = 3 is ok.
ml may have values of -3, -2, -1, 0, +1, +2, and +3 (that's -l to +l). It CAN'T have a value of 4 so that's what is wrong with that set.
You do the second one the same way. Jut analyze it step by step.
Okay, I understand now, it's much easier than I was making it out to be! Thanks so much for your help!
The sets you provided are stating the quantum numbers for an electron in an atom. Each electron is defined by a set of three quantum numbers: the principal quantum number (n), the azimuthal quantum number (l), and the magnetic quantum number (ml). These quantum numbers describe the energy state, the shape of the orbital, and the orientation of the electron within the orbital, respectively.
In the first set (n=4, l=3, ml=4), there is an issue with the values of l and ml. The azimuthal quantum number (l) can range from 0 to (n-1), so in this case, it should be between 0 and 3 (4-1). However, l is given as 3, which is correct. The magnetic quantum number (ml) can range from -l to +l, so in this case, ml should be between -3 and +3. However, ml is given as 4, which is incorrect. The correct set would be: n=4, l=3, ml=-3 to +3.
In the second set (n=2, l=-1, ml=1), there are multiple issues. Firstly, the azimuthal quantum number (l) cannot be negative. It must be a non-negative integer value ranging from 0 to (n-1). So, l=-1 is incorrect. Secondly, the magnetic quantum number (ml) cannot be greater than the absolute value of l. So, ml=1 is incorrect if l=-1. To fix this set, we need to adjust the values. We could choose a different value for l (e.g., 0 or 1) and then adjust ml accordingly. For example, we could have n=2, l=0, ml=0 or n=2, l=1, ml=-1,0,1.
Remember, to determine if a given set is valid or not, you need to consider the range of values for each quantum number.