Final answer:
The set of quantum numbers n = 3, l = 3, m = -1 is incorrect because l must be less than n, which can only be 0, 1, or 2 in this case, thus l = 3 is not allowed. Moreover, the m value is only valid if l is correct.
Step-by-step explanation:
The set of quantum numbers provided in the question: n = 3, l = 3, m = -1 are incorrect due to the relationship between the principal quantum number (n) and the azimuthal or angular momentum quantum number (l). According to the rules for quantum numbers, the value of l must be in the range of 0 to n-1. Since n is given as 3, l can only be 0, 1, or 2; consequently, l = 3 is not allowed because it equals n and does not fall within the acceptable range. The magnetic quantum number (m), which corresponds to the orientation of the orbital in space, can range from -l to +l; however, in this case, since l is not a valid value, m = -1 is also not valid within this context.
Allowed Values for the Quantum Numbers
n (principal quantum number): Any positive integer (1, 2, 3,...)
l (azimuthal or angular momentum quantum number): Integers ranging from 0 to n-1
m (magnetic quantum number): Integers ranging from -l to +l
ms (spin quantum number): Either +1/2 or -1/2
Therefore, an allowed set of quantum numbers for n=3 would have l values of 0, 1, or 2 and corresponding m values within the respective ranges for each l.