Final answer:
The set of quantum numbers n = 1, l = 0, ml = 0, ms = 1/2 is a valid combination for an electron in an atom, satisfying all the required quantum number rules.
Step-by-step explanation:
The set of quantum numbers in question is n = 1, l = 0, ml = 0, ms = 1/2. This set of quantum numbers is valid for an electron in an atom. The principal quantum number n describes the energy level of the electron and must be a positive integer. Here, n is 1, which is correct. The azimuthal quantum number l describes the subshell and must be in the range of 0 to n - 1. Since n is 1, l is correctly set to 0. The magnetic quantum number ml can take on integer values ranging from -l to l, including zero, so ml being 0 is also valid. Finally, the spin projection quantum number ms can be either +1/2 or -1/2, so ms = 1/2 is valid. Thus, the electron can have these quantum numbers, which aligns with the Pauli exclusion principle, stating that no two electrons in the same atom can have the same set of four quantum numbers.