Final answer:
The set of quantum numbers (1, 1, 0, +1/2) is not allowed for an electron in a ground state atom because it violates the Pauli exclusion principle and the restrictions on quantum numbers.
Step-by-step explanation:
The set of quantum numbers (1, 1, 0, +1/2) is not possible for an electron in a ground state atom because it violates the Pauli exclusion principle. According to this principle, no two electrons in an atom can have the same set of four quantum numbers.
The quantum numbers represent different properties of the electron, including its energy level (principal quantum number), orbital shape (azimuthal quantum number), orientation (magnetic quantum number), and spin (spin quantum number).
For an electron in a ground state atom, the quantum numbers must follow certain restrictions. The principal quantum number (n) must be an integer, the azimuthal quantum number (l) must be less than n, the magnetic quantum number (m) must be between -l and l, and the spin quantum number (ms) can only be +1/2 or -1/2.
In the given set of quantum numbers (1, 1, 0, +1/2), the azimuthal quantum number (l) is greater than the principal quantum number (n) which violates the restriction. Therefore, this set of quantum numbers is not possible for an electron in a ground state atom.