The set of quantum numbers given defines a specific orbital:

• n = 3: Principal quantum number (3rd shell).
• l = 1: Azimuthal quantum number (p-subshell).
• m = -1: Magnetic quantum number (represents one specific orbital among the three available 3p orbitals).

Since the set ($n, l, m$) specifies a single unique orbital, the Pauli Exclusion Principle states that this orbital can accommodate a maximum of 2 electrons (with opposite spins, $s = +1/2$ and $s = -1/2$).