Final answer:
The number of unpaired electrons for each option is zero for (a), one for (b), two for (c), and three for (d), based on the less than 1, 2, 3, and 4 electrons guidelines provided, respectively.
Step-by-step explanation:
The question requires us to determine the number of unpaired electrons in the ground state for each given option. Electrons will fill orbitals according to Hund's Rule, which states that every orbital in a subshell is singly occupied before any orbital is doubly occupied, and all of the electrons in singly occupied orbitals have the same spin.
Considering the reference information:
- (a) indicates that there are less than 1 electron (meaning no unpaired electrons), which aligns with having a fully paired electron configuration.
- (b) indicates less than 2 electrons, which implies there is one unpaired electron.
- (c) suggests there are less than 3 electrons, pointing to the presence of two unpaired electrons.
- (d) with less than 4 electrons, means there are three unpaired electrons.
Incorrect configurations such as "4s³" or "3p7" violate the Pauli exclusion principle or the electron capacity rules for orbitals, which determine the allowed number of electrons within a shell or subshell (2n² for a shell and 2(2l + 1) for a subshell).