Missing options
a. There are no sets of orbitals of equal energy
b. Two electrons will occupy the same orbital rather than separate orbitals
c. Two electrons will occupy different orbitals and have opposing spins.
d. Two electrons will occupy different orbitals and have like spins
Answer:
d. Two electrons will occupy different orbitals and have like spins
Step-by-step explanation:
When the orbitals are degenerate ( equal energy) pairing does not start until each orbital in a particular subshell gets one electron each. After that pairing start. This is the basis of Hund's rule of maximum multiplicity.
When the electrons have occupied different orbitals in the same subshell their spin remains same, because opposite spin electrons exist in the same orbitals. and this pattern continues in the second, so the electron in the second orbital will resemble to that of the first orbital electron