why do the degenerate d orbitals of a metal ion in a complex have higher energy than those of the free metal ion? group of answer choices the shared electrons in the metal-ligand bonding orbitals are repulsed by the other d electrons of the metal. it requires less energy to remove an electron from the higher energy d orbitals. transition metal complexes are not very stable. binding to a ligand uses up all of the metal ion's energy. the electrons in the metal ligand bond are destabilized and the other electrons in d orbitals around the metal are stabilized.