Answer: It points directly at the four ligands (sigma interaction); the other d orbitals are less directly aligned with ligands.
- A It points directly at the four ligands (sigma interaction); the other d orbitals are less directly aligned with ligands
- B It generally happens to contain more electrons than the other four d orbitals combined according to most researchers
- C The d<sup>8</sup> electron configuration is said to fill this particular orbital last by convention in the majority of cases studied
- D The four surrounding ligands are positioned specifically so as to avoid this orbital largely as widely reported in standard practice
Correct answer: A. It points directly at the four ligands (sigma interaction); the other d orbitals are less directly aligned with ligands
Explanation: In square planar geometry, dx2-y2 is destabilised most strongly as it lies in the xy plane pointing at all four ligands; dz<sup>2</sup> is intermediate; dxy is next; dxz and dyz are lowest.
The three common coordination geometries: octahedral (6 ligands), tetrahedral (4 ligands), and square planar (4 ligands in one plane).
Concept context
Study of compounds where a central metal atom is bonded to surrounding ligands. Covers nomenclature, types of isomerism, bonding theories (VBT, CFT), and applications in medicine, photography, and industry.