CHEM-002 Lecture Notes - Lecture 27: Square Planar Molecular Geometry, Ethylenediamine, Ammonia

• School: Georgetown University
• Department: Chemistry
• Course: CHEM-002
• Professor: Dedios Angel

Document Summary

X2-y(cid:1006) a(cid:374)d z(cid:1006) ha(cid:448)e highe(cid:396) e(cid:374)e(cid:396)gy (cid:271)e(cid:272)ause they"(cid:396)e i(cid:374) li(cid:374)e (cid:449)ith the liga(cid:374)ds. The diffe(cid:396)e(cid:374)(cid:272)e between these and dxy/dxz/dyz is the splitting difference. As lo(cid:374)g as (cid:449)e do(cid:374)"t ha(cid:448)e (cid:1005)(cid:1004) ele(cid:272)t(cid:396)o(cid:374)s i(cid:374) the oute(cid:396)(cid:373)ost d o(cid:396)(cid:271)ital, the o(cid:396)(cid:271)itals i(cid:374) d a(cid:396)e (cid:374)ot goi(cid:374)g to be filled u(cid:374)less it"s z(cid:374)(cid:1006)+, cd(cid:1006)+, a(cid:374)d hg(cid:1006)+ If the splitting is small, the d orbitals are filled before pairing. If the splitting is large, they pair in the dxy/dxz/dyz before filling the x2-y2 and z2. Diamagnetic pair before filling the higher energy d orbitals. We can observe this experimentally by seeing how they react to a magnet. Negati(cid:448)ely (cid:272)ha(cid:396)ged liga(cid:374)ds ha(cid:448)e a s(cid:373)alle(cid:396) splitti(cid:374)g the(cid:374) (cid:374)eut(cid:396)al o(cid:374)es. It"s depe(cid:374)de(cid:374)t o(cid:374) the ligand, not on the metal we need to memorize this in the book as well. The reason some ligands can split and others cant is because of the shape of the ligand.