1. Pengantar Kimia Koordinasi
Kimia Anorganik II

22. COMPOUNDS
NOMENCLATURE
[Co(NH3)3(NO2)3]
Triamintrinitrokobalt (III)
[Pt(NH3)2Cl2]
Diamindikloroplatina (II)
[Ni(DMG)2]
Bisdimetilglioksimatonikel (II)
[Cr(NH3)6](NO3)3
Heksaminkromium (III) nitrat
[Co(NH3)5H2O]Cl3
Akuopentaminkobalt (III) klorida
[Pt(NH3)4NO2Cl](SO4)2
Tetraminkloronitroplatina (IV) sulfat
K3[Al(C2O4)3]
Kalium trioksalatoaluminat (III)
NH4[Cr(NH3)2(NCS)4]
Ammonium diamintetratiosianatokromat (III)
Ca2[Fe(CN)6]
Kalsium heksasianoferrat (II)

40. d-Orbitals and Ligand Interaction (Octahedral Field)
Ligands approach metal
d-orbitals pointing directly at axis are affected most by electrostatic interaction
d-orbitals not pointing directly at axis are least affected (stabilized) by electrostatic interaction

41. The six negative charges are equally distributed
in a sphere around the metal

42. Crystal Field Theory (CFT)
6Dq = 0.6 o 4Dq = 0.4 o

43. High Spin Vs. Low Spin (d1 to d10)
Electron Configuration for Octahedral complexes of metal ion having d1 to d10 configuration [M(H2O)6]+n.
Only the d4 through d7 cases have both high-spin and low spin configuration.
Electron configurations for octahedral complexes of metal ions having from d1 to d10 configurations. Only the d4 through d7 cases have both high-spin and low-spin configurations.

44. CFSE (Crystal Field Stabilization Energy)
Octahedral complexes, weak field ligand, high spin complexes n
Konfiguration
Unpair electron
CFSE 1 2 3 4 5 6 7 8 9 10
t2g1
t2g2
t2g3
t2g3 eg1
t2g3 eg2
t2g4 eg2
t2g5 eg2
t2g6 eg2
t2g6 eg3
t2g6 eg4
-4Dq
-8Dq
-12Dq
-6Dq
0Dq
-4Dq + P
-8Dq + 2P
-12Dq + 3P
-6Dq + 4P
0Dq + 5P

45. Octahedral, Tetrahedral & Square Planar
dz2
dx2-y2
dxz
dxy
dyz
CF Splitting pattern for various molecular geometry
dxz
dz2
dx2-y2
dxy
dyz
dx2-y2
dz2
dxz
dxy
dyz
Octahedral
Tetrahedral
Square planar
Mostly d8
(Majority Low spin)
Strong field ligands
i.e., Pd2+, Pt2+, Ir+, Au3+
Pairing energy Vs. 
Weak field  < Pe
Strong field  > Pe
Small   High Spin

46. Color Absorption of Co3+ Complexes
The Colors of Some Complexes of the Co3+ Ion
Complex Ion Wavelength of Color of Light Color of Complex
light absorbed Absorbed
[CoF6] (nm) Red Green
[Co(C2O4)3] , 420 Yellow, violet Dark green
[Co(H2O)6] , 400 Yellow, violet Blue-green
[Co(NH3)6] , 340 Blue, violet Yellow-orange
[Co(en)3] , 340 Blue, ultraviolet Yellow-orange
[Co(CN)6] Ultraviolet Pale Yellow
The complex with fluoride ion, [CoF6]3+, is high spin and has one absorption band. The other complexes are low spin and have two absorption bands. In all but one case, one of these absorptions is in the visible region of the spectrum. The wavelengths refer to the center of that absorption band.

47. Colors & How We Perceive it
650
580
800
560
400
Artist color wheel
showing the colors which
are complementary to one
another and the wavelength
range of each color.
430
490

48. Black & White When a sample absorbs light, what we see is the sum
of the remaining colors that strikes our eyes.
If a sample absorbs all wavelength of visible light, none reaches our eyes from that sample. Consequently, it appears black.
If the sample absorbs no
visible light, it is white
or colorless.

49. Absorption and Reflection
If the sample absorbs
all but orange, the
sample appears orange.
750
430
650
580
560
490
400
Further, we also perceive orange color when visible light of all colors except blue strikes our eyes. In a complementary fashion, if the sample absorbed only orange, it would appear blue; blue and orange are said to be complementary colors.

50. Light absorption Properties of Metal Complexes
Recording the absorption Spectrum

51. Complex Influence on Color
Compounds of Transition metal complexes solution.
800
430
650
580
560
490
400
[Fe(H2O)6]3+
[Ni(H2O)6]2+
[Zn(H2O)6]2+
[Co(H2O)6]2+
[Cu(H2O)6]2+

52. Determine the field strength by measuring absorbed energy
Spectrophotometry method
Absorbancy
wavelength
 max
Absorded energy is energy used for exitation or the electrons from t2g to tg

53. TEORI ORBITAL MOLEKUL
Graphically these two orbitals look like this:

54. Constructive
Overlap
of two 1s orbitals
Destructive
Overlap of two
1s orbitals

55. Bonding orbital Anti-bonding orbital
Lower energy Higher energy
Stable Unstable
Favorable for electrons Unfavorable for electrons
Electrons exist between nuclei Electrons exist outside

56. Energetically, the molecular orbitals split.
The 1s lies lower in energy.
The 1s* is higher in energy.

57. The head-on overlap of two corresponding p atomic orbitals on different atoms, such as 2px with 2px, produces:
bonding orbital
antibonding orbital

58. Graphically, these orbitals look like this:

59. Graphically these orbitals look like this:

60. N N
7 electrons + 7 electrons

61. Orbital Molekul [Co(NH3)6]3+

62. Orbital Molekul [CoF6]3-