2. A central metal atom
bonded to a group of
molecules or ions is a
metal complex.
If the complex bears a
charge, it is a complex
ion.
Compounds containing
complexes are
coordination
compounds.
3. The molecules or ions coordinating to the
metal are the ligands.
They are usually anions or polar
molecules.
4. Three categories of isomerization
1. Structural isomers: atoms connected in different
ways
1. Coordination isomers
2. Linkage isomers
2. Geometric isomers: ligands have different spatial
arrangement
1. Cis-trans isomers
2. Octahedral complex isomers
3. Optical isomers: nonsuperimposable mirror-
images (enantiomers)
8. 8
MX3Y3
Fac (facial) isomer
Three identical ligands at corners of a
triangular face of octahedron
Mer (meridian) isomer
Three identical ligands at corners of a
triangular meridian (inside octahedron)
9. Absorbs all colors-but- the one you see or
Reflects most colors but absorbs the
complimentary
10. The colors of complex ions are due to
electronic transitions between the split d
sublevel orbitals
The wavelength of maximum absorbance can
be used to determine the size of the energy
gap between the split d sublevel orbitals
Ephoton = h = hc/ =
11. The strength of the crystal field depends in
large part on the ligands
strong field ligands include: CN─ > NO2
─ > en >
NH3
weak field ligands include:
H2O > OH─ > F─ > Cl─ > Br─ > I─
crystal field strength increases as the charge
on the metal cation increases
12. The electron configuration of the metal ion with
split d orbitals depends on the strength of the
crystal field
The 4th and 5th electrons will go into the higher
energy dx2-y2 and dz2 if the field is weak and the
energy gap is small – leading to unpaired
electrons and a paramagnetic complex
The 4th thru 6th electrons will pair the electrons
in the dxy, dyz and dxz if the field is strong and
the energy gap is large – leading to paired
electrons and a diamagnetic complex
14. Because the ligand approach interacts more
strongly with the planar orbitals in the
tetrahedral geometry, their energies are raised
Most high-spin complexes
15. d8 metals
The most complex splitting pattern
Most are low-spin complexes
16. Occurs when polar molecules are attracted to
each other.
Dipole interaction happens in water
positive region of one molecule attracts the
negative region of another molecule.
17. Occur when polar molecules are attracted to
each other.
Slightly stronger than dispersion forces.
Opposites attract, but not completely hooked
like in ionic solids.
H F H F
18.
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