1. Transition Metals Their Coordination Compounds & Isomers
AP Notes Chapter 22
Transition Metals Their Coordination Compounds & Isomers

2. Transition Elements
Metals capable of taking on multiple oxidation numbers.
Exist in 3 series 1st the 3d 2nd the 4d and the 3rd 5d
The 2nd and 3rd series are almost identical in radii size due to the 4f and 5f orbitals, the addition of these 14 protons and little shielding effect cause the similarity in size this is called the lanthanide contraction.

3. Transition Elements
Atomic Radii decrease from left to right, with a slight increase at the right end.
As Nuclear charge increases the s outer electrons are pulled closer initially making the atom smaller, near the end increased electron repulsion causes the slight increase.

4. Coordination Compounds or complex ions
Usually consist of a transition metal and the attraction of a unit called a Ligand with a coordinate covalent bond.
They take on a 3-D shape, those shapes or geometries use the naming methods you already know….and then add to them
Common coordination numbers are 2,4,and 6 they are associated with geometries linear, tetrahedral, square planar and octahedral.

5. Coordination Compounds
Linear – [CuCl2]- , [Ag(NH3)2]+
Tetrahedral – [CoCl4]2- , [NiCl4]2-
[Ni(CO)4] , [Zn(NH3)4]2+
Square Planar – [Ni(CN)4]2-
Octahedral – Fe(H2O)6]2+ , [Co(NH3)6]3+

6. Coordination Compounds
Monodentate - Ligands with one lone pair of electrons to donate
Polydentate – Ligands that have more than one lone pair to danate, often on different atoms (one bite)
Chelate ring – a polydentate ligand that coordinate bonds to the same atom (two bites)

7. Transition Elements
Melting Points increase toward the center of each series where the d orbital is about half-filled, where the largest number of unpaired electrons exist.
These metals can be isolated or extracted from ore by processes we call metallurgy
Pyrometallurgy – involves high temperatures
Hydrometallurgy – involves aqueous solutions

8. Isomerization Flow Chart
Isomers
Structural or Constitutional
(Different Bonds or connectivity)
Stereoisomerism
(Different arrangement same connectivity)
Geometric or Achiral
(Without stereocenters)
Optical or Chiral
(With stereocenters)
Coordination
(Different Bonds)
Cis-
(Same side)
Trans-
(Opposite side)
Linkage
(Different Connectivity)
Enantiomers
(Mirror images
Non-superimposible)
Diastereoisomer
(Non-mirror images)

9. Constitutional isomers: compounds that have the same molecular formula but different structural formulas (connected differently)

10. Cis- or Trans- isomers:
because of restricted rotation about a carbon-carbon double bond, an alkene with two different groups on each carbon of the double bond shows cis-trans isomerism

11. Crystal Field Theory
All the d orbitals are equal in energy they are said to be degenerate
Atomic bond theory and molecular orbital theory cannot explain many complexes and their behavior or bonding
The electrostatic field or ligand field exists when the atom or ion is approached by a legand.
Electrons lose degeneracy and are pushed into higher and lower spins split by energy

12. Crystal Field Theory Fe2+ has d6 electron configuration
Fe2+ [Fe(H2O)6]2+ [Fe(CN)6]4-
weak field strong field
high spin low spin DE

13. Colors & Coordination Componds
Transition metal complexes absorb light causing electrons to move from low to high energy levels.
The energy difference corresponds to a frequency in the visible portion of the spectrum … they appeared colored
Electron transition in the d orbital is responsible for this color
Changes in the splitting of the d orbital changes the observed color
Ligands ordered in ability to split d i.e. how strong the ligands are, ordering = spectrochemical series