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| Properties of Transition Metals |
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Colored compounds
Magnetic Properties
Catalytic Properties |
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| Most common oxidation numbers for transition metals |
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Definition
+2 and +3, max is +7 for MN
! tend to be higher when joined with electronegative nonmetals |
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| an atom with incompletely filled D-orbitals |
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| Electron configuration of Cr |
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| Electron configuration of Cu |
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| Number of nearest-neighbor atoms in a crystal or the number of donor ligands that surround a central metal ion in a complex |
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| prefix for 2 in coordination complexes |
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| Alphabetical, but ignore prefixes |
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| Transition metal in naming coordination complexes |
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Definition
always at the end of the complex followed by the roman numeral for its oxidation number;
When complex is the anion of the compound, metal edning is changed to -ate; iron and copper go to the latin ferrate and cuprate |
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Definition
Ethylenediamine; H2N-CH2-CH2-NH2
Since en already has a prefix in its name, we use Bis, Tris and Tetrakis when there are 2, 3 or 4 of them in the compound.
Also, en should be written in with parentheses surrounding it, to help distinguish it from the rest of the complex |
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| Geometry of most common coordination numbers |
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Definition
#2 - linear
#4 - square planar or tetrahedral
#6 - octahedral (the most common type) |
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I- < Br- < Cl- < F- < OH- < H2O < C2O4 2- < NH3 < en < NO2 - < CN
Oversimplification for use on test H2O and lower are the weak field ligands and NH3 and greater are strong field ligands |
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Complex with weak field ligands, so the energy gap is smaller.
!nearly all tetrahedral complexes are high spin
Octahedral crystal field diagram -
___ ___
___ ___ ___
Tetrahedral Crystal Field Diagram
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Square Planar Crystal Field Diagram
(not in notes) |
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Coordination complex where the metal ligands are joined to strong field ligands, there is a larger energy gap
Octahedral Crystal Theory Complex
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Tetrahedral Crystal-Field Digram
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| A greater total spin state usually makes the resulting atom more stable. Accordingly, it can be taken that if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs. |
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| orbitals are filled in both the top and bottom, there is little-to-no magnetism |
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| Orbitals are filled more so one level, there is magnetism |
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| Color and coordination chemistry |
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Definition
| Created when an electron absorbs light and goes up an energy level. Whatever the wavelength absorbed, the compound expresses the complimentary color of the color associated with that wavelength. |
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800nm - Red - 650nm - Orange - 600nm - Yellow - 560nm - Green - 490nm - Blue - 430nm - Violet - 400nm
!nano = 10x-9 |
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| Energy and wavelength absorption |
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Definition
DeltaE = h * c / (lambda)
h is 6.63e-34 J/s
c is 3e8 m/s |
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Definition
Molecular compounds with the same molecular formula but different structural formula
2 types: strctural and stereoisomers; of stereioisomers, there are geometric and optical |
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| 4 types of geometric isomers |
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Definition
Ionization isomer - atoms switching places to create an overall charge
Hydrate isomers - a special case of an ionization isomer where water moves
Coordination isomers - when the metal ion switches ligands
linkage isomer - the element the ligand is attached by changes |
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Definition
| the same ligands are on the same side |
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| The same ligands are opposite of eachother |
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| Stabilization and destabilization |
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Definition
___ ___ Destabilized e*3/5)Delta
___ ____ ___ Stabilized e*(2/5)Delta
e*(2/5)Delta - e*(3/5)Delta |
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| How many geometric isomers are possible for a octahedral complex with the structure MA4B2 or MA4BC? |
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| Can tetrahedral complexes have geometric isomers? |
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| No, everything is adjacent |
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| How many isomers can square planar complexes have if they are MA2B2 or MA2BC |
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| Spin based on d orbital configuration |
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d1 - d3: all electrons in lower energy orbitals - low spin
d8 - d10: Lower is completely full and upper is filled according to Hund's rule - high spin
d4-d7: low or high spin based on ligands |
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