Chapter 22

• typically have incompletely filled d subshells or readily give rise to ions with incompletely filled subshells (Zn, Cd, Hg are not considered T.M.'s)
• great tendency to from complex ions
• distinctive color
• paramagnetic compounds
• catalytic activity
• trend of size change is minimal - electrons go to inner shell instead out outer

• Small size and "closest packing" crystal structure give rise to strong metallic bonds
• high densities
• high melting/boiling points
• high ^ fus/vap
• highest oxidation states occur with very electronegative atoms like F or O

• a neutral species containing one or more complex ion
• -complex ion - contains a central metal cation bonded to one or more anions or molecules with lone pairs
• [Co(NH3)6]Cl3

• the small molecules or ions attached to the central metal
• has one or more electron pair that can be donated to the metal (they are Lewis bases)

the atom in a ligand bound directly to the metal atom

the number of donor atoms around a central atom

• ligand with one donor atom
• :C---O:

ligand with two donor atoms

ligand with more than two donor atoms

bidentate and polydentate ligands (Greek chele means "claw")

• Br-
• Bromo

• Cl-
• Chloro

• ethylenediamine (en) - neutral
• oxalate ion, 2-
• ethylenediaminetetraacetate (EDTA), 4-

• 1. Cation is named before the anion, regardless of which contains complex ion
• 2. Within a complex ion the ligands are named 1st in alphabetical order then the metal
• 3. Ligands: anionic end in -o, neutral usu name of molecule,
• 4. When several ligans: di, tri, tetra, penta, hexa
• 5. If the ligand itself already has the prefix in it's name: bis, tris, tetrakis
• 6. Give the oxidation # of the metal as a Roman Numeral
• 7.If complex is is an anion, its name ends in -ate

• CN-
• Cyano

• OH-
• Hydroxo

• O-2
• Oxo

• Co3 -2
• carbonato

• NO2 -
• nitro

• NH3
• ammine

• CO
• Carbonyl

• H2O
• aqua

Aluminate

cuprate

aurate

ferrate

plumbate

argentate

stannate

tungstate

compounds that are made up of the same types and numbers of atoms bonded together in the same sequence but with different spatial arrangements

• stereoisomers that cannot be converted without breaking chemical bonds
• cis - two groups are adjacent to each other
• trans - two groups are on opposite sides of the structure

• nonsuperimposable mirror images
• "chiral" (hand) mirror immage that isn't the same
• they are OPTICALLY ACTIVE 0 they can rotate plane-plarized light
• if compound rotates it right it is "dextrorotatory" (d)
• if it rotates light left it is "levorotatory" (l)

the d and l isomers of a chiral molecule

50/50 mixture of the two enantiomers

the bonding theory used to account for the color and magnetic properties of T.M. complexes

• ^ the energy difference between two sets of d orbitals in a metal atom when ligands are present
• the size of ^ is affected by the metal and the ligand
• ^ = hc/(lambda)

• an object appears black if it absorbs all colors of white light
• an object appears white if it does not absorb any colors of white light
• an object appears green if it absorbs all colors except green light (reflecting it back to your eye) or...
• an object appears green if it absorbs only the "complimentary" color

• is a list of ligands in order of increasing ability to split the d orbital energies
• the stronger field ligands will have a larger splitting ^ and higher energy light is being absorbed