Chem 20A

coordination complex 

metal + ligands, could be cation, neutral, or anion

Ligands

electron pair donor to central metal ion

coordination number

number of dative bonds (coordination covalent bonds)

oxidation number

charge of metal cation

crystal field theory

explains why complexes have different colors and different numbers of unpaired electrons

assumptions 

ligands behave like negatively charged spheres

spectrochemical series: weak field ligands

smaller splitting, absorbs longer wavelength

spectrochemical series: strong field ligands

bigger splitting, absorbs shorter wavelength

low-spin complexes

formed by strong field lignads, e will pair up in lower level first

high spin complexes 

formed by weak field lignands, e will fill all orbitals before pairing up

crystal field stabilization energy

energy difference between e in ligand field and those in spherical crystal field

polarizability

larger molecules are more polarizable (squisher) → stronger intermolecular force

increase in temp means

inc in vapor pressure

the stronger a liquid’s IMF

the lower its vapor pressure

greater numbers of electrons in a molecule means

stronger IMF, greater molar mass, lower vapor pressure, higher boiling point

higher the IMF or interatomic force means

higher boiling/melting point, lower water vapor and volatility