Inorganic Chem

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Start filling at lowest orbitals

Hunds

maximize spin

Pauli

every electron has a special quantum number configuration

Coulombic energy

destablizing energy from pairing

exchange energy

energy gained from unpaired electrons

n

principle number

l

angular momentum, can be up to n-1

l values

s=0, p=1, d=2, f=3

ml

magnetic spin- goes from negative l to l

ms

spin

Shielding

how much attraction your electron is feeling to the nucleus

Stability of half filled electrons

stabilized by the exchange energy, which encourages the promotion of the electron rather than pairing them

Nomenclature rules

1. cation before anion

2. ligands before metals

3. prefixes, is if doubled

4. alphabetical order

5. anions have -o

6. oxidation of metal

7. cis/trans prefix

8. u for bridging

9. -ate for anion ligands

Stereoisomers

same ligands, different arrangement

geometric isomers

diastereomers, look for different trans interactions

optical isomers

enantiomers, exist if you have chiral compounds, just mirror them. If they have enantiomers, there only group orbital is cn

structural/constitutional isomers

different bonding but same ligands

hydrate isomers

switches a ligand with aqua

ionization isomer

switching an ion in the ligand with an anion

coordination isomer

switchng metals for the ligand and anion, requires 2 metal ions

linkage isomer

switching the linking between ligand and metal

compounds with 2 ligands always have

cis and trans isomers

compounds with 3 ligands always have

mer and fac

mer

2 trans, 1 cis

fac

all cis

lambda

ccw

delta

clockwise

pi backbonding is

metal to ligand, the electrons come from the metal d orbitals, largest delta o

sigma bonding is

ligand to metal, ligand supplies electrons, smallest deltao

good sigma donors

low spin because they increase delta o by increasing the energy of e1g

good pi donor

high spin because they decrease delta o by raisng the energy of t2g

good pi acceptors

lo spin because they increase delta o from lowering t2g

metal oxidation state increases

delta o increases because your ligand and metal are going to bind more tightly, which causes energy orbitals to be more separated

2nd row and beyond TM

usually low spin because their d orbitals are larger, which causes a higher delta o, smaller pairing energy because there is more space and less repulsion

Compression

Stabilizes energy, the ligand is bonded more tightly

Expansion

Destabilizing energy, the ligand is bonded less tightly, pulled away

NH3 is

low spin

H2O is

high spin