CHEM H90 Lecture Notes - Lecture 20: Transition Metal, Octet Rule, Diamagnetism
Inorganic Chemistry
• periodic table
o d-orbitals
o lanthanides and actinides
• what makes metals so special?
o metals can have many oxidation states
▪ ex. chlorine, a non metal, is always Cl1-
▪ ex. iron, a transition metal, can be Fe1+, Fe2+, Fe3+
▪ allows for exciting reactions
o can have unpaired electrons
o can be magnetic
o come in many shapes and sizes and exhibit a large range of reactivity
o can make up to ~9 bonds
▪ don't obey octet rule
o play important biological roles
• d orbitals – transition metals
o 5 d orbitals
o fit 10 electrons
o 2 electrons per orbital
o orbitals are equal in energy
o creates degeneracy
o orbitals can split in multiple ways
o allows for interesting molecular shapes
• magnetism
o paramagnetic: element has unpaired electrons
▪ attracted to a magnetic field (magnetic)
o diamagnetic: all electrons are paired
▪ repelled by a magnetic field
• lanthanides and actinides
o f orbitals – rare earth metals
▪ 7 of orbitals
▪ fit 14 electrons
▪ 2 electrons per orbital
▪ split similarly to d orbitals
o metals make interesting complexes
▪ complex = ligands (primarily carbon based – organic) + metal center
o lanthanides have lots of unpaired electrons
▪ make strong magnets
o why study lanthanides?
▪ at this point, most of the periodic table is reasonably understood
▪ lanthanides and actinides were some of the most recently discovered
elements, so naturally, they are the LEAST understood
▪ so what do they do in the Evans lab
• make new molecules and do things with them
• see what they react with and what they make
o working with lanthanides
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