Orgo Lecture

goes between antibonding orbitals.

single fill orbitals of equal energy before pairing e-

stabilizes the resonance structure.

combining multiple individual wave functions to get a new wave function for a new orbital.

promote a 2s e- to a 2p e,- creating 3 sp2 orbitals.

combining wave functions linearly to get a new wave function for the molecular orbital.

orbitals filled from lowest to highest energy level.

sharing electrons between atoms.

atoms tend to gain or lose e- to obtain noble gas configuration (8 val e)-

coulombic attraction between an e- rich and e- poor atom.

the more EN atom is more stable with (--) charge.

sharing electrons between atoms

second row elements

very reactive with compounds that have LPE

have over-filled val shell

more stable than other versions of the same compound

more than one possible lewis structure

hybrid orbitals that exist in an inbetween form rather than multiple distinct resonance forms

multiple structures or one structure with delocalized e-

and the same net charge

predict molecular geometry

LPE will stay as far from each other as possible to minimize repulsion between them

predict molecular geometry

109.5°

120°

why atoms need to come together in covalent bonds (why bonding releases energy)

schrödingers equation and wave function

combining wave functions linearly to get a new wave function for the molecular orbital

fill the MOs according to Aufbau, Pauli, and Hund

orbitals filled from lowest to highest energy level

single fill orbitals of equal energy before pairing e-

combining multiple individual wave functions to get a new wave function for a new orbital

uneven dumbell

form sigma bonds with other s orbitals (bonding if same sign, antibonding if different)

effective overlap

ineffective overlap

tetrahedral

double bond, p orbital dumbells line up (either bonding or antibonding)

single bond only

goes between antibonding orbitals