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Nodal plane
goes between antibonding orbitals.
hund
single fill orbitals of equal energy before pairing e-
Electron delocalization
stabilizes the resonance structure.
Hybridization
combining multiple individual wave functions to get a new wave function for a new orbital.
Boron can
promote a 2s e- to a 2p e,- creating 3 sp2 orbitals.
LCAO
combining wave functions linearly to get a new wave function for the molecular orbital.
Aufbau
orbitals filled from lowest to highest energy level.
Covalent bond
sharing electrons between atoms.
Octet rule
atoms tend to gain or lose e- to obtain noble gas configuration (8 val e)-
Ionic bond
coulombic attraction between an e- rich and e- poor atom.
When 2+ atoms can support formal charge
the more EN atom is more stable with (--) charge.
covalent bond
sharing electrons between atoms
octet rule mainly applies to
second row elements
BF3 is
very reactive with compounds that have LPE
PCl5 and SF5
have over-filled val shell
balanced formal charge
more stable than other versions of the same compound
resonance structures
more than one possible lewis structure
resonance structures are really
hybrid orbitals that exist in an inbetween form rather than multiple distinct resonance forms
possible resonance structures can be drawn as
multiple structures or one structure with delocalized e-
each resonance structure should have the same e
and the same net charge
lewis structure cannot
predict molecular geometry
VSEPR
LPE will stay as far from each other as possible to minimize repulsion between them
lewis structure + VSEPR can
predict molecular geometry
tetrahedral bond angle
109.5°
trigonal planar bond angle
120°
molecular orbital theory question
why atoms need to come together in covalent bonds (why bonding releases energy)
LCAO derived from
schrödingers equation and wave function
LCAO
combining wave functions linearly to get a new wave function for the molecular orbital
e
fill the MOs according to Aufbau, Pauli, and Hund
Aufbau
orbitals filled from lowest to highest energy level
hund
single fill orbitals of equal energy before pairing e-
hybridization
combining multiple individual wave functions to get a new wave function for a new orbital
sp orbital shape
uneven dumbell
sp orbital can
form sigma bonds with other s orbitals (bonding if same sign, antibonding if different)
bonding orbital
effective overlap
antibonding orbital
ineffective overlap
sp3 hybridization molecular structure
tetrahedral
pi bond
double bond, p orbital dumbells line up (either bonding or antibonding)
sigma bond
single bond only
nodal plane
goes between antibonding orbitals
Note 
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