Acids and Bases
Bronsted Lowry = protons
Lewis = electrons
Lewis is more broad (bc/ all reactions involve electron movement)
Conjugate acid vs. conjugate base -> different forms of the same molecule
H3O+ <—-> H2O
Quantum Numbers
n, l, ml, ms
l = s, p, d, f, g…
l for s = 0, l for p = 1, l for d = 2…
ml is which orbital are you talking aobut
ml for s = 1 total
ml for p = 3 total (ml = -1, 0, 1)
ml for d = 5 total (ml = -2, -1, 0, 1, 2)
…
Magnetism
-paramagnetism involves at least one unpaired electron
-Ferromagnetism involves unpaired electrons
-ferromagnetic materials become permanent magnets when exposed to a magnetic field
Ionizing Atoms
Take Atoms from the higher energy level (n)
e.g. from Fe -> Fe2+
take two electrons from 4s2, despite 3d being a higher energy level
Exceptions
atoms want to fill the d suborbital
Effective Nuclear Charge
-basically, effective nuclear charge is the amount force from the nucleus experienced by each individual valence electron
-core electrons cancel out the protons
Hybridization
-to determine hybridization of an atom in a molecule: determine the number of domains (steric number)
1 domain = s hybridization
2 domains = sp hybridization
3 domains = sp2 hybridization
4 domains = sp3 hybridization
-if you have a lone pair on an atom, and that lone pair can contribute to resonance, then that lone pair is placed in a p orbital and the atom is sp2
Molecular Orbital Theory
Bonding order = 1/2(bonding MO e- – antibonding MO e-)
= 1/2(# of e- between the two atoms)
Lewis Structures
Least electronegative atom = central atom
VSEPR
Nomenclature
Strong Acids and Bases
Flame Test
