-
acids strongest to weakest
- hydronium
- carboxylic acid
- ammonium ion
- phenols
- H20
- alcohol
- carbonyls
- sp's
- nitrogens
- sp2's
- sp3
-
-
lewis acid/lewis base
- e- pair acceptor
- e- pair donor
-
strong lewis acid
carbocations
-
the 2 definitions for acid
and for base
- acid: proton donor/e- pair acceptor
- base: proton acceptor/e- pair donor
-
gain or lose electrons
ionic bonding
-
sharing electrons
covalent bonding
-
what is electropositive?
metals
-
big enough electronegative charge different for ionic bonding
2.2
-
same formula, different structures
isomers
-
any carbon with a lone pair
carboanion
-
carbon with one unpaired e-
carbon radical
-
sp3 bond type, shape and angle degree
- single bonds
- tetrahedral
- 109.5
-
sp2 hybridized bond type, shape and angle degree
- double bond (1 sigma, 2 pi)
- trigonal planar
- 120
-
sp hybridized bond type, shape and angle degree
- triple bond (1 sigma, 4 pi)
- planar
- 90
-
location of molecule with p orbitals where there's no chance of an e- being there
nodal plane
-
which shape is there some chance of e-'s being found at the nucleus?
spherical shape(s orbitals)
-
for orbital models, which is better?
molecular orbitals over atomic orbitals
-
direction of rxn for the different values of Keq
- if larger rxn to right
- if smaller rxn to the left
-
acid/base, which is solvent, which is solute?
- acid: solute
- base: solvent
-
Ka is ignored
strong acid, gives up H+ 100%
-
conversion of pKa to Ka
- pKa = -logKa
- negative log of 10^-3=3
-
stronger acids have negative values of
pKa
-
how many electrons in the first shell?
second shell?
third shell?
fourth shell?
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