The flashcards below were created by user
on FreezingBlue Flashcards.
acids strongest to weakest
- carboxylic acid
- ammonium ion
lewis acid/lewis base
- e- pair acceptor
- e- pair donor
strong lewis acid
the 2 definitions for acid
and for base
- acid: proton donor/e- pair acceptor
- base: proton acceptor/e- pair donor
gain or lose electrons
what is electropositive?
big enough electronegative charge different for ionic bonding
same formula, different structures
any carbon with a lone pair
carbon with one unpaired e-
sp3 bond type, shape and angle degree
- single bonds
sp2 hybridized bond type, shape and angle degree
- double bond (1 sigma, 2 pi)
- trigonal planar
sp hybridized bond type, shape and angle degree
- triple bond (1 sigma, 4 pi)
location of molecule with p orbitals where there's no chance of an e- being there
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
how many electrons in the first shell?