Module 2: Acids and Bases Flashcards
four main factors, in the following priority order, that affect the stability of the conjugate base
- Atom
- Resonance
- Induction
- Orbital
the acidity of H-A increases as the percent s-character of A increases
hybridization effects
measure of a compound’s affinity for a proton
basicity
Any species that is electron deficient and capable of accepting an electron also a?
lewis acid
The acidity relies on the stability of the?
conjugate base
Down the periodic table, the ___________________ determines the acidity
atomic size
acids that the net charge may be zero (+), or (-)
bronsted-lowry acids
The tendency of an acid to donate a proton
acid strength
these are more electronegative than p orbitals
s orbitals
Electron donor
lewis base
these contains a proton
all bronsted-lowry acids
this always favors formation of the weaker acid and base
equilibrium
the acidity of H-A inccreases both left-to-right across a row and down a column of the periodic table
element effects
this shows how greatly the acidity varied for different functional groups.
pKa table
this is the characteristic of a particular compound, which indicates the tendency of the compound to give up its proton.
pKa
Electron acceptor
lewis acid
the lewis acid is also called a ________________ or electron-rich
nucleophile
Proton acceptor
bronsted-lowry base
Increase the concentration of H+ions when dissolved in water
arrhenius acid
the acidity of H-A increases with the presence of electron-withdrawing groups in A
inductive effects
Increase the concentration of OH-ions when dissolved in water
arrhenius base
this is used to describe the acidity (concentration of positively charged hydrogen ions) of a solution
pH scale
The more readily the compound donates a proton, the?
stronger the acid
these contain a lone pair of electrons or a pi bond
all bronsted-lowry base
bases that the net charge may be zero or (-)
bronsted-lowry bases
The use of curved arrows to show simple proton-transfer reactions.
The Lewis Definition
Proton donor
bronsted-lowry acid
the acidity of H-A increases when the conjugate base A is resonance stabilized
resonance effects
An acid can be deprotonated by the conjugate base of any acid having a?
higher pKa
from left to right, acidity increases as the electronegativity _________________
increases
The ______________ the electronegativity, the stronger the inductive effect
stronger
Structural effects on acidity and basicity of organic molecules
The Brønsted–Lowry Definition
a lewis acid is also called an ________ or electron deficient
electrophile
the closer the electronegative atom to the hydrogen, the stronger the?
acid
this is due to differences in electronegativity (EN), the intrinsic ability of an atom to attract the shared electrons in a covalent bond
bond polarity
a weaker conjugate base means a more?
stable conjugate base
this is broader and more encompassing than the Bronsted-Lowry definition because it is not limited to substances that donate or accept protons only.
lewis definition of acids and bases
these are structurally the same as Brønsted–Lowry bases. Both have an available electron pair—a lone pair or an electron pair in a π bond.
lewis bases
measure of the tendency of a compound to give up a proton
acidity
the stronger the acid, the weaker its?
conjugate base
