Chapter 2 Book Flashcards
Bronsted Lowry Acid
Proton Donors
Bronsted Lowry Acid
Accepts protons
Lewis Acid
Electron pair acceptor
Lewis Base
Electron pair donors
Why can some compounds be both acid and bases
They have H and lone pairs
Is HBr and Acid or Base
Acid
IS NH3 an acid or base
Acid
IS (CH3)3CO- an acid or base
base
Reaction of Acid and Bases
HA+B=A-+HB+
Transfer Proton
Proton transfer reactions
What is the conjugate acid of CH3O-
CH3OH
What is the conjugate base of NH3
NH2-
What is Acid Strength
tendency to donate proton
What makes a compound more acidic when looking at Ka?
large Ka=stronger
What makes a compound more acidic when looking at pKa?
Smaller pKa is stronger
How do you find pKa from Ka?
- log which cancels out the base 10 so pKa is the positive exponent of Ka
If you have a strong acid what is the conjugate base strength?
Weak
If you have a strong Base what is the conjugate acid strength?
Weak
What side does equilibrium favor
the weaker acid and base
Element in same row which will be more acidic
acidity increases across periodic table as electronegativity increases
What how is acidity affected going down column of periodic table
As you go down the periodic table acidity increases because the size of the atom increases
inductive effect
electron deficent carbon pulls electron density through sigma bonds from negatively charged atoms
How does inductive effect effect acidity
More electronegative atoms more than C means more acidity as well that it is closers to each other
How does resonance effect acidity?
delocalization increases acidity due to base being stablilized
