ACDityBSCity Flashcards
What makes a more stable anion for a more acidic acid???
Electron withdrawing substituents :-)
What does basicity depend on?
Availability of lone pair of electrons for protonation
What makes lone pair of electrons on an atom more available for protonation, therefore higher basicity?
To attract the shitty H+ that likes negativity, you have to make lone pair of electrons very available for protonation- very negative. -» electron donating alkyl groups.
What does acidity depend on!
Stability of anion formed.
What do you strive for in making a strong acid??
NO NEGATIVITY.
You want to delocalise the negative charge over COO- group!!!!!
Acidity of carboxylic acids
Electron-donating groups _________ negative charge on COO- group -> ________ anion -> acid strength _________.
INTENSIFY negative charge
DESTABILISES anion
Strength REDUCED
Acidity of carboxylic acids
Electron-withdrawing groups ________ negative charge on COO- group (by _________ effect) -> ______________ anion -> acid strength __________
DISPERSE negative charge
INDUCTIVE effect
STABILISES anion
Acid strength INCREASED
Why benzoic acid stronger than aliphatic acid?
___________ of negative charge into benzene ring (_________ effect) -> benzoate ANION more stable than ethanoate anion
Delocalisation!!!
RESONANCE!!
Larger Kb value = smaller pKb value =?
Stronger base.
Larger Ka value = lower pKa value =?
Stronger acid.
Basicity
Electron-donating substituents make lone pair of electrons on atom more _________ for protonation, ________ basicity of compound
Rmb: you want them as neg as possible to attract emo H+
MORE AVAILABLE
INCREASE
Basicity
Electron-withdrawing substituents make lone pair of electrons on atom ____ ____________ for protonation, thus _________ basicity of amine.
Less available
Decrease
Bitch was made less negative, emo H+ not attracted
What makes a less stable anion for acids ; weaker acid??
Electron-donating substituents.
Acid wants to lose H+, acid cannot be negative, emo H+ loves it. Electron donating shit worsens it.
