Ch. 10: Acids and Bases (Complete) Flashcards
defn: Arrhenius acid vs. base
Arrhenius acid: will dissociate to form an excess of H+ in solution
Arrhenius base: will dissociate to form excess of OH- in solution
what types of substance are Arrhenius acids typically limited to?
aqueous acids and bases
what is the pattern for identifying Arrhenius acids? Give 3 common.
contain H at the beginning of their formula
HCl, HNO3, H2SO4
what is the pattern for identifying Arrhenius bases? Give 3 common.
contain OH at the end of their formula
NaOH, Ca(OH)2, Fe(OH)3
defn: Bronsted-Lowry acid vs. base
Bronsted-Lowry acid = a species that donates hydrogen ions (H+)
Bronsted-Lowry base = a species that accepts hydrogen ions
what is the advantage of the Bronsted-Lowry definition over the Arrhenius definition?
Bronsted-Lowry is not limited to aqueous solutions
will most acid-base chemistry reactions on the MCAT work in accordance with the Arrhenius definition or the Bronsted-Lowry definition?
Bronsted-Lowry
why do Bronsted-Lowry acids and bases always occur in pairs? what are these paired referred to as?
the definitions require the transfer of a proton from the acid to the base
referred to as conjugate acid-base pairs
defn: Lewis acid vs. base
Lewis acid: an electron pair acceptor
Lewis base: an electron pair donor
what type of electron pair is transferred in Lewis acid base chemistry?
a lone pair that is not involved in any other bonds
mnemonic: Bronsted Lowry vs. Lewis definitions
the brOnsted lOwry definition revolves around prOtOns
the lEwis definition around ElEctrons
what is the main idea behind what is going on in Lewis acid-base chemistry?
one species pushes a lone pair to form a bond with another
what are three alternative names/scenarios that are equivalent to Lewis acid-base chemistry?
- coordinate covalent bond formation
- complex ion formation
- nucleophile-electrophile interactions
which definition of acids and bases is the most inclusive?
lewis definition
why may we see lewis acids a lot in orgo?
lewis acids are often used as catalysts
defn: amphoteric species
one that reacts like an acid in a basic environment and like a base in an acidic environment
defn: amphiprotic
a substance that can either gain or lose a proton
what is the most common example of an amphoteric species on the MCAT?
water!
explain how water acts as an amphoteric species (how does it react with a base? how does it react with an acid?
what four categories of substances are usually considered amphoteric?
- the partially dissociated conjugate base of a polyvalent acid
- the hydroxides of certain metals
- species that can act as both oxidizing and reducing agents
- amino acids that have a zwitterion intermediate with both cationic and anionic character
nomenclature: acids formed from anions with names that end in -ide
prefix: hydro-
ending: -ic
name + nomenclature: acids formed with oxyanions
name: oxyacids
anion ends in -ite (less oxygen) –> acid ends in -ous acid
anion ends in -ate (more oxygen) –> acids ends in -ic acid
why is it so important to understand the behavior of acidic and basic compounds in water?
because many acid-base reactions take place in water, especially on the MCAT
defn + eqn + process: autoionization of water
water can react with itself
one water molecule donates a hydrogen ion to another water molecule to produce the hydronium ion (H3O+) and the hydroxide ion (OH-)