Chapter 17 Flashcards
(23 cards)
proton donor
acid
proton acceptor
base
proton transfer
acid/base reaction
what remains of the acid after it donates a proton
conjugate base
species formed when the base accepts a proton
conjugate acid
- strength of the H-X bond
- polarity of the H-X bond
2 factors that influence which acid undergoes ionization
hydrogen and nonmetal
binary acids
binary acids formed between hydrogen and halogens
hydrohalic acids
contain hydrogen, oxygen, and a central nonmetal (X)
- contain one or more O-H bonds
Oxoacids
organic acids with the structure
carboxylic acids
water can as act as either acid or base
- acts as a very weak electrolyte
-autoionization
Is an a amphoteric
can ionize by itself
auto ionization
ionize only to a limited extent in water
weak acids
similar treatment as for weak acids
Weak bases
undergo series of ionizations
Diprotic and polyprotic acids
sequential loss of protons by a polyprotic acid
-one proton at a time
stepwise ionization
the resulting anions and cations can all act like acids or bases
when salts dissociate in solution
depends on the relative strengths of the conjugate acid and base
pH
substance that can donate a pair of electrons
- must contain 1 or more lone pairs of e-
Lewis base
substance that can accept a pair of electrons
- contains incomplete valence shell, or multiple bonds that can shift to make room for lone pair
Lewis acid
is one that involves the donation of a pair of electrons form one species to another (formation of coordinate covalent bonds)
A lewis acid-base reaction
(those with empty orbitals are available to accept electrons) are Lewis acids
hydrated metals
(those with less than an octet of electrons) are lewis acids
electron-deficient molecules
