Chapter 6 Flashcards
acid
A substance that increases the concentration of H+ when added to water.
acidic solution
One in which the activity of H+ is greater than the activity of OH-
amine
A compound with the general formula RNH2, R2NH, or R3N, where R is any group of atoms.
ammonium ion
The ammonium ion is NH4+. An ammonium ion is any ion of the type RNH3+, R2NH2+, R3NH+, or R4N+, where R is an organic substituent.
aprotic solvent
One that cannot donate protons (hydrogen ions) in an acid-base reaction.
autoprotolysis
The reaction in which two molecules of the same species transfer a proton from one to the other.
base
A substance that decreases the concentration of H+ when added to water.
basic solution
One in which the activity of OH- is greater than the activity of H+.
Bronsted-Lowry acid
A proton donor.
Bronsted-Lowry base
A proton acceptor.
carboxylate anion
Conjugate base (RCO2-) of a carboxylic acid.
common ion effect
Occurs when a salt is dissolved in a solution already containing one of the ions of the salt. The salt is less soluble than it would be in a solution without that extra ion. An application of Le Chatelier’s principle.
complex ion
Historical name for any ion containing two or more ions or molecules that are each stable by themselves.
conjugate acid-base pair
An acid and a base that differ only through the gain or loss of a single proton.
coprecipitation
Occurs when a substance whose solubility is not exceeded precipitates along with one whose solubility is exceeded.
disproportionation
A reaction in which an element in one oxidation state gives products containing that element in both high and low oxidation states.
endothermic reaction
One for which deltaH is positive; heat must be supplied to reactants for them to react.
enthalpy change
The heat absorbed or released when a reaction occurs at constant pressure.
entropy
A measure of the disorder of a substance.
exothermic reaction
One for which deltaH is negative; heat is liberated when products are formed.
hydronium ion
H3O+; What we really mean when we write H+.
ion pair
A closely associated anion and cation, held together by electrostatic attraction. In solvents less polar than water, ions are usually found as ion pairs.
Le Chatelier’s principle
If a system at equilibrium is disturbed, the direction in which it proceeds back to equilibrium is such that the disturbance is partly offset.
Lewis acid
One that can form a chemical bond by sharing a pair of electrons donated by another species.
Lewis base
One that can form a chemical bond by sharing a pair of its electrons with another species.
ligand
An atom or a group attached to a central atom in a molecule. The term is often used to mean any group attached to anything else of interest.
neutralization
Process in which a stoichiometric equivalent of acid is added to a base (or vice versa).
polyprotic acid or base
Compound that can donate or accept more than one proton.
protic solvent
One with an acidic hydrogen atom.
salt
An ionic solid.
saturated solution
One that contains the maximum amount of a compound that can dissolve at equilibrium.
standard state
The standard state of a solute is 1 M and the standard state of a gas is 1 bar. Pure solids and liquids are considered to be in their standard states. In equilibrium constants, dimensionless concentrations are expressed as a ratio of the concentration of each species to its concentration in its standard state.
