Chapter 4 Study Cards

Front 1

the substance that dissolves in the solvent

Back 1

Solute

Front 2

The substance in which the solute(s) dissolve

Back 2

Solvent

Front 3

Has an uneven distribution of electron charge, polar bonds, and a bent molecular shape

Back 3

Polar molecule

Front 4

Surrounded closely by solvent molecules

Back 4

solvated

Front 5

A substance that conducts a current when dissolved in water

Back 5

electrolyte

Front 6

An aqueous solution that does not conduct an electric current

Back 6

nonelectrolyte

Front 7

The quantity of solute dissolved in a given quantity of solution (or of solvent).

Back 7

concentration

Front 8

most common unit of concentration... expressed as the moles of solute dissolved in 1 L of solution

M = (mol solute) / (L soln)

Back 8

Molarity (M)

Front 9

A chemical equation showing a reaction in solution in which reactants and products appear as intact, undissociated compounds

Back 9

molecular equation

Front 10

An equation for an aqueous reaction that shows all the soluble ionic substances dissociated into ions.

Back 10

total ionic equation

Front 11

An ion that is present as part of a reactant but is not involved in the chemical change.

Back 11

spectator ion

Front 12

A chemical equation of a reaction in solution in which spectator ions have been eliminated to show the actual chemical change.

Back 12

net ionic equation

Front 13

A reaction in which two soluble ionic compounds form an insoluble product, a precipitate.

Back 13

precipitation reaction

Front 14

The insoluble product of a precipitation reaction.

Back 14

precipitate

Front 15

A reaction in which atoms or ions of two compounds exchange bonding partners. Precipitation and acid-base reactions are examples.

Back 15

metathesis reaction aka double displacement reaction

Front 16

Any reaction between an acid and a base. An acid-base reaction that yields water and a solution of a salt; when the H+ ions of a strong acid react with an equivalent amount of the OH- ions of a strong base, the solution is neutral.

Back 16

acid-base (neutralization) reaction

Front 17

Any species that produces H+ ions when dissolved in water.

Back 17

acid

Front 18

Any species that produces OH- ions when dissolved in water.

Back 18

base

Front 19

An ionic compound that results from an Arrhenius acid-base reaction after solvent is removed.

Back 19

salt

Front 20

A method of determining the concentration of a solution by monitoring relative amounts during its reaction with a solution of known concentration.

Back 20

titration

Front 21

The point in a titration when the number of moles of the added species is stoichiometrically equivalent to the original number of moles of the other species.

Back 21

equivalence point

Front 22

The point in a titration at which the indicator changes color caused by a tiny excess of OH- ions.

Back 22

end point

Front 23

A process in which there is a net movement of electrons from one reactant (reducing agent) to another (oxidizing agent).

Back 23

oxidation-reduction (redox) reaction

Front 24

The loss of electrons by a species, accompanied by an increase in oxidation number.

Back 24

oxidation

Front 25

The gain of electrons by a species, accompanied by a decrease in oxidation number.

Back 25

reduction

Front 26

The substance that accepts electrons in a reaction and undergoes a decrease in oxidation number.

Back 26

oxidizing agent

Front 27

The substance that donates electrons in a redox reaction and undergoes an increase in oxidation number.

Back 27

reducing agent

Front 28

A number equal to the magnitude of the charge an atom would have if its shared electrons were held completely by the atom that attracts them more strongly.

Back 28

oxidation number (O.N.) or (oxidation state)

Front 29

A listing of metals arranged in order of decreasing strength of the metal as a reducing agent in aqueous reactions.

Back 29

activity series of the metals

Front 30

The condition at which the forward and reverse reactions are taking place at the same rate, so there is no net change in the amounts of reactants or products.

Back 30

dynamic equilibrium

Front 31

List strong acids:

Back 31

Hydrochloric acid, HCl
Hydrobromic acid, HBr

Hydriodic acid, HI

Nitric acid, HNO₃

Sulfuric acid, H₂SO₄

Perchloric acid, HClO₄

Front 32

List strong bases:

Back 32

Group 1A (1) hydroxides:

Lithium hydroxide, LiOH

Sodium hydroxide, NaOH

Potassium hydroxide, KOH

Rubidium hydroxide, RbOH

Cesium hydroxide, CsOH

Heavy Group 2A (2) hydroxides:
Calcium hydroxide, Ca(OH)₂

Strontium hydroxide, Sr(OH)₂
Barium hydroxide, Ba(OH)

Front 33

List weak acids:

Back 33

Hydrofluoric acid, HF

Phosphoric acid, H₃PO₄

Acetic acid, CH₃COOH

(three of many)

Front 34

List weak bases

Back 34

Ammonia, NH3

(one of many)

Front 35

These types of acids and bases dissociate very little into ions...

Back 35

WEAK acids and bases

Front 36

These types of acids and bases dissociate completely into ions...

Back 36

STRONG acids and bases