Chapter 4 rxns in aqueous solutions

Question 1

solution

Answer 1

homogeneous misture of 2 or more substances

Question 2

solvent

Answer 2

substance with greatest quantity

Question 3

solute

Answer 3

other substance, dissolved in the solvent

Question 4

electrolyte

Answer 4

a substance whose aq solution contains ions

Question 5

nonelectrolte

Answer 5

does no form ions in solutioon

Question 6

solvation

Answer 6

helps stabilize the ions in solution and prevents cations and anions from recombing

Question 7

strong electrolytes

Answer 7

those solutes that exist in solution completely or nearly completely as ions

Question 8

weak electolytes

Answer 8

those solutes that exist in solution mostly in the form of neutral molecules with onlu a small fraction in the form of ions

Question 9

chemical equillibrium

Answer 9

relative number of each type of ion or molecule in the rxn is constant over time

Question 10

->

Answer 10

represents ionization of strong electrolytes.

water soluable ionic cmpds are strong electrolytes

Question 11

precipitation rxns

Answer 11

rxns that result in the formation of an insoluable product

Question 12

solubility

Answer 12

the amount of the substance that can be dissolved in a given amount of solvent

Question 13

exchange (metathesis) rxns

Answer 13

rxn in which cations and anions appear to exchange partners.

have to check solubilities, for precip to occur, 1 product must be insoluable in water

Question 14

complete ionic equation

Answer 14

all soluble strong electrolytes shown as ions

Question 15

spectator ions

Answer 15

plays no direct role in the rxn, are exactly the same on both sides of the equation

Question 16

net ionic equation

Answer 16

includes only ions and molecules directly invovled in the rxn. the sum of the ionic charges must be the same on both sides of the balanced net ionic equation.
steps on p 123

Question 17

acids

Answer 17

substances that ionize in aq solutions to form H ions. Proton donors

Question 18

bases

Answer 18

substances that accept (react with) H ions. produce OH- ions with dissolved in water

Question 19

neutralization rxns

Answer 19

when a soluton of an acid and a solution of a base are mixed

Question 20

salt

Answer 20

any ionic compound whose cations comes from a base

Question 21

redox rxn

Answer 21

electrons are transferred from one reactant to another

Question 22

oxidation

Answer 22

loss of elctrons, becomse + charged

Question 23

reduction

Answer 23

gain of electrons, becomes - charged

when one substance is oxidized, another must be reduced

Question 24

oxidation #s rules

Answer 24

1. for an atom in its elemental form, the oxidation # is always 0.
2. for any monatomic ion the oxidation # = the ionic charge
3. nonmetals usually have negative oxidation numbers, although they can sometimes be positive.
   - the oxidation # of oxygen is usually -2. EXCEPT peroxides O2, oxidation # is -1
   - oxidation # of H is +1 when bonded to nonmetals and -1 when bonded to metals
   - F is always -1. other halogens have an oxidation number of -1 in most binary compunds. when combined with oxygen, they have positive oxidation states
4. the sume of the oxidation # of all atoms in a neutral compound is 0. the sum of the oxidation #s in a polyatomic ion = the charge of the ion.

Question 25

activities series

Answer 25

a list of metals arranged in order of decreasing ease of oxidation . any metal ion on the list can be oxidized by the ions of elements below it.

Question 26

concentrations

Answer 26

desgnate the amount of solute dissolveed in a given quanitity of solvent or quantity of solutoions

Question 27

Molarity, M

Answer 27

M= moles solute/volume of soln in L

Question 28

dilutoin

Answer 28

solution of lower concertrations can be obtained by adding water M1xV1=M2V2