Chapter 4

Question 1

solutions

Answer 1

homogeneous mixtures of 2+ substances

Question 2

solvents

Answer 2

present in greatest abundance

Question 3

solutes

Answer 3

present in lesser abundance

Question 4

aqueous solution

Answer 4

w/ water

Question 5

solvation

Answer 5

surrounding of solute by solvent (water); molecular and ionic

Question 6

dissociation

Answer 6

ionic compounds dissolve by separation into ions

Question 7

electrolyte

Answer 7

dissociates into ions in aqueous solution; ionic, conducts electricity

Question 8

nonelectrolyte

Answer 8

doesn’t dissociate (doesn’t form ions); molecular, doesn’t conduct electricity

Question 9

strong electrolyte

Answer 9

dissociates completely when dissolved
- water-soluble ionic compounds

Question 10

all ionic compounds =

Answer 10

strong electrolytes

Question 11

weak electrolytes

Answer 11

only dissociate partially when dissolved
- chemical equilibrium; reaction goes forwards and backwards

Question 12

precipitation reactions

Answer 12

2 solutions w/ soluble salts –> insoluble salt (precipitate)

Question 13

precipitate

Answer 13

insoluble solid formed by 2 soluble salts

Question 14

solubility

Answer 14

amount of substance can be dissolved in solvent

Question 15

metathesis reactions (exchange)

Answer 15

partner switching

Question 16

steps to metathesis reactions

Answer 16

• determine ions present
• write formulas for product, cation from 1 reaction w/ anion from other reaction
• check solubility; if insoluble, precipitate forms

Question 17

molecular equation

Answer 17

lists reactants and products w/o ionic values

Question 18

complete ionic equation

Answer 18

all strong electrolytes dissociated into ions
- breaks down aqueous species

Question 19

net ionic equations

Answer 19

doesn’t include spectator ions (cancel out what’s on both sides)

Question 20

acids

Answer 20

substances that ionize in aqueous solutions to form H+ ions (protons)
- proton donors

Question 21

monocratic acids

Answer 21

donate 1 H+ per molecule

Question 22

diprotic acid

Answer 22

donates 2 H+ per molecule

Question 23

bases

Answer 23

increase amount of OH- ions or accepts H+ ions

Question 24

strong acids

Answer 24

Hydrochloric acid, HCl
hydrobromic acid, HBr
Hydroiodic acid, HI
Chloric acid, HClO3
perchloric acid, HClO4
nitric acid, HNO3
sulfuric acid, H2SO4

Question 25

strong bases

Answer 25

Group 1A metal hydroxides (LiOH, NaOH, KOH, RbOH, CsOH heavy group 2A metal hydroxides (Ca(OH)2, Sr(OH)2, Ba(OH)2)

Question 26

strong acids and bases

Answer 26

completely dissociate in aq (completely ionized)

Question 27

weak acids and bases

Answer 27

don't completely dissociate (partially ionized)

Question 28

identifying strong/weak electrolytes

Answer 28

- ionic or molecular? --> ionic = strong - molecular = acid or base? - if starts w/ H or ends w/ COOH = acid

Question 29

neutralization reaction

Answer 29

reaction b/w acid and base

Question 30

neutralization reaction w/ metal hydroxide (base)

Answer 30

product = water + salt

Question 31

neutralization reaction w/ gas

Answer 31

carbonate/bicarbonate react w/ acid --> water + salt + CO2

Question 32

oxidation

Answer 32

loss of electrons

Question 33

reduction

Answer 33

gain of electrons

Question 34

oxidation number

Answer 34

assigned; determines if redox reaction occured

Question 35

oxidation number: pure element

Answer 35

0

Question 36

oxidation number: monatomic ion

Answer 36

same as charge

Question 37

oxidation number: nonmetals

Answer 37

usually (-)

Question 38

oxidation number: sum of oxidation numbers

Answer 38

neutral = 0 polyatomic ion = charge of ion(s)

Question 39

displacement reactions

Answer 39

ion oxidize an element - reaction b/w metal + acid/metal salt (partner switching)

Question 40

becoming more (+)

Answer 40

loss of electrons

Question 41

becoming more (-)

Answer 41

gain electrons

Question 42

activity series

Answer 42

list of metals in order of decreasing oxidation - elements higher = more reactive = more easily oxidized

Question 43

active metals

Answer 43

metals at top of series = most easily oxidized

Question 44

noble metals

Answer 44

metals at bottom of series = low reactivity

Question 45

reducing agent

Answer 45

loses electrons (more +), is oxidized

Question 46

oxidizing agent

Answer 46

gains electrons (more -), is reduced

Question 47

concentration

Answer 47

amount of solute dissolved in solvent

Question 48

molarity (M)

Answer 48

concentration of solution M = (moles of solute)/(volume of solution (L))

Question 49

dilution

Answer 49

adding solvent to solution; lowers concentration, moles stay the same - molarity(initial) x volume(initial) = molarity(final) x volume(final)

Question 50

titration: to calculate concentration of solute in solution

Answer 50

- m1v1 = m2v2 - mL1=? M1=, M2=, ML2=

Question 51

standard solution

Answer 51

reagent solution of known concentration

Question 52

equivalence point

Answer 52

point of which equivalent quantities are brought together