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Chem 101 > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

solutions

A

homogeneous mixtures of 2+ substances

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2
Q

solvents

A

present in greatest abundance

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3
Q

solutes

A

present in lesser abundance

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4
Q

aqueous solution

A

w/ water

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5
Q

solvation

A

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

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6
Q

dissociation

A

ionic compounds dissolve by separation into ions

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7
Q

electrolyte

A

dissociates into ions in aqueous solution; ionic, conducts electricity

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8
Q

nonelectrolyte

A

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

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9
Q

strong electrolyte

A

dissociates completely when dissolved
- water-soluble ionic compounds

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10
Q

all ionic compounds =

A

strong electrolytes

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11
Q

weak electrolytes

A

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

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12
Q

precipitation reactions

A

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

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13
Q

precipitate

A

insoluble solid formed by 2 soluble salts

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14
Q

solubility

A

amount of substance can be dissolved in solvent

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15
Q

metathesis reactions (exchange)

A

partner switching

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16
Q

steps to metathesis reactions

A
  • determine ions present
  • write formulas for product, cation from 1 reaction w/ anion from other reaction
  • check solubility; if insoluble, precipitate forms
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17
Q

molecular equation

A

lists reactants and products w/o ionic values

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18
Q

complete ionic equation

A

all strong electrolytes dissociated into ions
- breaks down aqueous species

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19
Q

net ionic equations

A

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

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20
Q

acids

A

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

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21
Q

monocratic acids

A

donate 1 H+ per molecule

22
Q

diprotic acid

A

donates 2 H+ per molecule

23
Q

bases

A

increase amount of OH- ions or accepts H+ ions

24
Q

strong acids

A

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

25
Q

strong bases

A

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

26
Q

strong acids and bases

A

completely dissociate in aq (completely ionized)

27
Q

weak acids and bases

A

don’t completely dissociate (partially ionized)

28
Q

identifying strong/weak electrolytes

A
  • ionic or molecular? –> ionic = strong
  • molecular = acid or base?
    • if starts w/ H or ends w/ COOH = acid
29
Q

neutralization reaction

A

reaction b/w acid and base

30
Q

neutralization reaction w/ metal hydroxide (base)

A

product = water + salt

31
Q

neutralization reaction w/ gas

A

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

32
Q

oxidation

A

loss of electrons

33
Q

reduction

A

gain of electrons

34
Q

oxidation number

A

assigned; determines if redox reaction occured

35
Q

oxidation number: pure element

A

0

36
Q

oxidation number: monatomic ion

A

same as charge

37
Q

oxidation number: nonmetals

A

usually (-)

38
Q

oxidation number: sum of oxidation numbers

A

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

39
Q

displacement reactions

A

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

40
Q

becoming more (+)

A

loss of electrons

41
Q

becoming more (-)

A

gain electrons

42
Q

activity series

A

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

43
Q

active metals

A

metals at top of series = most easily oxidized

44
Q

noble metals

A

metals at bottom of series = low reactivity

45
Q

reducing agent

A

loses electrons (more +), is oxidized

46
Q

oxidizing agent

A

gains electrons (more -), is reduced

47
Q

concentration

A

amount of solute dissolved in solvent

48
Q

molarity (M)

A

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

49
Q

dilution

A

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

50
Q

titration: to calculate concentration of solute in solution

A
  • m1v1 = m2v2
  • mL1=? M1=, M2=, ML2=
51
Q

standard solution

A

reagent solution of known concentration

52
Q

equivalence point

A

point of which equivalent quantities are brought together

Chem 101 (11 decks)

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