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chemistryyyy > unit 4 test > Flashcards

unit 4 test Flashcards

1
Q

results a chem rxn took place

A

the temp of the rxn mixture increases

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2
Q

is conducting electricity a sign if a chem rxn

A

no becuase if the initial solutions are ions they will anywyas

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3
Q

what is the best way to determine a change occurred when water and X are mixed

A

measure the electrical conductivities of water and X mixture

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4
Q

what is a compound that is an electrolyte

A

an ion compound

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5
Q

strong electrolytes

A

strong acids bases and ionic compounds

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6
Q

non electrolytes

A

covalently bonded molecular substances

except acids and bases

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7
Q

weak electrolytes

A

weak acids

weak bases

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8
Q

what is always a product for any combustion reaction

A

H2O is always a product in a combustion reaction

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9
Q

what is broken in a chemical change

A

covalent and ionic bonds

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10
Q

physical change breaks what attractions

A

intermolecular

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11
Q

chemical change breaks what attractions

A

intra molecular attractions

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12
Q

evidence of chem change

A 
production of gas
formation of precipitate or solid
change in color 
production of heat- combustion produces heat
sounds
light
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13
Q

for strong electrolytes to be separated into ions they have to be in what state of matter

A

they have to be aqueous

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14
Q

strong electrolytes

A

are soluble ionic substances

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15
Q

know your 7 strong acids

A

know your 7 strong bases

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16
Q

know your polyatomic ions memorized

A

ok

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17
Q

what happens to weka electrolytes

A

nothing they remain in tact(since they ar won’t aqueous?)

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18
Q

as soon as you are given a particle diagram

A

count the number of particles

circle the groups based on the balanced equation

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19
Q

always use law of conservation of mass

A

products equals reactants

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20
Q

molar volume is used to

A

convert between moles and literdy

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21
Q

what is molar volume

A

22.4 mol/1 L at STP

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22
Q

what is density

A

grams per litee

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23
Q

what is percent yield

A

what you got in the lab over what you are supposed to get based on stoich times 100

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24
Q

the point of a titration

A

determine the mass of an unknown

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25
Q

analyze

A

what we are analyzing with the unknown concentration

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26
Q

titrant

A

in the burrette what we have a known concentration of

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27
Q

burrette

A

most precise piece of glassware in a lab

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28
Q

equivalence point

A

when the analyte is totally consumed by the titrant

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29
Q

end point

A

when the color has changed

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30
Q

based on the volume of the flask and the volume of what is in the burrette you cna

A

determine the concentration at equivalence point

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31
Q

precipitation reaction is a

A

DR (double replacement) reaction that creates a solid

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32
Q

acid base reaction

A

a neutralization reaction where an acid donates a proton and a salt and water are formed

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33
Q

neutralization run means

A

we form water

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34
Q

redox

A

involves transfer of electrons

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35
Q

combustion runs are

A 
a subclass of redox reactions 
carbon and water are always formed
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36
Q

an acid according to bronsted lowry

A

an acid is. proton donor

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37
Q

base according to bronsted lowry

A

proton acceptor

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38
Q

what is an amphoteric substance

A

water, it cna be an acid or a base

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39
Q

what are elements

A

substances that can’t be decomposed into simpler substances by chemical or physical means

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40
Q

what is important to to note about physical changes

A

they are usually reversible

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41
Q

Na + Cl2 -> NaCl

A

composition (synthesis) rxn

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42
Q

KClO3 -> KCl + O2

A

Decompostion

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43
Q

Mg+HCl-> MgCl2 + H2

A

single ionic replacement

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44
Q

LiCl + AgNO3 -> LiNO3 + AgCl

A

double ionic replacement

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45
Q

C3H8 + O2 -> CO2 + H2O

A

combustion of a hydrocarbon

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46
Q

Mg + O2 -> MgO

A

combustion of a metal

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47
Q

what reaction is NOT a double replacement rxn

A

redox rxns

48
Q

gas to liquid

A

condensation

49
Q

liquid to gas

A

vaporization

50
Q

solid to liquid

A

fusion(melting)

51
Q

liquid to solid

A

freezing

52
Q

solid to gas

A

sublimation

53
Q

gas to solid

A

deposition

54
Q

7 diatomic elements

A

H2 N2 O2 F2 Cl2 Br2

55
Q

dissolution example w ionic and strong acids and bases

NaCl(s)->NaCl(aq)

A

NaCl(s)-> Na+(aq) + Cl-(aq)

56
Q

dissolution example: non ionic and weak acids/bases

C6H12O6(s) -> C6H12O6(aq)

A

no change

C6H12O6(s) -> C6H12O6(aq)

57
Q

the theoretical yield is also the

A

limiting reactant

58
Q

acid base titration

A

either acid or base is titrant, pH meters cna determine equivalence point

59
Q

redox titration

A

a color change is produced when oxidation state of a metal ion in the rxn changes

60
Q

precipitation titration

A

when the titrant reacts w ions in the analyze a precipitation can occur

61
Q

how will a strong acid or base act in water

A

it will completely ionize or be soluble

62
Q

how will a weak aoc dot base act in water

A

it will have less than 100% ionization

63
Q

strong acids

A

HClO3 HBr HCl HI HNO3 HClO4 H2SO4

64
Q

strong bases

A

LiOH NaOH KOH RbOH Ca(OH)2 Sr(OH)2 Ba(OH)2

65
Q

a strong acid forms a

A

a weak conjugate base and vice versa

66
Q

a weak acid forms a

A

strong conjugate base and vice versa

67
Q

What happens to the IMF

melting

A

weakening

68
Q

What happens to the IMF

boiling

A

breaking

69
Q

What happens to the IMF

condensing

A

forming

70
Q

What happens to the IMF

sublimation

A

breaking

71
Q

What happens to the IMF

deposition

A

forming

72
Q

What happens to the IMF

freezing

A

forming

73
Q

metal and strong acid form a

Mg+2HCl ->

A

salt and gas(usually H2)

MgCl2 + H2

74
Q

carbonate and strong acid form a

MgCO3 + HCl ->

A

combustion reaction is an ion in addition to water and carbon dioxide
MgCl2+H2O +CO2

75
Q

weak electrolyte have

A

partial dissociation

76
Q

strong electrolytes have

A

complete dissociation

77
Q

completing the following equations for an ionic compound place in water means

A

do the mismatching compound thing and find the solubility of the products(should be aqueous)
usually decomposition or double replacement

78
Q

is the LR bigger or smaller than the ER

A

the LR is smaller

79
Q

what do you use to find the excess reactant

A

the limiting reactant

80
Q

what type of compounds are non electrolytes

A

polar covalen

81
Q

what types of compounds are weak electrolytes

A

weak acids

82
Q

what type of compounds are strong electrolytes

A

ionic compounds

83
Q

If acid/ base is stronger than CA/CB which direction does the reaction proceed

A

To the right

84
Q

If CA/CB is stronger than the acid/ base which direction does the reaction proceed

A

To the left

85
Q

What is a neutralization reaction

A

Acid reacting with a base

86
Q

What are the products of a neutralization reaction

A

Salt and water

87
Q

What si the net ionic reaction for any strong acid/strong base rxn

A

H+ +OH- -> H2O

88
Q

What is a salt

A

A compound with no net charge, the opposing charges balance out

89
Q

What elements tend to be good oxidizing agents

A

No metals

90
Q

What elements tend to be good reducing agents

A

Metals

91
Q

What does acid base titration do

A

It determines how much volume acid or base is in a solution

That will completely react with it

92
Q

As we add base what happens to the pH

A

As the volum of the base increases the pH slowly rise then sharply increases at the equivalence point

93
Q

What’s the titrant

A

The known concentration

94
Q

What’s the analyte/titrand

A

The unknown solution your want to known the concentration of

95
Q

What’s the point of a titration

A

Determine concentration of unknown solution by adding a concentration of a known solution

96
Q

What does an indicator do

A

Mark the endpoint of a titration

97
Q

As the volume of the titrant increases what happens to the color of the indicator

A

It appears then disappears as you swirl and infills it becomes a colored solution

98
Q

Typically titrations are formed how many times

A

3 times and average volume is used

99
Q

If a molecule is a weak acid what happens to it in a net ionic equation
Like HC2H3O2

A

You do not break it up for net charge because weak acids(or electrolytes) don’t fully dissociate or ionize

100
Q

If HCl is an acid what is it’s conjugate

And why

A

Cl-

1 less H and 1 less charge

101
Q

If H2O is a base what is its conjugate

A

H3O+

One extra H and one extra positive charge

102
Q

Amohoteric

A

Substances that are able to act as an acid or base (water?)

103
Q

What can MV = MV be used for

A

Determining molarity of unknown solution that reacts with known sokution(titration)
M is moles and v is volume in L

104
Q

What does a non electrolyte do

A

Not dissociate at all

105
Q

What does a weak electrolyte do

A

Some molecules dissociate some do not

106
Q

What does a strong electrolyte do

A

Everything completely dissociates

107
Q

What is the driving force in the net equation

A

Something that isn’t (aq) aka something that can’t be ionized and broken up in the net equation

108
Q

When does M1V1=M2V2 work

A

In neutralization reaction
When there is one OH in one equation and one H in the other
1:1 ratio

109
Q

What is a neutralization reaction

A

Moles of acid must equal moles of base

110
Q

For solution equations first

A

Find the products side and balance the equation to use for mol ratio!

111
Q

What product should you always try to get in a neutralization reaction

A

Water H2O

112
Q

when u add base to a strong acid to a strong base solution what happens to the pH

A

it increases

113
Q

when you add acid to a strong base to a a strong acid solution what happens to the pH

A

it decreases

114
Q

in pH titration curve the volume corresponds to what

A

the titration in the left of the solution

115
Q

the equivalence point occurs when the slope is

A

vertical

116
Q

when calculating charges for redox rxns consider

A

the coefficient multiply the eco efficient by the charge!!

chemistryyyy (40 decks)

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