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CHM 115 Blechle > Chapter 4 > Flashcards

Chapter 4 Flashcards

1
Q

What needs to happen for a reaction to occur?

A

reactants must come into physical contact

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2
Q

What phase does reactions happen best in?

A

gas or liquid

b/c more movement occurs

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3
Q

What is a homogeneous mixture?

A

two or more components mix freely

molecules or ions are completely intermingled

contain at least two substances

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4
Q

What is the medium that dissolves the solute?

A

solvent

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5
Q

What is the substance dissolved in solvent?

A

solute

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6
Q

What is the component is large amounts in a solution?

A

solvent

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7
Q

What does an aqueous solution mean?

A

a solute dissolved in water as the solvent

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8
Q

A method characterizing solution broadly defined as a solute to solvent ratio, though the method of measurement can change?

A

concentration

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9
Q

Formula for the concentration?

A

C = solute / solvent

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10
Q

What is a concentration called when the solution is a small solute to solvent ratio?

Give example

A

dilute solution

eye drops

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11
Q

What is a concentration called when the solution is a large solute to solvent ratio?

Give example

A

concentrated solution

brine

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12
Q

Why do you have to be careful when you use ‘dilute’ and ‘concentrated’ ?

A

they are relative terms

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13
Q

What do chemists use as a unit of absolute concentration?

A

M = molarity

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14
Q

What are the units for molarity (M)?

A

moles / liter

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15
Q

Formula for solute

A

g solute needed to make saturated solution / 100g solvent

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16
Q

What does solubility depend on?

A

temperature

also the type of solvent

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17
Q

Solution in which no more solute can be dissolved at a given temperature?

A

saturated solution

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18
Q

Solution containing less solute than the maximum amount (able to dissolve more solute)?

A

unsaturated solution

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19
Q

Solution that holds more than the maximum solute because its temp went up, solute was added, and then the temp cooled?

A

super saturated solution

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20
Q

What does it mean for a solution to be an electrolyte?

A

it conducts charge

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21
Q

Which compounds conduct electricity and which ones do not?

A

ionic compounds do

molecular compounds do not

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22
Q

What is a strong vs weak electrolyte?

A 
strong = conducts electricity well
weak = conducts electricity but not well
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23
Q

What happens when molecular compounds dissolve in water?

A

particles are surrounded by water

do not dissociate

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24
Q

What happens when ionic compounds dissolve in water?

A

water arranges itself around ions snd removes lattice (bonds?)
dissociate
(unless its a polyatomic)

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25
Q

What is dissociation?

A

salt breaks apart into ions when entering solution

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26
Q

What conducts electricity when ionic compound dissociate?

A

the separated ions

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27
Q

What do ionic compounds dissolved form?

A

hydrated ions

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28
Q

What does hydrated mean?

A

surrounded by water

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29
Q

How are ions indicated in a chemical equations?

A

aqueous (aq) written behind it
or
the ions are separated

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30
Q

What equation has substances listed as complete formulas?

A

molecular equation

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31
Q

What equation has all soluble substances broken into ions?

A

ionic equation

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32
Q

What equation only lists substances that actually take part in the reaction?

A

net ionic equation

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33
Q

What do net ionic equations get rid of from ionic equations?

A

spectator ions

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34
Q

What equation gives the identity of all compounds?

A

molecular eqation

35
Q

What dissociates into ions?

A

All strong electrolytes

36
Q

What equation is used to visualize what is actually occurring in solution?

A

ionic equation

37
Q

What are spectator ions?

A

ions that don’t take part in reaction

they sit and watch

38
Q

What equation emphasizes the actual reaction?

A

net ionic equations

39
Q

What equation focuses on the chemical change that occurs?

A

net ionic equations

40
Q

What is the criteria for ionic and net ionic equations?

A

material balance - same # of atom on both sides

electrical balance - same net electrical charge on both sides

41
Q

What type of reaction is when two ions change partners?

A

metathesis / double replacement reaction

42
Q

What type of reaction is when one ion changes to the other ion in the equation?

A

single replacement reaction

43
Q

Give a sample formula for metathesis?

Give sample for single replacement?

A

AB + CD –> AD + BD (cation always go with anion)

AB + C –> A + CB

44
Q

When does metathesis reactions occur?

A 
solid
liquid
gas
weak electrolyte
non-electrolyte

*if one of those forms as a product
(if not then it doesn’t react and all ions are spectator ions)

45
Q

Name the Solubility Rules

A
  1. all salts of alkali metal (G1A)
  2. all salts containing NH4(+) , NO3(-) , ClO4(-), ClO3(-) , C2H3O2(-)
  3. all chlorides, iodides, and bromides
    * except with Ag(+) , Pb(2+) , Hg2(2+)
  4. all salts containing SO4(2-)
    * except with Ca(2+) , Sr(2+) , Ba(2+) , Hg2(2+) , Pb(2+)
46
Q

Name the Insolubility Rules

A
  1. all metal hydroxides and metal oxides [OH(-) and O(2-)]
    * except with G1A , Ca(2+) , Sr(2+) , Ba(2+)
  2. all salts containing PO4(3-) , CO3(2-) , SO3(2-) , S(2-)
    * except G1A and NH4(+)
47
Q

Acids and Bases are common lab Reagan’s…name some common household acids and bases?

A

acids - vinegar, citrus juice, cola

bases - drain cleaners, ammonia

48
Q

What is an Arrhenius Acid?

A

substance that reacts with water to produce hydronium ion, H3O(+)

49
Q

What is an Arrhenius Base?

A

substance that reacts with water to produce the hydroxide ion, OH(-)

50
Q

Give example equation for Arrhenius Acid…

A

HA + H2O –> A(-) + H3O(+)

51
Q

Give example equation for Arrhenius Base…

A

metal hydroxide –> metal + hydroxide

NaOH (s) –> Na(+)(aq) + OH(-) (aq)

52
Q

Name the Strong Acids

A 
HClO4 (Perchloric acid)
HCl (Hydrochloric acid)
HBr (Hydrobromic acid)
HI (Hydroiodic acid)
HNO3 (Nitric acid)
H2SO4 (sulfuric acid)
^^all aqueous
53
Q

What is the electrical conduction dissociation of strong acids and bases?

A 
good electrical conduction
dissociate completely (aq)
54
Q

Name the Strong Bases

A 
G1A metal hydroxides
LiOH
NaOH
KOH
PbOH
CsOH

G2A metal hydroxides
Ca(OH)2
Sr(OH)2
Ba(OH)2

55
Q

What is the electricity conduction of weak acids and bases?

A

weak electrolyte

56
Q

What strength is acetic acid?

What is it?

A

weak
CH3COOH (aq)

CH3COO(-) (aq)

57
Q

What is it called when 2 opposing reactions are occurring at the same rate?

A

Dynamic Equilibrium

Chemical Equilibrium

58
Q

What is it called when concentrations of substances present in solution do not change with time?

A

equilibrium

59
Q

What is it called when both opposing reactions occur continuously?

A

dynamic

60
Q

How are dynamic equilibrium equations represented?

A

a double arrow

61
Q

In a dynamic equilibrium reaction…which reaction forms what?

A

forward reaction = forms ions

backward reaction = reverse ions

62
Q

Do weak acids and bases dissociate?

A

weak acids = yes

weak bases = no

63
Q

Write basic formula for a STRONG ACID IN WATER

A

HA (aq) + H2O –> H3O(+) + A(-)

64
Q

Write basic formula for a STRONG BASE ex:M(OH)n

A

M(OH)n –> M(n+) (aq) + nOH(-) (aq)

65
Q

Write basic formula for a WEAK ACID IN WATER

A

HA (aq) + H2O H3O(+) + A(-)

66
Q

Write basic formula for a WEAK BASE IN WATER

A

B (aq) + H2O HB(+) (aq) + OH(-) (aq)

67
Q

What is a neutralization reaction?

A

reaction that results is production of water and salt
product is neither acidic or basic
HA +BOH –> AB + H2O

68
Q

neutralization reaction between STRONG ACID and STRONG BASE

2HCl + Ca(OH)2 (aq) –>

A

2HCl + Ca(OH)2 (aq) –> 2H2O (l) + CaCl2 (aq)

69
Q

neutralization reaction between WEAK ACID and STRONG BASE

HC2H3O2 (aq) + NaOH(-) –>

A

HC2H3O2 (aq) + NaOH(-) –> H2O (l) + NaC2H3O2(-)

70
Q

neutralization reaction between STRONG ACID and WEAK BASE

HNO3 (aq) + NH3 (aq) –>

A

HNO3 (aq) + NH3 (aq) –> NH4NO3 (aq)

71
Q

neutralization reaction between WEAK ACID and WEAK BASE

HC2H3O2 (aq) + NH3 (aq) –>

A

HC2H3O2 (aq) + NH3 (aq) –> NH4C2H3O2 (aq)

72
Q

What are oxidation-reduction reactions?

A

electron transfer reactions

- from 1 substance to another

73
Q

What is another name for oxidation-reduction reactions?

A

redox reactions

74
Q

When do redox reactions occur?

A

combustion of fuels

metal reacting with oxygen

75
Q

What are the 2 processes of redox reactions?

A

oxidation = loss of electrons
reduction = gain electrons
LEO goes GER

76
Q

What is the oxidizing agent?

What is the reducing agent?

A

ox=substance that accepts electron

re=substance that donates electrons

77
Q

Split into half reactions

2Na + Cl2 –> 2 Na(+) + 2Cl(-)

A

reduction half reaction
Cl2 + 2e(-) –> 2Cl(-)

oxidation half reaction
Na –> Na(+) + e(-)

78
Q

What use happen for redox reactions to occur?

A

one substance must accept the electrons lost by another

79
Q

Can oxidation numbers be fractions?

A

yes but not common

80
Q

What is oxidation state?

A

oxidation #

81
Q

List then hierarchy of asigning Oxidation Number

A
  1. oxidation numbers must add to = charge of unit
  2. atoms of free elements have oxidation numbers of 0
  3. metals in G1A, G2A, and Al have ox. numbers of +1 , +2 , +3
  4. H and F in compounds have +1 , -1 ox. numbers
  5. oxygen has a ox. number of = -2
  6. G7A elements have ox. number of -1
  7. G6A elements have ox. number of -2
  8. G5A elements have ox. number of -3
  9. when there is a conflict between rules, use rule with lower ox. number or higher on list
82
Q

How do you know if a single replacement reaction will take place?

A

looking at the metal activity series

83
Q

Is the top or bottom of the metal activity series list more reactive?

A

the top
meaning the higher ones displace lower ones
the more active element must be by itself equation

84
Q

What equations do you use to figure of the molarity or volume of a dilute or concentration solution?

A

(V1)(M1) = (V2)(M2)

1 = dilute
2 = concentrated

CHM 115 Blechle (8 decks)

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