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unit 6 Flashcards

1
Q

solution

A

homogeneous mixture of 2 substances

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2
Q

solvent

A

majority component of a solution

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3
Q

aqueous solution

A

a solution where water acts as a solvent

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4
Q

solute

A

minority component of a mixture

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5
Q

dilute solution

A

small amount of solute dissolved in the solvent

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6
Q

concentrated solution

A

large amount of solute dissolved in the solvent

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7
Q

saturated solution

A

a solution in which the solution is in equilibrium with the undissolved state

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8
Q

unsaturated solution

A

has less than the maximum amount of solute dissolved in the solvent

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9
Q

supersaturated solution

A

more than the maximum amount of solute is dissolved

can be obtained by preparing a saturated solution at a high temperature, then cooled carefully to avoid crystallizing the excess solute

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10
Q

metastable

A

in a saturated solution, excess solute will crystallize if the solution is shaken or if a seed crystal is added to start crystallization

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11
Q

concentration

A

expression of solute : solvent in a solution and is often expressed as amount of solute per volume of solution

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12
Q

molarity

A

the number of moles of solute per liter of solution

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13
Q

molar concentration conversion factors

A

1.5 mol x = 1 L x soln

1.5 mol x / 1 L x soln

1 L x soln / 1.5 mol x

ratios are just for example*

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14
Q

standard solution

A

solution of a known concentration

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15
Q

stock solution

A

solutions stored in concentrated forms

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16
Q

formula used in dilution problems

A

m1v1 = m2v2

m1: concentration of stock solution
v1: volume of stock solution
m2: concentration of desired solution
v2: volume of desired solution

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17
Q

entropy

A

measure of energy randomization or dispersal in a system

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18
Q

how does entropy work?

A

-gases have kinetic energy due to particle motion
-when barrier is removed, each gas and its kinetic energy is dispersed
-the gas mixture has a greater energy dispersal than the separated components

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19
Q

steps of dissolving

A
  1. energy is used to break attractions between solvent particles
  2. energy is used to break attractions between solute particles
  3. energy is released when new attractions are formed between solvent and solute particles, energy is used as heat
    -when the energy released is less than the energy used, the shortfall is compensated by the increased entropy of the solution
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20
Q

entropy strength when dissolved: solids

A

greatest increase

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21
Q

entropy strength when dissolved: liquids

A

moderate increase

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22
Q

entropy strength when dissolved: gases

A

no increase

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23
Q

lattice energy

A

energy needed to disrupt the crystal
-very strong
-lattice breaking should not occur

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24
Q

why do strong electrolyte solutions conduct electricity strongly?

A

-ionic substances dissociate completely into ions when dissolved in water
-some molecular compounds ionize when dissolved in water

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25
ionization
molecule breaks apart into ions
26
why do weak electrolyte solutions conduct electricity weakly?
-other compounds dissociate/ionize less than 10% -most common are weak acids and weak bases
27
why do nonelectrolyte solutions not conduct electricity?
molecular compounds are soluble in water, but form no compounds
28
dynamic equillibrium
rate of dissolving = rate of crystallization
29
how do you show equillibrium in a chemical equation?
double arrow
30
proportion of solubility (solids) to temperature
directly proportional
31
proportion of temperature to entropy (solids/liquids)
directly proportional
32
the solubility of a gas in a liquid is affected by:
temperature and pressure
33
proportion of solubility (gases) and temperature
inversely proportional
34
proportion of solubility (gases) and pressure
directly proportional higher pressure of gas above a liquid = more soluble the gas is
35
Henry's law
quantifies the solubility of gases with increasing pressure and shows solubility of a gas in a liquid = pressure of gas above the liquid S(gas) = k(H) P (gas) S(gas) = solubility of the gas (usually in M k(H) = Henry's law constant P(gas) = partial pressure of the gas
36
3 steps of chemical reactions
1. bonds in reactants are broken 2. atoms/ groups of atoms rearrange 3. atoms form new bonds and combinations to make products
37
clues that a reaction has occurred
-absorption/release of energy -color change -production of a gas (bubbles) -precipitates
38
precipitate
formation of a solid product from two solutions
39
purpose of chemical equations
shorthand ways of representing chemical reactions that use the chemical formulas of the reactants separated from the products by an arrow also includes physical states of the reactants
40
reactant types
solid (s) liquid (l) gas (g)
41
aqueous (aq) meaning
substances dissolved in water
42
aqueous other names
dissolved in water in solution dilute
43
how is heat portrayed as a catalyst in a reaction
triangle over the arrow
44
catalyst
something used to speed up a reaction, not used up in it chemical formula written over the arrow
45
law of conservation of mass
in any chemical reaction, the mass remains constant mass of reactants = mass of products
46
coefficient uses in balancing equations
placed before the formula to support to law of conservation of mass
47
when balancing, never change:
subscripts in a chemical formula
48
why should we classify chemical reactions?
-predict products in a chemical reaction -predict if a chemical reaction will occur
49
synthesis (combustion) reaction
two or more simple substances react, one complex product -might require a small of heat/light energy -forms binary/complex compounds
50
decomposition reaction
one complex substance reacts, two or more simple products -opposite of a synthesis reaction -most require a continuous supply of energy, used to break bonds in reactants -reactions that absorb more energy to break bonds than released when forming are endothermic -some form simple compounds instead of elements
51
single replacement reaction
an uncombined element and compound react, so the element displaces the same type of element in the compound, new element and compound produce -to determine if this will occur, the uncombined reactant must be higher on the reactivity series than the similar element in the compound
52
double replacement reaction
two compounds react and exchange cations/anions, two new compounds produce
53
neutralization reaction
acid and base react, a salt and water produce
54
combustion reaction
hydrocarbon/carbohydrate and oxygen gas reacts, carbon dioxide and water produce -heat/other energy also produced -exothermic reaction -water releases as vapor
55
activation energy
energy required to start a reaction
56
exothermic reaction
release of energy in the form of heat or light
57
when nonmetal oxides react with water
acid is produced
58
when metal oxides react with water
it forms a base
59
when metal oxides react with nonmetal oxides
ternary ionic compounds are produced
60
endothermic reaction
reactions that absorb more energy to break bonds than released when forming
61
precipitation reaction
two soluble ionic compounds in an aqueous solution exchange cations to produce two new ionic compounds -at least one solid (precipitate) formed
62
neutralization reaction
reaction between an acid and a base to produce an ionic compound and water -ionic compound composed of cation from base and anion from acid -water formed from hydrogen ion from the acid and the hydroxide ion from the base -some products are unstable and spontaneously dissolve and decompose to form a water and a gas
63
when an ionic compound dissolves in water, the resulting solution contains
the component ions
64
what happens when neither products are precipitates
no reaction
65
molecular equation
shows the complete neutral formulas for each compound in the aqueous reaction as if they existed as molecules
66
complete ionic equations
equations that describe the material's structure when dissolved
67
spectator ions
ions that don't participate in the reaction
68
net ionic equation
ionic equation where spectator ions are removed
69
Some laboratory procedures involving oxygen-sensitive reactants or products call for using water that has been boiled and then cooled. Why?
When the water is heated to boiling, oxygen becomes less soluble and will bubble out leaving the water oxygen-deficient

ap chem (11 decks)

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