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unit 6 Flashcards

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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
Q

ionization

A

molecule breaks apart into ions

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26
Q

why do weak electrolyte solutions conduct electricity weakly?

A

-other compounds dissociate/ionize less than 10%
-most common are weak acids and weak bases

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27
Q

why do nonelectrolyte solutions not conduct electricity?

A

molecular compounds are soluble in water, but form no compounds

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28
Q

dynamic equillibrium

A

rate of dissolving = rate of crystallization

29
Q

how do you show equillibrium in a chemical equation?

A

double arrow

30
Q

proportion of solubility (solids) to temperature

A

directly proportional

31
Q

proportion of temperature to entropy (solids/liquids)

A

directly proportional

32
Q

the solubility of a gas in a liquid is affected by:

A

temperature and pressure

33
Q

proportion of solubility (gases) and temperature

A

inversely proportional

34
Q

proportion of solubility (gases) and pressure

A

directly proportional

higher pressure of gas above a liquid = more soluble the gas is

35
Q

Henry’s law

A

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
Q

3 steps of chemical reactions

A
  1. bonds in reactants are broken
  2. atoms/ groups of atoms rearrange
  3. atoms form new bonds and combinations to make products
37
Q

clues that a reaction has occurred

A

-absorption/release of energy
-color change
-production of a gas (bubbles)
-precipitates

38
Q

precipitate

A

formation of a solid product from two solutions

39
Q

purpose of chemical equations

A

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
Q

reactant types

A

solid (s)
liquid (l)
gas (g)

41
Q

aqueous (aq) meaning

A

substances dissolved in water

42
Q

aqueous other names

A

dissolved in water
in solution
dilute

43
Q

how is heat portrayed as a catalyst in a reaction

A

triangle over the arrow

44
Q

catalyst

A

something used to speed up a reaction, not used up in it

chemical formula written over the arrow

45
Q

law of conservation of mass

A

in any chemical reaction, the mass remains constant

mass of reactants = mass of products

46
Q

coefficient uses in balancing equations

A

placed before the formula to support to law of conservation of mass

47
Q

when balancing, never change:

A

subscripts in a chemical formula

48
Q

why should we classify chemical reactions?

A

-predict products in a chemical reaction
-predict if a chemical reaction will occur

49
Q

synthesis (combustion) reaction

A

two or more simple substances react, one complex product

-might require a small of heat/light energy
-forms binary/complex compounds

50
Q

decomposition reaction

A

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
Q

single replacement reaction

A

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
Q

double replacement reaction

A

two compounds react and exchange cations/anions, two new compounds produce

53
Q

neutralization reaction

A

acid and base react, a salt and water produce

54
Q

combustion reaction

A

hydrocarbon/carbohydrate and oxygen gas reacts, carbon dioxide and water produce

-heat/other energy also produced
-exothermic reaction
-water releases as vapor

55
Q

activation energy

A

energy required to start a reaction

56
Q

exothermic reaction

A

release of energy in the form of heat or light

57
Q

when nonmetal oxides react with water

A

acid is produced

58
Q

when metal oxides react with water

A

it forms a base

59
Q

when metal oxides react with nonmetal oxides

A

ternary ionic compounds are produced

60
Q

endothermic reaction

A

reactions that absorb more energy to break bonds than released when forming

61
Q

precipitation reaction

A

two soluble ionic compounds in an aqueous solution exchange cations to produce two new ionic compounds

-at least one solid (precipitate) formed

62
Q

neutralization reaction

A

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
Q

when an ionic compound dissolves in water, the resulting solution contains

A

the component ions

64
Q

what happens when neither products are precipitates

A

no reaction

65
Q

molecular equation

A

shows the complete neutral formulas for each compound in the aqueous reaction as if they existed as molecules

66
Q

complete ionic equations

A

equations that describe the material’s structure when dissolved

67
Q

spectator ions

A

ions that don’t participate in the reaction

68
Q

net ionic equation

A

ionic equation where spectator ions are removed

69
Q

Some laboratory procedures involving oxygen-sensitive reactants or products call for using water that has been boiled and then cooled. Why?

A

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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