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AP Chem > Chapter 4 Key Terms > Flashcards

Chapter 4 Key Terms Flashcards

1
Q

the dissolving medium in a solution

A

solvent

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2
Q

a solution in which water is the solvent

A

aqueous solution

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3
Q

__ of water gives it its great ability to dissolve compounds

A

polarity

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4
Q

a molecule that has a permanent dipole moment. Positive ends attracted to anions, negative ends attracted to cations

A

polar molecules

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5
Q

the interaction between solute particles and water molecules

A

hydration

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6
Q

the amount of a substance that dissolves in a given volume of solvent at a given temperature

A

solubility

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7
Q

__ dissolves polar, __ dissolves non polar

A

polarnonpolar

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8
Q

a substance dissolved in a liquid to form a solution

A

solute

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9
Q

the ability to conduct an electric current

A

electrical conductivity

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10
Q

material that, when dissolved in water, gives a solution that conducts an electric current very efficiently. more ions available

A

strong electrolyte

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11
Q

material which, when dissolved in water, gives a solution that conducts only a small electric current. less ions available

A

weak electrolyte

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12
Q

a substance that, when dissolved in water, gives a nonconducting solution

A

nonelectrolyte

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13
Q

What is the Arrhenius definition of an acid?

A

substance that produces H+ ions in solution

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14
Q

an acid that completely dissociates to produce an H+ ion and the conjugate base

A

strong acid

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15
Q

a metal hydroxide salt that completely dissociates into its ions in water

A

strong bases

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16
Q

an acid that dissociates only slightly in aqueous solution

A

weak acid

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17
Q

base that reacts with water to produce hydroxide ions to only a slight extent in aqueous solution

A

weak base

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18
Q

What is the Arrhenius definition of a base?

A

substance that produces OH- ions in solution

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19
Q

What is the Bronsted-Lowry definitions of acids and bases?

A

Acid: proton donor, Base: proton acceptor

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20
Q

moles of solute per volume of solution in liters

A

Molarity (M)

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21
Q

solution whose concentration is accurately known

A

standard solution

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22
Q

solutions purchased or prepared in concentrated form

A

stock solutions

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23
Q

process of adding solvent to lower the concentration of solute in a solution

A

dilution

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24
Q

device for accurately measuring and transferring a given volume of solution

A

pipet

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25
Q

Molarity equation

A

M = Moles of solute / Liters of solution

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26
Q

Dilution equation

A

M1V1 = M2V2

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27
Q

the ions of 2 compounds exchange places in an aqueous solution to form two new compounds

A

double replacement reaction

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28
Q

in a double replacement reaction, one of the compounds formed is a __, insoluble __, or molecular __

A

precipitategascompound

29
Q

What are the 3 types of solution reactions?

A

precipitation reactions, acid base reactions, oxidation reduction reactions

30
Q

a reaction in which an insoluble substance forms and separates from the solution

A

precipitation reaction

31
Q

solid that forms in a double replacement reaction

A

precipitate

32
Q

If both ions are colorless, the solid formed should be the color __

33
Q

tiny amount of solid that dissolves, is not noticeable

A

slightly soluble

34
Q

3 simple rules for the solubility of salts in water

A

1) Nitrate salts are soluble 2) Salts containing the alkali metal ions and the ammonium ion are soluble 3) all acids, perchlorates, and hallides are soluble

35
Q

an equation representing a reaction in solution showing the reactant and products in undissociated form whether they are strong or weak electrolytes

A

formula equation

36
Q

an equation that shows all substances that are strong electrolytes as ions

A

complete ionic equation

37
Q

ions present in solution that don’t precipitate directly in a reaction

A

spectator ions

38
Q

an equation for a reaction in solution where strong electrolytes are written as ions, showing only those components that are directly involved in the chemical change

A

net ionic equations

39
Q

Solving Stoichiometry Problems for Reactions in Solutions (6 steps)

A

1) Identify species present in combined solution and determine what reaction occurs2) Write balanced net ionic equation3) Calculate moles of reactants4) Determine limiting reactant5) Calculate moles of product or products, as required6) Convert to grams or other units, as required

40
Q

Performing Calculations for Acid-Base Reactions (6 steps)

A

1) List species present in combined solution and decide what reaction occurs2) Write balanced net ionic equation3) Calculate moles of reactants4) Determine limiting reactant5) Calculate moles of required reactant or product6) Convert to grams or volume as required

41
Q

an acid-base reaction

A

neutralization reaction

42
Q

a process involving titration of one solution with another

A

volumetric analysis

43
Q

technique in which one solution is used to analyze another

44
Q

Describe process of titration

A

Involves delivery (from a buret) of a measured volume of a solution of known concentration (titrant) into a solution containing the substance being analyzed (analyte)

45
Q

the point in titration when enough titrant has been added to react exactly with the substance in solution being titrated

A

equivalence point (stoichiometric point)

46
Q

chemical that changes color and is used to mark the endpoint of a titration

47
Q

the point in a titration at which the indicator changes color

48
Q

3 requirements that must be met for a titration to be successful

A

1) Exact reaction between titrant and analyte must be known (and rapid) 2) The stoichiometric (equivalence) point must be marked accurately 3) The volume of titrant required to reach the stoichiometric point must be known accurately

49
Q

titration of an acid with a standard solution containing OH- ions

A

standardizing the solution

50
Q

Properties of acids (6)

A

Proton donors, pH lower than 7, taste sour, reacts with active metals producing H2 (fizzing) & salts, react with carbonates, neutralizes bases

51
Q

How does acids effect indicators?

A

Blue litmus turns redMethyl orange turns red

52
Q

Strong acids assumed __% in solution, weak acids less than __% ionized

53
Q

Neutralization reactions always produce a __ and __

54
Q

Properties of bases (5)

A

proton acceptors, pH greater than 7, taste bitter, feel slippery, neutralizes acids

55
Q

How does bases effect indicators?

A

Red litmus turns bluePhenolphthalein turns purple

56
Q

a reaction in which one or more electrons are transferred

A

Oxidation-reduction (redox) reactions

57
Q

Spontaneous redox rxns can transfer __. Nonspontaneous redox rxns can be made to happen with __

A

energyelectricity

58
Q

a concept that provides a way to keep track of electrons in oxidation reduction reactions according to certain rules

A

Oxidation states (numbers)

59
Q

Rules for Assigning Oxidation numbers (7)

A

1) Oxidation # of any uncombined element is 0 2) Oxidation # of a monatomic ion equals its charge 3) Oxidation # of Oxygen in compounds is -2 4) Oxidation # of hydrogen in compounds is +1 5) Sum of the oxidation #s in the formula of a compound is 0 6) Sum of the oxidation #s in the formula of a polyatomic ion is equal to its charge 7) Oxidation # of Fluorine is -1

60
Q

an increase in oxidation state (a loss of electrons)

61
Q

a decrease in oxidation state (a gain of electrons)

62
Q

Oxidized: __ electrons, __ agentReduced: __ electrons, __ agent

A

loses, reducinggains, oxidizing

63
Q

a reactant that accepts electrons from another reactant

A

oxidizing agent (electron acceptor)

64
Q

a reactant that donates electrons to another substance to reduce the oxidation state of one of its atoms

A

reducing agent (electron donor)

65
Q

the 2 parts of an oxidation reduction reaction; one representing oxidation, the other reduction

A

half-reactions

66
Q

The half-reaction method for balancing equations for oxidation-reduction reactions occurring in acidic solution(5 steps)

A

1) Write separate equations for the oxidation and reduction half-reactions 2) For each half reaction: a) balance all elements except hydrogen and oxygen b) balance oxygen using water c) balance hydrogen using H+ d) balance the charge using electrons 3) If needed, multiply one or both balanced half-reactions by an integer to equal the # of electrons transferred in the 2 half-reactions 4) Add the half reactions, cancel identical species 5) Check that the elements and charges are balanced

67
Q

The half-reaction method for balancing equations for oxidation-reduction reactions occurring in basic solution(5 steps)

A

1) Use half-reaction method as specified for acidic solutions to obtain the final balanced equation as if H+ ions were present 2) To both sides of the equation, add a # of OH- ions that is equal to the # of H+ ions (want to eliminate H+ by forming water) 3) Form water on the side containing both H+ and OH- ions, eliminate # of water molecules that appear on both sides of the equation 4) Check that the elements and charges are balanced

68
Q

Active Metals: __ electrons easily, easily __Active Nonmetals: __ electrons easily, easily __

A

lose, oxidizedgain, reduced

69
Q

What does OILRIG stand for?

A

Oxidation is Loss, Reduction is Gain

AP Chem (11 decks)

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