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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
Molarity equation
M = Moles of solute / Liters of solution
26
Dilution equation
M1V1 = M2V2
27
the ions of 2 compounds exchange places in an aqueous solution to form two new compounds
double replacement reaction
28
in a double replacement reaction, one of the compounds formed is a __, insoluble __, or molecular __
precipitategascompound
29
What are the 3 types of solution reactions?
precipitation reactions, acid base reactions, oxidation reduction reactions
30
a reaction in which an insoluble substance forms and separates from the solution
precipitation reaction
31
solid that forms in a double replacement reaction
precipitate
32
If both ions are colorless, the solid formed should be the color __
white
33
tiny amount of solid that dissolves, is not noticeable
slightly soluble
34
3 simple rules for the solubility of salts in water
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
an equation representing a reaction in solution showing the reactant and products in undissociated form whether they are strong or weak electrolytes
formula equation
36
an equation that shows all substances that are strong electrolytes as ions
complete ionic equation
37
ions present in solution that don't precipitate directly in a reaction
spectator ions
38
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
net ionic equations
39
Solving Stoichiometry Problems for Reactions in Solutions (6 steps)
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
Performing Calculations for Acid-Base Reactions (6 steps)
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
an acid-base reaction
neutralization reaction
42
a process involving titration of one solution with another
volumetric analysis
43
technique in which one solution is used to analyze another
titration
44
Describe process of titration
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
the point in titration when enough titrant has been added to react exactly with the substance in solution being titrated
equivalence point (stoichiometric point)
46
chemical that changes color and is used to mark the endpoint of a titration
indicator
47
the point in a titration at which the indicator changes color
endpoint
48
3 requirements that must be met for a titration to be successful
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
titration of an acid with a standard solution containing OH- ions
standardizing the solution
50
Properties of acids (6)
Proton donors, pH lower than 7, taste sour, reacts with active metals producing H2 (fizzing) & salts, react with carbonates, neutralizes bases
51
How does acids effect indicators?
Blue litmus turns redMethyl orange turns red
52
Strong acids assumed __% in solution, weak acids less than __% ionized
100%5%
53
Neutralization reactions always produce a __ and __
saltwater
54
Properties of bases (5)
proton acceptors, pH greater than 7, taste bitter, feel slippery, neutralizes acids
55
How does bases effect indicators?
Red litmus turns bluePhenolphthalein turns purple
56
a reaction in which one or more electrons are transferred
Oxidation-reduction (redox) reactions
57
Spontaneous redox rxns can transfer __. Nonspontaneous redox rxns can be made to happen with __
energyelectricity
58
a concept that provides a way to keep track of electrons in oxidation reduction reactions according to certain rules
Oxidation states (numbers)
59
Rules for Assigning Oxidation numbers (7)
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
an increase in oxidation state (a loss of electrons)
oxidation
61
a decrease in oxidation state (a gain of electrons)
reduction
62
Oxidized: __ electrons, __ agentReduced: __ electrons, __ agent
loses, reducinggains, oxidizing
63
a reactant that accepts electrons from another reactant
oxidizing agent (electron acceptor)
64
a reactant that donates electrons to another substance to reduce the oxidation state of one of its atoms
reducing agent (electron donor)
65
the 2 parts of an oxidation reduction reaction; one representing oxidation, the other reduction
half-reactions
66
The half-reaction method for balancing equations for oxidation-reduction reactions occurring in acidic solution(5 steps)
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
The half-reaction method for balancing equations for oxidation-reduction reactions occurring in basic solution(5 steps)
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
Active Metals: __ electrons easily, easily __Active Nonmetals: __ electrons easily, easily __
lose, oxidizedgain, reduced
69
What does OILRIG stand for?
Oxidation is Loss, Reduction is Gain

AP Chem (11 decks)

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