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Pre-Pharm > Chemistry - Ch 4 > Flashcards

Chemistry - Ch 4 Flashcards

1
Q

Aqueous solution

A

a solution in which water is the dissolving medium

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2
Q

Solution

A

homogeneous mixture of 2+ substances

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3
Q

Solvent

A

substance present in the greatest quantity in a solution

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4
Q

Solutes

A

other substances in the solution, said to be dissolved in the solvent

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5
Q

Electrolyte

A

a substance whose aqueous solutions contain ions (ex. NaCl)

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6
Q

Nonelectrolyte

A

a substance that does not form ions in solution (ex. C12H22O11)

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7
Q

Dissociates

A

an ionic solid breaking up into its component ions as it dissolves

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8
Q

Solvation

A

process that helps stabilize the ions in solution and prevents cations and ions from recombining; water molecules surround the ions as an ionic compound dissolves (ions are solvated)

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9
Q

Strong electrolytes

A

solutes that exist in solution completely or nearly completely as ions (all soluble ionic compounds, like NaCl, and a few molecular compounds, like H20 are strong electrolytes)

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10
Q

Weak electrolytes

A

solutes that exist in solution mostly in the form of molecules with only a small fraction in the form of ions

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11
Q

Chemical equilibrium

A

relative numbers of each type of ion or molecule in the reaction are constant over time

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12
Q

Soluble ionic compounds are ___ electrolytes

A

strong

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13
Q

Precipitation reactions

A

reactions that result in the formation of an insoluble product

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14
Q

precipitate

A

insoluble solid formed by a reaction in solution

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15
Q

Solubility

A

amount of the substance that can be dissolved in a given quantity of solvent at the given temperature

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16
Q

Insoluble

A

any substance with a solubility less than .01 mol/L

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17
Q

all common ionic compounds of the ______ and of the ____ ion are soluble in water

A

alkali metal ions; ammonium

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18
Q

Exchange reactions (metathesis reactions)

A

reactions in which positive ions and negative ions appear to exchange partners (AX + BY –> AY + BX), like precipitation reactions

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19
Q

Molecular equation

A

equation showing the complete chemical formulas of the reactants and the products; shows the chemical formulas of reactants/products without indicating their ionic character

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20
Q

Complete ionic equation

A

equation written with all soluble strong electrolytes shown as ions

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21
Q

Spectator ions

A

ions that appear in identical forms among both the reactants and the products of a complete ionic equation (play no direct role in the reaction)

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22
Q

Net ionic equation

A

when spectator ions are omitted from the equation (cancel like algebraic quantities)

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23
Q

If every ion in a complete ionic equation is a spectator, then __ _______ ________

A

No reaction occurs

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24
Q

Acids

A

substances that ionize in aqueous solutions to form hydrogen ions, thereby increasing the concentration of H+ (aq) ions; AKA “proton donors”

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25
Monoprotic acids
HCl & HNO3; yield one H+ per molecule of acid
26
Diprotic acid
Yields 2 H+ per molecule of acid (ex. sulfuric acid, H2SO4)
27
Bases
substances that accept (react with) H+ ions; produce OH- when they dissolve in water (ex. NaOH, KOH, Ca(OH)2; NH3)
28
Strong acids, strong bases
acids and bases that are strong electrolytes (completely ionized in solution)
29
Weak acids, weak bases
weak electrolytes (partly ionized)
30
Hydrochloric acid
HCl
31
Hydrobromic acid
HBr
32
Hydroiodic acid
HI
33
Chloric acid
HClO3
34
Perchloric acid
HClO4
35
Nitric acid
HNO3
36
Sulfuric acid
H2SO4
37
Group 1A Metal hydroxides (strong bases)
LiOH, NaOH, KOH, RbOH, CsOH
38
Heavy group 2A metal hydroxides
Ca(OH)2, Sr(OH)2, Ba(OH)2
39
Neutralization reaction
when a solution of an acid and a solution of a base are mixed
40
Salt
any ionic compound whose cation comes from a base and whose anion comes from an acid; a neutralization reaction between an acid and a metal hydroxide produces water and a salt
41
Antacids
substances that remove excess acid
42
Acid inhibitors
substances that decrease the production of acid
43
Oxidation-reduction (redox) reactions
electrons are transferred between reactants
44
Corrosion
conversion of a metal into a metal compound by a reaction between the metal and some substance in its environment
45
Oxidation
loss of electrons by a substance
46
Reduction
when an atom, ion, or molecule has become more negatively charged (gained electrons)
47
Oxidation number
actual charge for a monatomic ion
48
For an atom in its elemental form, the oxidation number is always _____
zero
49
For any monatomic ion, the oxidation number equals ____________
the charge on the ion
50
Nonmetals usually have _____ oxidation numbers
negative
51
The sum of the oxidation numbers of all atoms in a neutral compound is ____
zero
52
Displacement reactions
the ion in solution is displaced or replaced through oxidation of an element
53
Activity series
a list of metals arranged in order of decreasing ease of oxidation; any metal on the list can be oxidized by the ions of elements below it
54
Active metals
alkali metals, alkaline earth metals are most easily oxidized (they react most readily to form compounds)
55
Noble metals
transition metals from groups 8B & 1B very stable and form compounds less readily
56
Concentration
the amount of a solute dissolved in a given quantity of solvent or quantity of solution
57
Aqua regia
royal water; gold dissolved in a 3:1 mixture of concentrated hydrochloric and nitric acids
58
Molarity (M)
concentration of a solution as the number of moles of solute in a liter of solution; moles solute/volume of solution in liters
59
Stock solutions
solutions that are used routinely in the lab, often purchased or prepared in concentrated form
60
Dilution
solutions of lower concentrations can be obtained by adding water to stock solution
61
hyponatremia
a condition in which the concentration of sodium ion in the blood is too low due to excess water consumption
62
titration
combining a sample of the solution with a reagent solution of known concentration (standard solution); used to determine the concentration of a particular solute in a solution; can be conducted using acid-base, precipitation, or oxidation-reduction reactions
63
Standard solution
reagent solution of known concentration
64
Equivalence point (of the titration)
the point at which stoichiometrically equivalent quantities are brought together
65
Acid-base indicators
dyes used in acid-base titrations to determine when the equivalence point of the titration has been reached

Pre-Pharm (182 decks)

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