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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
Q

Monoprotic acids

A

HCl & HNO3; yield one H+ per molecule of acid

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26
Q

Diprotic acid

A

Yields 2 H+ per molecule of acid (ex. sulfuric acid, H2SO4)

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27
Q

Bases

A

substances that accept (react with) H+ ions; produce OH- when they dissolve in water (ex. NaOH, KOH, Ca(OH)2; NH3)

28
Q

Strong acids, strong bases

A

acids and bases that are strong electrolytes (completely ionized in solution)

29
Q

Weak acids, weak bases

A

weak electrolytes (partly ionized)

30
Q

Hydrochloric acid

31
Q

Hydrobromic acid

32
Q

Hydroiodic acid

33
Q

Chloric acid

34
Q

Perchloric acid

35
Q

Nitric acid

36
Q

Sulfuric acid

37
Q

Group 1A Metal hydroxides (strong bases)

A

LiOH, NaOH, KOH, RbOH, CsOH

38
Q

Heavy group 2A metal hydroxides

A

Ca(OH)2, Sr(OH)2, Ba(OH)2

39
Q

Neutralization reaction

A

when a solution of an acid and a solution of a base are mixed

40
Q

Salt

A

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
Q

Antacids

A

substances that remove excess acid

42
Q

Acid inhibitors

A

substances that decrease the production of acid

43
Q

Oxidation-reduction (redox) reactions

A

electrons are transferred between reactants

44
Q

Corrosion

A

conversion of a metal into a metal compound by a reaction between the metal and some substance in its environment

45
Q

Oxidation

A

loss of electrons by a substance

46
Q

Reduction

A

when an atom, ion, or molecule has become more negatively charged (gained electrons)

47
Q

Oxidation number

A

actual charge for a monatomic ion

48
Q

For an atom in its elemental form, the oxidation number is always _____

49
Q

For any monatomic ion, the oxidation number equals ____________

A

the charge on the ion

50
Q

Nonmetals usually have _____ oxidation numbers

51
Q

The sum of the oxidation numbers of all atoms in a neutral compound is ____

52
Q

Displacement reactions

A

the ion in solution is displaced or replaced through oxidation of an element

53
Q

Activity series

A

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
Q

Active metals

A

alkali metals, alkaline earth metals are most easily oxidized (they react most readily to form compounds)

55
Q

Noble metals

A

transition metals from groups 8B & 1B very stable and form compounds less readily

56
Q

Concentration

A

the amount of a solute dissolved in a given quantity of solvent or quantity of solution

57
Q

Aqua regia

A

royal water; gold dissolved in a 3:1 mixture of concentrated hydrochloric and nitric acids

58
Q

Molarity (M)

A

concentration of a solution as the number of moles of solute in a liter of solution; moles solute/volume of solution in liters

59
Q

Stock solutions

A

solutions that are used routinely in the lab, often purchased or prepared in concentrated form

60
Q

Dilution

A

solutions of lower concentrations can be obtained by adding water to stock solution

61
Q

hyponatremia

A

a condition in which the concentration of sodium ion in the blood is too low due to excess water consumption

62
Q

titration

A

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
Q

Standard solution

A

reagent solution of known concentration

64
Q

Equivalence point (of the titration)

A

the point at which stoichiometrically equivalent quantities are brought together

65
Q

Acid-base indicators

A

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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