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Chemistry 1a > Ch 4 - Chemical Quantities and Aqueous Reactions > Flashcards

Ch 4 - Chemical Quantities and Aqueous Reactions Flashcards

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1
Q

Stoichiometry

A

the numerical relationships between chemical amounts in a balanced chemical equation.

Allows us to predict the amounts of products that will form from a chemical reaction based on the amount of reactants that react.

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2
Q

limiting reactant

A

the reactant that limits the amount of product in a chemical reaction.

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3
Q

Reactant in excess

A

the reactant that does not limit the reaction and has some left over.

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4
Q

Theoretical Yield

A

the maximum amount of product that can be made in a chemical reaction based on the amount of the limiting reactant.

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5
Q

Actual Yield

A

the amount of product actually produced by a chemical reaction.

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6
Q

Percent Yield

A

actual yield/theoretical yield.

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7
Q

Solution

A

a homogeneous mixture of two substances

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8
Q

Solvent

A

the majority component in a solution

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9
Q

Solute

A

the minority component in a solution

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10
Q

Aqueous Solution

A

A solution where water acts as the solvent

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11
Q

Dilute Solution

A

a solution that contains a small amount of solute relative to the solvent

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12
Q

Concentrated Solution

A

a solution that contains a large amount of solute relative to the solvent

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13
Q

Molarity(M)

A

the amount of solute(in moles) divided by the volume of solution(in liters)

M = Amount of solute(in moles) / volume of solution(in L)

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14
Q

Stock Solution

A

Concentrated solution forms which can be diluted to desired concentrations

M1V1 = M2V2

V1 = (0.500 * 3.00) / 10.0 = 0.150 L

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15
Q

Electrolyte

A

Substances that dissolve in water to form solutions that conduct electricity

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16
Q

Strong Electrolyte

A

Substances that completely dissolve in water

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17
Q

Nonelectrolyte

A

Compounds who do not dissociate into ions when dissolved in water.

Do not conduct electricity

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18
Q

Strong Acid

A

An acid that completely ionizes in solution.

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19
Q

Weak Acid

A

An acid that does not completely ionize in water

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20
Q

Weak electrolyte

A

typically composed of weak acids.

Conduct electricity weakly

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21
Q

Soluble

A

a compound that can be dissolved in water

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22
Q

Insoluble

A

a compound that can not be dissolved in water

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23
Q

Soluble Rules:

Li^+, Na^+, K^+, and NH4^+

A

Always soluble. No exceptions.

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24
Q

Soluble Rules:

NO3^- and C2H3O2^-

A

Always soluble. No exceptions.

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25
Q

Soluble Rules:

Cl^-, Br^-, and I^-

A

Typically soluble.

Exceptions: Insoluble when paired with:
Ag^+, Hg^2+, or Pb^2+

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26
Q

Soluble Rules:

SO4^2-

A

Typically soluble.

Exceptions: Insoluble when paired with:
Sr^2+, Ba^2+, Pb^2+, Ag^+, or Ca^2+

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27
Q

Soluble Rules:

OH^- and S^2-

A

Typically insoluble.

Exceptions: Soluble when paired with:
Li^+, Na^+, K^+, or NH4^+

or

Ca^2+, Sr^2+, or Ba^2+

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28
Q

Soluble Rules:

CO3^2- and PO4^3-

A

Typically Insoluble.

Exceptions: Soluble when paired with:
Li^+, Na^+, K^+, or NH4^+

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29
Q

Precipitation Reaction

A

reactions in which a solid, a precipitate, forms when we mix two solutions

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30
Q

Precipitate

A

a solid formed from mixing two solutions.

Only insoluble compounds form precipitates.

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31
Q

Molecular Equation

A

an equation showing the complete neutral formulas for each compound in a reaction as if they existed as molecules.

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32
Q

Complete Ionic Equation

A

an equation which list all of the ions present as either reactants or products in a chemical reaction.

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33
Q

Spectator Ions

A

in a complete ionic equation the ions in solution that appear unchanged on both sides of the equation.

34
Q

Net Ionic Equation

A

an equation that show only the species that actually changed during a reaction.

Spectator ions are left out of this equation.

Only the interesting stuff stays in the equation.

35
Q

Acid-Base Reaction(Neutralization Reaction)

A

an aqueous reaction where and acid and a base react to neutralize each other while producing water and sometimes a weak electrolyte.

36
Q

Gas-Evolution Reaction

A

a reaction in which a gas is formed resulting in bubbling

Many acid-base reactions are this.

37
Q

Acid

A

substance that produces H^+ ions in aqueous solution

38
Q

Base

A

substance that produces OH^- ions in aqueous solution

39
Q

Arrhenius Definitions

A

Named after Svante Arrhenius. Defined Acids and Bases.

40
Q

Hydronium Ion

A

H^+ is a bare proton and in solution they typically associate with H2O

H^+(aq) + H2O(l) -> H3O^+(aq)

H^+ or H3O^+ both mean a hydronium ion.

41
Q

Polyprotic Acids

Example with a Diprotic Acid

A

an acid containing more than one ionizable proton and release them sequentially.

First it is strong(one way reaction)
H2SO4(aq) -> H^+(aq) + HSO4^-(aq)

Second it is weak(the reaction can go both ways)

HSO4^-(aq) -><- H^+(aq) + SO4^2-(aq)

42
Q

Hydrochloric Acid

A

HCl

43
Q

Hydrobromic Acid

A

HBr

44
Q

Hydroiodic Acid

A

HI

45
Q

Nitric Acid

A

HNO3

46
Q

Sulfuric Acid

A

HSO4

47
Q

Perchloric Acid

A

HCLO4

48
Q

Acetic Acid

A

weak acid.

HC2H3O2

49
Q

Hydroflouric Acid

A

Weak acid.

HF

50
Q

Sodium Hydroxide

A

NaOH

51
Q

Lithium Hydroxide

A

LiOH

52
Q

Potassium Hydroxide

A

KOH

53
Q

Calcium Hydroxide

A

Ca(OH)2

54
Q

Barium Hydroxide

A

Ba(OH)2

55
Q

Ammonia

A

Weak Base.

NH3

56
Q

Salt

A

typically formed in an acid-base reaction. Stays dissolved in the solution but is an ionic compound.

57
Q

Acid + Base ->

A

Water + salt

58
Q

Titration

A

a substance in a solution of known concentration is reacted with another substance in a solution of unknown concentration. Used to determine concentration of unknown solution.

59
Q

Equivalence Point

A

the point in the titration when the number of moles of OH^- added = the number of moles of H^+ initially in the solution.

60
Q

Indicator

A

signals the equivalency point of a titration by using a dye whose color depends on the acidity or basicity of the solution.

61
Q

Intermediate Product

A

an unstable and quickly decomposing product in a Gas-Evolution Reaction

62
Q

Reactant Type:

Sulfides

A

Intermediate Product: None

Gas Evolved: H2S

63
Q

Reactant Type:

Carbonates and bicarbonates

A

Intermediate Product: H2CO3

Gas Evolved: CO2

64
Q

Reactant Type:

Sulfites and bisulfites

A

Intermediate Product: H2SO3

Gas Evolved: SO2

65
Q

Reactant Type:

Ammonium

A

Intermediate Product: NH4OH

Gas Evolved: NH3

66
Q

Oxidation-Reduction Reactions(redox reactions)

A

reactions in which electrons transfer from one reactant to the other.

Many involve a substance with oxygen.

67
Q

Oxidation

A

the loss of an electron.

68
Q

Reduction

A

the gain of electrons.

69
Q

Oxidation State(number)

A

A theoretical number given to each atom based on the electron assignments.

Noted as “-1” instead of an ionic charge of “1-“

70
Q

Oxidation State Rule 1

A

The Ox State of an atom in a free element is 0.

Cl2 = 0 ox state.

71
Q

Oxidation State Rule 2

A

The Ox State of a monoatomic ion is equal to its charge.

Ca^2+ = +2 Ox State

72
Q

Oxidation State Rule 3

A

the sum of the oxidation states of all atoms in:

  • A neutral molecule or formula unit = 0
    H20 = 2(H ox state) + 1(O ox state) = 0
  • An ion is equal to the charge of the ion.
    NO3^- = 1(N ox state) + 3(O ox state) = -1
73
Q

Oxidation State Rule 4

A

In their compounds, metals have positive ox states

  • Group 1A always have an ox state of +1
  • Group 2A always have an ox state of +2
74
Q

Oxidation State Rule 5

A

in their compounds nonmetals are assigned ox state as follows:

Flourine = -1
Hydrogen = +1
Oxygen = -2
Group 7A = -1
Group 6A = -2
Group 5A = -3
75
Q

Oxidation

A

An increase in oxidation state

76
Q

Reduction

A

A decrease in oxidation state

77
Q

Oxidizing Agent

A

a substance that causes the oxidation of another substance

78
Q

Reducing Agent

A

a substance that causes the reduction of another substance

79
Q

The Only 7 Strong Acids

A 
HCl - Hydrochloric Acid
HBr - Hydrobromic Acid
HI - Hydroiodic Acid
HNO3 - Nitric Acid
H2SO4 - Sulfuric Acid
HClO3 - Chloric Acid
HClO4 - Perchloric Acid
80
Q

Strong Bases

A

Alkali Metals
Calcium
Strontium
Barium

Chemistry 1a (15 decks)

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