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Gen Chem 01 > Chapter 04: Chemical Quantities and Aqueous Reactions > Flashcards

Chapter 04: Chemical Quantities and Aqueous Reactions Flashcards

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1
Q

Stoichiometry

A

Quantitative relationships between products and reactants in chemical equations

Requires use of:

1) Balanced chemical equation
2) Conversion factor: mole ratios

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2
Q

Mole ratio

A

Ratio in units of moles relating any two species in a chemical reaction

Used as a conversion factor

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3
Q

Solving stoichoimetry problems

A

Mass (g) of compound A
to
Moles of compound A
using molar mass
Then to
Moles of compound B
using mole ratio
Then to
mass (g) of compound B
using molar mass

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4
Q

Limiting reactant (reagent)

A

Reactant that limits the amount of product that can be made

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5
Q

Excess reactant

A

Leftover reactant (not reacted) in a chemical reaction

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6
Q

Reaction yield: theoretical yield

A

The amount of product that would result if all the limiting reactant reacted

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7
Q

Reaction yield: actual yield

A

The amount of product that is actually obtained from a reaction

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8
Q

% yield

A

% yield = actual yield x 100
theoretical yield

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9
Q

Solution

A

Homogenous mixture of 2+ substances

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10
Q

Solvent

A

Substance present in larger amount within solution

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11
Q

Solute

A

Substance(s) present with smaller amounts dissolved in solvent

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12
Q

Aqueous solution

A

Solution with water as solvent

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13
Q

Solution concentration

A

Qualitative and/or quantitative description of amount of solute in a solvent/solution

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14
Q

Molarity

A

Molarity (M) = moles of solute (n)
liters of solution (V)

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15
Q

Dilute solution

A

Relatively small amount of dissolved solute

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16
Q

Concentrated solution

A

Relatively large amount of dissolved solute

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17
Q

Dilution

A

Procedure for preparing a less concentrated solution from a more concentrated solution

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18
Q

Dilution formula

A

M1V1=M2V2

Where M = molarity
V = volume

*moles (n) of solute remain the same

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19
Q

Solute and solvent interactions

A

Attractive forces between solute particles, between solvent particles, and between solute and solvent particles

If attractions between solute and solvent are strong enough –> dissolve

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20
Q

Charge distribution in water molecule

A 
Oxygen = partial charge negative
Hydrogen = partial charge positive
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21
Q

Hydration

A

Process in which an ion is surrounded by water molecules arranged in a specific manner

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22
Q

Electrolyte

A

Substance that, when dissolved in water, conducts electricity

Contain cations and anions –> dissolve into ions
(Ionic compounds, some acids, some bases)

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23
Q

Nonelectrolyte

A

Substance that, when dissolved in water, does not conduct electricity

No cations, no anions
(Molecular substances)

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24
Q

Strong electrolyte

A

Dissolve completely as ions

*Irreversible reaction.

Most salts, some acids and bases

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25
Q

Weak electrolyte

A

Do not dissolve completely as ions

*Reversible reaction

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26
Q

Dissociation

A

Ions of a salt separate as salt dissolves

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27
Q

Ionization

A

Process of ion formation in solution
Results from chemical reaction between water + compound
(acids, bases)

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28
Q

Soluble

A

A compound that dissolves in water

29
Q

Insoluble

A

A compound that does not dissolve in water

30
Q

Solubility

A

The maximum amount of solute that will dissolve in a given quantity of solvent at a specifc temperature

31
Q

Precipitation reactions & preciptate

A

Reactions that produce precipitate

&

An insoluble solid that separates from solution

32
Q

Spectator ions

A

Ion that exists in the same form on both sides of chemical reaction

33
Q

Complete ionic equation

A

Molecular equation’s aqueous solutions are broken down to ions

Solids, liquids, and gases are still written as compounds

34
Q

Net ionic equation

A

A complete ionic equation with spectator ions cancelled out

A shorthand way of showing what ions react

35
Q

Gravimetric Analysis

A

Make aqueous solution with unknown substance

React unknown with known –> form precipitate

Filter & dry precipitate

Weigh precipitate

Use chemical formula and mass of precipitate to determine amount of unknown ion

36
Q

Acid properties (6)

A
  • sour taste
  • blue litmus paper –> red (red means acid)
  • reacts with certain metals to produce H2 (g) (as H is less reactive than most metals and displaced)
  • reacts with carbonates and bicarbonates to produce CO2 gas
  • reacts with bases to produce salt and water (neutralization)
  • aqueous acid solutions conduct electricity
37
Q

Base properties (5)

A
  • bitter taste
  • feel slippery
  • red litmus –> blue (blue means base)
  • reacts with acids to produce salt and water (neutralization)
  • aqueous base solutions conduct electricity
38
Q

Arrhenius acid

A

Produces H+ (H3O+) in water

39
Q

Arrhenius base

A

Produces OH- in water

40
Q

H3O+

Hydronium ion

A

Hydrated proton (i.e. H+ + H2O)

(Remember: H+ has 0 electrons, 0 neutrons, 1 proton)

41
Q

Brønsted acid

A

Proton donor (donor = acid)

Must contain at least one ionizable proton

42
Q

Brønsted base

A

Proton acceptor (acceptor = base)

43
Q

Acid ionization

A 
Acids = molecular compounds
Ionization = ion formation in solution from compound + H<sub>2</sub>O reaction

Thus:

  • Acid molecules are pulled apart by attraction for water
  • When acids ionize, H+ and counter anions form
  • % of acid molecules that ionize varies
44
Q

Strong acids

A

Acids that ionize virtually 100%

(Irreversible)

45
Q

Weak acids

A

Ionize only a small percentage

(Reversible)

46
Q

Monoprotic acids

A

Each unit of acid yields one H+ ion

47
Q

Diprotic acids

A

Each unit of acid yields two H+​ ions

48
Q

Triprotic acids

A

Each unit of acid yields three H+​ ions

49
Q

Neutralization reactions

A

Acid + base –> salt + water

Weak acid + base –> salt + water

50
Q

Gas-evolving reactions

A

Reactions that form gas directly (from ion exchange) or indirectly (from decomposition; reactants –> ion exchange –> gas + water)

acid + salt –> salt + gas + water

compared to

acid + base –> salt + water

51
Q

Compounds that undergo gas-evolution reactions (4)

A

Sulfides –> H2S (g)

(Bi)carbonates –> H2CO3 –> CO2 (g)

(Bi)sulfites –> H2SO4 –> SO2 (g)

Ammonium –> NH4OH –> NH3 (g)

52
Q

Oxidation-reduction reactions

(Redox reactions)

A

Electron transfer reactions

Uses chemical “bookkeeping” of election transfers

53
Q

Oxidation half-reaction

A

Shows the loss of electron(s)

OIL = oxidiation is loss [of elections]

54
Q

Reduction half-reaction

A

Shows the gaining of electron(s)

RIG = reduction is gaining [of electrons]

55
Q

Oxidation reaction

A

Half-reaction that involves loss of electron(s)

56
Q

Reduction reaction

A

Half-reaction that involves gain of electron(s)

57
Q

Oxidizing agents

A

Oxidizing agents are reduced and gain electron(s)

RIG = reduction is gain –> oxidizing agent reduces

58
Q

Reduction agents

A

Reducing agents are always oxidized and lose electron(s)

OIL = oxidization is loss – reducing agents oxidize

59
Q

Combination reaction

A

Type of redox reaction

A + B –> C

60
Q

Decomposition reaction

A

Type of redox reaction

C –> A + B

61
Q

Combustion reaction

A

Type of redox reaction

A + O2 –> B

Substance + O2 –> [1+ O-containing substances] + water

Emits heat (exothermic)

62
Q

Displacement reaction

A

Type of redox reaction

A + BC –> AC + B

3 subtypes:

  • *Hydrogen** displacement
  • *Metal** displacement
  • *Halogen** displacement
63
Q

Activity series for halogens

A

F2 > Cl2 > Br2 > I2

Note: order from top to bottom = decreasing activity

Note: diatomic!

64
Q

Disproportionation reaction

A

Type of redox reaction

Same element is simultaneously oxided and reduced

65
Q

Titrations

A

Measure the volume of one reagent required to react with a measured mass or volume of another reagent

  • *Often** used to determine amount of acid or base in sample
  • *Also** used for redox reactions

Buret drips into Erlenmeyer flask

66
Q

Indicator

A

Used in titrations to indicate when amount of known substance has neutralized unknown

67
Q

Endpoint (equivalence point)

A

When an acid and base have become neutralized

68
Q

Modified dilution equation

A

MacidVacid(# of H+) = MbaseVbase(# of OH-)

Gen Chem 01 (21 decks)

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