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General Chemistry > Exam 2 > Flashcards

Exam 2 Flashcards

1
Q

Balanced Chemical Equation

A

Every atom on the reactant side ends up on the product side. Vice versa.

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2
Q

Limiting Reagent

A

Reactant in the shortest supply limits the amount of product

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3
Q

Excess Reagent

A

Reactant with excess amount after the reaction

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4
Q

Percent Yield

A

Actual Yield/ Theoretical Yield * 100

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5
Q

Solution

A

a homogenous mixture of two or more substances in which the ions or molecules intermingle freely

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6
Q

Solvent

A

component of a solution present in the largest amount. It is the medium into which solutes are mixed or dissolved.

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7
Q

Solute

A

Substance dissolved in the solvent.

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8
Q

Concentration

A

Ratios between the solute, solvent, and solution.

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9
Q

Dilute Solution

A

Has a small solute-solvent ratio

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10
Q

Concentrated Solution

A

Has a large solute-solvent ratio

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11
Q

Saturated Solution

A

Limit to how much solute can go into a solvent. When amount of solute added exceeds the limit, solution is saturated.

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12
Q

Unsaturated Solution

A

Less solute present than required for saturation.

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13
Q

Solubility and Temperature

A

Directly proportional. Increase temperature, increase solubility. Sometimes can dissolve MORE solute by heating the mixture. i.e. sugar water vs. simple syrup

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14
Q

Supersaturated Solution

A

Solution that contains more solute than required for saturation at a given temperature. Usually unstable.

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15
Q

Precipitation Reactions

A

Reactions that form precipitates

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16
Q

Electrolyte

A

a compound that conducts electricity either in solution or in a molten state.

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17
Q

Dissociation of Ionic Compound

A

Particles surrounded by solvent

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18
Q

Nonelectrolytes

A

aqueous solutions of most molecular compounds that do not conduct electricity

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19
Q

Hydrated

A

When a solute particle is surrounded by water

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20
Q

Ionic Equation

A

All soluble strong electrolytes are written in dissociated form.

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21
Q

Spectator Ions

A

Ions present in the reaction that do not participate.

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22
Q

Net Ionic Equation

A

Ionic equation without spectator ions. Allow us to generalize/ predict future relations. Charges on each side MUST balance.

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23
Q

Double Replacement Definition

A

a reaction of two salts in which the cations and the anions switch places.

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24
Q

Types of Replacement (single or double) Rx

A

gas forming, precipitation, acid-base

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25
Q

Gas forming rx

A
  • Type of replacement

- One product is a gas

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26
Q

Precipitation Rx

A
  • Type of replacement
  • use solubility rules
  • one product is a solid
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27
Q

Molarity

A

M

The number of moles of solute per liter of solution

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28
Q

Electrolyte

A

compound that conducts electricity in solution or molten state

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29
Q

Conductivity

A

get definition from Pam!

30
Q

dissociated vs. dissolved

A

dissociate: break into ions
dissolve: stay in lattice surrounded by H2O

31
Q

Dissociate

A

break up into ions

32
Q

Base

A

a substance that produces hydroxide in water

33
Q

Ionization Reaction

A

reaction that forms ions from neutral reactants

34
Q

Acid/Water Rx

A

Acid + H2O –> H3O+ + anion

35
Q

Monoprotic Acid

A

Only 1 H+ per molecule of acid

36
Q

Polyprotic Acid

A

Many H+ per molecule of acid

37
Q

Base/Water Rx

A

Base + H2O –> BaseH+ + OH-

38
Q

Binary Acids

A

binary compounds of hydrogen with nonmetals

39
Q

Oxoacids

A

acids that contain H, O, and another element

40
Q

Acid Salt

A

Salt of a partially neutralized polyprotic acid

41
Q

Naming Oxoacids

A

ate –> -ic + acid

ite –> -ous + acid

42
Q

Naming Binary Acids

A

‘hydro’ + nonmetal stem + ‘-ic’ acid.

43
Q

Naming Bases with O2-

A

(metal) oxide

44
Q

Strong Acid Definition

A

acids that are strong electrolytes

45
Q

Strong Acid List

A 
HClO4- perchloric acid
HCL- hydrochloric acid
HBr- hydrobromic acid
HI- hydroiodic acid
HNO3 - nitric acid
H2SO4 - sulfuric acid
46
Q

Strong Base Definition

A

metal hydroxide that dissociates essentially 100% in water

47
Q

Strong Bases in Group IIA

A

Ca(OH)2 - calcium hydroxide
Sr(OH)2 - strontium hydroxide
Ba(OH)2 - barium hydroxide
Mg(OH)2 - magnesium hydroxide

48
Q

weak electrolyte

A

substance that has low percent ionization or dissociation in water

49
Q

weak acid

A

acid that has low % ionization in solutions, poor proton donor

50
Q

weak base

A

base with low % ionization in solution, poor proton acceptor.

51
Q

forward reaction

52
Q

reverse reaction

53
Q

dynamic equilibrium

A
  • forward and reverse rx occurring at the same rate

- double arrows

54
Q

chemical equilibrium

A

dynamic equilibrium of a chemical system

55
Q

Coulomb’s Law

A

F = k (q1q2)/(d^2)

56
Q

ion charge to force

A

directly proportional

57
Q

distance to force

A

inversely proportional

58
Q

conjugate acid

A

a base that has gained a proton

59
Q

conjugate base

A

an acid that has lost a proton

60
Q

metal oxide

A
  • strong bases

- deprotonate water to make 2OH-

61
Q

metal hydroxide

62
Q

Molarity

A

moles of solute / liters of solution

63
Q

weight percent

A

(mass solute/ mass solution) * 100

64
Q

1 ppm

A

1 mg solute/kg of solution

65
Q

1 ppb

A

1 ug (microgram) solute/kg of solution

66
Q

When preparing solutions

A

add solid first, then liquid!

67
Q

Molarity of hydrates

A
  • use H2O in molar mass

- ignore after that

68
Q

moles in stock =

A

moles final

69
Q

moles =

A

Molarity * Volume (L)

70
Q

M1V1 =

General Chemistry (3 decks)

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