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Bettelheim and Chang > Chemical Reactions > Flashcards

Chemical Reactions Flashcards

1
Q

is the sum of the atomic weights in atomic mass units (amu) of all the atoms in the compound’s formula. It is used for ionic and molecular compounds.

A

Formula weight

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2
Q

sum of the atomic weights in atomic mass units (amu) of all the atoms and is used only for covalent compounds

A

atomic weight

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3
Q

The formula weight of a substance expressed in grams

A

mol

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4
Q

the amount of any substance that contains as many formula units as the number of atoms in 12 g of carbon-12.

A

Avogadro’s number (6.022x10^23)

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5
Q

Avogadro’s number from

A

Amadeo Avogadro

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6
Q

is the formula weight of the substance expressed in grams.

A

molar mass

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7
Q

reactants that are converted to the products carbon dioxide and water in a chemical reaction called

A

combustion

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8
Q

A representation using chemical formulas of the process that occurs when reactants are converted to products

A

chemical reaction

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9
Q

To balance an equation, we place numbers in front of the formulas until the number of each kind of atom in the products is the same as the number in the starting materials. These numbers are called

A

coefficients

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10
Q

The mass relationships in a chemical reaction

A

stoichiometry

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11
Q

“Stoichiometry” comes from the Greek

A

Stoicheion = element; metron = measure

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12
Q

The reactant that is consumed, leaving an excess of another reagent or reagents unreacted

A

Limiting reagent

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13
Q

A reaction that does not give the main product is called a

A

Side reaction

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14
Q

The mass of product formed in a chemical reaction

A

Actual yield

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15
Q

The mass of product that should form in a chemical reaction according to the stoichiometry of the balanced equation

A

Theoretical yield

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16
Q

The actual yield divided by the theoretical yield times 100

A

percent yield

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17
Q

ionic compounds always consist of both positive and negative ions. When they dissolve in water, the positive and negative ions become separated from each other by water molecules.

A

Dissociation

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18
Q

Ions that do not participate in a reaction are called

A

spectator ions

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19
Q

kind of equation that we write for ions in solution is called a

A

net ionic equation

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20
Q

is the loss of electrons

A

oxidation

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21
Q

the gain of electrons.

A

reduction

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22
Q

involves the transfer of electrons from one species to another

A

oxidation–reduction reaction/redox reaction

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23
Q

An entity that accepts electrons in an oxidation–reduction reaction

A

oxidizing agent

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24
Q

An entity that donates electrons in an oxidation–reduction reaction

A

reducing agent

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25
Q

are redox reactions in which the compounds or mixtures that are burned are oxidized by oxygen, O2.

A

Combustion

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26
Q

The oxygen in the air we breathe oxidizes carbon-containing compounds in our cells to produce CO2 and H2O.

A

Respiration

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27
Q

When iron or steel objects are left out in the open air, they eventually rust

A

Rusting

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28
Q

involves oxidation, and common bleaches are oxidizing agents.

A

Bleaching

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29
Q

A voltaic cell is a device in which electricity is generated from a chemical reaction.

A

Batteries

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30
Q

The heat given off or absorbed in a chemical reaction

A

Heat of reaction

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31
Q

A chemical reaction that gives off heat

A

Exothermic reaction

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32
Q

A chemical reaction that absorbs heat

A

Endothermic reaction

33
Q

The heat given off in a combustion reaction is called the

A

Heat of combustion

34
Q

The ionization of acetic acid is written with a double arrow to show that it is a ________; that is, the reaction can occur in both directions.

A

reversible reaction

35
Q

results in the formation of an insoluble product, or precipitate

A

precipitation reaction

36
Q

an insoluble solid that separates from the solution

A

precipitate

37
Q

the formulas of the compounds are written as though all species existed as molecules or whole units

A

molecular equation

38
Q

shows dissolved species as free ions

A

ionic equation

39
Q

ions that are not involved in the overall reaction

A

spectator ions

40
Q

shows only the species that actually take part in the reaction

A

net ionic equation

41
Q

as substances that ionize in water to produce H+ ions

42
Q

substances that ionize in water to produce OH- ions

43
Q

classify substances whose properties in aqueous solutions were well known.

A

Svante Arrhenius

44
Q

Notes for acid

A

*Acids have a sour taste
*Acids cause color changes in plant dyes (Blue to red)
* Acids react with certain metals, such as zinc, magnesium, and iron, to produce hydrogen gas.
* Acids react with carbonates and bicarbonates, such as Na2CO3, CaCO3, and NaHCO3, to produce carbon dioxide gas
* Aqueous acid solutions conduct electricity.

45
Q

Notes for base

A
  • Bases have a bitter taste
  • Bases feel slippery
  • Bases cause color changes in plant dyes (red to blue)
  • Aqueous base solutions conduct electricity
46
Q

a proton donor

A

Bronsted acid

47
Q

a proton acceptor

A

Bronsted base

48
Q

hydrated proton, H3O+, is called the

A

hydronium ion

49
Q

each unit of the acid yields one hydrogen ion upon ionization

A

monoprotic acid

50
Q

Acids commonly used in the laboratory include

A

Hydrochloric acid, acetic acid, sulfuric acid, phosphoric acid

51
Q

each unit of the acid gives up two H+ ions

A

diprotic acid

52
Q

yield three H+ ions, are relatively few in number

A

Triprotic acid

53
Q

a reaction between an acid and a base

A

Neutralization reaction

54
Q

an ionic compound made up of a cation other than H+ and an anion other than OH- or O2-

55
Q

Whereas acid-base reactions can be characterized as proton-transfer processes, the class

A

Oxidation-reduction or redox reactions

56
Q

refers to the half-reaction that involves loss of electrons

A

Oxidation reaction

57
Q

half-reaction that involves gain of electrons

A

Reduction reaction

58
Q

donates electrons to oxygen and causes oxygen to be reduced

A

reducing agent

59
Q

it accepts electrons from calcium, causing calcium to be oxidized

A

oxidizing agent

60
Q

signifies the number of charges the atom would have in a molecule (or an ionic compound) if electrons were transferred completely

A

oxidation number

61
Q

Rules to assign oxidation number

A
  1. In free elements (that is, in the uncombined state), each atom has an oxidation number of zero. Thus each atom in H2, Br2, Na, Be, K, O2, and P4 has the same oxidation number: zero.
  2. For ions composed of only one atom (that is, monatomic ions) the oxidation number is equal to the charge on the ion. All alkali metals have an oxidation number of +1 and all alkaline earth metals have an oxidation number of +2 in their compounds. Aluminum has an oxidation number of +3 in all its compounds.
  3. The oxidation number of oxygen in most compounds (for example, MgO and H2O) is -2, but in hydrogen peroxide (H2O2) and peroxide ion (O22-), it is -1.
  4. The oxidation number of hydrogen is +1, except when it is bonded to metals in binary compounds. In these cases (for example, LiH, NaH, CaH2), its oxidation number is -1.
  5. Fluorine has an oxidation number of -1 in all its compounds. Other halogens (Cl, Br, and I) have negative oxidation numbers when they occur as halide ions in their compounds.
  6. In a neutral molecule, the sum of the oxidation numbers of all the atoms must be zero. In a polyatomic ion, the sum of oxidation numbers of all the elements in the ion must be equal to the net charge of the ion.
  7. Oxidation numbers do not have to be integers.
62
Q

Four general types of redox reactions

A

combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions

63
Q

two or more substances combine to form a single product

A

Combination reaction

64
Q

the breakdown of a compound into two or more components

A

decomposition reaction

65
Q

an ion (or atom) in a compound is replaced by an ion (or atom) of another element

A

displacement reaction

66
Q

Most displacement reactions fit into one of three subcategories:

A

hydrogen displacement, metal displacement, or halogen displacement

67
Q

All alkali metals and some alkaline earth metals (Ca, Sr, and Ba), which are the most reactive of the metallic elements, will displace hydrogen from cold water. Less reactive metals, such as aluminum and iron, react with steam to give hydrogen gas

A

Hydrogen displacement

68
Q

A metal in a compound can be displaced by another metal in the elemental state.

A

Metal displacement

69
Q

a convenient summary of the results of many possible displacement reactions

A

activity series

70
Q

Another activity series summarizes the halogens’ behavior in halogen displacement reaction

A

Halogen displacement

71
Q

an element in one oxidation state is simultaneously oxidized and reduced.

A

Disproportionation reaction

72
Q

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

A

concentration of solution

73
Q

the procedure for preparing a less concentrated solution from a more concentrated one.

74
Q

an analytical technique based on the measurement of mass

A

gravimetric analysis

75
Q

the determination of the amount or concentration of a substance in a sample

A

quantitative analysis

76
Q

a solution of accurately known concentration

77
Q

is added gradually to another solution of unknown concentration, until the chemical reaction between the two solutions is complete

A

standard solution

78
Q

the point at which the acid has completely reacted with or been neutralized by the base

A

equivalence point

79
Q

substances that have distinctly different colors in acidic and basic media

A

indicators

Bettelheim and Chang (7 decks)

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