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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
are redox reactions in which the compounds or mixtures that are burned are oxidized by oxygen, O2.
Combustion
26
The oxygen in the air we breathe oxidizes carbon-containing compounds in our cells to produce CO2 and H2O.
Respiration
27
When iron or steel objects are left out in the open air, they eventually rust
Rusting
28
involves oxidation, and common bleaches are oxidizing agents.
Bleaching
29
A voltaic cell is a device in which electricity is generated from a chemical reaction.
Batteries
30
The heat given off or absorbed in a chemical reaction
Heat of reaction
31
A chemical reaction that gives off heat
Exothermic reaction
32
A chemical reaction that absorbs heat
Endothermic reaction
33
The heat given off in a combustion reaction is called the
Heat of combustion
34
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.
reversible reaction
35
results in the formation of an insoluble product, or precipitate
precipitation reaction
36
an insoluble solid that separates from the solution
precipitate
37
the formulas of the compounds are written as though all species existed as molecules or whole units
molecular equation
38
shows dissolved species as free ions
ionic equation
39
ions that are not involved in the overall reaction
spectator ions
40
shows only the species that actually take part in the reaction
net ionic equation
41
as substances that ionize in water to produce H+ ions
acids
42
substances that ionize in water to produce OH- ions
base
43
classify substances whose properties in aqueous solutions were well known.
Svante Arrhenius
44
Notes for acid
*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
Notes for base
* Bases have a bitter taste * Bases feel slippery * Bases cause color changes in plant dyes (red to blue) * Aqueous base solutions conduct electricity
46
a proton donor
Bronsted acid
47
a proton acceptor
Bronsted base
48
hydrated proton, H3O+, is called the
hydronium ion
49
each unit of the acid yields one hydrogen ion upon ionization
monoprotic acid
50
Acids commonly used in the laboratory include
Hydrochloric acid, acetic acid, sulfuric acid, phosphoric acid
51
each unit of the acid gives up two H+ ions
diprotic acid
52
yield three H+ ions, are relatively few in number
Triprotic acid
53
a reaction between an acid and a base
Neutralization reaction
54
an ionic compound made up of a cation other than H+ and an anion other than OH- or O2-
salt
55
Whereas acid-base reactions can be characterized as proton-transfer processes, the class
Oxidation-reduction or redox reactions
56
refers to the half-reaction that involves loss of electrons
Oxidation reaction
57
half-reaction that involves gain of electrons
Reduction reaction
58
donates electrons to oxygen and causes oxygen to be reduced
reducing agent
59
it accepts electrons from calcium, causing calcium to be oxidized
oxidizing agent
60
signifies the number of charges the atom would have in a molecule (or an ionic compound) if electrons were transferred completely
oxidation number
61
Rules to assign oxidation number
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
Four general types of redox reactions
combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions
63
two or more substances combine to form a single product
Combination reaction
64
the breakdown of a compound into two or more components
decomposition reaction
65
an ion (or atom) in a compound is replaced by an ion (or atom) of another element
displacement reaction
66
Most displacement reactions fit into one of three subcategories:
hydrogen displacement, metal displacement, or halogen displacement
67
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
Hydrogen displacement
68
A metal in a compound can be displaced by another metal in the elemental state.
Metal displacement
69
a convenient summary of the results of many possible displacement reactions
activity series
70
Another activity series summarizes the halogens’ behavior in halogen displacement reaction
Halogen displacement
71
an element in one oxidation state is simultaneously oxidized and reduced.
Disproportionation reaction
72
the amount of solute present in a given quantity of solvent or solution
concentration of solution
73
the procedure for preparing a less concentrated solution from a more concentrated one.
Dilution
74
an analytical technique based on the measurement of mass
gravimetric analysis
75
the determination of the amount or concentration of a substance in a sample
quantitative analysis
76
a solution of accurately known concentration
titration
77
is added gradually to another solution of unknown concentration, until the chemical reaction between the two solutions is complete
standard solution
78
the point at which the acid has completely reacted with or been neutralized by the base
equivalence point
79
substances that have distinctly different colors in acidic and basic media
indicators

Bettelheim and Chang (7 decks)

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