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CHEM 1030 > Chapter 8 > Flashcards

Chapter 8 Flashcards

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1
Q

A type of matter that consists of more than one substance and can be separated into its components by making use of the different physical properties of the substances present

A

mixture

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2
Q

A ______ has a fixed composition, whereas the composition of a mixture can vary.

A

compound

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3
Q

A mixture in which the individual components are uniformly mixed, even on the molecular scale

A

Homogeneous Mixture

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4
Q

A homogeneous mixture is also known as a

A

solution

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5
Q

Solutions are made by dissolving a ______ into the _____

A

solute

solvent

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6
Q

A solution in which the solvent is water

A

Aqueous solution

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7
Q

The quantity of substance in a given volume

A

Concentration (mol/L)

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8
Q

A common way to express a solution concentration is ______
the amount of solute (in moles) divided by the volume of
solution (in liters).

A

Molarity (M)

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9
Q

a _____ is when a new solution is prepared from a stock solution (more concentrated solution)
To make solutions of lower concentrations from these stock solutions, more ______ is added.
The amount of solute doesn’t change; just the _____ of solution changes

A

dilution
solvent
volume

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10
Q

The mathematical relationship of a dilution is

A

M1V1 = M2V2

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11
Q

When a substance _____ in water to make a solution, the substance breaks into its component ions or molecules.

A

dissolves

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12
Q

When a substance _____ in water to make a solution, the substance separates into its component ions, which allows the solution to conduct electricity (electrolytes dissociate).

A

dissociates

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13
Q

Soluble ionic compounds ______when they dissolve in water

A

dissociate

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14
Q

Many molecular compounds dissolve, but do not _____

A

dissociate

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15
Q

solute that produces ions in solution which enables its solution to conduct electricity

A

Electrolyte

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16
Q

molecular substance that does not dissociate into ions when it dissolves in water and will not conduct electricity (such as C12H22O11, H2O, CH3OH, many carbon compounds)

A

Nonelectrolyte

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17
Q

______ electrolytes completely dissociate into ions

A

Strong

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18
Q

_____ electrolytes partially dissociation into their ions

A

Weak

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19
Q

compounds that when dissolved in water dissociate into ions.

Depending on what kind it is, their dissociation in water can be complete or partial.

A

acids and bases

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20
Q

Strong electrolytes include

A

soluble ionic compounds; strong acids; strong bases

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21
Q

Weak electrolytes include

A

weak acids, weak bases

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22
Q

electrolytes include

A

any molecular compound that is not a weak or strong electrolyte

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23
Q

When an ionic compound dissolves in water, the resulting solution contains:
Not the intact ionic compound itself but ________

A

component ions dissolved in water

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24
Q

NOT all ionic compounds dissolve in water. In general, a compound is termed _____ if it dissolves in water and ______ if it does not.

A

soluble

insoluble

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25
What compounds are soluble no exceptions?
Li+, Na+, K+, NH4+ | NO3- (nitrates) and C2H3O2- (acetate) or CH3COO-
26
Cl-, Br-, and I- are soluble except when paired with
Ag+, Hg2^2+, or Pb2+
27
SO4^2- is soluble except when paired with
Sr^2+, Ba^2+, Pb^2+, Ag+, or Ca^2+
28
OH- and S^2- are insoluble except when paired with
Li+, Na+, K+, NH4+ | Ca^2+, Sr^2+, Ba^2+
29
CO3^2- and PO4^3- are insoluble except when paired with
Li+, Na+, K+, NH4+
30
Precipitation reactions are reactions in which a ______ forms when two solutions are mixed. Reactions between _____ solutions of ionic compounds produce an ionic compound that is insoluble in water. • The insoluble product is called a _______
solid aqueous precipitate
31
Precipitation reactions do not always occur when two aqueous solutions are mixed. The product is written as ______
no reaction
32
How do you predict precipitation reactions?
1. Determine what ions each of the aqueous reactants has. 2. Determine formulas of possible products. • Exchange (switch) ions. • Balance charges of combined ions to get the formula of each product. 3. Determine the solubility of each product in water. • Use the solubility rules to determine if a product is insoluble or slightly soluble (i.e., it will precipitate) or if it forms a soluble compound. 4. If neither product will precipitate, write “no reaction” after the arrow. 5. If products are insoluble, write their formulas as the products of the reaction using (s) after the formula to indicate solid. Write any soluble products with (aq) after the formula to indicate aqueous. 6. Balance the equation.
33
An equation showing the complete neutral formula for each compound in the aqueous reaction as if they existed as molecules is called a
molecular equation.
34
In actual solutions of soluble ionic compounds, dissolved substances are present as ions. Equations that describe the material’s structure when dissolved are called
complete ionic equations.
35
What are the rules of writing a complete ionic equation?
Aqueous (aq) strong electrolytes are written as ions. Soluble salts, strong acids, strong bases Insoluble substances, weak electrolytes, and nonelectrolytes are written in molecular form. Solids (s), liquids (l), and gases (g) are not dissociated; hence, they remain in molecular form.
36
Notice that in the complete ionic equation, some of the ions in the solution appear unchanged on both sides of the equation. These ions are called ________ because they do not participate in the reaction.
spectator ions
37
A net ionic equation differs from a complete ionic equation because it does NOT have ______ in the equation.
spectator ions
38
Arrhenius Definition of Acid
Acid: a substance that dissociates to produce H+ in an aqueous solution (H+ is the same as H3O+)
39
Arrhenius Definition of Base
Base: a substance that dissociates to produce OH- in aqueous solutions
40
Strong acids and strong bases will dissociate _______ into their ions. Therefore, they are also strong electrolytes and will conduct electricity!
completely
41
Name strong acids
Hydrochloric acid HCl Hydrobromic acid HBr Hydroiodic acid HI Nitric acid HNO3 Perchloric acid HClO4 Sulfuric acid H2SO4
42
Name strong bases
Any group 1 or group 2 metal (Ca^2+, Sr^2+, Ba^2+) with an OH- Examples: NaOH LiOH Ba(OH)2
43
Brønsted-Lowry Definition of an acid
substance donates (loses) a proton (H+ ion)
44
Brønsted-Lowry Definition of a base
substance accepts a proton (H+ ion)
45
NH3 (aq) + H2O (l) ->
NH3 - base (accepts proton) H2O - acid (donates proton) NH4+ acid (lost proton) OH- - base (accepts proton)
46
NH3 and H2O are not a strong base or a strong acid, so they must be a weak base and a weak acid. Weak acids and weak bases are weak ______, so they weakly conduct electricity.
electrolytes
47
______ acids and bases are also Brønsted-Lowry acids and bases, but Brønsted- Lowry acids and bases may not be _____ acids and base
Arrhenius | Arrhenius
48
When an acid and a base react, the reaction is called a
neutralization reaction
49
In a neutralization reaction, an acid reacts with a base, and __________
the two neutralize each other, producing water (or in some cases a weak electrolyte)
50
As long as the salt that forms is soluble in water, the net ionic equation for an acid–base reaction involving a strong acid is:
H+ (aq) + OH- (aq) -> H2O (l)
51
A neutralization reaction is completed when the moles of acid ____ the moles of base in the solution.
equal
52
In a _______, a substance in a solution of known concentration is reacted with another substance in a solution of unknown concentration. In many cases the known solution (the _____) is added slowly to a flask containing the unknown solution from an instrument called a ____
titration titrant buret
53
In acid–base titrations, because both the reactant and product solutions are colorless, a chemical is added that changes color when the solution undergoes large changes in acidity/alkalinity. The chemical is called a(n) _____
indicator
54
Titration | The ______ of a reaction is when the indicator color changes.
endpoint
55
Titration The indicator is selected so that the endpoint is reached when the number of moles of H+ equals the number of moles of OH– . This is known as the __________
equivalence point.
56
The reactions in which electrons are transferred from one reactant to the other are called
oxidation– reduction reactions | These are also called redox reactions.
57
Many redox reactions involve the reaction of a substance with
oxygen
58
In a redox reaction, electrons are exchanged between species. Oxidation occurs when a species ____ electrons Reduction occurs when a species _____ electrons It is important to know that oxidation and reduction must take place together; whenever a species is oxidized, another species is reduced.
loses gains OIL RIG
59
An oxidation number is the “charge” it would have if it all shared electrons were assigned the
most electronegative atom.
60
Each atom in a pure element has oxidation number of
zero
61
For monatomic ions, the oxidation number is equal to the
charge on the ion
62
Group 1 metals always have a charge of | group 2 metals always have a charge of
+1 | +2
63
When combined with another element, fluorine always has an oxidation state of
-1
64
The oxidation number of oxygen in most compounds is | Except when combined with
-2 | fluorine F2O and peroxides.
65
The oxidation number of H in most compounds is | except with
+1 | metals
66
Cl, Br, and I have oxidation numbers of _ in compounds | except when combined with
-1 | oxygen and fluorine
67
The algebraic sum of the oxidation numbers for atoms in a neutral compound must add to
zero
68
in a polyatomic ion, the oxidation number of each atom must be equal to
the ion charge
69
The reactant that reduces an element in another reactant is called the
reducing agent
70
The reducing agent contains the element that is
oxidized
71
The reactant that oxidizes an element in another reactant is called the
oxidizing agent.
72
The oxidizing agent contains the element that is
reduced
73
Oxidizing and reducing agents can only be in the _____ of an equation
reactant

CHEM 1030 (8 decks)

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