Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CHEM 401 > CHAPTER 4 > Flashcards

CHAPTER 4 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

A homogeneous mixture of two or more substances and components are mixed uniformly together.

A

solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

A substance that is present in a smaller amount.

A

solute

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

The substance is present in a larger amount and may be a solid, liquid, or gas.

A

solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

The solute initially is a liquid or a solid and the solvent is water.

A

aqueous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

A substance that, when dissolved in water, results in a solution that can conduct electricity.

A

electrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

A substance that does not conduct electricity when dissolved in water.

A

non-electrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What allows the solutions to conduct electricity?

A

The movements of ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Breaking up of the compound into cations and anions.

A

dissociation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

They have large dipole moments (“partial charges”) and contain bonds between atoms with very different electronegativities such as oxygen and hydrogen.

A

polar solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

The process in which an ion is surrounded by water molecules.

This also helps to stabilize ions in solution and prevents cations from recombining with anions.

the result of a strong interaction between solute particles and H2O molecules.

A

hydration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

The separation of acids and bases into ions.

A

ionization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

The reaction can occur in both directions.

A

reversible reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Most ____ substances, aside from acids and bases, are nonelectrolytes and do not conduct electricity in aqueous solutions.

A

molecular substances

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why does an aqueous solution of an ionic substance conduct an electric current?

A

The solution contains ions that are free to move.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What structural feature will allow a substance to conduct an electric current?

A

The presence of charged particles that are free to move independently.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Dissociates or ionizes 100% in water and conducts an electric current in aqueous solution.

A

strong electrolyte

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Dissociates or ionizes less than 100% in water, and conducts a limited amount of electric current in aqueous solution.

A

weak electrolyte

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Does not dissociate or ionize in water and does not conduct an electric current in aqueous solution.

A

nonelectrolyte

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What ions are released when the ionic compound Fe2(SO4)3 dissociates in aqueous solution?

A

SO42–

Fe3+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

When an ionic compound dissolved in water, the cations are attracted to the ___ atom(s) of the H2O molecule, while the anions are attracted to the ___ atom(s).

A

oxygen; hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

In aqueous solution, a soluble ionic compound dissociates into its ___, which are free to move independently, allowing the solution to conduct electricity. Ionic compounds are therefore classified as ___.

A

ions; electrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

An electric current is a flow of charge through a medium, and can be carried by the movement of ___.

A

electrons and ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

___ will not ionize or dissociate in water and is therefore a nonelectrolyte.

A

Glucose (C6H12O6)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

___ will ionize in the presence of water to a small extent (< 100%) and is therefore a weak electrolyte.

A

Ammonia (NH3)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Which of the following balanced equations correctly represents the dissociation of Ni(NO3)2 in water?

A

Ni(NO3)2(s) → Ni2+(aq) + 2NO3–(aq)

Ni(NO3)2 consists of Ni2+ ions and NO3– ions, which dissociate from each other in aqueous solution. Each unit of Ni(NO3)2 forms one Ni2+ ions and two NO3– ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Why is an acid able to produce ions in aqueous solution?

A

An acid (H-X) dissociates into H+ and X- in solution. Each ion is surrounded by water and stabilized by hydration.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Strong acids and bases ___ completely to form ___ in water. The resulting solution conducts electricity well; hence these compounds are classified as ___ electrolytes.

A

ionize: gas: strong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Acids (e.g. HCl) are ___ compounds that nonetheless produce ions in aqueous solutions as the H2O molecules attract the ionizable hydrogen atoms in the compound, causing the ___ H-X bond to break. Acids are therefore electrolytes.

A

ionic; covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

The formation of an insoluble product, known as a precipitate.

One common type of reaction that occurs in aqueous solution.

____ reactions usually involve ionic compounds.

A ___ reaction is a reaction in which two or more water-soluble ionic compounds react in aqueous solution to form one or more insoluble/solid precipitates.

A

precipitation reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

An insoluble solid that separates from the solution.

A

precipitate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

A reaction that involves the exchange of parts between the two compounds.

Also called as a double-displacement reaction.

A

metathesis reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

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

A

solubility

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

A substance is ____ if a fair amount of it visibly dissolves when added to water.

A

soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

All ___ compounds are strong electrolytes, but they are not equally soluble.

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

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

It identifies the reagents; however, it does not describe in detail what actually is happening in solution.

A

molecular equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Dissolved species are free, hydrated ions.

Charges and atoms must be balanced in an ___equation.

Charges must be included where relevant in an ___equation.

The ___equation includes all ions, including spectator ions.

A

ionic equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Ions that are not involved in the overall reaction.

They appear on both sides of an equation, they can be eliminated from the ionic equation.

Ions that do not participate in the reaction although they are present

A

spectator ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Shows only the species that actually take part in the reaction.

A

net ionic equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

PROCEDURE FOR WRITING IONIC AND NET IONIC EQUATIONS

A
  1. balance molecular equation
  2. write ionic equation
  3. cancel spectator ions
  4. net ionic equation
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Which of the following options correctly contrast strong and weak acids in terms of electrolyte behavior?

A

Both strong and weak acids are electrolytes.

A solution of a weak acid always contains some unionized acid molecules.

All molecules of a strong acid will ionize in aqueous solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Match each type of hydrogen atom in the formula CH3COOH.

A

H of CH3 group -> NOT readily ionizable

H of COOH group -> READILY ionizable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

What ions are released when the ionic compound Fe2(SO4)3 dissociates in aqueous solution?

A

SO42–

Fe3+

The cation in this compound is Fe3+. You can determine this from SO42– present. If there are 3 SO42– ions, the total negative charge is 3(–2) = –6. The total positive charge must therefore be +6, meaning that each Fe ion must carry a 3+ charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

The symbol ⇌ indicates that a reaction is ___, meaning that reactants are converted to products and products are in turn reconverted to reactants.

An acid undergoes partial ionization in water.

An aqueous solution contains a weak electrolyte.

A

reversible

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

Ionize completely in aqueous solution

A

strong acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Strong acids are classified as ___

A

strong electrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

They form very few ions in aqueous solution

A

weak acids

47
Q

Weak acids are classified as ___

A

weak electrolytes

48
Q

Why is the formula for acetic acid typically written as CH3COOH instead of C2H4O2?

A

The H of the COOH group is ionizable, while the H atoms bonded in the CH3 group are not.

49
Q

When a chemical reaction is reversible _____.

A

reactants and products are present together

products react to form reactants

reactants continuously form products

50
Q

When a reversible chemical reaction occurs in a closed system, a state of dynamic chemical equilibrium is reached when the ____ of the forward and reverse reactions are equal. At this point the ____ of the reactants and products no longer change, although the forward and reverse reactions continue to occur.

A

rates; concentrations

51
Q

There appears to be no visible change in the concentrations of reactants or products.

The forward and reverse reactions occur at equal rates.

A

chemical system at equilibrium

52
Q

Readily reversible and reaches chemical equilibrium under ordinary conditions

A

The ionization of CH3COOH in aqueous solution

53
Q

Ions that always form soluble ionic compounds

A

NO3–

Group 1A cations

NH4+

54
Q

The balanced equation below is not a representation of metathesis reaction.

Pb(NO3)2(aq) + 2NaCH3COO(aq) → Pb(CH3COO)2(aq) + 2NaNO3(aq)

A

This reaction is NOT a metathesis reaction. A metathesis reaction is one in which two compounds exchange partners. Although it appears that this happens in the equation shown here, because both products are soluble in water all the ions simply remain dissociated and separate in solution. No actual exchange of partners has occurred.

55
Q

A reversible reaction in a closed system can reach a state of chemical ___, in which the rate of the forward reaction is equal to the rate of the reverse reaction.

A

equilibrium

56
Q

These compounds are ___ in water
NH4Cl

Pb(NO3)2

Na3PO4

(NH4)2CO3

Ca(ClO3)2

K2SO4

A

soluble

57
Q

What are the influences in the solubility of a solute in a solvent?

A

Quantity of solvent

Chemical nature of the solute

Temperature

58
Q

The following cations often produce water- ___ salts, even with anions such as SO4 2-
Ag+

Hg2 2+

Pb2+

A

insoluble

59
Q

A chemical equation that shows all reactants and products as intact, undissociated compounds is called a(n)
____. The name is misleading because not all compounds are composed of ____.

A

molecular

molecules

60
Q

An ionic equation shows species ____ in solution. This equation is the ____ accurate representation of the chemical change occurring.

A

An ionic equation shows ALL species present, not just spectator ions. This gives the most accurate representation of the chemical reaction occurring.

61
Q

Ions that typically form water-___salts, except when partnered with a Group 1A cation or NH4+

OH–

PO43–

CO32–

A

insoluble

62
Q

new ion combination that may form a precipitate

A

cation-anion

63
Q

will not form a precipitate

A

soluble ion combination

64
Q

cannot combine to form a compound

A

cation-cation

65
Q

will precipitate from solution

A

insoluble ion combination

66
Q

compounds that are correctly paired with their solubility in water at 25°C.
CaSO4, ___

(NH4)2S, ___

A

insoluble; soluble

67
Q

A ___equation will not include any charges on any of the species.

This equation represents all reactants and products as if they were intact and undissociated.

A

molecular equation

68
Q

It is the ___ in solution that will combine to form a precipitate in this type of reaction, not molecules. A precipitate is an ___ salt.

A

ions; insoluble

69
Q

Substances that ionize in water to produce H+ ions.

have a sour taste

cause color changes in plant dyes; for example, they change the color of litmus from blue to red.

They react with certain metals such as zinc, magnesium and iron to produce hydrogen gas.

They react with carbonates and bicarbonates such as Na2CO3, CaCO3, and NaHCO3, to produce carbon dioxide gas.

A

acids

70
Q

____ acid solutions conduct electricity

A

aqueous

71
Q

Substances that ionize in water to produce OH- ions.

Have a bitter taste

slippery

cause color changes in plant dyes; for example, they change the color of litmus from red to blue.

example of this:
Ba(OH)2
NH3
NaOH

A

bases

72
Q

____ base solutions conduct electricity.

A

aqueous

73
Q

Swedish chemist who defined acids and bases to classify substances whose properties in aqueous solutions were well known.

A

Svante Arrhenius

74
Q

Acid increases the concentration of H+ ions in aqueous solution

A

Acid according to Arrhenius

75
Q

Base increases the concentration of OH- ions in aqueous solution

A

Base according to Arrhenius

76
Q

Danish chemist

A

Johannes Bronsted

77
Q

proton donor

A

Acid according to Bronsted-Lowry

78
Q

proton acceptor

A

Base according to Bronsted-Lowry

79
Q

Each unit of the acid yield one hydrogen ion upon ionization.

A

monoprotic acids

80
Q

ionizes completely in aqueous solution

A

strong acid

81
Q

has a low percentage ionization in aqueous solution

A

weak acid

82
Q

there are no intact molecules

A

in a solution of a strong acid

83
Q

there will be intact acid molecules as well as ions

A

in a solution of a weak acid

84
Q

The following substances are ____:
H2O

HSO4–

HCO3–

A

amphoteric

85
Q

The following substances are ____:
HBr(aq)

H3PO4(aq)

CH3CH2COOH(aq)

A

acidic

86
Q

neutralization occurs between _____ and _____.

their products are typically ionic compound which is called salt and the neutral molecule water

The net ionic equation is typically given by H+ (aq) + OH–(aq) → H2O(l).

A

strong acid and strong base

87
Q

The reaction between an acid and a base is often called a(n) ____ reaction because the H+ ions produced by the acid react with OH– ions produced by the base, thus ____ each other.

A

neutralization; neutralizing

88
Q

The following are considered ___ in the aqueous solution:

Ca(OH)2

NaOH

NH3

Na2O

A

basic

89
Q

transfer of electrons from one atom or ion to another

A

electrons

90
Q

The transfer of electrons in a redox reaction is tracked using a(n) ___ number. This number is the charge an atom would have if all bonds were ___ in nature.

A

oxidation; ionic

91
Q

the species being reduced in oxidation

the species that shows a decrease in oxidation number

gains electrons

A

oxidizing agent

92
Q

the species oxidized in oxidation

the species that shows an increase in oxidation number

loses electrons

A

reducing agent

93
Q

half-reaction that involves loss of electrons

A

oxidation reaction

94
Q

half-reaction that involves gain of electrons

In a decomposition reaction a single reactant forms two or more different products.

A thermal decomposition involves heat and is indicated using the symbol Δ.

In a displacement reaction the number of substances on both sides of the equation remains the same.

A

reduction reaction

95
Q

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

track movement of electrons in chemical reactions

the charge of an atom WOULD have if electrons were always transferred, but it is NOT an actual charge.

A

oxidation number or oxidation state

96
Q

Rules for assigning oxidation numbers

A

(1) The sum of the oxidation numbers for the atoms in a neutral compound is zero
(2) The oxidation number for a monatomic ion is the same as its charge

97
Q

the highest oxidation number any main-group element from period 3 onward can have is equal to ____

A

the A-group number

98
Q

Displacement reactions are a type of oxidation-reduction reaction.

Displacement reactions involve an ion (or atom) in a compound that is replaced by an ion (or atom) of another element.

A

Displacement reactions

99
Q

All elements can have an oxidation state of 0.

Metals tend to have positive oxidation numbers only.

Transition metals usually have more than one possible oxidation number.

A

periodic trends in oxidation number

100
Q

the ___ of a substance results in an increase in its oxidation number and lose electrons.

A

oxidation

101
Q

the ___ of a substance results in a decrease in its oxidation number and gain electrons

A

reduction

102
Q

any metal listed in activity series will react with any ____ (in a compound) below it)

A

metal

103
Q

All elements can have an oxidation state of 0.

Metals tend to have positive oxidation numbers only.

Transition metals usually have more than one possible oxidation number.

A

periodic trends in oxidation number

104
Q

a convenient summary of the results of many possible displacement reactions

A metal higher up on the list will displace the ions of another metal further down the list from solution.

Metals become less reactive the further down the series you go.

Metals high on the list react more easily with cold water than metals low on the list.

A

activity series

105
Q

any metal above ___ will displace it from water or from an acid, but metals below ____ will not react with either water or an acid

A

hydrogen

106
Q

reaction in which two or more substances combine to form a single product

A

combination

107
Q

the breakdown of a compound into two or more components

A

decomposition

108
Q

a reaction in which a substance reacts with oxygen, usually with the release of heat and light to produce a flame

A

combustion

109
Q

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

fit into one of three subcategories: hydrogen ___, metal ___, or halogen ___

A

displacement

110
Q

all alkali and some alkaline earth metals (Ca, Sr, and Ba), which most reactive of the metallic elements will displace hydrogen from cold water

A

hydrogen displacement

111
Q

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

A

metal displacement

112
Q

another activity series summarizes the halogens’ behavior

F2 > Cl2 > Br2 > I2

A

Halogen displacement

113
Q

an element in one oxidation state is simultaneously oxidized and reduced

one reactant always contains an element that can have at least three oxidation states

A

disproportionation

CHEM 401 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions