Unit 5 and 6 Flashcards
1
Q
Homogeneous mixture of two or more substances
A
Solution
2
Q
The most abundant component of a solution in terms of moles
A
Solvent
3
Q
Any component in a solution other than the solvent.
A
Solute
4
Q
Water is a (blank) but aqueous describes (blank)
A
Solvent, solution
5
Q
A substance that dissociates into ions when it dissolves enhancing the conductivity of the solvent
A
Electrolyte
6
Q
A substance that dissociates completely into ions when it dissolves in water
A
Strong electrolyte
7
Q
What is an example of a strong electrolyte?
A
Sodium chloride
8
Q
A substance that does not dissociate into ions and therefore does not enhance the conductivity of water when dissolved
A
Non electrolyte
9
Q
A substance that only partly dissociates into ions when it dissolves in water
A
Weak electrolyte
10
Q
Few ions =
A
Poor conductivity
11
Q
What is an example of a weak electrolyte?
A
Acetic acid
12
Q
A solution in which the solvent is water
A
Aqueous
13
Q
Interaction of water with ions
Positive H atoms attracted to (blank)
Negative O atom attracted to (blank)
A
Negative ion (anion) Positive ion (cation)
14
Q
The feature of water relates to the concept of (blank)
A
Polarity
15
Q
How do we know ions are present in aqueous solutions?
A
Solutions conduct electricity
16
Q
Homogeneous mixture of two or more substances
A
Solution
17
Q
What two things is a solution composed of?
A
Solute and solvent
18
Q
Substances that ionize in water to form electrically conducting solutions
A
Electrolytes
19
Q
Dissociates completely in solution
A
Strong electrolyte
20
Q
(Blank) conducts electricity
A
Strong electrolyte
21
Q
Dissociate partially in solution
A
Weak electrolyte
22
Q
Dissolve in solution but do not ionize
A
No electrolytes
23
Q
What are two examples of nonelectrolytes?
A
Ethanol and sugar
24
Q
When oxides of sulfur, nitrogen, or other Nonmetals dissolve in water, they produce (blank)
A
Hydrogen ions
25
A H+ bonded to a molecule of water, H2O
| The form in which the hydrogen ion is found in an aqueous solution
Hydronium ion (H3O+)
26
Proton donor
Acid
27
Proton acceptor
Base
28
Reaction that takes place when an acid reacts with a base and produces a solution of salt in water
Neutralization
29
The product of a neutralization reaction- made up of the cation of the base in the reaction plus the anion of the acid
Salt
30
A balanced equation describing a reaction in solution in with the reactants and products are written as undissociated molecules
Molecular equation
31
A balanced equation that shows all the species, both ionic and molecular, present in a reaction occurring in aqueous solution
Overall ionic equation
32
A balanced equation that describes the actual reaction taking place in aqueous solution; it is obtained by eliminating the spectator ions from the overall ionic equation
Net ionic equation
33
An ion that is present in a reaction vessel when a chemical reaction takes place but is unchanged by the reaction
Spectator ion
34
The reaction of water with another material
Hydrolysis
35
An acid that completely dissociates into ions in aqueous solution
Strong acids
36
An acid that only partially dissociates in aqueous solution and has a limited capacity to donate protons to the medium
Weak acid
37
A base that completely dissociates into ions in aqueous solution
Strong base
38
A base that only partially dissociates in aqueous solution and has a limited capacity to accept protons
Weak base
39
A substance that can behave as either a proton acceptor or proton donor
Amphiprotic
40
An analytical method for determining the concentration of a solute in a sample by reacting the solute with a standard solution of known concentration
Titration
41
The standard solution added to the sample in a titration
Titrant
42
Solution of known concentration used in titrations
Standard solution
43
A solid product formed from a reaction in a solution
Precipitate
44
A reaction that produces an insoluble product upon mixing two solutions
Precipitation reaction
45
(Blank) can be used to synthesize water-insoluble salts
Precipitation reactions
46
Common minerals that are often formed with anions that lead to insolubility
Sulfides, carbonates, oxides, hydroxides
47
A substance that produces hydrogen ions in solution
Acid
48
A substance that produces hydroxide ions in solution
Base
49
An acid ------- (blank) in water
H+
50
(Blank) are strong electrolytes and are completely ionized
Strong acids
51
(Blank) are weak electrolytes and only partially ionize
Weak acids
52
What is he chemical produced in the largest quantity in the US
Sulfuric acid
53
Acid that can furnish more than one proton
Polyprotic acid
54
Base -----(blank) in water
OH
55
(Blank) are strong electrolytes and are completely ionized
Strong bases
56
An important weak base
Ammonia (NH3)
57
Four steps to writing net ionic equation
1) write a balanced chemical equation
2) write a complete ionic equation
3) identify spectator ions
4) write the net ionic equation
58
The amount of solute in a particular amount of solvent or solution
Concentration
59
The concentration of a solution expressed in moles of solute per liter of solution
Molarity
60
A concentrated solution of a substance used to prepare solutions of lower concentration
Stock solution
61
The process of lowering the concentration of a solution by adding more solvent
Dilution
62
Driving force of a net ionic equation
Formation of an insoluble compound, a precipitate gas forming reaction
63
In acid base reaction the driving force is
The formation of water
64
A way to express acidity- the concentration of H+ in a solution
pH
65
Acidic solution pH
<7
66
Neutral solution pH
7
67
Basic solution pH
>7
68
The medium in which a solute is dissolved to form a solution
Solvent
69
The substance dissolved in a solvent to form a solution
Solute
70
Amount of solute in a solution is given by its concentration
Solution concentration
71
Molarity (M)
Moles of solute / liter of solution
72
Concentration M =
moles/ volume
73
Important point in dilution problems
Moles in initial solution = moles in final solution
74
Dilution equation
M(initial) x V (initial) = M (final) x V (final)
75
Millimolarity
Millimoles of solute / L of solution
76
Parts per million (ppm)
(Mass of substance / mass of sample)x 10^6
77
Parts per billion
(Mass of substance / mass of sample)x 10^9
78
A solution that contains the maximum concentration of a solute possible at a given temperature
Saturated solution
79
The maximum amount of a substance that dissolves in a given quantity of solvent at a given temperature
Solubility
80
Increase in temp = blank solubility of solids in water
Greater
81
A solution that contains more than the maximum quantity of solute predicted to be soluble in a given volume of solution at a given temperature
Supersaturated solution
82
Process by which one ion is displaced by another
Ion exchange
83
What is ion exchange important in?
Water purification
84
Neutral crystalline minerals or synthetic materials consisting of 3D networks of channels that contain sodium for other 1+ cations
Zeolite
85
All zeolites have a rigid (blank) structure
3D
86
Combination reactions of oxygen with Nonmetals such as carbon, sulfur, and nitrogen produce
Volatile oxides
87
Oxidation
Increase in oxygen
88
Reduction
Decrease in oxygen
89
A chemical changes in which a species loses electrons
Oxidation
90
The ON increases
Oxidation
91
The ON decreases
Reduction
92
A chemical change in which a species gains electrons
Reduction
93
Change in ON reflects the change in (blank) associated with an atom or ion
of electrons
94
A positive or negative # based on the number of electrons an atom gains or loses when it forms an ion, or that it shares when it forms a covalent bond with another element
Oxidation number or state
95
ON of atoms in neutral molecule sum
Zero
96
ON of atoms in ion sum to
Charge on ion
97
Each atom in pure element has an ON # of
0
98
In monatomic ions, the ON is the charge (blank)
ON the ion
99
In compounds containing fluorine and 1+ elements, ON is
-1
100
In most compounds the ON of hydrogen is (blank) and oxygen is (blank)
1+
| 2-
101
ON of metal hydrides
-1
102
ON of O in peroxide ion (O2_^2)
-1
103
A substance in a redox reaction that contains the element being reduced
Oxidizing agent
104
Electron acceptor
Oxidizing agent
105
A substance in a redox reaction that contains the element being oxidized
Reducing agent
106
Electron donor
Reducing agent
107
One of the two halves of an oxidation- reduction reaction
Half reaction
108
Step 1 to balance redox reaction
1) write one equation for the oxidation half reaction and a separate equation for the reduction half reaction
109
Step 2 to balance redox reaction
Balance the # of particles in each half reaction
110
Step 3 to balance redox reaction
Balance the charge in each half reaction (always ADD electrons)
111
Step 4 to balance redox reaction
Multiply each half-reaction by the appropriate whole #
112
Step 5 to balance redox reaction
Add the the two half reactions to generate the equation representing the redox reaction
113
A qualitative ordering of the oxidizing ability of metals and their cations
Activity series
114
A chemical equation describing the redox reaction in nature will be balanced when
1) the # of atoms of each element on both sides of the reaction are the same
2) the total charges on each side of the reaction arrow are the same
115
General approach to solution stoichiometry problem
Mass zinc- moles zinc- stoichiometric factor - moles HCl- volume or mass HCl
116
Steps to solve a solution stoichiometry problem
1) write the balanced equation
2) calculate the moles of Zn
3) use the stoichiometric factor
4) calculate the volume of HCl required
117
Acronym for oxidation reduction reactions
OIL-RIG
118
Oxidation involves (blank) of electrons
Loss
119
Reduction involves (blank) of electrons
Gains
120
6 rules for assigning oxidation states
1) the oxidation state of an atom in its natural form is 0
2) simple ions = oxidation # = charge on ion
3) oxygen has a oxidation # of 2- in compounds
4) oxidation # of H- +1
5) Fluorine always has an oxidation # of -1 in compounds
6) sum of ON in neutral compound =0
Sum of ON of a polyatomic ion = charge on ion
121
Redox reactions are characterized by (blank) between an electron donor and electron acceptor
Electron transfer
122
Increase in ON of some element
Oxidation
123
Decrease in ON of some element
Reduction
124
The point in a titration at which the # of moles of titrant added is stoichiometrically = to the # of moles of the substance being analyzed
Equivalence point
125
The point in a titration that is reached when just enough standard solution has been added to cause the indicator to change color
End point
126
Law of thermodynamics
Energy is neither created nor destroyed during chemical reactions
127
The chemical equation of a reaction that includes energy as a reactant or product
Thermochemical equation
128
Describes whether energy is absorbed or released when reaction occurs
Thermochemical equation
129
A form of energy required to move an object through a given distance
Work
130
The study of energy and its transformations
Thermodynamics
131
The study of the relation between chemical reactions and changes in energy
Thermochemistry
132
Process by which energy moves from a warmer object to a cooler object
Heat transfer
133
Energy transferred between objects because different temps
Heat
134
A condition in which temperature is uniform throughout a material and no energy flows from one point to another
Thermal equilibrium
135
Work =
Force x distance
136
Energy stored in an object because of its position
Potential energy
137
Potential energy equation
PE = mass x g (acceleration due to gravity) x h (vertical distance)
138
A property of an entity based solely on its chemical or physical state or both, but not how it achieved that state
State function
139
State function does not depend on
How object gets to a particular point
140
The energy of an object in motion due to its mass (m) and its speed (u)
Kinetic energy
141
Energy cannot be created nor destroyed but can be converted from one form into another
Law of conservation of energy
142
The kinetic energy of atoms, ions, and molecules
Thermal energy
143
Increase in particles = increase in
Thermal energy
144
Energy a particle has because of its electrostatic charge and its position relative to another particle
Electrostatic potential energy (Eel)
145
Electrostatic energy is directly proportional to the product of the charged of the particles and inversely proportional to the distance between them
Coulombic interaction
146
A lower electrostatic potential energy corresponds to
Greater stability
147
The part of the universe that is the focus of a thermochemical study
System
148
Everything that is not part of the system
Surroundings
149
A system that exchanges neither energy nor matter with the surroundings
Isolated system
150
A thermos bottle containing hot soup with the lid screwed on tightly
Isolated system
151
A system that exchanges energy but not matter with the surroundings
Closed system
152
A cup of hot soup with a lid
Closed system
153
A system that exchanges both energy and matter with the surroundings
Open system
154
An open cup of hot soup
Open system
155
Energy flows from a system into its surroundings
Exothermic
156
(Blank) process is a combustion reaction
Exothermic
157
Energy flows from the surroundings into the system
Endothermic process
158
Ice cubes in warm water = (blank) process
Endothermic process
159
Releases energy = (blank) process
Exothermic
160
Absorbs energy = (blank) process
Endothermic
161
System loses energy to its surroundings
Exothermic
162
System gained energy from surroundings
Endothermic
163
Q
Exothermic
164
Q>O
Endothermic
165
The sum of all the kinetic and potential energies of all the components of a system
Internal energy (E)
166
Delta E =
E final - E initial
167
Reducing agents are electron
Donors
168
Reducing agents get
Oxidized
169
Oxidizing agents are electron
Acceptors
170
Oxidizing agents get
Reduced
171
Represent two parts of a redox reaction
Half reactions
172
A technique in which one solution is used to analyze another
Titration
173
Procedure to determine the concentration of a solution in a titration
Standardization
174
Occurs when exact stoichiometric amounts of both reagents have been added in a titration
Equivalence point
175
Steps to find concentration
1) balance the equation
2) calculate amount of (blank)
3) calculate amount of (blank) required
4) calculate concentration
176
The study of energy and its inter conversions
Thermodynamics
177
Capacity to do work or transfer heat
Energy
178
Energy transferred between two objects due to a temperature difference between them
Heat
179
The energy required at a constant pressure to raise the temperature of 1 mole of a substance by 1 degree C
Molar heat capacity
180
Q =
M C dT
181
The energy required to raise the temperature of 1g of a substance 1 degree C at constant pressure
Specific heat
182
The quantity of energy needed to raise the temperature of a particular object 1 degree C at constant pressure
Heat capacity
183
The energy required to convert 1 mole of a solid substance at its melting point into the liquid state
Molar heat of fusion (delta Hfus)
184
Enthalpy change
Q = ndeltaHfus
185
The energy required to convert 1 mole of a liquid substance at its boiling point to the vapor state
Molar heat of vaporization (deltaHvap)
186
System takes in energy = blank value
+
187
Ability of water to absorb large quantities of energy
Heat sink
188
To calculate the enthalpy change that takes place when 1 g of methane or 1 g of propane burns in air, producing CO2 and liquid water, we
Divide the absolute value of change in reaction for each reaction by the mm of hydrocarbon
189
The energy released during the complete combustion of 1 g of a substance
Fuel value
190
As the # of carbon atoms/ molecules increases, the hydrogen to carbon ratio
Decreases
191
The amount of energy released during the complete combustion of 1 liter of a liquid fuel
Fuel density
192
The quantity of energy produced when a material consumed by an organism for sustenance is burned completely
Food value
193
A condition in which the system and its surroundings are at the same Temp and heat transfer stops
Thermal equilibrium
194
The collection of molecules we are studying
System
195
Results in the evolution of heat
| Heat flows from system to surroundings
Exothermic reactions
196
Absorbs energy
| Energy flows into system from surroundings
Endothermic reactions
197
Heat required to raise temp of 1 g of H2O by 1 degree C
1 calorie
198
1000 calorie
1 kc
199
1 kc
1 kcal
200
Amount of energy required to raise an objects temperature by 1 degree C
Heat capacity
201
The heat capacity per gram of substance
Specific heat capacity
202
Problems involving heat transfer can be approached by assuming the sum of the heat changes within a given substance is zero
Complex heat transfer
203
The amount of energy necessary to raise the temperature of 1 g of water by 1 degree C
Calorie
204
The total increase in the internal energy of a closed system is the
Sum of the work done on it (w) and any other energy (q) gained
Q + w
205
The energy gained or lost by a system must equal the energy lost or gained by the surroundings
First law of thermodynamics
206
Work done by a system on its surroundings internal energy (blank)
Decreases
207
The work associated with the expansion or compression of a gas
Pressure-volume (PV work)
208
System heated by surroundings (q blank)
>O
209
Work done by system (w blank)
210
Energy transferred from system to surroundings (q blank)
211
Heat absorbed by an endothermic process or given off by an exothermic process occurring at constant pressure
Enthalpy change (delta H)
212
Sum of the internal energy and the pressure to volume product of a system
Enthalpy (H)
213
All the energy (heat and work) exchanged by the system with surroundings
Delta E
214
Only q, heat exchanged at constant pressure
Delta H
215
Energy flows out of system
Endothermic
216
Endothermic, q and H
Q -
| Delta H
217
Heat flows into system
Exothermic
218
Exothermic, q and H
Q+
| h>O
219
The standard enthalpy of reaction delta Hrxn for a reaction that is the sum of two or more reactions is equal to the sum of the delta H run values of the constituent reactions
Hess's law
220
The capacity to do work or transfer heat
Energy
221
Thermal energy transferred from a warmer to a cooler object
Heat
222
Mechanical energy that moves an object from one place to another
Work
223
Heat into system = blank q
+
224
Heat out of system equals blank q
-
225
Work done on system
+
226
Work done by system
-
227
Heat transfer in
Endothermic
228
Heat transfer out
Exothermic
229
Work done on system
+w
230
Work done by system
-w
231
Heat content of a substance at constant pressure
Enthalpy
232
If Hfinal > H initial
Change in H- endothermic +
233
If H final < H initial then
Change in H - exothermic
234
Formation of water endothermic or exothermic
Exothermic
235
If a reaction is the sum of two or more reactions, the net delta H is the sum of the delta Hs of each reaction
Hess's law
236
Property that is independent of pathway
State function
237
The measurement of the quantity of heat transferred during a physical change or chemical process
Calorimetry
238
A device used to measure the absorption or release of energy by a physical change or chemical process
Calorimeter
239
The energy absorbed or given off by a chemical reaction = heat of reaction
Enthalpy of reaction
240
A constant volume device used to measure the energy released during a combustion reaction
Bomb calorimeter
241
Heat capacity of a calorimeter
Calorimeter constant
242
The enthalpy change of a formation reaction- also called standard heat of formation
Standard enthalpy of formation
243
A reaction in which 1 mole of substance is formed from its component elements in their standard states
Formation reaction
244
The most stable form of a substance under 1 bar pressure and some specified temperature
Standard state
245
The energy associated with a reaction that takes place under standard conditions
Standard enthalpy of reaction
246
More negative the heat of formation of a subsgance, the (blank)
More stable
247
Change in Hrxn
Sum of nproducts -sum of nreactants
248
Science of measuring heat
Calorimetry
249
Device used to experimentally determine the heat associated with a chemical reaction
Calorimeter
