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Chemisty > Unit 5 and 6 > Flashcards

Unit 5 and 6 Flashcards

1
Q

Homogeneous mixture of two or more substances

A

Solution

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2
Q

The most abundant component of a solution in terms of moles

A

Solvent

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3
Q

Any component in a solution other than the solvent.

A

Solute

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4
Q

Water is a (blank) but aqueous describes (blank)

A

Solvent, solution

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5
Q

A substance that dissociates into ions when it dissolves enhancing the conductivity of the solvent

A

Electrolyte

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6
Q

A substance that dissociates completely into ions when it dissolves in water

A

Strong electrolyte

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7
Q

What is an example of a strong electrolyte?

A

Sodium chloride

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8
Q

A substance that does not dissociate into ions and therefore does not enhance the conductivity of water when dissolved

A

Non electrolyte

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9
Q

A substance that only partly dissociates into ions when it dissolves in water

A

Weak electrolyte

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10
Q

Few ions =

A

Poor conductivity

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11
Q

What is an example of a weak electrolyte?

A

Acetic acid

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12
Q

A solution in which the solvent is water

A

Aqueous

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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)
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14
Q

The feature of water relates to the concept of (blank)

A

Polarity

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15
Q

How do we know ions are present in aqueous solutions?

A

Solutions conduct electricity

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16
Q

Homogeneous mixture of two or more substances

A

Solution

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17
Q

What two things is a solution composed of?

A

Solute and solvent

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18
Q

Substances that ionize in water to form electrically conducting solutions

A

Electrolytes

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19
Q

Dissociates completely in solution

A

Strong electrolyte

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20
Q

(Blank) conducts electricity

A

Strong electrolyte

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21
Q

Dissociate partially in solution

A

Weak electrolyte

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22
Q

Dissolve in solution but do not ionize

A

No electrolytes

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23
Q

What are two examples of nonelectrolytes?

A

Ethanol and sugar

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24
Q

When oxides of sulfur, nitrogen, or other Nonmetals dissolve in water, they produce (blank)

A

Hydrogen ions

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25
Q

A H+ bonded to a molecule of water, H2O

The form in which the hydrogen ion is found in an aqueous solution

A

Hydronium ion (H3O+)

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26
Q

Proton donor

A

Acid

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27
Q

Proton acceptor

A

Base

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28
Q

Reaction that takes place when an acid reacts with a base and produces a solution of salt in water

A

Neutralization

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29
Q

The product of a neutralization reaction- made up of the cation of the base in the reaction plus the anion of the acid

A

Salt

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30
Q

A balanced equation describing a reaction in solution in with the reactants and products are written as undissociated molecules

A

Molecular equation

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31
Q

A balanced equation that shows all the species, both ionic and molecular, present in a reaction occurring in aqueous solution

A

Overall ionic equation

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32
Q

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

A

Net ionic equation

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33
Q

An ion that is present in a reaction vessel when a chemical reaction takes place but is unchanged by the reaction

A

Spectator ion

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34
Q

The reaction of water with another material

A

Hydrolysis

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35
Q

An acid that completely dissociates into ions in aqueous solution

A

Strong acids

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36
Q

An acid that only partially dissociates in aqueous solution and has a limited capacity to donate protons to the medium

A

Weak acid

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37
Q

A base that completely dissociates into ions in aqueous solution

A

Strong base

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38
Q

A base that only partially dissociates in aqueous solution and has a limited capacity to accept protons

A

Weak base

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39
Q

A substance that can behave as either a proton acceptor or proton donor

A

Amphiprotic

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40
Q

An analytical method for determining the concentration of a solute in a sample by reacting the solute with a standard solution of known concentration

A

Titration

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41
Q

The standard solution added to the sample in a titration

A

Titrant

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42
Q

Solution of known concentration used in titrations

A

Standard solution

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43
Q

A solid product formed from a reaction in a solution

A

Precipitate

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44
Q

A reaction that produces an insoluble product upon mixing two solutions

A

Precipitation reaction

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45
Q

(Blank) can be used to synthesize water-insoluble salts

A

Precipitation reactions

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46
Q

Common minerals that are often formed with anions that lead to insolubility

A

Sulfides, carbonates, oxides, hydroxides

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47
Q

A substance that produces hydrogen ions in solution

A

Acid

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48
Q

A substance that produces hydroxide ions in solution

A

Base

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49
Q

An acid ——- (blank) in water

A

H+

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50
Q

(Blank) are strong electrolytes and are completely ionized

A

Strong acids

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51
Q

(Blank) are weak electrolytes and only partially ionize

A

Weak acids

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52
Q

What is he chemical produced in the largest quantity in the US

A

Sulfuric acid

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53
Q

Acid that can furnish more than one proton

A

Polyprotic acid

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54
Q

Base —–(blank) in water

A

OH

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55
Q

(Blank) are strong electrolytes and are completely ionized

A

Strong bases

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56
Q

An important weak base

A

Ammonia (NH3)

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57
Q

Four steps to writing net ionic equation

A

1) write a balanced chemical equation
2) write a complete ionic equation
3) identify spectator ions
4) write the net ionic equation

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58
Q

The amount of solute in a particular amount of solvent or solution

A

Concentration

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59
Q

The concentration of a solution expressed in moles of solute per liter of solution

A

Molarity

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60
Q

A concentrated solution of a substance used to prepare solutions of lower concentration

A

Stock solution

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61
Q

The process of lowering the concentration of a solution by adding more solvent

A

Dilution

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62
Q

Driving force of a net ionic equation

A

Formation of an insoluble compound, a precipitate gas forming reaction

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63
Q

In acid base reaction the driving force is

A

The formation of water

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64
Q

A way to express acidity- the concentration of H+ in a solution

A

pH

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65
Q

Acidic solution pH

A

<7

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66
Q

Neutral solution pH

A

7

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67
Q

Basic solution pH

A

> 7

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68
Q

The medium in which a solute is dissolved to form a solution

A

Solvent

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69
Q

The substance dissolved in a solvent to form a solution

A

Solute

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70
Q

Amount of solute in a solution is given by its concentration

A

Solution concentration

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71
Q

Molarity (M)

A

Moles of solute / liter of solution

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72
Q

Concentration M =

A

moles/ volume

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73
Q

Important point in dilution problems

A

Moles in initial solution = moles in final solution

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74
Q

Dilution equation

A

M(initial) x V (initial) = M (final) x V (final)

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75
Q

Millimolarity

A

Millimoles of solute / L of solution

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76
Q

Parts per million (ppm)

A

(Mass of substance / mass of sample)x 10^6

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77
Q

Parts per billion

A

(Mass of substance / mass of sample)x 10^9

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78
Q

A solution that contains the maximum concentration of a solute possible at a given temperature

A

Saturated solution

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79
Q

The maximum amount of a substance that dissolves in a given quantity of solvent at a given temperature

A

Solubility

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80
Q

Increase in temp = blank solubility of solids in water

A

Greater

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81
Q

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

A

Supersaturated solution

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82
Q

Process by which one ion is displaced by another

A

Ion exchange

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83
Q

What is ion exchange important in?

A

Water purification

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84
Q

Neutral crystalline minerals or synthetic materials consisting of 3D networks of channels that contain sodium for other 1+ cations

A

Zeolite

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85
Q

All zeolites have a rigid (blank) structure

A

3D

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86
Q

Combination reactions of oxygen with Nonmetals such as carbon, sulfur, and nitrogen produce

A

Volatile oxides

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87
Q

Oxidation

A

Increase in oxygen

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88
Q

Reduction

A

Decrease in oxygen

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89
Q

A chemical changes in which a species loses electrons

A

Oxidation

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90
Q

The ON increases

A

Oxidation

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91
Q

The ON decreases

A

Reduction

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92
Q

A chemical change in which a species gains electrons

A

Reduction

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93
Q

Change in ON reflects the change in (blank) associated with an atom or ion

A

of electrons

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94
Q

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

A

Oxidation number or state

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95
Q

ON of atoms in neutral molecule sum

A

Zero

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96
Q

ON of atoms in ion sum to

A

Charge on ion

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97
Q

Each atom in pure element has an ON # of

A

0

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98
Q

In monatomic ions, the ON is the charge (blank)

A

ON the ion

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99
Q

In compounds containing fluorine and 1+ elements, ON is

A

-1

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100
Q

In most compounds the ON of hydrogen is (blank) and oxygen is (blank)

A

1+

2-

101
Q

ON of metal hydrides

A

-1

102
Q

ON of O in peroxide ion (O2_^2)

A

-1

103
Q

A substance in a redox reaction that contains the element being reduced

A

Oxidizing agent

104
Q

Electron acceptor

A

Oxidizing agent

105
Q

A substance in a redox reaction that contains the element being oxidized

A

Reducing agent

106
Q

Electron donor

A

Reducing agent

107
Q

One of the two halves of an oxidation- reduction reaction

A

Half reaction

108
Q

Step 1 to balance redox reaction

A

1) write one equation for the oxidation half reaction and a separate equation for the reduction half reaction

109
Q

Step 2 to balance redox reaction

A

Balance the # of particles in each half reaction

110
Q

Step 3 to balance redox reaction

A

Balance the charge in each half reaction (always ADD electrons)

111
Q

Step 4 to balance redox reaction

A

Multiply each half-reaction by the appropriate whole #

112
Q

Step 5 to balance redox reaction

A

Add the the two half reactions to generate the equation representing the redox reaction

113
Q

A qualitative ordering of the oxidizing ability of metals and their cations

A

Activity series

114
Q

A chemical equation describing the redox reaction in nature will be balanced when

A

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
Q

General approach to solution stoichiometry problem

A

Mass zinc- moles zinc- stoichiometric factor - moles HCl- volume or mass HCl

116
Q

Steps to solve a solution stoichiometry problem

A

1) write the balanced equation
2) calculate the moles of Zn
3) use the stoichiometric factor
4) calculate the volume of HCl required

117
Q

Acronym for oxidation reduction reactions

A

OIL-RIG

118
Q

Oxidation involves (blank) of electrons

A

Loss

119
Q

Reduction involves (blank) of electrons

A

Gains

120
Q

6 rules for assigning oxidation states

A

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
Q

Redox reactions are characterized by (blank) between an electron donor and electron acceptor

A

Electron transfer

122
Q

Increase in ON of some element

A

Oxidation

123
Q

Decrease in ON of some element

A

Reduction

124
Q

The point in a titration at which the # of moles of titrant added is stoichiometrically = to the # of moles of the substance being analyzed

A

Equivalence point

125
Q

The point in a titration that is reached when just enough standard solution has been added to cause the indicator to change color

A

End point

126
Q

Law of thermodynamics

A

Energy is neither created nor destroyed during chemical reactions

127
Q

The chemical equation of a reaction that includes energy as a reactant or product

A

Thermochemical equation

128
Q

Describes whether energy is absorbed or released when reaction occurs

A

Thermochemical equation

129
Q

A form of energy required to move an object through a given distance

A

Work

130
Q

The study of energy and its transformations

A

Thermodynamics

131
Q

The study of the relation between chemical reactions and changes in energy

A

Thermochemistry

132
Q

Process by which energy moves from a warmer object to a cooler object

A

Heat transfer

133
Q

Energy transferred between objects because different temps

A

Heat

134
Q

A condition in which temperature is uniform throughout a material and no energy flows from one point to another

A

Thermal equilibrium

135
Q

Work =

A

Force x distance

136
Q

Energy stored in an object because of its position

A

Potential energy

137
Q

Potential energy equation

A

PE = mass x g (acceleration due to gravity) x h (vertical distance)

138
Q

A property of an entity based solely on its chemical or physical state or both, but not how it achieved that state

A

State function

139
Q

State function does not depend on

A

How object gets to a particular point

140
Q

The energy of an object in motion due to its mass (m) and its speed (u)

A

Kinetic energy

141
Q

Energy cannot be created nor destroyed but can be converted from one form into another

A

Law of conservation of energy

142
Q

The kinetic energy of atoms, ions, and molecules

A

Thermal energy

143
Q

Increase in particles = increase in

A

Thermal energy

144
Q

Energy a particle has because of its electrostatic charge and its position relative to another particle

A

Electrostatic potential energy (Eel)

145
Q

Electrostatic energy is directly proportional to the product of the charged of the particles and inversely proportional to the distance between them

A

Coulombic interaction

146
Q

A lower electrostatic potential energy corresponds to

A

Greater stability

147
Q

The part of the universe that is the focus of a thermochemical study

A

System

148
Q

Everything that is not part of the system

A

Surroundings

149
Q

A system that exchanges neither energy nor matter with the surroundings

A

Isolated system

150
Q

A thermos bottle containing hot soup with the lid screwed on tightly

A

Isolated system

151
Q

A system that exchanges energy but not matter with the surroundings

A

Closed system

152
Q

A cup of hot soup with a lid

A

Closed system

153
Q

A system that exchanges both energy and matter with the surroundings

A

Open system

154
Q

An open cup of hot soup

A

Open system

155
Q

Energy flows from a system into its surroundings

A

Exothermic

156
Q

(Blank) process is a combustion reaction

A

Exothermic

157
Q

Energy flows from the surroundings into the system

A

Endothermic process

158
Q

Ice cubes in warm water = (blank) process

A

Endothermic process

159
Q

Releases energy = (blank) process

A

Exothermic

160
Q

Absorbs energy = (blank) process

A

Endothermic

161
Q

System loses energy to its surroundings

A

Exothermic

162
Q

System gained energy from surroundings

A

Endothermic

163
Q

Q

A

Exothermic

164
Q

Q>O

A

Endothermic

165
Q

The sum of all the kinetic and potential energies of all the components of a system

A

Internal energy (E)

166
Q

Delta E =

A

E final - E initial

167
Q

Reducing agents are electron

A

Donors

168
Q

Reducing agents get

A

Oxidized

169
Q

Oxidizing agents are electron

A

Acceptors

170
Q

Oxidizing agents get

A

Reduced

171
Q

Represent two parts of a redox reaction

A

Half reactions

172
Q

A technique in which one solution is used to analyze another

A

Titration

173
Q

Procedure to determine the concentration of a solution in a titration

A

Standardization

174
Q

Occurs when exact stoichiometric amounts of both reagents have been added in a titration

A

Equivalence point

175
Q

Steps to find concentration

A

1) balance the equation
2) calculate amount of (blank)
3) calculate amount of (blank) required
4) calculate concentration

176
Q

The study of energy and its inter conversions

A

Thermodynamics

177
Q

Capacity to do work or transfer heat

A

Energy

178
Q

Energy transferred between two objects due to a temperature difference between them

A

Heat

179
Q

The energy required at a constant pressure to raise the temperature of 1 mole of a substance by 1 degree C

A

Molar heat capacity

180
Q

Q =

A

M C dT

181
Q

The energy required to raise the temperature of 1g of a substance 1 degree C at constant pressure

A

Specific heat

182
Q

The quantity of energy needed to raise the temperature of a particular object 1 degree C at constant pressure

A

Heat capacity

183
Q

The energy required to convert 1 mole of a solid substance at its melting point into the liquid state

A

Molar heat of fusion (delta Hfus)

184
Q

Enthalpy change

A

Q = ndeltaHfus

185
Q

The energy required to convert 1 mole of a liquid substance at its boiling point to the vapor state

A

Molar heat of vaporization (deltaHvap)

186
Q

System takes in energy = blank value

A

+

187
Q

Ability of water to absorb large quantities of energy

A

Heat sink

188
Q

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

A

Divide the absolute value of change in reaction for each reaction by the mm of hydrocarbon

189
Q

The energy released during the complete combustion of 1 g of a substance

A

Fuel value

190
Q

As the # of carbon atoms/ molecules increases, the hydrogen to carbon ratio

A

Decreases

191
Q

The amount of energy released during the complete combustion of 1 liter of a liquid fuel

A

Fuel density

192
Q

The quantity of energy produced when a material consumed by an organism for sustenance is burned completely

A

Food value

193
Q

A condition in which the system and its surroundings are at the same Temp and heat transfer stops

A

Thermal equilibrium

194
Q

The collection of molecules we are studying

A

System

195
Q

Results in the evolution of heat

Heat flows from system to surroundings

A

Exothermic reactions

196
Q

Absorbs energy

Energy flows into system from surroundings

A

Endothermic reactions

197
Q

Heat required to raise temp of 1 g of H2O by 1 degree C

A

1 calorie

198
Q

1000 calorie

A

1 kc

199
Q

1 kc

A

1 kcal

200
Q

Amount of energy required to raise an objects temperature by 1 degree C

A

Heat capacity

201
Q

The heat capacity per gram of substance

A

Specific heat capacity

202
Q

Problems involving heat transfer can be approached by assuming the sum of the heat changes within a given substance is zero

A

Complex heat transfer

203
Q

The amount of energy necessary to raise the temperature of 1 g of water by 1 degree C

A

Calorie

204
Q

The total increase in the internal energy of a closed system is the

A

Sum of the work done on it (w) and any other energy (q) gained
Q + w

205
Q

The energy gained or lost by a system must equal the energy lost or gained by the surroundings

A

First law of thermodynamics

206
Q

Work done by a system on its surroundings internal energy (blank)

A

Decreases

207
Q

The work associated with the expansion or compression of a gas

A

Pressure-volume (PV work)

208
Q

System heated by surroundings (q blank)

A

> O

209
Q

Work done by system (w blank)

A
210
Q

Energy transferred from system to surroundings (q blank)

A
211
Q

Heat absorbed by an endothermic process or given off by an exothermic process occurring at constant pressure

A

Enthalpy change (delta H)

212
Q

Sum of the internal energy and the pressure to volume product of a system

A

Enthalpy (H)

213
Q

All the energy (heat and work) exchanged by the system with surroundings

A

Delta E

214
Q

Only q, heat exchanged at constant pressure

A

Delta H

215
Q

Energy flows out of system

A

Endothermic

216
Q

Endothermic, q and H

A

Q -

Delta H

217
Q

Heat flows into system

A

Exothermic

218
Q

Exothermic, q and H

A

Q+

h>O

219
Q

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

A

Hess’s law

220
Q

The capacity to do work or transfer heat

A

Energy

221
Q

Thermal energy transferred from a warmer to a cooler object

A

Heat

222
Q

Mechanical energy that moves an object from one place to another

A

Work

223
Q

Heat into system = blank q

A

+

224
Q

Heat out of system equals blank q

A

-

225
Q

Work done on system

A

+

226
Q

Work done by system

A

-

227
Q

Heat transfer in

A

Endothermic

228
Q

Heat transfer out

A

Exothermic

229
Q

Work done on system

A

+w

230
Q

Work done by system

A

-w

231
Q

Heat content of a substance at constant pressure

A

Enthalpy

232
Q

If Hfinal > H initial

A

Change in H- endothermic +

233
Q

If H final < H initial then

A

Change in H - exothermic

234
Q

Formation of water endothermic or exothermic

A

Exothermic

235
Q

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

A

Hess’s law

236
Q

Property that is independent of pathway

A

State function

237
Q

The measurement of the quantity of heat transferred during a physical change or chemical process

A

Calorimetry

238
Q

A device used to measure the absorption or release of energy by a physical change or chemical process

A

Calorimeter

239
Q

The energy absorbed or given off by a chemical reaction = heat of reaction

A

Enthalpy of reaction

240
Q

A constant volume device used to measure the energy released during a combustion reaction

A

Bomb calorimeter

241
Q

Heat capacity of a calorimeter

A

Calorimeter constant

242
Q

The enthalpy change of a formation reaction- also called standard heat of formation

A

Standard enthalpy of formation

243
Q

A reaction in which 1 mole of substance is formed from its component elements in their standard states

A

Formation reaction

244
Q

The most stable form of a substance under 1 bar pressure and some specified temperature

A

Standard state

245
Q

The energy associated with a reaction that takes place under standard conditions

A

Standard enthalpy of reaction

246
Q

More negative the heat of formation of a subsgance, the (blank)

A

More stable

247
Q

Change in Hrxn

A

Sum of nproducts -sum of nreactants

248
Q

Science of measuring heat

A

Calorimetry

249
Q

Device used to experimentally determine the heat associated with a chemical reaction

A

Calorimeter

Chemisty (10 decks)

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