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AP Chemistry > Chapter 10 > Flashcards

Chapter 10 Flashcards

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1
Q

Dipole-Dipole Forces

A

Attraction between molecules with dipole moments

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2
Q

The larger the difference in electromagnetic, what happens to dipole moment?

A

increases in size

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3
Q

Inter-molecular Forces

A

Forces that exist between the molecules/atoms that a substance is composed of

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4
Q

What bonds are INTRAMOLECULAR?

A

ionic and covalent bonding

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5
Q

Dipole-Dipole forces are considered?

A

uneven, polar, and weak

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6
Q

Dipole Dipole force interactions maximize what between the atoms?

A

attractive forces

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7
Q

Dipole Dipole force interactions minimize what between the atoms?

A

repulsive forces

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8
Q

Dipole dipole forces compared to ionic solids?

A

1% as strong

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9
Q

Dipole Dipole forces only exist in what phases?

A

solid and liquid

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10
Q

Hydrogen bonding is what strength?

A

strong

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11
Q

Hydrogen bonding is a specific example of?

A

Dipole-Dipole attraction

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12
Q

Hydrogen bonding is only between?

A

hydrogen and oxygen, fluorine, nitrogen

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13
Q

What gives water its unique properties?

A

hydrogen bonding

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14
Q

London dispersion forces are considered?

A

non-polar and most weak

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15
Q

In London dispersion forces what are formed?

A

instantaneous dipoles

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16
Q

Molecules without dipole moments still need to have?

A

ability to exert force on one another

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17
Q

instantaneous dipoles exist in?

A

non-polar molecules and diatomic gases

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18
Q

The random movement of electrons can create?

A

non-symmetrical electron distribution

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19
Q

Instantaneous dipoles can induce?

A

short lived dipole in neighboring molecules

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20
Q

London dispersion forces exist between all molecules but are?

A

the weakest forces of attraction

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21
Q

Polarizability

A

how easy the electron cloud of an atom can be distorted to give a dipole charge

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22
Q

Polarizability increases with?

A

the number of electrons in a molecule

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23
Q

the more electrons a molecule has the more chances for?

A

a momentary dipole interaction to occur

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24
Q

CCl₄ experiences greater London dispersion forces than?

A

CH₄

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25
Q

Surface tension

A

the resistance of a liquid to an increase in its surface area

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26
Q

Which shape has the smallest surface area?

A

sphere

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27
Q

the higher the intermolcular forces, the greater?

A

the surface tension can be

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28
Q

Have higher surface tensions in liquid state?

A

polar substances

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29
Q

Capillary action

A

based upon cohesive forces between liquid molecules

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30
Q

Adhesive forces are between?

A

polar liquid molecules and polar bonds in the material and the container

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31
Q

glass has partial negative charges and attracted to?

A

positive end of polar molecules

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32
Q

Waters adhesive forces are greater than

A

cohesive forces

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33
Q

cohesive forces

A

the force of attraction between the same molecules

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34
Q

adhesive forces

A

forces between the liquid molecules and their container

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35
Q

what in glass is attracted to hydrogen in water?

A

oxygen

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36
Q

Viscosity

A

resistance to flow

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37
Q

structural models for a liquid are dependent on? (3)

A

-Intermolecular forces
-polar or nonpolar
-what adding to liquid

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38
Q

Is there a definite model for liquids?

A

no

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39
Q

Crystalline solids have a highly ______ arrangement of components?

A

regular

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40
Q

The components of a crystalline solid arrange themselves how?

A

3D lattice network that is repeated throughout the structure

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41
Q

Unit Cell

A

smallest repeating 3D lattice

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42
Q

a solid can be composed of?

A

atoms, ions, or molecules

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43
Q

The type of component found at the lattice point determines?

A

what type of solid that you are

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44
Q

Types of solids

A

molecular, ionic, atomic

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45
Q

What type of solid has the lowest melting point?

A

molecular

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46
Q

What type of solid has lowest enthalpy of fusion?

A

molecular

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47
Q

Order of weakest to strongest attractive forces?

A

molecular, ionic, metallic, network covalent

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48
Q

Amorphous solid

A

Components are “frozen in place” before they can achieve an ordered arrangement

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49
Q

What do amorphous solids lack?

A

ordered arrangement

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50
Q

examples of amorphous solids?

A

glass and plastic

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51
Q

Ionic solids are composed of?

A

hard, high melting point, conduct when dissolved in water

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52
Q

In ionic solids ions occupy?

A

lattice points

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53
Q

Molecular solids

A

discrete covalent bonded molecules at each lattice points

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54
Q

lattice point

A

a point at the intersection of grid lines in a regularly spaced array of points

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55
Q

examples of molecular solids

A

ice and sucrose

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56
Q

3 subgroups of atomic solids?

A

metallic, network, group 8A

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57
Q

network solids

A

atomic solids with strong directional covalent bonds

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58
Q

closet packing

A

arrangement of packing uniform hard spheres into the most efficient use of available space

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59
Q

spheres are arranged in?

A

layers

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60
Q

each sphere is surrounded by?

A

6 others

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61
Q

In the second layer, how are the spheres arranged?

A

to fill in the dimples formed by three spheres in the first layer

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62
Q

In the 3rd layer what are the two ways the particles can arrange themselves?

A

aba, abc

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63
Q

hexagonal closest packing

A

has hexagonal unit cell structure

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64
Q

In hexagonal closest packing each layer is?

A

identical

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65
Q

In hexagonal closest packing the spheres in _____ occupy the same ________?

A

every other level, vertical positional

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66
Q

Aba is also known as?

A

hexagonal closest packing

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67
Q

Hexagonal closest packing abbreviated is?

A

hcp packing

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68
Q

Cubic Closest Packing

A

has a face centered cubic unit cell

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69
Q

Cubic Closest Packing is also referred to as?

A

ccp

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70
Q

In Cubic Closest Packing the spheres in every _____ layer occupy the same ________.

A

4th, vertical position

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71
Q

What is common in both ccp and hcp?

A

-12 equivalent nearest neighbors
-6 in the same layer
-3 in layer above
-3 in layer below

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72
Q

Where does an intermolecular force occur?

A

between molecules

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73
Q

changes in state of matter are due to ___________ among the molecules rather than those ________ the molecules.

A

changes in force, within

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74
Q

how much energy is needed to vaporize 1 mole of water?

A

40.7 kJ

75
Q

how much energy is needed to break the O-H bond in 1 mole of water molecules?

A

934 kJ

76
Q

dipole moment

A

molecules with polar bonds behaving as if they had a center of positive and negative charge.

77
Q

as the distance between the dipoles increases, the force of attraction?

A

weakens

78
Q

the formation of a temporary dipole can affect?

A

electron distribution of a neighboring atom

79
Q

Instantaneous dipole

A

The separation of charges in a non-polar molecule at an instant due to sudden disturbance in the electron cloud around the molecule

80
Q

The formation of a temporary dipole is also called?

A

instantaneous dipole

81
Q

the instantaneous dipole that occurs accidentally can induce?

A

a similar dipole in a neighboring atom

82
Q

Why does the freezing point rise as you go down group 18?

A

increased polarizability

83
Q

To increase a liquid’s surface area, molecules must?

A

move from the interior to the surface

84
Q

Which liquids have relatively large intermolecular forces?

A

polar molecules

85
Q

Liquids with large intermolecular forces tend to have high?

A

surface tensions

86
Q

When do adhesive forces occur?

A

When a container is made of a substance with polar bonds

87
Q

The concave shape of a meniscus shows water’s ___________ are greater than _______.

A

adhesive forces, cohesive forces

88
Q

liquids with large intermolcular forces tend to be?

A

highly viscous

89
Q

When does a convex meniscus occur?

A

when a liquid has stronger cohesive forces than adhesive forces.

90
Q

Crystalline Solids

A

highly regular arrangement of components

91
Q

lattice

A

3D system of points designating the position of substances that make up a substance

92
Q

The structure of crystalline solids are most commonly determined by?

A

x-ray diffraction

93
Q

atomic solids include?

A

carbon, boron, silicon and all metals

94
Q

Two types of alloys

A

substitutional and interstitial

95
Q

electron sea model

A

explains how metals can conduct electricity and are malleable and ductile

96
Q

In electron sea model where are metal cations found?

A

in a “sea” of valence electrons

97
Q

The valance electrons found in the electron sea model are?

A

mobile

98
Q

The mobile electrons in the electron sea model can?

A

conduct heat and electricity

99
Q

The metal ions in the electron sea model can be easily moved around as?

A

metal is hammered into a sheet or pulled into a wire

100
Q

Alloy

A

substance that contains a mixture of elements and has metallic properties

101
Q

What happens in a substitutional alloy?

A

some of the host metals are replaced by other metal atoms of similar size

102
Q

What happens in a interstitial alloy?

A

holes in closest packed metal structure are occupied by small atoms

103
Q

Network solids are composed of?

A

brittle, do not efficiently conduct heat or electricity.

104
Q

Two most common forms of carbon?

A

diamond and graphite

105
Q

diamond and graphite are?

A

network solids

106
Q

The differences in diamond and graphite arise from?

A

differences in bonding

107
Q

silica is composed of?

A

oxygen, quartz, and some types of sand

108
Q

silicates are found in most?

A

rocks, soils, and clays

109
Q

O/Si ratio

A

2:1

110
Q

Silicates O/Si ratio is?

A

greater than 2:1

111
Q

Silicates contain?

A

silicon-oxygen anions

112
Q

When silica is heated above its melting point and cooled rapidly what happens?

A

an amorphous solid called glass results

113
Q

Silicon is a ___________ element

A

semiconducting

114
Q

how can the conductivity of silicon be enhanced at normal temperature?

A

doping the silicon crystal with certain other elements

115
Q

When molecules have dipole moments, their intermolecular forces are?

A

significantly greater, especially when hydrogen bonding is possible

116
Q

Ionic solids are ________, ____________ substances

A

stable, high melting

117
Q

how are ionic solids held together?

A

by strong electrostatic forces that exist between oppositely charged ions

118
Q

Three types of holes in closet packing structures?

A

Trigonal, tetrahedral, octahedral

119
Q

Trigonal holes

A

formed by 3 spheres in same layer

120
Q

Tetrahedral holes

A

formed when a sphere sits in the dimple of 3 spheres in an adjacent layer

121
Q

octahedral holes

A

formed between two sets of three spheres in adjoining layers

122
Q

example of substitutional alloy

A

brass

123
Q

example of interstitial alloy

A

steel

124
Q

by adding smaller atoms to a interstitial alloy, you alter?

A

the properties of the host metal

125
Q

diamonds are composed entirely of?

A

carbon-60

126
Q

each carbon in a diamond is?

A

surrounded by a tetrahedral arrangement of other carbon atoms

127
Q

network solids can be viewed as?

A

giant molecules

128
Q

the structure of diamond is held together and stabilized with?

A

covalent bonds that are formed by the overlap of sp3 hybrid orbitals

129
Q

Why is diamond a poor conductor of heat but a good insulator?

A

Because of large gap between the occupied and unoccupied orbitals

130
Q

graphite is made of?

A

carbon-10

131
Q

Graphite is a great conductor of?

A

electricity

132
Q

The structure of graphite is based on?

A

layers of carbon atoms in 6 member rings

133
Q

Each carbon in one layer is surrounded by?

A

3 other carbons in a trigonal planar arrangement with sp2 hybridization

134
Q

There are what kind of bonds in graphite’s layers?

A

pie bonds

135
Q

Pie bonds in graphite contribute to?

A

stablization and conductivity because of delocalized electrons associated with them.

136
Q

In graphite there are ______ bonds within the layers and ____ between the layers.

A

strong, weak

137
Q

The more London dispersion forces the _________ the boiling point?

A

higher

138
Q

In non-metals, metallic bonds are present in?

A

aluminum foil and copper wire

139
Q

What solid has valance electrons delocalized over huge array of atoms?

A

network solids

140
Q

Vaporization or evaporation is clear evidence that?

A

the molecules of a liquid can escape the liquid’s surface and form a gas

141
Q

What type of process is vaporization?

A

endothermic

142
Q

Why is vaporization endothermic?

A

energy is required to overcome the strong intermolecular forces in the liquid

143
Q

heat of vaporization

A

the energy required to vaporize 1 mole of a liquid at a pressure of 1 atm.

144
Q

Heat of vaporization is also called?

A

enthalpy of vaporization

145
Q

Condensation

A

the process by which vapor molecules reform into a liquid

146
Q

A system is a equilibrium when no further net charges occur in?

A

the amount of liquid or vapor

147
Q

In any closed container at equilibrium, the rate of condensation and vaporization

A

exactly balance each other out

148
Q

Equilibrium Vapor Pressure

A

the pressure of the vapor present at equilibrium

149
Q

Equilibrium Vapor Pressure is also called?

A

vapor pressure

150
Q

Silicon is different from carbon because?

A

it cannot use 3p orbitals to form pie bonds with oxygen due to its large size

151
Q

The silica structure has all ___ bonds?

A

single

152
Q

Why does silica have only single bonds?

A

silica cannot form a double bond with oxygen

153
Q

quartz is based on a?

A

SiO4 tetrahedron

154
Q

Silica is the main component of _____ which is an amorphous solid.

A

glass

155
Q

Molecular solids can be though of as?

A

one giant molecule

156
Q

In molecular solids what takes place within the molecules?

A

strong covalent bonding

157
Q

In molecular solids what takes place between the molecules?

A

weak attractive forces

158
Q

Examples of molecular solids

A

Ice, Dry Ice, S8

159
Q

Generally the attractive forces between the molecules in molecular solids are?

A

London Dispersion

160
Q

What happens to the London dispersion forces in a molecular solid as the size of the molecules increase?

A

increase in strength

161
Q

Vapor Pressure is very dynamic on the molecular level because?

A

molecules are constantly escaping and entering the liquid phase

162
Q

Why is equilibrium established in a closed container?

A

because molecules are constantly escaping and entering the liquid phase

163
Q

Once vapor pressure is ______kPa or ________atm or _____mmHg that is boiling point.

A

101.3, 1, 760

164
Q

Lower vapor pressure means ____ ______ _______ in liquids.

A

greater intermolecular forces

165
Q

High vapor pressure means ____ _______ _______ in liquids.

A

lower intermolecular forces

166
Q

Why do liquids with greater intermolecular forces have low vapor pressures?

A

the significant attractions between the molecules need to be overcome before the liquid particles can move into the gas phase

167
Q

Sublimation

A

substance goes from solid to gas phase.

168
Q

Reasons for sublimation

A

-solids have low vapor pressures
-solids with little intermolecular attraction are able to sublime at room temperatures

169
Q

heat of fusion

A

energy required to co convert 1 mole of solid substance into a mole of liquid substance

170
Q

Normal melting point

A

temperature at which the solid and liquid states have same vapor pressure under 1 atm

171
Q

Normal boiling point

A

temperature at which the vapor pressure of a liquid is exactly 1 atm

172
Q

Super cooling

A

liquid is cooled below 0 degrees Celsius and remains in a liquid state

173
Q

In super cooling the quick temperature change does not allow time for?

A

the organization of the molecules into an orderly solid structure

174
Q

Super heating

A

when a liquid is heated above its boiling point

175
Q

How is super heating avoided in lab?

A

boiling chips

175
Q

In super heating, there is not enough _____ _____ _______ accumulated in one place to form bubbles and escape.

A

high energy molecules

176
Q

Most slopes in a closed diagram have?

A

positive slope between liquid and solid

177
Q

The water in a closed diagram has a _______ slope between the _____ & _______ phase.

A

negative, solid, liquid

178
Q

What occurs at triple point?

A

-solids and liquids have identical vapor pressure
-all three phases exist together in equilibrium

179
Q

Critical Temperature

A

temperature where substances can not exist as a liquid no matter the pressure.

180
Q

Critical Pressure

A

the pressure needed to produce a liquid at critical temperature

181
Q

Critical point

A

point where critical temp and critical pressure meet

182
Q

Melting Point ____ as pressure increases for water.

A

decreases

183
Q

Why does Melting point decreases as pressure increases for water?

A

the density of ice is less than that of water thus the volume increases.

AP Chemistry (16 decks)

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