Chapter 10 Liquids & Solids Flashcards
(198 cards)
1
Q
What are the three physical states of matter?
A
Solid, Liquid, and Gas
These are the basic phases in which matter can exist.
2
Q
What is a characteristic of solids?
A
Particles are tightly packed, fixed in place, and incompressible
Solids have a definite shape and volume due to strong intermolecular forces.
3
Q
What is a characteristic of liquids?
A
Particles are still attracted to each other but can move past one another
Liquids have a definite volume but take the shape of their container.
4
Q
What is a characteristic of gases?
A
Particles are far apart, move freely, and are compressible
Gases fill the entire volume of their container and have no definite shape or volume.
5
Q
What type of energy is associated with the motion of particles?
A
Kinetic Energy (KE)
Kinetic energy increases with temperature, affecting the state of matter.
6
Q
What determines the phase of a substance?
A
Intermolecular forces (IMF) and kinetic energy
The balance between these factors dictates whether a substance is solid, liquid, or gas.
7
Q
How do intermolecular forces affect the melting point of a solid?
A
Stronger intermolecular forces result in a higher melting point
This is because more energy is required to overcome these forces.
8
Q
What is the relationship between temperature and intermolecular forces?
A
Higher temperatures can weaken intermolecular forces
This can lead to a phase change, such as melting or boiling.
9
Q
Fill in the blank: Solids have ______ intermolecular forces than liquids.
A
stronger
This strength keeps the particles in a fixed position.
10
Q
True or False: Gases have definite shape and volume.
A
False
Gases do not have a definite shape or volume; they expand to fill their container.
11
Q
What happens to particles in a liquid when heat is added?
A
They gain kinetic energy and may overcome intermolecular forces
This can cause the liquid to transition into a gas.
12
Q
What are dispersion forces?
A
Dispersion forces are a type of intermolecular force (IMF) present in all atoms and molecules. They are the weakest of all intermolecular forces.
13
Q
What is the nature of London dispersion forces?
A
London dispersion forces are present in all atoms and molecules and are the weakest intermolecular forces.
14
Q
What type of molecules exhibit dispersion forces?
A
Dispersion forces are found in nonpolar molecules.
15
Q
What causes the temporary dipoles in molecules?
A
Temporary dipoles are caused by the constant shifting of electrons in nonpolar molecules, leading to slight negative and positive charges.
16
Q
How do dispersion forces affect molecular interactions?
A
Dispersion forces result in weak electrostatic forces due to the temporary dipoles formed in molecules.
17
Q
What is polarizability?
A
Polarizability is a measure of how easy or difficult it is for an electron to be displaced by an electric field.
18
Q
What happens to polarizability as size increases?
A
As size increases, polarizability increases.
19
Q
What are stronger intermolecular forces associated with?
A
Stronger intermolecular forces are associated with higher boiling points.
20
Q
What is the molar mass of C6H12?
A
The molar mass of C6H12 is 84 g/mol.
21
Q
What is the relationship between intermolecular forces and boiling point?
A
Stronger intermolecular forces lead to higher boiling points.
22
Q
What is the characteristic of the most compact compound regarding boiling point?
A
The most compact compound has the weakest intermolecular forces and the lowest boiling point.
23
Q
What is the significance of the heat of vaporization?
A
The heat of vaporization is significant as it indicates the strength of intermolecular forces.
24
Q
What are the forces that attract molecules?
A
Attractive forces include dipole-dipole interactions and dispersion forces.
25
What is the effect of strong intermolecular forces?
Strong intermolecular forces result in higher boiling points.
26
What is the significance of charge in molecules?
Electrostatic charge can influence molecular interactions continuously.
27
What is a dipole moment?
A dipole moment occurs in polar molecules, leading to dipole-dipole attractions.
28
What factors affect the strength of intermolecular attractions?
The strength of intermolecular attractions is affected by the size of the contact area.
29
What happens with less surface area in molecular interactions?
Less surface area results in weaker attractions.
30
What are dispersion forces?
Dispersion forces are weak attractions that occur due to temporary dipoles.
31
What is hydrogen bonding?
Hydrogen bonding occurs in molecules with H-F, H-O, and H-N bonds.
32
What type of bond is a hydrogen bond?
A hydrogen bond is a strong dipole-dipole interaction due to highly polar bonds.
33
What are the strongest hydrogen bonds responsible for?
They are responsible for the high boiling points of molecules like H2O and NH3.
34
How does hydrogen bonding explain the density of water?
Hydrogen bonding explains why the density of water is higher than that of ice.
35
What happens to water molecules in H2O?
In H2O, hydrogen bonds attract to lone pairs, creating clusters of water molecules.
36
What is the effect of hydrogen bonding on water's boiling point?
Hydrogen bonding results in strong forces of attraction, affecting the boiling point.
37
What are the types of molecules based on polarity?
Polar and nonpolar.
38
What type of intermolecular forces are present in polar molecules?
Dipole-dipole interactions.
39
What is required to overcome attractions between molecules in liquids and solids?
The stronger the intermolecular forces, the more energy is required.
40
What is surface tension?
Resistance to flow exhibited by all liquids and gases, resulting from attraction between molecules.
41
What does surface tension explain about water?
It explains why water beads.
42
What affects surface tension?
Surface tension is affected by dissolved substances (e.g., soap).
43
What happens to insects on water?
Insects float on water but sink if soap is added.
44
What is a water droplet?
A water droplet is a small, spherical mass of liquid water.
## Footnote
It is formed due to the surface tension of the liquid.
45
What happens to the surface area of a liquid when it is reduced?
The surface area of the liquid is reduced when the liquid is attracted to gas.
46
What is the curvature of a water droplet when liquid is attracted to gas?
The curvature is concave.
47
What is the curvature of a droplet of mercury when liquid is not attracted to gas?
The curvature is convex.
48
What is capillary rise?
Capillary rise occurs when a very small diameter glass tube is placed in a liquid, causing the liquid to rise in the tube.
49
What happens to the liquid when it is attracted to the glass in capillary rise?
The liquid climbs up the glass tube.
50
What is the effect of surface tension in capillary rise?
Surface tension causes the liquid to expand and create a meniscus in the tube.
51
What is a phase transition in chemistry?
A phase transition is a change from one state of matter to another, such as from solid to liquid.
52
What is melting?
Melting is the phase transition from solid to liquid.
53
What is freezing?
Freezing is the phase transition from liquid to solid.
54
What is boiling?
Boiling is the phase transition from liquid to gas.
55
What is condensation?
Condensation is the phase transition from gas to liquid.
56
What is sublimation?
Sublimation is the phase transition from solid to gas without passing through the liquid phase.
57
What is deposition?
Deposition is the phase transition from gas to solid without passing through the liquid phase.
58
True or False: Evaporation is the same as boiling.
False
59
What is the process of a solid turning directly into a gas called?
Sublimation
60
What happens to molecular motion during melting?
Molecular motion increases as the solid absorbs heat and transitions to a liquid.
61
Fill in the blank: The temperature at which a liquid becomes a solid is called the ________ point.
freezing
62
What is the reverse process of sublimation?
Deposition
63
What is the critical point in phase transitions?
The critical point is the temperature and pressure at which the distinction between liquid and gas phases disappears.
64
True or False: All substances can undergo all types of phase transitions.
False
65
What phase transition occurs when a gas becomes a liquid?
Condensation
66
What is the term for the phase transition from liquid to gas at temperatures below boiling point?
Evaporation
67
What is the latent heat of fusion?
The latent heat of fusion is the amount of energy required to change a substance from solid to liquid at its melting point.
68
What is the latent heat of vaporization?
The latent heat of vaporization is the amount of energy required to change a substance from liquid to gas at its boiling point.
69
Fill in the blank: The process of turning liquid water into ice is called ________.
freezing
70
What phase transition occurs at the boiling point of a liquid?
Boiling
71
What is the relationship between temperature and phase transitions?
Temperature changes can cause phase transitions by providing or removing energy from a substance.
72
What is the significance of phase diagrams?
Phase diagrams illustrate the conditions of temperature and pressure under which distinct phases occur and coexist.
73
True or False: Phase transitions are always reversible.
False
74
What is a common example of sublimation?
Dry ice turning into carbon dioxide gas.
75
What happens to the kinetic energy of molecules during condensation?
The kinetic energy decreases as molecules lose energy and transition from gas to liquid.
76
Fill in the blank: The transition from solid to liquid involves an increase in ________ energy.
thermal
77
What is the process of fusion?
Fusion is the process of melting, where a solid turns into a liquid.
78
True or False: Sublimation is the transition from a solid directly to a gas.
True
79
Fill in the blank: The process of turning from a gas to a liquid is called __________.
condensation
80
What is vaporization?
Vaporization is the process where a liquid turns into a gas.
81
Which of the following is an example of deposition? A) Ice melting B) Water boiling C) Frost forming on a window
C) Frost forming on a window
82
What occurs during the freezing process?
Freezing is the transition from a liquid to a solid.
83
True or False: In sublimation, heat is released.
False
84
What happens to molecules during vaporization?
Molecules gain enough energy to break free from the liquid state and enter the gas state.
85
Define condensation.
Condensation is the process where gas molecules lose energy and transition into a liquid state.
86
What is the reverse process of vaporization?
The reverse process of vaporization is condensation.
87
Fill in the blank: During __________, a gas changes directly into a solid without becoming a liquid first.
deposition
88
What type of energy change occurs during freezing?
During freezing, heat energy is released.
89
True or False: Fusion requires heat energy to occur.
True
90
What is the term for the phase change from solid to gas?
Sublimation
91
What is required for vaporization to occur?
Vaporization requires the addition of heat energy.
92
Multiple Choice: Which phase change involves cooling? A) Freezing B) Vaporization C) Fusion
A) Freezing
93
What happens to the temperature of a substance during fusion?
The temperature remains constant while the substance is melting.
94
Fill in the blank: The process of __________ involves a solid gaining energy and becoming a liquid.
fusion
95
True or False: Deposition is the process of a solid turning into a gas.
False
96
What is a common example of condensation?
Water droplets forming on a cold glass.
97
What phase change occurs when ice melts?
Fusion
98
Fill in the blank: The opposite of freezing is __________.
melting
99
What is the significance of temperature during sublimation?
Sublimation occurs at temperatures below the melting point of the solid.
100
Multiple Choice: Which process involves a liquid becoming a gas? A) Freezing B) Vaporization C) Deposition
B) Vaporization
101
What is the main difference between evaporation and boiling?
Evaporation occurs at any temperature, while boiling occurs at a specific temperature.
102
True or False: Energy is absorbed during the process of freezing.
False
103
What is required for a substance to vaporize?
A substance must overcome the intermolecular forces to escape.
## Footnote
Example: Molecules must be attracted to the body of liquid.
104
What happens to molecules in vapor?
Some molecules in vapor collide with liquid and stick.
105
What affects the rate of condensation?
The rate of condensation is affected by the number of molecules in the vapor phase.
106
What continues to happen during the transfer of molecules?
There is a continuous transfer of molecules between liquid and vapor.
107
What occurs eventually with molecules in vapor?
Eventually, the rate of molecules condensing equals the rate of molecules vaporizing.
108
What is vapor pressure?
Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid at a given temperature.
109
How does vapor pressure vary with temperature?
Vapor pressure depends on temperature. For example, water has a vapor pressure of 0.03 atm at 25°C.
110
What is the vapor pressure of chloroform (CHCl3) at 25°C?
The vapor pressure of chloroform (CHCl3) is 0.7 atm at 25°C.
111
What is the boiling point?
The boiling point is the temperature where the vapor pressure of a liquid equals the external atmospheric pressure.
112
What is normal boiling point?
Normal boiling point is the boiling point of a liquid at 1 atm of atmospheric pressure.
113
How does boiling point vary with pressure?
The boiling point varies with pressure; for example, water boils at 100°C at 1 atm but at lower temperatures at lower pressures.
114
What is the term for the temperature at which a pure liquid changes to a crystalline solid?
The temperature at which a pure liquid changes to a crystalline solid is called the freezing point.
115
What is the term for the temperature at which a crystalline solid changes?
The temperature at which a crystalline solid changes is referred to as the melting point.
116
What is the energy required to melt 1 mole of solid?
The energy required to melt 1 mole of solid is known as the molar enthalpy of fusion (ΔH_fus).
## Footnote
Example: For H2O, ΔH_fus = 0 kJ/mol.
117
What is the energy required to vaporize 1 mole of liquid?
The energy required to vaporize 1 mole of liquid is known as the molar enthalpy of vaporization (ΔH_vap).
## Footnote
Example: For H2O, ΔH_vap = 40.7 kJ/mol.
118
What are phase diagrams?
Phase diagrams are graphical representations that show the conditions under which a substance exists as a solid, liquid, or gas.
119
What do phase diagrams help determine?
They help determine melting points and the effect of external pressures on phases.
120
What do lines in a phase diagram indicate?
Lines in a phase diagram indicate the boundaries separating different regions.
121
What are the conditions when both phases exist?
Conditions when both phases exist are represented by points where curves meet.
122
What is a point where three curves meet called?
A point where three curves meet is known as a triple point.
123
124
What is the core of atoms held together by?
The positive core of atoms is held together by a strong force.
125
What is an example of a solid?
Ice is an example of solid water.
## Footnote
Example sentence: 'Solid ice is formed from water.'
126
What do solids not do?
Solids do not mix by diffusion.
127
What are the two types of solids?
Crystalline and non-crystalline.
128
What factors affect the properties of solids?
Temperature, pressure, and composition.
129
What is the state of matter that is not solid?
Liquid.
130
What type of solid is characterized by molecules held together by intermolecular forces?
Molecular solids
131
True or False: Metallic solids have a fixed structure and do not conduct electricity.
False
132
Fill in the blank: Ionic solids are formed by the electrostatic attraction between ______ and ______.
cations, anions
133
Which type of solid is known for having a high melting point and being hard due to a network of covalent bonds?
Covalent network solids
134
What is the primary force that holds metallic solids together?
Metallic bonding
135
Multiple choice: Which of the following is NOT a characteristic of ionic solids? A) High melting points B) Conduct electricity in solid state C) Brittle D) Formed from metal and non-metal
B) Conduct electricity in solid state
136
What type of bonding is primarily responsible for the properties of molecular solids?
Intermolecular forces
137
True or False: Covalent network solids can conduct electricity.
False
138
Name one example of a metallic solid.
Copper
139
What is the typical physical state of molecular solids at room temperature?
Solid or liquid
140
What is the chemical composition of diamond?
Diamond is composed of carbon atoms arranged in a crystal structure.
141
What is silicon dioxide commonly known as?
Silicon dioxide is commonly known as silica.
142
What is the primary element in graphite?
The primary element in graphite is carbon.
143
What type of bond does carbon form in diamond?
Carbon exists as a covalent network in diamond.
144
What is the appearance of diamond?
Diamond is a solid with a crystalline structure.
145
What are the physical properties of solids?
Melting point, hardness, electrical conductivity.
146
What is the melting point of molecular solids?
Molecular solids have a low melting point.
147
How does the melting point of covalent network solids compare?
Covalent network solids have a high melting point due to strong bonding.
148
What affects the melting point of metallic solids?
The melting point varies widely depending on the metallic bonding.
149
What is an example of the order of melting points in metals?
The order of melting points: Na, NaCl, Si, NH3, Ne, Li, Na, Li, SiO2.
## Footnote
Example melting points of various substances.
150
What does hardness depend on in solids?
Hardness depends on how easily the structural units can be moved relative to one another.
151
How do molecular solids behave in terms of hardness?
Molecular solids tend to be soft.
152
What is an example of a covalent network solid?
Diamond is an example of a covalent network solid.
## Footnote
Example of a covalent network solid.
153
What is a characteristic of ionic solids?
Ionic solids are brittle and tend to fracture easily along crystal planes.
154
What is a property of metals regarding shape?
Metals are malleable and can be easily shaped by hammering.
155
What is a property of metals in terms of electrical conductivity?
Metals are good electrical conductors due to delocalized valence electrons.
156
What is a crystalline solid?
A crystalline solid is a material whose atoms are arranged in a highly ordered, repeating pattern.
157
True or False: Amorphous solids have a long-range order in their atomic structure.
False
158
Fill in the blank: The basic repeating unit in a crystalline solid is called a _________.
unit cell
159
What defines the lattice structure of a crystalline solid?
The lattice structure is defined by the arrangement of lattice points and the geometric arrangement of the unit cells.
160
Which of the following is NOT a characteristic of crystalline solids? (a) Definite melting point (b) Anisotropy (c) Random arrangement of atoms (d) Long-range order
c) Random arrangement of atoms
161
What are lattice points?
Lattice points represent the positions of atoms, ions, or molecules in a crystal lattice.
162
True or False: Amorphous solids exhibit isotropy in their physical properties.
True
163
What is the primary difference between crystalline and amorphous solids?
The primary difference is the order in their atomic arrangement; crystalline solids have a defined order, while amorphous solids do not.
164
Which type of solid typically has a sharp melting point?
Crystalline solids
165
Fill in the blank: The three-dimensional arrangement of unit cells in a crystalline solid is known as a _________.
lattice structure
166
How many types of unit cells are there based on their geometry?
There are seven types of unit cells based on their geometry.
167
True or False: The properties of amorphous solids can change with temperature and pressure.
True
168
What is a simple cubic unit cell?
A simple cubic unit cell is a cube where each corner is occupied by an atom.
169
What type of solid is glass considered to be?
Glass is considered an amorphous solid.
170
Which unit cell type has atoms at each corner and the center of each face?
Face-centered cubic unit cell
171
Fill in the blank: The arrangement of particles in a crystalline solid can be described as _________.
periodic
172
What is the significance of unit cells in understanding crystalline solids?
Unit cells help to describe the structure and properties of the entire crystal.
173
Which of the following is a property of crystalline solids? (a) Isotropic (b) Anisotropic (c) Amorphous (d) None of the above
b) Anisotropic
174
What is the term for the energy required to break the bonds in a crystalline solid?
Bond energy
175
True or False: Lattice points can only be occupied by atoms.
False
176
What type of arrangement do ionic solids exhibit in their lattice structure?
Ionic solids exhibit a regular arrangement of alternating positive and negative ions.
177
Fill in the blank: The distance between lattice points in a crystal is known as the _________.
lattice parameter
178
What does the term 'coordination number' refer to in a crystal lattice?
The coordination number refers to the number of nearest neighbors surrounding a lattice point.
179
Which type of unit cell is characterized by a body-centered arrangement?
Body-centered cubic unit cell
180
True or False: Crystalline solids can be formed from both organic and inorganic materials.
True
181
What is the role of symmetry in crystalline solids?
Symmetry helps to determine the properties and classification of the crystal structure.
182
Do ionic solids conduct electricity?
They do NOT conduct electricity.
When melted they DO conduct electricity and when dissolved in H2O.
183
What are the three types of cubic unit cells?
Simple cubic, body-centered cubic, and face-centered cubic.
184
True or False: In a simple cubic unit cell, atoms are located only at the corners.
True.
185
Fill in the blank: The body-centered cubic unit cell has atoms at the _____ and one atom in the center.
corners
186
Which cubic unit cell has the highest packing efficiency?
Face-centered cubic.
187
What is the coordination number of atoms in a face-centered cubic unit cell?
12.
188
Multiple choice: Which unit cell has a total of 2 atoms per unit cell? A) Simple cubic B) Body-centered cubic C) Face-centered cubic
B) Body-centered cubic.
189
What is the packing efficiency of a simple cubic unit cell?
Approximately 52.4%.
190
True or False: The face-centered cubic unit cell has atoms located at the corners and the centers of each face.
True.
191
Short answer: How many total atoms are effectively present in a face-centered cubic unit cell?
4 atoms.
192
What distinguishes a body-centered cubic cell from a simple cubic cell?
A body-centered cubic cell has an additional atom in the center of the cube.
193
What does 'n' represent in X-ray diffraction?
n = order of selection
194
What is 'E' in the context of X-ray diffraction?
E = wavelength of incident X-rays
195
What does 'd' represent in X-ray diffraction?
d = interplanar spacing
196
What does the Bragg equation compute?
The Bragg equation may be used to compute measurements from such measurements.
197
What is analyzed to determine the crystal structure?
The angles at which X-rays are diffracted are analyzed to determine the crystal material.
198
What is produced from the diffraction pattern?
A diffraction pattern can be produced, resulting in a crystal structure analysis.
