Chapter 11 Concepts

Question 1

Kinetic Molecular Theory

The kinetic molecular theory states that gases..

Answer 1

are compressible fluids because they are composed of molecules or single atoms that are in constant random motion throughout mostly empty space (unless the gas is highly compressed.) Because the molecules of a gas can be pushed into a smaller space, it means that gases are compressible. They are also considered fluids because individual molecules can move easily relative to one another.

Question 2

Kinetic Molecular Theory

The kinetic molecular theory states that liquids..

Answer 2

are relatively incompressible fluids because although the molecules of a liquid are in constant random motion (similar to a gas), they are tightly packed and have less free space. Molecules of a liquid can move relative to each other, making it a fluid like gas. But it is important to remember that the lack of empty space is what differentiates a liquid and a gas because it makes liquid a nearly imcompressible fluid.

Question 3

Kinetic Molecular Theory

The kinetic molecular theory states that solids..

Answer 3

are nearly incompressible and are rigid, not fluid like gas and liquid. This is because the particles making up the solid exist in close contact and do not move like gases and liquid. The particles vibrate in fixed sites instead. Furthermore, having a compact structure explains its incompressibility.

Question 4

Ideal Gas Law

The ideal gas law is..

Answer 4

PV=nRT

Question 5

van der Waals

The van der Waals equation is

Answer 5

Question 6

Phase Change

Solid to Liquid

Answer 6

Fusion

Question 7

Phase Change

Solid to Gas

Answer 7

Sublimination

Question 8

Phase Change

Gas to Solid

Answer 8

Deposition

Question 9

Phase Change

Gas to Liquid

Answer 9

Condensation

Question 10

Phase Change

Liquid to Solid

Answer 10

Freezing

Question 11

Phase Change

Liquid to Gas

Answer 11

Vaporization

Question 12

Vapor Pressure

Vapor Pressure of a liquid is..

Answer 12

the partial pressure of the vapor over the liquid, measured at equilibrum at a given temperature.

Question 13

Relationship between Temperature and Vapor Pressure

The relationship between temperature and vapor pressure is..

Answer 13

As temperature increases, vapor pressure also increases

Question 14

Dynamic Equilibrium

Dynamic Equilibrium is when..

Answer 14

a molecular process is continously occuring.

In order to represent the dynamic equilibrium for the vaporization and condensation of water by the equation with a double arrow. H2O (l) –> H2O (g) (–> is double arrow)

Question 15

Equilibrium

Equilibrium is when..

Answer 15

a molecular process peaks and then remains unchanged.

Question 16

Boiling Point

Boiling point is..

Answer 16

the temperature at which the vapor pressure is equal to the pressure of the liquid, usually atmoshperic pressure. Furthermore, when vapor pressure equals atmospheric pressure, bubbles of gas form within the liquid.

Question 17

Relationship between Pressure of a liquid and Boiling Point

The relationship between pressure of a liquid and boiling point is..

Answer 17

When the pressure of a liquid increases so does boiling point. When the pressure of a liquid decreases so does boiling point.

Question 18

Phase Diagram

A phase diagram is..

Answer 18

a graphical way to summarize the conditions under which the different states of a substance are stable.

Question 19

Melting Point Curve

The melting point curve is..

Answer 19

a phase diagram for water. It consists of three curves that divide the diagram into regions labeled “solid,” “liquid,” and “gas.”

Every point on each of the curves indicates experimentally determined temperatures and pressures at which two states are in equilibrium.

Question 20

Vapor Pressure Curves for the Liquid and the Solid

The curve AC that divides the liquid region from the gaseous region gives the vapor pressures of the liquid at various temperatures. It also gives the boiling points of the liquid at various temperatures. Meanwhile, the curve AD divides the solid region from the gaseous region gives the vapor pressures of the solid at various temperatures.

Triple Point is the point on a phase representing the temperature and pressure at which three phases of a substance coexist in equilibrium.

Answer 20

Question 21

Criticial Temperature and Pressure

The critical temperature is..

Answer 21

the temperature above which the liquid state of a substance no longer exists regardless of the pressure.

Question 22

Critical Pressure

The critical pressure is..

Answer 22

the vapor pressure at the critical temperature. It is also known as the minimum pressure that must be applied to a gas at the critical temperature to liquefy it. Most gases cannot be liquefied at room temperature, this is because it is must be below their critical temperature and be applied sufficent pressure.

Question 23

Surface Tension

Surface tension is..

Answer 23

the energy required to increase the surface area of a liquid by a unit amount.

Question 24

Capillary Rise

Capillary Rise is..

Answer 24

a phenomenon related to surface tension. When a capillary is placed upright in water, a column of the liquid rises in the tube.

Question 25

# Viscosity Viscosity is..

Answer 25

the resistance to flow that is exhibited by all liquids and gases.

Question 26

# Intermolecular Forces Dipole-Dipole is..

Answer 26

an attractive intermolecular force resulting from the tendency of polar molecules to align themselves such that the positive end of one molecule is near the negative end of another. | In simpler words, dipole dipole deals with electronegativity. ## Footnote Also known as the second strongest IMF.

Question 27

# Intermolecular Forces London Diespersion is..

Answer 27

the weak attractive forces between molecules resulting from the small, instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei. | London forces tend to increase with molecular weight.

Question 28

# Intemolecular Forces Hydrogen Bonding is..

Answer 28

the strongest intermolecular force and can only be present in molecules that have a hydrogen connecting to at least one or more of F.O.N | Flourine, Oxygen, and Nitrogen

Question 29

# Relationship between Boiling Point and Intermolecular Forces The relationship between Boiling Point and IMF is..

Answer 29

Stronger IMF = Higher Boiling Point

Question 30

# Relationship between Surface Tension and Intermolecular Forces The relationship between Surface Tension and IMF is..

Answer 30

Stronger IMF = Higher Surface Tension

Question 31

# Relationship between Viscosity and Intermolecular Forces The relationship between Viscosity and IMF is..

Answer 31

Stronger IMF = Higher Viscosity

Question 32

# Relationship between Vapor Pressure and Intermolecular Forces The relationship between Vapor Pressure and IMF is..

Answer 32

Stronger IMF = Lower Vapor Pressure

Question 33

# Types of Solids A Molecular Solid is..

Answer 33

A solid that consists of atoms or molecules held together by intermolecular forces. ## Footnote Examples include solid neon, solid water (ice), and solid carbon dioxide (dry ice).

Question 34

# Types of Solids A Metallic Solid is..

Answer 34

a solid that consists of positive cores of atoms held together by a surrounding "sea" of electrons (metallic bonding). ## Footnote Examples include iron, copper, and silver.

Question 35

# Types of Solids A Ionic Solid is..

Answer 35

a solid that consists of cations and anions held together by the electrical attraction of opposite charges (ionic bonds). ## Footnote Examples include cesium chloride, sodium chloride, and zinc sulfide.

Question 36

# Types of Solids A Covalent Network Solid is..

Answer 36

a solid that consists of atoms held together in large networks or chains by covalent bonds. ## Footnote Examples include diamond, graphite, graphene.

Question 37

# Identifying Types of Solids The best way to identify the type of solid is..

Answer 37

The metallic elements, of course, have metallic bonding. The nonmetallic elements in Groups 5A to 7A, which are rather reactive, are usually molecu-lar, whereas those in Group 8A (the noble gases) are atomic. The nonmetals in Groups 3A (B) and 4A (C and Si) often occur with network bonding. A compound of two non-metals is likely to be molecular, although in some cases network bonding occurs (involv-ing Groups 3A and 4A elements especially, such as BN, SiO2, and SiC, with strong single bonds). A compound of a metal and a nonmetal is likely to have ionic bonds.

Question 38

# Melting Point and Structure The relationship between the Melting Point and Molecular Solid is..

Answer 38

For a solid to melt, the forces holding the structural units in their sites must be overcome, at least partially. In a molecular solid, these forces are weak intermolecular attractions. ## Footnote Both molecular and covalent network solids have covalent bonds, but none of the covalent bonds are broken dur-ing the melting of a molecular solid.

Question 39

# Melting Point and Structure The relationship between the Melting Point and Ionic Solid and Covalent Solid is..

Answer 39

For ionic solids and covalent network solids to melt, chemical bonds must be broken. For that reason, the melting points of these types of solids are rela-tively high.

Question 40

# Properties of the Different Types of Solid Molecular Solid's melting point is..

Answer 40

Low

Question 41

# Properties of the Different Types of Solid Molecular Solid's Hardness and Brittleness is..

Answer 41

Soft and Brittle

Question 42

# Properties of the Different Types of Solid Molecular Solid's Electrical Conductivity is..

Answer 42

Nonconducting

Question 43

# Properties of the Different Types of Solid Metallic Solid's Melting Point is..

Answer 43

variable

Question 44

# Properties of the Different Types of Solid Metallic Solid's Hardness and Brittleness is..

Answer 44

variable hardness, malleable

Question 45

# Properties of the Different Types of Solid Metallic Solid's Electrical Conductivity is..

Answer 45

conducting

Question 46

# Properties of the Different Types of Solid Ionic Solid's Melting Point is..

Answer 46

high to very high

Question 47

# Properties of the Different Types of Solid Ionic Solid's Electrical Conductivity is..

Answer 47

nonconducting solid (conducting liquid)

Question 48

# Properties of the Different Types of Solid Ionic Solid's Hardness and Brittleness is..

Answer 48

hard and brittle

Question 49

# Properties of the Different Types of Solid Covalent network solid's melting point

Answer 49

very high

Question 50

# Properties of the Different Types of Solid Covalent network solid's hardness and brittleness

Answer 50

very hard

Question 51

# Properties of the Different Types of Solid Covalent network solid's electrical conductivity

Answer 51

Usually nonconducting

Question 52

# Crystalline Solids Crystalline solid is..

Answer 52

composed of one or more crystals. each crystal has a well-defined, ordered structure in three dimensions.

Question 53

# Amorphous Solid Amorphous solid is..

Answer 53

has a disordered structure; it lacks the well-defined arrangement of basic units (atoms, molecules, or ions) found in a crystal.

Question 54

# Crystal Lattice Crystal Lattice is..

Answer 54

the geometric arrangement of lattice points of a crystal, in which we choose one lattice point at the same location within each of the basic units of the crystal.

Question 55

# Cubic Unit Cells A simple cubic unit cell is..

Answer 55

a cubic unit cell in which lattice points are stiuated only at the corners. | 1

Question 56

# Cubic Unit Cells A body centered cubic unit cell is..

Answer 56

a cubic unit cell in which there is a lattice point at the center of the cubic cell in addition to those at the corners. | 2

Question 57

# Cubic Unit Cells A face centered cubic unit cell is..

Answer 57

a cubic unit cell which there are lattice points at the centers of each face of the unit cell in addition to those at the corners. | 4