Chapter 11 Concepts Flashcards
Kinetic Molecular Theory
The kinetic molecular theory states that gases..
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.
Kinetic Molecular Theory
The kinetic molecular theory states that liquids..
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.
Kinetic Molecular Theory
The kinetic molecular theory states that solids..
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.
Ideal Gas Law
The ideal gas law is..
PV=nRT
van der Waals
The van der Waals equation is
Phase Change
Solid to Liquid
Fusion
Phase Change
Solid to Gas
Sublimination
Phase Change
Gas to Solid
Deposition
Phase Change
Gas to Liquid
Condensation
Phase Change
Liquid to Solid
Freezing
Phase Change
Liquid to Gas
Vaporization
Vapor Pressure
Vapor Pressure of a liquid is..
the partial pressure of the vapor over the liquid, measured at equilibrum at a given temperature.
Relationship between Temperature and Vapor Pressure
The relationship between temperature and vapor pressure is..
As temperature increases, vapor pressure also increases
Dynamic Equilibrium
Dynamic Equilibrium is when..
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)
Equilibrium
Equilibrium is when..
a molecular process peaks and then remains unchanged.
Boiling Point
Boiling point is..
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.
Relationship between Pressure of a liquid and Boiling Point
The relationship between pressure of a liquid and boiling point is..
When the pressure of a liquid increases so does boiling point. When the pressure of a liquid decreases so does boiling point.
Phase Diagram
A phase diagram is..
a graphical way to summarize the conditions under which the different states of a substance are stable.
Melting Point Curve
The melting point curve is..
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.
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.
Criticial Temperature and Pressure
The critical temperature is..
the temperature above which the liquid state of a substance no longer exists regardless of the pressure.
Critical Pressure
The critical pressure is..
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.
Surface Tension
Surface tension is..
the energy required to increase the surface area of a liquid by a unit amount.
Capillary Rise
Capillary Rise is..
a phenomenon related to surface tension. When a capillary is placed upright in water, a column of the liquid rises in the tube.
Viscosity
Viscosity is..
the resistance to flow that is exhibited by all liquids and gases.
Intermolecular Forces
Dipole-Dipole is..
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.
Also known as the second strongest IMF.
Intermolecular Forces
London Diespersion is..
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.
Intemolecular Forces
Hydrogen Bonding is..
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
Relationship between Boiling Point and Intermolecular Forces
The relationship between Boiling Point and IMF is..
Stronger IMF = Higher Boiling Point
Relationship between Surface Tension and Intermolecular Forces
The relationship between Surface Tension and IMF is..
Stronger IMF = Higher Surface Tension
Relationship between Viscosity and Intermolecular Forces
The relationship between Viscosity and IMF is..
Stronger IMF = Higher Viscosity
Relationship between Vapor Pressure and Intermolecular Forces
The relationship between Vapor Pressure and IMF is..
Stronger IMF = Lower Vapor Pressure
Types of Solids
A Molecular Solid is..
A solid that consists of atoms or molecules held together by intermolecular forces.
Examples include solid neon, solid water (ice), and solid carbon dioxide
(dry ice).
Types of Solids
A Metallic Solid is..
a solid that consists of positive cores of atoms held together by a surrounding “sea” of electrons (metallic bonding).
Examples include iron, copper, and silver.
Types of Solids
A Ionic Solid is..
a solid that consists of cations and anions held together by the electrical attraction of opposite charges (ionic bonds).
Examples include cesium chloride, sodium chloride, and zinc sulfide.
Types of Solids
A Covalent Network Solid is..
a solid that consists of atoms held together in large networks or chains by covalent bonds.
Examples include diamond, graphite, graphene.
Identifying Types of Solids
The best way to identify the type of solid is..
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.
Melting Point and Structure
The relationship between the Melting Point and Molecular Solid is..
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.
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.
Melting Point and Structure
The relationship between the Melting Point and Ionic Solid and Covalent Solid is..
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.
Properties of the Different Types of Solid
Molecular Solid’s melting point is..
Low
Properties of the Different Types of Solid
Molecular Solid’s Hardness and Brittleness is..
Soft and Brittle
Properties of the Different Types of Solid
Molecular Solid’s Electrical Conductivity is..
Nonconducting
Properties of the Different Types of Solid
Metallic Solid’s Melting Point is..
variable
Properties of the Different Types of Solid
Metallic Solid’s Hardness and Brittleness is..
variable hardness, malleable
Properties of the Different Types of Solid
Metallic Solid’s Electrical Conductivity is..
conducting
Properties of the Different Types of Solid
Ionic Solid’s Melting Point is..
high to very high
Properties of the Different Types of Solid
Ionic Solid’s Electrical Conductivity is..
nonconducting solid (conducting liquid)
Properties of the Different Types of Solid
Ionic Solid’s Hardness and Brittleness is..
hard and brittle
Properties of the Different Types of Solid
Covalent network solid’s melting point
very high
Properties of the Different Types of Solid
Covalent network solid’s hardness and brittleness
very hard
Properties of the Different Types of Solid
Covalent network solid’s electrical conductivity
Usually nonconducting
Crystalline Solids
Crystalline solid is..
composed of one or more crystals. each crystal has a well-defined, ordered structure in three dimensions.
Amorphous Solid
Amorphous solid is..
has a disordered structure; it lacks the well-defined arrangement of basic units (atoms, molecules, or ions) found in a crystal.
Crystal Lattice
Crystal Lattice is..
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.
Cubic Unit Cells
A simple cubic unit cell is..
a cubic unit cell in which lattice points are stiuated only at the corners.
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Cubic Unit Cells
A body centered cubic unit cell is..
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.
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Cubic Unit Cells
A face centered cubic unit cell is..
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.
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