Download Chapter 12 - Humble ISD

CHAPTER
CHEMISTRY
Matter and Change
Chapter 12: States of Matter
SECTION
12.1
Gases
States of Matter
12
Section 12.1
Gases
Section 12.2
Forces of Attraction
Section 12.3
Liquids and Solids
Section 12.4
Phase Changes
SECTION
Gases
12.1
• Use the kinetic-molecular theory to explain the
behavior of gases.
kinetic-molecular theory
pressure
elastic collision
barometer
• Describe how mass affects the rates of diffusion and
effusion.
temperature
pascal
diffusion
atmosphere
Graham’s law of
effusion
Dalton’s law of partial
pressures
• Explain how gas pressure is measured and calculate
the partial pressure of a gas.
kinetic energy: energy due to motion
Gases expand, diffuse, exert pressure,
and can be compressed because they
are in a low density state consisting of
tiny, constantly-moving particles.
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SECTION
SECTION
12.1
12.1
Gases
The Kinetic-Molecular Theory
• Kinetic-molecular theory explains the
different properties of solids, liquids, and
gases.
• Atomic composition affects chemical
properties.
Gases
The Kinetic-Molecular Theory (cont.)
• Gases consist of small particles separated
by empty space.
• Gas particles are too far apart to experience
significant attractive or repulsive forces.
• Atomic composition also affects physical
properties.
• The kinetic-molecular theory describes the
behavior of matter in terms of particles in
motion.
SECTION
SECTION
12.1
12.1
Gases
The Kinetic-Molecular Theory (cont.)
• Gas particles are in constant random
motion.
Gases
The Kinetic-Molecular Theory (cont.)
• Kinetic energy of a particle depends on
mass and velocity.
• An elastic collision is one in which no kinetic
energy is lost.
• Temperature is a measure of the average
kinetic energy of the particles in a sample of
matter.
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SECTION
SECTION
12.1
12.1
Gases
Explaining the Behavior of Gases
• Great amounts of space exist between gas
particles.
• Compression reduces the empty spaces
between particles.
Gases
Explaining the Behavior of Gases (cont.)
• Gases easily flow past each other because
there are no significant forces of attraction.
• Diffusion is the movement of one material
through another.
• Effusion is a gas escaping through a tiny
opening.
SECTION
SECTION
12.1
12.1
Gases
Explaining the Behavior of Gases (cont.)
• Graham’s law of effusion states that the
rate of effusion for a gas is inversely
proportional to the square root of its molar
mass.
Gases
Gas Pressure
• Pressure is defined as force per unit area.
• Gas particles exert pressure when they
collide with the walls of their container.
• Graham’s law also applies to diffusion.
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SECTION
12.1
Gases
SECTION
12.1
Gases
Gas Pressure (Cont.)
Gas Pressure (Cont.)
• The particles in the earth’s atmosphere
exert pressure in all directions called air
pressure.
• Torricelli invented the barometer.
• There is less air pressure at high altitudes
because there are fewer particles present,
since the force of gravity is less.
SECTION
12.1
Gases
• Barometers are
instruments used to
measure atmospheric
air pressure.
SECTION
12.1
Gases
Gas Pressure (Cont.)
Gas Pressure (Cont.)
• Manometers measure gas pressure in a
closed container.
• The SI unit of force is the newton (N).
• One pascal(Pa) is equal to a force of one
Newton per square meter or N/m2.
• One atmosphere is equal to 760 mm Hg or
101.3 kilopascals.
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SECTION
Gases
12.1
SECTION
Gases
12.1
Gas Pressure (Cont.)
• Dalton’s law of partial pressures states that
the total pressure of a mixture of gases is equal
to the sum of the pressures of all the gases of
the mixture.
• The partial pressure of a gas depends on the
number of moles, size of the container, and
temperature and is independent of the type of
gas.
• At a given temperature and pressure, the partial
pressure of 1mol of any gas is the same.
SECTION
Gases
12.1
Gas Pressure (Cont.)
Ptotal = P1 + P2 + P3 +...Pn
SECTION
12.1
Section Check
The average of kinetic energy of
particles in a substance is measured
by its ____.
A. mass
B. density
C. temperature
• Partial pressure can be used to calculate the
amount of gas produced in a chemical reaction.
D. pressure
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SECTION
12.1
Section Check
One mole of oxygen in a 5.0 liter container
has the same partial pressure as one mol
of hydrogen in the same container. This is
a demonstration of what law?
SECTION
12.2
• Describe intramolecular
forces.
• Compare and contrast
intermolecular forces.
A. law of conservation of mass
D. Dalton’s law of partial pressures
dipole-dipole force
hydrogen bond
Intermolecular forces—including dispersion
forces, dipole-dipole forces, and hydrogen
bonds—determine a substance’s state at a given
temperature.
SECTION
SECTION
12.2
12.2
Forces of Attraction
Intermolecular Forces
• Attractive forces between molecules cause
some materials to be solids, some to be
liquids, and some to be gases at the same
temperature.
polar covalent: a type
of bond that forms when
electrons are not shared
equally
dispersion force
B. law of definite proportions
C. law of conservation of energy
Forces of Attraction
Forces of Attraction
Intermolecular Forces (cont.)
• Dispersion forces are weak forces that
result from temporary shifts in density of
electrons in electron clouds.
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SECTION
SECTION
12.2
12.2
Forces of Attraction
Intermolecular Forces (cont.)
• Dipole-dipole forces are attractions between
oppositely charged regions of polar molecules.
Forces of Attraction
Intermolecular Forces (cont.)
• Hydrogen bonds are special dipole-dipole
attractions that occur between molecules that
contain a hydrogen atom bonded to a small,
highly electronegative atom with at least one
lone pair of electrons, typically fluorine, oxygen,
or nitrogen.
SECTION
SECTION
12.2
12.2
Forces of Attraction
Intermolecular Forces (cont.)
• Hydrogen bonds explain
why water is a liquid at
room temperature while
compounds of comparable
mass are gases.
• Methane is nonpolar, so
relatively weak dispersion
forces holding the molecule
together.
Section Check
A hydrogen bond is a type of ____.
A. dispersion force
B. ionic bond
C. covalent bond
D. dipole-dipole force
• Ammonia and Water both form hydrogen bonds but oxygen
is more electronegative than nitrogen making O-H bonds
more polar and thus stronger.
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SECTION
Section Check
12.2
SECTION
12.3
Liquids and Solids
Which of the following molecules can
form hydrogen bonds?
• Contrast the arrangement of particles in liquids and
solids.
A. CO2
• Describe the factors that affect viscosity.
B. C2H6
• Explain how the unit cell and crystal lattice are
related.
C. NH3
D. H2
meniscus: the curved surface of a column of liquid
SECTION
Liquids and Solids
12.3
SECTION
12.3
Liquids and Solids
Liquids
viscosity
unit cell
surface tension
allotrope
surfactant
amorphous solid
crystalline solid
The particles in solids and liquids have
a limited range of motion and are not
easily compressed.
• Forces of attraction keep molecules closely
packed in a fixed volume, but not in a fixed
position.
• Liquids are much denser than gases because
of the stronger intermolecular forces holding
the particles together.
• Large amounts of pressure must be applied
to compress liquids to very small amounts.
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SECTION
Liquids and Solids
12.3
Liquids (Cont.)
• Viscosity is a measure of the resistance of a
liquid to flow and is determined by the type of
intermolecular forces, size and shape of
particles, and temperature.
SECTION
Liquids and Solids
Liquids (Cont.)
• Fluidity is the ability to flow and diffuse;
liquids and gases are fluids.
Liquids and Solids
12.3
SECTION
12.3
• The stronger the intermolecular attractive forces,
the higher the viscosity.
• In glycerol, it is the
hydrogen bonding that
makes it so viscous.
• The hydrogen atoms
attached to the oxygen
atoms in each molecule are
able to form hydrogen
bonds with other glycerol
molecules.
SECTION
Liquids and Solids
12.3
Liquids (Cont.)
Liquids (Cont.)
• Particle size and shape:
• Surface tension is the energy required to increase
the surface area of a liquid by a given amount.
–Larger molecules create greater viscosity.
–Long chains of molecules result in a higher
viscosity: cooking oils and motor oils.
• Temperature:
–Increasing the temperature decreases viscosity
because the added energy allows the molecules to
overcome intermolecular forces and flow more
freely.
– Surface tension is the a measure of the inwards pull by
particles in the interior.
– The stronger the attraction between particles the stronger
the surface tension. Ex. Water
• Surfactants are compounds that lower the surface
tension of water.
– Surface tension is why water alone will not clean your
clothes, you need soap to break down the hydrogen
bonds so the water will carry the dirt away.
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SECTION
12.3
Liquids and Solids
SECTION
Liquids and Solids
12.3
Liquids (Cont.)
Solids
• Cohesion is the force of attraction between
identical molecules.
• Solids contain particles with strong
attractive intermolecular forces.
• Adhesion is the force of attraction between
molecules that are different.
• Particles in a solid vibrate in a fixed position.
• Most solids are more dense than liquids.
• Capillary action is the upward movement of
liquid into a narrow cylinder, or capillary tube.
SECTION
12.3
Liquids and Solids
– One exception to this is water. Ice is less dense
than liquid water. The hydrogen bonding in ice
results in an open symmetrical structure that
keeps the water molecules in ice farther apart
than in water in a liquid state.
SECTION
12.3
Liquids and Solids
Solids (Cont.)
Solids (Cont.)
• Crystalline solids are solids with atoms,
ions, or molecules arranged in an orderly,
geometric shape.
• A unit cell is the smallest arrangement of
atoms in a crystal lattice that has the same
symmetry as the whole crystal.
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SECTION
12.3
Liquids and Solids
SECTION
12.3
Liquids and Solids
Solids (Cont.)
• Amorphous solids are solids in which the
particles are not arranged in a regular,
repeating pattern.
• Amorphous solids form when molten material
cools quickly.
SECTION
12.3
Section Check
The smallest arrangement of atoms in a
crystal that has the same pattern as the
crystal is called ____.
A. crystal lattice
B. unit cell
C. crystalline
SECTION
12.3
Section Check
The viscosity of a liquid will increase
as:
A. particle size decreases
B. temperature increases
C. intermolecular forces decrease
D. particle size increases
D. geometric cell
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SECTION
12.4
Phase Changes
• Explain how the addition
and removal of energy
can cause a phase
change.
phase change: a
change from one state
of matter to another
• Interpret a phase
diagram.
SECTION
Phase Changes
12.4
melting point
freezing point
vaporization
condensation
evaporation
deposition
vapor pressure
phase diagram
boiling point
triple point
Matter changes phase when energy is
added or removed.
SECTION
SECTION
12.4
12.4
Phase Changes
Phase Changes That Require Energy
• Melting occurs when heat flows into a solid
object.
• Heat is the transfer of energy from an object
at a higher temperature to an object at a
lower temperature.
Phase Changes
Phase Changes That Require Energy (cont.)
• When ice is heated, the ice eventually
absorbs enough energy to break the
hydrogen bonds that hold the water
molecules together.
• When the bonds break, the particles move
apart and ice melts into water.
• The melting point of a crystalline solid is the
temperature at which the forces holding the
crystal lattice together are broken and it
becomes a liquid.
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SECTION
SECTION
12.4
12.4
Phase Changes
Phase Changes That Require Energy (cont.)
• Particles with enough energy escape from
the liquid and enter the gas phase.
Phase Changes
Phase Changes That Require Energy (cont.)
• Vaporization is the process by which a
liquid changes to a gas or vapor.
• Evaporation is vaporization only at the
surface of a liquid.
SECTION
SECTION
12.4
12.4
Phase Changes
Phase Changes That Require Energy (cont.)
• In a closed container, the pressure exerted
by a vapor over a liquid is called vapor
pressure.
Phase Changes
Phase Changes That Require Energy (cont.)
• The boiling point is the temperature at
which the vapor pressure of a liquid equals
the atmospheric pressure.
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SECTION
SECTION
12.4
12.4
Phase Changes
Phase Changes That Require Energy (cont.)
• Sublimation is the process by which a solid
changes into a gas without becoming a
liquid.
Phase Changes
Phase Changes That Require Energy (cont.)
• As heat flows from water to the
surroundings, the particles lose energy.
• The freezing point is the temperature at
which a liquid is converted into a crystalline
solid.
SECTION
SECTION
12.4
12.4
Phase Changes
Phase Changes That Require Energy (cont.)
• As energy flows from water vapor, the
velocity decreases.
• The process by which a gas or vapor
becomes a liquid is called condensation.
Phase Changes
Phase Diagrams
• A phase diagram is a graph of pressure
versus temperature that shows in which
phase a substance will exist under different
conditions of temperature and pressure.
• Deposition is the process by which a gas or
vapor changes directly to a solid, and is the
reverse of sublimation.
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SECTION
SECTION
12.4
12.4
Phase Changes
Phase Diagrams (cont.)
• The triple point is the point on a phase
diagram that represents the temperature
and pressure at which all three phases of a
substance can coexist.
SECTION
12.4
Section Check
Phase Changes
• The phase diagram for different substances are
different from water.
SECTION
12.4
Section Check
The addition of energy to water molecules
will cause them to ____.
The transfer of energy from one object to
another at a lower temperature is ____.
A. freeze
A. heat
B. change to water vapor
B. degrees
C. form a crystal lattice
C. conductivity
D. move closer together
D. electricity
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SECTION
12.1
Study Guide
Gases
SECTION
12.2
Study Guide
Forces of Attraction
Key Concepts
Key Concepts
• The kinetic-molecular theory explains the properties
of gases in terms of the size, motion, and energy of
their particles.
• Intramolecular forces are stronger than intermolecular
forces.
• Dalton’s law of partial pressures is used to determine
the pressures of individual gases in gas mixtures.
• Graham’s law is used to compare the diffusion rates of
two gases.
SECTION
12.3
Study Guide
Liquids and Solids
• Dispersion forces are intermolecular forces between
temporary dipoles.
• Dipole-dipole forces occur between polar molecules.
SECTION
12.4
Study Guide
Phase Changes
Key Concepts
Key Concepts
• The kinetic-molecular theory explains the behavior of
solids and liquids.
• States of a substance are referred to as phases
when they coexist as physically distinct parts of a
mixture.
• Intermolecular forces in liquids affect viscosity, surface
tension, cohesion, and adhesion.
• Crystalline solids can be classified by their shape and
composition.
• Energy changes occur during phase changes.
• Phase diagrams show how different temperatures and
pressures affect the phase of a substance.
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CHAPTER
12
Chapter Assessment
States of Matter
760 mm Hg is equal to ____.
A. 1 Torr
B. crystalline
C. liquids
D. amorphous
A collision in which no kinetic energy is lost is
a(n) ____ collision.
D. conserved
States of Matter
Solids with no repeating pattern are ____.
A. ionic
States of Matter
C. inelastic
D. 1 atmosphere
Chapter Assessment
Chapter Assessment
B. elastic
C. 1 kilopascal
12
12
A. net-zero
B. 1 pascal
CHAPTER
CHAPTER
CHAPTER
12
Chapter Assessment
States of Matter
What is the point at which all six phase
changes can occur?
A. the melting point
B. the boiling point
C. the critical point
D. the triple point
17
CHAPTER
12
Chapter Assessment
States of Matter
What are the forces that determine a
substance’s physical properties?
A. intermolecular forces
B. intramolecular forces
C. internal forces
CHAPTER
12
Chapter Assessment
States of Matter
What do effusion rates depend on?
A. temperature of the gas
B. temperature and pressure of the gas
C. molar mass of the gas
D. molar mass and temperature of the gas
D. dispersal forces
CHAPTER
12
Chapter Assessment
States of Matter
A sealed flask contains helium, argon, and
nitrogen gas. If the total pressure is 7.5 atm,
the partial pressure of helium is 2.4 atm and the
partial pressure of nitrogen is 3.7 atm, what is
the partial pressure of argon?
A. 1.3 atm
B. 6.1 atm
CHAPTER
12
Chapter Assessment
States of Matter
Adding energy to a liquid will:
A. cause it to form crystal lattice
B. increase the viscosity
C. compress the particles closer together
D. increase the velocity of the particles
C. 1.4 atm
D. 7.5 atm
18
CHAPTER
12
Chapter Assessment
States of Matter
Hydrogen bonds are a special type of ____.
A. ionic bond
B. covalent bond
C. dipole-dipole force
D. dispersion force
CHAPTER
12
Chapter Assessment
States of Matter
How many atoms of oxygen are present in 3.5
mol of water?
A. 2.1 x 1024
B. 3.5 x 1023
C. 6.02 x 1023
D. 4.2 x 1024
19