CHAPTER 10: STATES OF MATTER CH 10 Notes.pdf · 2020. 7. 17. · CHAPTER 10.1 KINETIC MOLECULAR...
Transcript of CHAPTER 10: STATES OF MATTER CH 10 Notes.pdf · 2020. 7. 17. · CHAPTER 10.1 KINETIC MOLECULAR...
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CHAPTER 10:
STATES OF MATTER
Honors Chemistry
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CHAPTER 10.1
KINETIC MOLECULAR THEORY
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Kinetic-Molecular Theory of Matter
All particles of matter are in constant
motion – even the solids!
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This is a model for the behavior of
an ideal gas. It is useful for
predicting the behavior of gases.
Kinetic Molecular Theory
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Kinetic Molecular Theory
1. Gases are composed of tiny particles and mainly empty space
2. Collisions are perfectly elastic
3. Gas particles move in constant, rapid,
random motion
4. There are no attractive forces
between gas particles
5. Volume of individual gas particles is zero
6. The temperature of the gas depends on the average kinetic energy. (KE = ½mv2)
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Applies to only ideal gases
Ideal Gas: hypothetical gas that perfectly fits
all the assumptions of the kinetic-molecular
theory
Real Gases
Expand, are fluid, have relatively low
densities, compressible, and diffuse & effuse
Kinetic Molecular Theory
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CHAPTER 10.2
LIQUIDS
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10.2 Liquids
Properties of Liquids:
1. Definite volume
2. Indefinite shape
3. Free flowing particles; fluidity
4. Condensed state of matter with higher density
5. Relatively incompressible
6. Ability to diffuse
7. Surface tension
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Surface Tension
Definition: The force that tends to pull adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size.
Causes bugs and leaves to walk/float on water
Causes droplets to occur
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Capillary Action
Definition: the attraction of the surface of a
liquid to the surface of a solid
Related to surface tension
Responsible for a meniscus, xylem & phloem, &
paper product absorption
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Capillary Action
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Vaporization
Definition: term used for the
conversion of a liquid to a gas or
vapor below its boiling point
General term for the escape of
molecules at the surface
Can be an open or closed container
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Evaporation
Process by which
particles escape
from the surface of
a non-boiling liquid
and enter the gas
state
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Vaporization Pressure
Vapor Pressure: vaporized particles collide
with the walls of a sealed container, and
create a pressure above the surface of the
liquid.
particles enter the vapor
some particles condense back to the liquid
Ex) The “Sssst” in soda!
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CHAPTER 10.3
SOLIDS
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Types of Solids
Crystalline Solids: highly regular
arrangement of their components
[table salt (NaCl), pyrite (FeS2)].
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Lattice: A 3-
dimensional system
of points
designating the
centers of
components (atoms,
ions, or molecules)
that make up the
substance.
Crystalline Solids
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7 Basic Crystal Units
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Amorphous
solids:
considerable
disorder in their
structures (glass
and plastic).
Types of Solids
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Substances with very little intermolecular
attraction exist as gases
Substances with strong intermolecular
attraction exist as liquids
Substances with very strong intermolecular
(or ionic) attraction exist as solids
Forces and Phases
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Intermolecular Forces
Forces of attraction between different
molecules rather than bonding forces within
the same molecule.
Dipole-dipole attraction
Hydrogen bonds
Dispersion forces
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Phase Differences
Solid – definite volume and shape; particles
packed in fixed positions; particles are not
free to move
Liquid – definite volume but indefinite
shape; particles close together but not in
fixed positions; particles are free to move
Gas – neither definite volume nor definite
shape; particles are at great distances from
one another; particles are free to move
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CHAPTER 10.4
CHANGES OF STATE
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Changes of State
Common ones:
Condensation
Evaporation
Melting
Freezing
Sublimation
Deposition
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Sublimation
Sublimation is the phase change from solid to gas
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Deposition
Deposition is the phase change from gas to solid
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Phase: A phase is any part of a system that
has uniform composition and properties.
Condensation: is the process by which a gas
changes to a liquid. A gas that is in contact with
its solid or liquid phase is called a vapor.
Equilibrium: is a dynamic condition in which two
opposing changes occur at equal rates in a
closed system.
Phases
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Equilibrium
Dynamic Equilibrium: After time, the amount
of particles vaporizing equals the particles
condensing
rate of evaporation = rate of condensation
Particles are still vaporizing and still
condensing…it doesn’t stop!!!
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Phase Diagrams
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Phase Diagram
A diagram that represents the
phases of a substance as a function
of temperature and pressure.
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Gives:
Critical temperature
Critical pressure.
Critical point
Phase Diagram
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Phase Diagram for Water
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Carbon dioxide
CO2
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Phase Diagram
Critical temperature: the highest
temperature at which the solid and
liquid phases can exist. (Above the
critical temperature, the substance
can only be found as a gas)
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Critical pressure: the pressure
required to liquefy a gas at its
critical temperature (The pressure
needed to turn the gas into a
liquid)
Phase Diagram
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Critical point: temperature and
pressure above which a
substance can only exist as a
gas (substance cannot exist as a
solid or liquid above this
temperature)
Phase Diagram
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Phase Diagram
Critical point: critical temperature
and pressure
For water, Tc = 374°C and
Tp = 218 atm
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Phase Diagram: How to Read
Melting/Freezing occurs at the line
between the solid and liquid
Boiling/Condensing occurs at the
line between the liquid and gas
Sublimation/Deposition occurs at
the line between the solid and gas
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Phase Diagram: How to Read
The “normal” boiling point refers
to the temperature a substance
boils at Standard Pressure
The “normal” freezing point refers
to the temperature a substance
freezes at Standard Pressure
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Phase Diagram: How to Read
The “normal” condensation point
refers to the temperature a
substance condenses at Standard
Pressure
The “normal” melting point refers
to the temperature a substance
melts at Standard Pressure
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VAPOR PRESSURE
A liquid will begin to boil when its
vapor pressure equals the external
pressure
Thus, as the pressure in the room
changes, the boiling point of the
liquid will change as well.
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Vapor Pressure
The IUPAC standard boiling point of
water at standard pressure is 99.61 °C
On top of Mount Everest, at 29,029 ft
the pressure is about 255 Torr and the
boiling point of water is 71 °C.
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At standard pressure (1 atm) the temperature at which a liquid will boil is called the normal boiling point
You can use a vapor pressure graph to determine the boiling point of a liquid at any pressure
VAPOR PRESSURE
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Vapor Pressure Diagrams
At standard
pressure
(760mmHg),
liquid A will boil
around 72oC.
Liquid B will boil
around 115oC.
At what temps
will they boil at
400mmHg?
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Vapor Pressure Diagrams
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Boiling and Freezing
When a substance boils or freezes
(or melts or condenses) the
temperature of the system will
remain constant (does not change)
until the phase change is complete
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Boiling
This means, boiling water has a temp of 100oC, not higher.
The temp will begin to rise when all the water is boiled away into steam
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Freezing/ melting
This also means melting ice has a
temp of 0oC, not lower, not higher.
The temp will begin to rise when all
the ice is melted
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Water phase changes
Temperature remains constant
during a phase change.
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Boiling and Freezing
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Specific Heats of Water
Constants
Water: 4.184 J/g·oC
Ice: 2.03 J/g·oC
Steam: 2.01 J/g·oC
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Heat During Phase Change
Examples:
Heats of fusion (melting) = Hfus
Heats of solidification (freezing) = Hsolid
Heats of vaporization (boiling)= Hvap
Heats of condensation = Hcond
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Heat of Vaporization & Condensation:
The amount of heat necessary to vaporize one mole of water is its molar heat of vaporization
For water = Hvap = 40.7 kJ/mol
The amount of heat necessary to melt one mole of ice is its molar heat of fusion.
For water Hfus = 6.01 kJ/mol
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Specific Heats of Water
ΔHfus = 333.6 J/g Specific heat of water: 4.184 J/g0C
ΔHsolid = -333.6 J/g
ΔHvap = 2259.6 J/g Specific heat of ice: 2.108 J/g0C
ΔHcon = -2259.6 J/g
ΔHfus = 6.01 kJ/mole Specific heat of steam: 1.996 J/g0C
ΔHvap = 40.7 kJ/mole q = mc ΔT q = ΔH x m
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Water phase changes
Temperature remains constant
during a phase change.
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Distillation
Uses the specific boiling point of each liquid to
separate a mixture of liquids
Boiling point is a physical property and unique
to each substance
As a substance is boiling the temperature
remains CONSTANT regardless of how much
energy is added to the system
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Distillation Apparatus