I. Kinetic Molecular Theory KMT. Assumptions of KMT All matter is composed of tiny particles These...
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Transcript of I. Kinetic Molecular Theory KMT. Assumptions of KMT All matter is composed of tiny particles These...
I. Kinetic Molecular Theory
KMT
I. Kinetic Molecular Theory
KMT
Assumptions of KMTAssumptions of KMT
•All matter is composed of tiny particles
•These particles are in constant, random motion.
•Some particles are moving fast, some are moving slowly.
•Temperature is a measure of the average Kinetic Energy and is proportional to the average speed of the molecules.
KMT ModelKMT Model
http://preparatorychemistry.com/Bishop_KMT_frames.htm
Click on the link above to see how particles of matter behave according to the KMT.
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
II. Intermolecular ForcesII. Intermolecular Forces
Definition of IMFDefinition of IMF
Attractive forces between molecules.
Much weaker than chemical bonds within molecules.
a.k.a. van der Waals forces
Types of IMFTypes of IMF
London Dispersion Forces
View animation online.
Types of IMFTypes of IMF
Dipole-Dipole Forces
+ -
View animation online.
Types of IMFTypes of IMF
Hydrogen Bonding
Types of IMFTypes of IMF
III. Physical PropertiesIII. Physical Properties
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
Liquids vs. SolidsLiquids vs. Solids
LIQUIDS
Stronger than in gases
Y
high
N
slower than in gases
SOLIDS
Very strong
N
high
N
extremely slow
IMF Strength
Fluid
Density
Compressible
Diffusion
Liquid PropertiesLiquid Properties
Surface Tension• attractive force between particles in a
liquid that minimizes surface area
Liquid PropertiesLiquid Properties
Capillary Action• attractive force between the surface of
a liquid and the surface of a solid
water mercury
Types of SolidsTypes of Solids
Crystalline - repeating geometric pattern• covalent network• metallic• ionic• covalent molecular
Amorphous - no geometric pattern
decreasingm.p.
Types of SolidsTypes of Solids
Ionic(NaCl)
Metallic
Types of SolidsTypes of Solids
CovalentMolecular
(H2O)
CovalentNetwork
(SiO2 - quartz)
Amorphous(SiO2 - glass)
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
IV. Changes of StateIV. Changes of State
Phase ChangesPhase Changes
Most substances can exist in 3 states:• Solid• Liquid • Gas
Depends on temperature and pressure
Phase ChangesPhase Changes
Phase ChangesPhase Changes
Each state is referred to as a “Phase”• Ice water is a heterogeneous
mixture of 2 phasesWhen energy is added or removed,
one phase can change into another
Phase Changes Requiring Energy
Phase Changes Requiring Energy
MeltingVaporizationSublimation
MeltingMelting
Amount of energy needed to melt a substance depends on forces keeping particles together.• Melting water requires a high amount of energy
because of hydrogen bonding• Adding energy allows molecules to move
faster, breaking the hydrogen bonds• Melting point - Temperature at which the
forces holding crystal lattice together are broken and substance becomes liquid
Which has a higher m.p.?• polar or nonpolar?• covalent or ionic?
Phase ChangesPhase Changes
Melting Point• equal to freezing point
polar
ionic
IMF m.p.
VaporizationVaporization
In liquid water, some particles will have more kinetic energy than others.• When the particles have enough energy to
overcome the forces of attraction they will escape the liquid as a gas.
• Vapor - A substance that is liquid at room temperature and becomes gas.
• Vaporization - the process of changing a liquid to a gas
VaporizationVaporization
Evaporation - Vaporization that occurs at the surface of a liquid, molecules at the surface gain enough energy to overcome IMF
• Evaporation is gradual• Even at cold temperatures, some molecules have
enough energy to break the attractions and become gas.
Evaporation is how your body cools itself• Water in sweat absorbs heat from your body• Water evaporates leaving less heat in your body and a
lower ‘average kinetic energy’ (lower temperature)
Phase ChangesPhase Changes
Vapor PressureVapor Pressure• pressure of vapor above
a liquid at equilibrium
IMF v.p.temp v.p.
• depends on temp & IMF
p.478
temp
v.p
.
Phase ChangesPhase Changes
Boiling Point
IMF b.p.Patm b.p.
• Temperature at which the vapor pressure of a liquid equals the external atmospheric pressure
• depends on Patm & IMF
• Normal B.P. - b.p. at 1 atm
SublimationSublimation
Sublimation - when a substance goes from solid directly to gas without becoming a liquid• Solid iodine• Frozen carbon dioxide (dry ice)• Moth balls (p-dichlorobenzene)• Solid air fresheners• Ice cubes left in a freezer for a long time
Phase Changes the Release Energy
Phase Changes the Release Energy
CondensationDepositionFreezing
CondensationCondensation
Condensation – process of changing from gas to liquid• When molecule s lose energy,• Velocity of the molecules is reduced• Intermolecular forces take over• Hydrogen bonds form, energy is released (heat
comes out)• There are different causes for condensation,
however, all involve loss of energy:• Contact with cold item
Phase ChangesPhase Changes
EquilibriumEquilibrium• trapped molecules reach a balance
between evaporation & condensation
DepositionDeposition
Deposition – changing from gas directly to solid
• Snowflakes
FreezingFreezing
Freezing – process of changing from liquid to solid• Remove energy from liquid• Molecules don’t move past each other any
longer• Molecules stay in fixed, set position• Become solid
Phase ChangesPhase Changes
Energy Required Energy Released
Solid LiquidMelting or fusion
Liquid Solidfreezing
Liquid GasVaporization, evaporation or boiling
Gas Liquidcondensation
Solid Gassublimation
Gas Solidsolidification
Phase DiagramsPhase Diagrams
Phase diagram shows phase of matter at different temperatures and pressures• Each substance is unique• X-axis usually temperature• Y-axis usually pressure• There is usually a “Triple Point” where all
three phases can coexist• “Critical Point” – temperature and pressure
above which substance cannot exist as liquid
Phase Diagram - WaterPhase Diagram - Water
Phase Diagram CO2Phase Diagram CO2
Heating CurvesHeating Curves
Kinetic Energy Changes – Heat Energy speeds up the molecules.
Potential Energy Changes – Heat energy separates the molecules from solid to liquid, liquid to gas.
Heating CurvesHeating Curves
Temperature Change• change in KE (molecular motion) • depends on heat capacity
Heat Capacity• energy required to raise the temp of 1
gram of a substance by 1°C
Phase ChangePhase Change
The energy involved in a phase change is calculated using:
Heat of Fusion (Hfus)
Heat of Vaporization (Hvap)
Heat of FusionHeat of Fusion
Heat of Fusion is the energy required to change 1 gram of a substance from the solid to the liquid state without changing its temperature.
Heat of Fusion is used for calculations involving the phase changes of solid liquid or liquid solid
Heat of VaporizationHeat of Vaporization
Heat of Vaporization (Hvap)
• energy required to boil 1 gram of a substance at its b.p.
EX: sweating, steam burns, the drinking bird