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I. Kinetic Molecular Theory
KMT
I. Kinetic Molecular Theory
KMT
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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.
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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.
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Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
II. Intermolecular ForcesII. Intermolecular Forces
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Definition of IMFDefinition of IMF
Attractive forces between molecules.
Much weaker than chemical bonds within molecules.
a.k.a. van der Waals forces
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Types of IMFTypes of IMF
London Dispersion Forces
View animation online.
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Types of IMFTypes of IMF
Dipole-Dipole Forces
+ -
View animation online.
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Types of IMFTypes of IMF
Hydrogen Bonding
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Types of IMFTypes of IMF
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Ion-DipoleIon-Dipole
Attraction between an Ion and a polar covalent bond (dipole)
IMF responsible for salts dissolving in water.
Strength determines salt solubility.
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III. Physical PropertiesIII. Physical Properties
Liquids & SolidsLiquids & SolidsLiquids & SolidsLiquids & Solids
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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
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Liquid PropertiesLiquid Properties
Surface Tension• attractive force between particles in a
liquid that minimizes surface area
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Liquid PropertiesLiquid Properties
Capillary Action• attractive force between the surface of
a liquid and the surface of a solid
water mercury
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Types of SolidsTypes of Solids
Crystalline - repeating geometric pattern• covalent network• metallic• ionic• covalent molecular
Amorphous - no geometric pattern
decreasingm.p.
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Types of SolidsTypes of Solids
Ionic(NaCl)
Metallic
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Types of SolidsTypes of Solids
CovalentMolecular
(H2O)
CovalentNetwork
(SiO2 - quartz)
Amorphous(SiO2 - glass)
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Solvation In Aqueous Solutions
Solvation In Aqueous Solutions
Solvation – process of surrounding solute particles with solvent particles
Why are some substances soluble in a solvent and some others are not?
must be compatibility between solute and solvent
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“like dissolves like”“like dissolves like”
Defn – rule used to determine if substance will dissolve in another
- based on attractive forces between solute and solvent
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SolubilitySolubility
Defn – max amt of solute that can dissolve in a solvent at a specific temp
how much solute can be put into solvent?
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Unsaturated SolutionUnsaturated Solution
Defn – less than max amt of solute dissolved
if I put sugar into water and all sugar is dissolved, solution is unsaturated
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Saturated SolutionSaturated Solution
Defn – contains max amt of solute dissolved
if I put sugar into water and not dissolves (you can see the sugar), the solution is saturated
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Supersaturated SolutionSupersaturated Solution
Defn – contains more solute than saturated solution at the same conditions
a saturated solution made at high temp cools slowly. Slow cooling allows excess solute to remain dissolved in solution at lower temperature
very unstable
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Solubility Curve (generic)Solubility Curve (generic)
Curve represents max amount solute allowed
Temperature
Solu
bili
ty(g
solu
te/
10
0 g
H2O
)
Unsaturated(below line)
Saturated(above line)
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Solubility RulesSolubility Rules
Some ions always form water soluble compounds.
Other ions always form water insoluble compounds
The rest are sometimes water soluble and sometimes insoluble
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Always SolubleAlways Soluble
The following ions are always soluble, no matter what the other ion is.• Group IA (Li, Na…)
• Ammonium (NH4+)
• Nitrates (NO3-)
• Chlorates (ClO3-)
• Acetates (C2H3O2-)
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Almost always solubleAlmost always soluble
Halides (Cl, Br…)• Except for fluorides• Except for silver, mercury(I) and lead
Sulfates• Except for barium, calcium, lead,
mercury(I)
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Mostly insolubleMostly insoluble
Hydroxide (OH-)
• Except for barium, strontium and calcium (these ARE soluble along with the always soluble ions)
Sulfides, carbonates, chromates, and phosphates.