Intermolecular Forces Intermolecular Forces: weaker interactions that occur between molecules. These...
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Intermolecular Forces Intermolecular Forces: weaker interactions that occur between molecules. These are collectively known as Van der Waals forces. Intramolecular
Intermolecular Forces Intermolecular Forces: weaker
interactions that occur between molecules. These are collectively
known as Van der Waals forces. Intramolecular Forces: Do not
confuse Inter with Intra! Intramolecular forces are how we describe
bonding between atoms.
Slide 3
Intermolecular Forces
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Types of IMF London Dispersion Forces View animation
online.animation
Slide 5
Types of IMF Dipole-Dipole Forces + + - - View animation
online.animation
Slide 6
Types of IMF Hydrogen Bonding
Slide 7
Liquids vs. Solids IMF Strength Fluid Density Compressible
Diffusion LIQUIDS Stronger than in gases Y high N slower than in
gases SOLIDS Very strong N high N extremely slow
Slide 8
Liquid Properties Surface Tension attractive force between
particles in a liquid that minimizes surface area
Slide 9
Liquid Properties Capillary Action attractive force between the
surface of a liquid and the surface of a solid watermercury
Slide 10
Viscosity: Resistance to flow (molecules with large
intermolecular forces). Liquid Properties
Types of Solids: Metals The electron sea model for metals
postulates a regular array of cations in a "sea" of valence
electrons. (a) Representation of an alkali metal (Group 1A) with
one valence electron. (b) Representation of an alkaline earth metal
(Group 2A) with two valence electrons.
Slide 16
Types of Solids: Metals Alloy: A substance that contains a
mixture of elements and has metallic properties Substitutional
Alloy (a): some of the host metal atoms are replaced with atoms
similar size metal atom Interstial Alloy (b): some of holes between
the metal atoms are filled with smaller atoms
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Phase Changes
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Evaporation Evaporation molecules at the surface gain enough
energy to overcome IMF Volatility Volatility measure of evaporation
rate depends on temp & IMF
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Phase Changes Equilibrium Equilibrium trapped molecules reach a
balance between evaporation & condensation
Slide 20
Phase Changes Vapor Pressure Vapor Pressure pressure of vapor
above a liquid at equilibrium IMFv.p.tempv.p. depends on temp &
IMF directly related to volatility temp v.p.
Slide 21
Phase Changes Boiling Point temp at which v.p. of liquid equals
external pressure IMFb.p.P atm b.p. depends on P atm & IMF
Normal B.P. - b.p. at 1 atm
Slide 22
Which has a higher m.p.? polar or nonpolar? covalent or ionic?
Phase Changes Melting Point equal to freezing point polar ionic
IMFm.p.
Slide 23
Phase Changes Sublimation solid gas v.p. of solid equals
external pressure EX: dry ice, mothballs, solid air fresheners
Slide 24
Heating and Cooling curve
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Heating 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 1C -
Slide 26
Heating Curves Phase Change change in PE (molecular
arrangement) temp remains constant Heat of Fusion ( H fus ) energy
required to melt 1 gram of a substance at its m.p.
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Heating Curves Heat of Vaporization ( H vap ) energy required
to boil 1 gram of a substance at its b.p. usually larger than H fus
why? EX: sweating, steam burns, the drinking bird
Slide 28
Temperature Pressure Phase Diagrams We know that different
compounds can have different phases. These phases depend on the
temperature and pressure of the substance. We can then use that
information to create a diagram of the different phases called a
PHASE DIAGRAM.
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Looking at Phase Diagrams The boundaries between phases occur
at phase changes (ie. melting, freezing, vaporizing, etc.) A -
melting, freezing B - vaporization, condensation C - sublimation,
deposition S L G Temperature Pressure A B C
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S L G Temperature Pressure Looking at Phase Diagrams The triple
point is where the boundaries converge at one point and all three
phases are present at the same time. Triple Point
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S L G Temperature Pressure Looking at Phase Diagrams Critical
Point The critical point is the point at which the distinction
between the liquid phase and gas phase ceases to exist.
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S L G Temperature Pressure Determining the Melting Point 1.
Find the current pressure 2. Draw a line across the diagram 3. At
the boundary between the solid and liquid phase, draw a line down
to the temperature 4. Determine the temperature 1 atm
Slide 33
Phase Change of Water
Slide 34
Phase Diagrams Each substance or compound has different
melting/freezing points, boiling/condensing points, and
sublimation/deposition points. Therefore, each substance or
compound has a different phase diagram. Carbon