1 chapter 12: liquids, solids and interparticle forces
TRANSCRIPT
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Chapter 12: Liquids, Solids and Interparticle Forces
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What is a liquid? A solid?
Properties of liquids and solids: depend on Interparticle (Intermolecular) forces- vaporization/condensation/freezing- equilibrium vapor pressure/volatility- surface tension- boiling point/freezing point
We are going to learn about Interparticle or Intermolecular forces first!
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TYPES OF INTERPARTICLE FORCES - SEE HANDOUT
All forces of attraction between atoms, ions, molecules are “Interparticle” forces
Includes ionic bonding, covalent bonding, metallic bonding, and ion-dipole attraction
Important Subcategory is Intermolecular Forces Also called Van Der Waal’s forcesWeak to moderate forces of attractionNot a type of bondingIncludes three main ones: London Dispersion Forces, Dipole-dipole Attraction and Hydrogen Bonding Attraction
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Intermolecular Forces
1. London dispersion forces (LDF)- Small to moderate strength- Depend on size of electron cloud (and so also molar mass) of atom or molecule- Noble gases, diatomic elements, and many other nonpolar compounds
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Nonpolar molecules such as H2 can develop instantaneous dipoles and induced dipoles. The attractions between such dipoles, even through they are transitory, create London dispersion forces. (See figures 12.17 & 18)
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Noble Gas
Molar Mass, (g/mol)
Boiling Point, (K)
He 4.00 4.2
Ne 20.18 27
Ar 39.95 87
Kr 83.80 120
Xe 131.29 165
Table 12.4: Dispersion Force and Molar Mass
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Relationship between Dispersion Force and Molecular Size
-300
-250
-200
-150
-100
-50
0
50
100
150
200
250
1 2 3 4 5 6
Period
Boi
ling
Poi
nt, °
C
BP, Noble Gas
BP, Halogens
BP, XH4
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Intermolecular Forces
2. Dipole-dipole attraction- Moderate strength- Molecules that have polar covalent bonds- Polar molecules + and - attraction
Table of Properties of HydrohalogensH-F H-Cl H-Br H-I
EN 1.4 1.1 0.8 0.4# e-s 10 18 36 54BP 291 188 206 238
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There are many dipole-dipole interactions possible between randomly arranged ClF molecules. In each interaction, the positive end of one molecule is attracted to the negative end of a neighboring ClF molecule.
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MolarMass (g/mol)
Boiling Point, °C
Dipole Size, D
CH3CH2CH3 44 -42 0
CH3-O-CH3 46 -24 1.3
CH3 - CH=O 44 20.2 2.7
CH3-CN 41 81.6 3.9
Polarity and Dipole-to-Dipole Attraction
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Intermolecular Forces
3. Hydrogen-bonding (enhanced dipole-dipole)- Strong force, but much less than real bonding- Memory helper: E.T. FON Home: only F-H, O-H and N-H have this type of force- Due to small radius and high EN- See in boiling point data
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Depiction of hydrogen bonding among water molecules. The dotted lines are the hydrogen bonds.
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Figures 12.22 & 24: Intermolecular H-Bonding
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Hydrogen Bonding and Water:Water - 80% hydrogen-bonded - very tight
arrangement (also high viscosity high density and high specific heat)
Ice - crystal is very open, less dense than liquid
(4. Dipole - induced dipole between diff types of molecules, O2 in H2O)
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Diagrams of hydrogen bonding involving selected simple molecules. The solid lines represent covalent bonds; the dotted lines represent hydrogen bonds.
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If there were no hydrogen bonding between water molecules, the boiling point of water would be approximately - 80C.
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Relationship between H-bonding and Intermolecular Attraction
-200
-150
-100
-50
0
50
100
150
1 2 3 4 5
Period
Bo
ilin
Po
int,
°C
BP, HX
BP, H2X
BP, H3X
BP, XH4
CH4
NH3
HF
H2O
SiH4
GeH4
SnH4
H2S H2Se
H2Te
Notice that molecules with F-H, O-H and N-H have HIGH BPs because of Hydrogen-bonding forces of attraction.
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Properties and H-Bonding
NameNameForm-Form-
ulaula
Molar Molar MassMass StructureStructure
BP,BP,
°C°CMP,MP,
°C°C
Sol’b Sol’b in in
WaterWater
EthaneEthane CC22HH66 30.030.0 -88-88 -172-172 immisimmiscc
MethanMethanolol
CHCH33OOHH
32.032.0 64.764.7 -97.8-97.8misc-misc-
bleble
H C
H
H
C H
H
H
H C
H
H
O H
Table on page 411 in Tro.
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Chemistry at a Glance:Intermolecular Forces
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PRACTICE IDENTIFYING THE TYPE OF IM FORCE:
CH4(g) C6H6(l)
Br2(l) HBr(l)
IBr(s) CH3OH(l)
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There are six changes of state possible for substances: learn all 6
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Distinguishing Properties of Solids, Liquids, and Gases
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BP, FP, Phase Changes, and Ho
phase
Boiling point: temperature at which the vapor pressure of a liquid is equal to the external pressure above the liquid, usually atmospheric pressure of 1 atm
Freezing point: temperature at which a liquid changes into a solid at 1 atm
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BP, FP, Phase Changes, and DHo
phase
Phase changes: changes of stateLearn all sixAccompanied by heat flow called
Enthalpy of phase change or Hophase
Heat of vaporization: liquid to vapor; energy (J) to vaporize 1 mol at constant T & P
Heat of fusion: solid to liquid; energy (J) to melt 1 mol at constant T & P
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BP, FP, Phase Changes, and Ho
phase
Sensible heat transfer: temperature is changed but not phase
q = m * cp * Tm is mass, cp is specific heat and T is Tf – Ti
See example (13.1***)Latent heat transfer using Ho
phase: phase changes but not temperature
q = m * Hophase
m is mass or moles depending on unitsSee example (13.2***)
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BP, FP, Phase Changes, and Ho
phase
Specific heat: energy required to raise temperature of 1.00 gram of substance by 1.00oC
cp for water is 4.184 J/g.oC
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In the evaporation of a liquid in a closed container (a), the liquid level drops for a time (b) and then becomes constant (ceases to drop). At that point a state of equilibrium has been reached in which the rate of evaporation equals the rate of condensation (c).
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Equilibrium Vapor Pressure
In closed system: at any given temperature, rate of vaporization = rate of condensation
At dynamic equilibrium: means number of molecules in gas phase and number of molecules in liquid phase stay the same, but processes still happening
Vapor pressure taken at equilibrium = the partial pressureVapor pressure changes with change in temperature
(listen to weather)Plot as vapor pressure curves: pressure vs. temperature
(see Fig 13.6)Boiling point anywhere along curve: see bubbles rise to
surfaceNormal boiling point is when vapor pressure is 1.00 atm or
760. Torr
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Vapor Pressure of Water at Various Temperatures.
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Boiling Point of Water at Various Locations That Differ in Elevation
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Just read about surface tension and capillary action
Just read section (****13.10 and skip section 13.11