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Inter- molecular Forces. Have studied INTRA molecular forces—the forces holding atoms together to form molecules. Now turn to forces between molecules — INTER molecular forces. Forces between molecules, between ions, or between molecules and ions. Ion-Ion Forces for comparison of magnitude. - PowerPoint PPT Presentation
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© 2006 Brooks/Cole - Thomson
Inter-Inter-moleculamolecular Forcesr Forces
Have studied Have studied INTRAINTRAmolecular molecular forces—the forces holding forces—the forces holding atoms together to form atoms together to form molecules.molecules.
Now turn to forces between Now turn to forces between molecules —molecules — INTERINTERmolecular forces. molecular forces.
Forces between molecules, Forces between molecules, between ions, or between between ions, or between molecules and ions.molecules and ions.
© 2006 Brooks/Cole - Thomson
Ion-Ion Forcesfor comparison of
magnitudeNaNa++—Cl—Cl-- in salt in saltThese are the These are the
strongest forces.strongest forces. Lead to solids with Lead to solids with
high melting high melting temperatures.temperatures.
NaCl, mp = 800 NaCl, mp = 800 ooCCMgO, mp = 2800 MgO, mp = 2800 ooCC
© 2006 Brooks/Cole - Thomson
Covalent Bonding Forcesfor comparison of
magnitude
C–H, 413 kJ/molC–H, 413 kJ/mol
C=C, 610 kJ/molC=C, 610 kJ/molC–C, 346 kJ/molC–C, 346 kJ/mol
CN, 887 kJ/molCN, 887 kJ/mol
© 2006 Brooks/Cole - Thomson
Attraction Between Ions and Permanent
Dipoles
Water is highly polar Water is highly polar and can interact and can interact with positive ions to with positive ions to give give hydratedhydrated ions in water.ions in water.
HH
water dipole••
••
O-
+
© 2006 Brooks/Cole - Thomson
Attraction Between Ions and Permanent
Dipoles
Water is highly polar Water is highly polar and can interact and can interact with positive ions to with positive ions to give give hydratedhydrated ions in water.ions in water.
HH
water dipole••
••
O-
+
© 2006 Brooks/Cole - Thomson
Attraction Between Ions and Permanent
Dipoles
Many metal ions are hydrated. This is Many metal ions are hydrated. This is the reason metal salts dissolve in the reason metal salts dissolve in waterwater..
© 2006 Brooks/Cole - Thomson
Attraction between ions and dipole depends on Attraction between ions and dipole depends on ion chargeion charge and and ion-dipole distanceion-dipole distance..
Measured by ∆H for MMeasured by ∆H for Mn+n+ + H + H22O --> [M(HO --> [M(H22O)O)xx]]n+n+
-1922 kJ/mol-1922 kJ/mol-405 kJ/mol-405 kJ/mol-263 kJ/mol-263 kJ/mol
Attraction Between Ions and Permanent
Dipoles
OH
H+
-• • • O
H
H+
-• • • O
H
H+
-• • •
Na+Mg2+
Cs+
© 2006 Brooks/Cole - Thomson
Dipole-Dipole Forces
Such forces bind molecules having Such forces bind molecules having permanent dipoles to one another.permanent dipoles to one another.
© 2006 Brooks/Cole - Thomson
Dipole-Dipole Forces
Influence of dipole-dipole forces is seen in Influence of dipole-dipole forces is seen in the boiling points of simple molecules.the boiling points of simple molecules.
CompdCompd Mol. Wt.Mol. Wt. Boil PointBoil PointNN22 2828 -196 -196 ooCCCOCO 2828 -192 -192 ooCCBrBr22 160160 59 59 ooCCIClICl 162162 97 97 ooCC
© 2006 Brooks/Cole - Thomson
Hydrogen BondingA special form of dipole-dipole attraction, A special form of dipole-dipole attraction,
which enhances dipole-dipole attractions.which enhances dipole-dipole attractions.
H-bonding is strongest when X and Y are H-bonding is strongest when X and Y are N, O, N, O, or For F
© 2006 Brooks/Cole - Thomson
Hydrogen Bonding in H2O
H-bonding is especially H-bonding is especially strong in water strong in water becausebecause
• the O—H bond is very the O—H bond is very polarpolar
• there are 2 lone pairs there are 2 lone pairs on the O atomon the O atom
Accounts for many of Accounts for many of water’s unique water’s unique properties.properties.
© 2006 Brooks/Cole - Thomson
Hydrogen Bonding in H2OIce has open Ice has open
lattice-like lattice-like structure.structure.
Ice density is Ice density is < liquid.< liquid.
And so solid And so solid floats on floats on water.water.
Snow flake: www.snowcrystals.com
© 2006 Brooks/Cole - Thomson
Hydrogen Bonding in H2OIce has open lattice-like structure.Ice has open lattice-like structure.Ice density is < liquid and so solid floats on Ice density is < liquid and so solid floats on
water.water.
One of the VERY One of the VERY few substances few substances where solid is LESS where solid is LESS DENSE than the DENSE than the liquid.liquid.
© 2006 Brooks/Cole - Thomson
Hydrogen Bonding in H2OH bonds ---> abnormally high specific heat capacity of H bonds ---> abnormally high specific heat capacity of
water (4.184 J/g•K)water (4.184 J/g•K)This is the reason water is used to put out fires, it is the This is the reason water is used to put out fires, it is the
reason lakes/oceans control climate, and is the reason reason lakes/oceans control climate, and is the reason thunderstorms release huge energy.thunderstorms release huge energy.
© 2006 Brooks/Cole - Thomson
Boiling Points of Boiling Points of Simple Hydrogen-Simple Hydrogen-
Containing Containing CompoundsCompounds
Active Figure 13.8Active Figure 13.8
© 2006 Brooks/Cole - Thomson
Portion of Portion of a DNA a DNA chainchain
Double Double helix of helix of
DNADNA
H-bonding is especially strong in biological systems — such as H-bonding is especially strong in biological systems — such as DNA. DNA. DNA — helical chains of phosphate groups and sugar molecules. DNA — helical chains of phosphate groups and sugar molecules. Chains are helical because of tetrahedral geometry of P, C, and O.Chains are helical because of tetrahedral geometry of P, C, and O.Chains bind to one another by specific hydrogen bonding between Chains bind to one another by specific hydrogen bonding between pairs of Lewis bases.pairs of Lewis bases. ——adenine with thymineadenine with thymine ——guanine with cytosineguanine with cytosine
© 2006 Brooks/Cole - Thomson
Base-Pairing through H-Bonds
© 2006 Brooks/Cole - Thomson
Base-Pairing through H-Bonds
© 2006 Brooks/Cole - Thomson
FORCES INVOLVING INDUCED DIPOLES
How can non-polar molecules such as OHow can non-polar molecules such as O2 2 and Iand I22 dissolve in water? dissolve in water?
The water dipole The water dipole INDUCESINDUCES a a dipole in the Odipole in the O22 electric electric cloud. cloud.
Dipole-Dipole-induced induced dipoledipole
© 2006 Brooks/Cole - Thomson
FORCES INVOLVING INDUCED DIPOLES
Solubility increases with mass the gasSolubility increases with mass the gas
© 2006 Brooks/Cole - Thomson
FORCES INVOLVING INDUCED DIPOLES
•Process of Process of inducing a dipole inducing a dipole is is polarizationpolarization
•Degree to which Degree to which electron cloud of electron cloud of an atom or an atom or molecule can be molecule can be distorted in its distorted in its polarizabilitypolarizability..
© 2006 Brooks/Cole - Thomson
IM FORCES — INDUCED DIPOLES
Consider IConsider I22 dissolving dissolving in ethanol, in ethanol, CHCH33CHCH22OH.OH.
OH
-
+
I-I
R-
+
OH
+
-
I-I
R
The alcohol The alcohol temporarily temporarily creates or creates or
INDUCESINDUCES a a dipole in Idipole in I22..
© 2006 Brooks/Cole - Thomson
FORCES INVOLVING INDUCED DIPOLES
Formation of a dipole in two nonpolar IFormation of a dipole in two nonpolar I22 molecules.molecules.
Induced dipole-induced dipole
The induced forces between IThe induced forces between I22 molecules are very weak, so molecules are very weak, so solid Isolid I22 sublimes (goes from a solid to gaseous molecules). sublimes (goes from a solid to gaseous molecules).
© 2006 Brooks/Cole - Thomson
FORCES INVOLVING INDUCED DIPOLES
The magnitude of the induced dipole The magnitude of the induced dipole depends on the tendency to be distorted. depends on the tendency to be distorted.
Higher molec. weight ---> larger induced Higher molec. weight ---> larger induced dipoles.dipoles.
MoleculeMolecule Boiling Point Boiling Point ((ooC)C) CHCH44 (methane) (methane) - 161.5- 161.5 CC22HH66 (ethane) (ethane) - 88.6 - 88.6 CC33HH88 (propane) (propane) - 42.1- 42.1 CC44HH1010 (butane) (butane) - 0.5- 0.5
© 2006 Brooks/Cole - Thomson
Boiling Points of Hydrocarbons
Note linear relation between bp and molar mass.
CHCH44
CC22HH66
CC33HH88
CC44HH1010
© 2006 Brooks/Cole - Thomson
Intermolecular Forces Summary
© 2006 Brooks/Cole - Thomson
Equilibrium Vapor PressureActive Figure 13.18
© 2006 Brooks/Cole - Thomson
Liquids Equilibrium Vapor Pressure
FIGURE 13.18:FIGURE 13.18: VP as a function of T.VP as a function of T.1. The curves show all conditions of P and T where LIQ 1. The curves show all conditions of P and T where LIQ
and VAP are in and VAP are in EQUILIBRIUMEQUILIBRIUM2. The VP rises with T.2. The VP rises with T.3. When VP = external P, the liquid boils.3. When VP = external P, the liquid boils. This means that BP’s of liquids change with altitude.This means that BP’s of liquids change with altitude.4. If external P = 760 mm Hg, T of boiling is the 4. If external P = 760 mm Hg, T of boiling is the
NORMAL BOILING POINTNORMAL BOILING POINT5. VP of a given molecule at a given T depends on IM 5. VP of a given molecule at a given T depends on IM
forces. Here the VP’s are in the orderforces. Here the VP’s are in the order
CC 22HH 55HH 55CC22 HHHH 55CC 22 HHHH
waterwateralcoholalcoholetherether
increasing strength of IM interactionsincreasing strength of IM interactions
extensiveextensiveH-bondsH-bondsH-bondsH-bonds
dipole-dipole-dipoledipole
OOOOOO
© 2006 Brooks/Cole - Thomson
Liquids
HEAT OF VAPORIZATIONHEAT OF VAPORIZATION is the heat is the heat req’d (at constant P) to vaporize the liquid.req’d (at constant P) to vaporize the liquid.
LIQ + heat ---> VAPLIQ + heat ---> VAPCompd.Compd. ∆H∆Hvapvap (kJ/mol) (kJ/mol) IM ForceIM ForceHH22OO 40.7 (100 40.7 (100 ooC)C) H-bondsH-bondsSOSO22 26.8 (-47 26.8 (-47 ooC)C) dipoledipoleXeXe 12.6 (-107 12.6 (-107 ooC)C) induced induced
dipole dipole
© 2006 Brooks/Cole - Thomson
Phase Diagrams
Lines connect all conditions of T and P where EQUILIBRIUM exists Lines connect all conditions of T and P where EQUILIBRIUM exists between the phases on either side of the line. (At equilibrium between the phases on either side of the line. (At equilibrium particles move from liquid to gas as fast as they move from gas to particles move from liquid to gas as fast as they move from gas to liquid, for example.)liquid, for example.)
© 2006 Brooks/Cole - Thomson
Phase Equilibria — WaterSolid-liquidSolid-liquid
Gas-LiquidGas-Liquid
Gas-SolidGas-Solid
© 2006 Brooks/Cole - Thomson
Triple Point — Water
At the TRIPLE POINT all three phases are in equilibrium.
© 2006 Brooks/Cole - Thomson
Phases Diagrams—Important Points for Water
T(˚C)T(˚C)P(mmHg)P(mmHg)Normal boil point Normal boil point 100100 760 760Normal freeze pointNormal freeze point 00 760 760Triple point Triple point 0.00980.0098 4.58 4.58
© 2006 Brooks/Cole - Thomson
Critical T and P
.
LIQUID
GAS
Pcritical
Hig
h Pr
essu
re
High Temperature
Tcritical
Note that linegoes straight up
Above Above critical T no critical T no liquid exists liquid exists no matter no matter how high the how high the pressure.pressure.
As P and T increase, you finally reach the CRITICAL T and PAs P and T increase, you finally reach the CRITICAL T and P
At P < 4.58 mmHg and T < 0.0098 ˚C solid HAt P < 4.58 mmHg and T < 0.0098 ˚C solid H22O O can go directly to vapor. This process is called can go directly to vapor. This process is called SUBLIMATIONSUBLIMATIONThis is how a frost-free refrigerator works.This is how a frost-free refrigerator works.
© 2006 Brooks/Cole - Thomson
Critical T and PCOMPDCOMPD TTcc((ooC)C) PPcc(atm)(atm)HH22OO 374374 218218COCO22 3131 7373CHCH44 -82-82 4646Freon-12Freon-12 112112 4141
(CCl(CCl22FF22))Notice that TNotice that Tcc and P and Pcc depend on depend on
intermolecular forces.intermolecular forces.
© 2006 Brooks/Cole - Thomson
Solid-Liquid Equilibria
Raising the pressure at constant Raising the pressure at constant T causes water to melt.T causes water to melt.
The NEGATIVE SLOPE of the S/L The NEGATIVE SLOPE of the S/L line is unique to Hline is unique to H22O. Almost O. Almost everything else has positive everything else has positive slope.slope.
LIQUID H2OICEfavored atlow P
favored athigh P
SolidH2O
LiquidH2O
P
T
760mmHg
0 °C
Normalfreezingpoint
The behavior of water under pressure is an example of The behavior of water under pressure is an example of LE LE CHATELIER’S PRINCIPLE CHATELIER’S PRINCIPLE At Solid/Liquid equilibrium, At Solid/Liquid equilibrium, raising P squeezes the solid. raising P squeezes the solid. It responds by going to phase with greater density, i.e., the It responds by going to phase with greater density, i.e., the liquid phase.liquid phase.In any system, if you increase P the In any system, if you increase P the DENSITYDENSITY will go up. will go up.
Therefore — as P goes up, equilibrium favors phase with Therefore — as P goes up, equilibrium favors phase with the larger density (or the larger density (or SMALLERSMALLER volume/gram). volume/gram).