Condensed Phases and Intermolecular Forces. Fundamentals How do particle diagrams of liquids &...
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Transcript of Condensed Phases and Intermolecular Forces. Fundamentals How do particle diagrams of liquids &...
![Page 1: Condensed Phases and Intermolecular Forces. Fundamentals How do particle diagrams of liquids & solids compare to those of gases?](https://reader034.fdocuments.us/reader034/viewer/2022042613/551b09f45503465e7d8b5c7b/html5/thumbnails/1.jpg)
Condensed Phases
and
Intermolecular Forces
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Fundamentals
How do particle diagrams of liquids & solids compare to those of gases?
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Describe relative positions and motions of particles in each of 3 phases
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The Question
Why do some substances exist as gases, some as liquids, and some as solids
at room temp?
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Part of answer has to do with forces between separate molecules
2 broad categories of forces need to be aware of
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Forces
INTERMOLECULAR INTRAMOLECULAR
Dispersion
Dipole-Dipole
Hydrogen Bonding
Covalent
Ionic
Metallic
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#1: Intramolecular ForcesIntramolecular forces = attractive
forces that hold particles together in bonds (ionic, covalent, or metallic)
Intra means “within”Intramolecular forces = bonding forces
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# 2: Intermolecular Forces-IMF (aka: van der Waals forces) Inter means “between” or “among”
Intermolecular forces = forces between neighboring molecules
Intermolecular forces are weaker than Intramolecular forces
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Intermolecular forces determine Intermolecular forces determine phasephase
“Competition” between strength of IMF & KE determines phase
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If IMF are strong, substance will be solid or liquid at room tempParticles want to clump together
If IMF are weak, substance will be gas at room temp
Particles free to spread apart
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It’s a balancing act!
Intermolecular Forces
Kinetic Energy
[this substance = a gas at room temperature]
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Intermolecular Forces vs. Kinetic Energy
Intermolecular Forces
Kinetic Energy
[this substance = a condensed phase (solid/liquid)]
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Why Temperature Changes Affect PhaseSince T is measure of average KE, changing T can change phase
Changing T will change average KE
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Changing the temperature
Intermolecular Intermolecular ForcesForces
KineticEnergy
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Intermolecular Forces:≈ 5% to 15% of strength of
intramolecular or bonding forces
Account for phase at room tempAccount for phase at room temp
Strong IMF condensed phase
Weak IMF gas phase
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3 types of intermolecular forces (IMF):
1.Dispersion forces2.Dipole-Dipole forces3.Hydrogen bonds
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1. 1. Dispersion ForcesDispersion Forces:
● weakest IMF ● occur between nonpolar molecules
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2. 2. Dipole-dipole Dipole-dipole forcesforces:
• intermediate IMF • occur between polar molecules
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3. 3. Hydrogen bondsHydrogen bonds:
• strongest IMF • occur between molecules that have:
H-F H-O or H-N bonds
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Dispersion Forces & Nonpolar molecules
•instantaneous and momentary•fluctuate•results from motion of electrons
if charge cloud not symmetrical will induceinduce asymmetry in neighbor’s charge cloud!
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Nonpolar molecules
NonNonpolar means nono poles• Can’t tell one end of molecule from other end•electrons are evenly distributed
Symmetrical
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Examples of Nonpolar Molecules
monatomic gas molecules: He, Ne, Ar, Kr, Xe, Rn
diatomics if both atoms are same: H2, N2, O2, Cl2, F2, I2, Br2
symmetrical molecules: CH4, C2H6, C3H8
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Dispersion Forces and Size
Dispersion forces ↑ with molecule size
larger the electron cloud, the greater the fluctuations in charge can beRn > Xe > Kr > Ar > Ne > HeI2 > Br2 > Cl2 > F2
C8H18 > C5H12 > C3H8 > CH4
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Boiling point of N2 is 77 K (-196˚C)IMF are very weak dispersion forces
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Dipole-dipole Forces & Polar Molecules
Molecule shows permanent separation of charge; has poles: one end partly (-) & one end partly (+)
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Polar means molecule has poles: (+) & (-) geometry and electron distribution are not symmetrical
Polar Molecules
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What do you know about charge?
Opposites Attract!this time, situation is permanent!
Examples: HI, CH3Cl
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Hydrogen Bonding
H-O N-H
Occurs between molecules with H-F, H-O, or H-N bonds (FON!!!)
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Hydrogen Bonding
Hydrogen bonding is extreme case of dipole-dipole bondingF, O, and N are all small and
electronegative strong electrons attraction H has only 1 electron, so if being pulled
away H proton is almost “naked” H end is always positive & F, O, or N end is always negative
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Hydrogen bonding: • strongest IMF• influences physical props a great deal
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Strength of Hydrogen BondingFluorine most electronegative element, so H-F bonds are most polar and exhibit
strongest hydrogen bonding
H-F > H-O > H-N
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IMF vs. Physical Properties
If IMF then:Boiling point Melting point Heat of Fusion Heat of Vaporization while: Evaporation Rate
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Intermolecular Force vs. TemperatureIMF more important as
temperature is loweredLow temperature – low evaporation rate
High temperature – high evaporation rate
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Indicate type of IMF for each molecule:NH3
ArN2
HClHFNeO2
HBrCH3NH2
• Hydrogen bonding• Dispersion forces• Dispersion forces• Dipole-dipole
forces• Hydrogen bonding• Dispersion• Dispersion• Dipole-dipole• Hydrogen bonding