topic: intermolecular forces part 2: dipole- dipole and hydrogen bonding do now: list the 4...
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TOPIC: Intermolecular ForcesPart 2: Dipole- Dipole and Hydrogen Bonding
Do Now: List the 4 categories of Nonpolar Molecules – all of these have DISPERSION FORCES Noble Gas –group 18:
He, Ne, Ar, Kr, Xe, Rn
7 diatomic elements
H2, N2, O2, Cl2, F2, I2, Br2
Pure Hydrocarbons – molecules with only C and H
General formula CxHy : examples = CH4, C2H6, C3H8
these 3 small symmetrical molecule
CO2, CF4, CCl4
All molecules have Dispersion forces (the regents calls these Van der Waals)
2 other types of forces (IMF): 1. Dipole-Dipole forces2. Hydrogen bonds
-if one of these are present, they are more important.
2. Dipole-dipole forces: • Stronger then dispersion forces• occur between polar (asymmetrical)
molecules (they have a partial charge at each pole – one is typically much larger than the other)
• Click here for animation (slide 3 of 13)
Dipole-dipole Forces & Polar Molecules
Polar Molecule shows permanent separation of charge; has poles: one end partially (-) & one end partially (+);Asymmetrical
3. Hydrogen bonds:
• strongest IMF • occur between molecules that have an :
H-F H-O or H-N bonds ONLY
Strongest Intermolecular Force
Hydrogen Bonding
Dipole-Dipole
Dispersion
Hydrogen Bonding
H-O N-H
Occurs between molecules with H-F, H-O, or H-N bonds
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
Strength of Hydrogen BondingFluorine most electronegative element, so
H-F bonds are most polar and exhibit strongest hydrogen bonding, so strongest IMF
H-F is stronger than H-O which is stronger than H-N
(H-bonding…sound like FON to me!!!)
OH
H
OH
H
H-Bonding = strongest IMFmuch harder to “pull” molecules apart
C
Dispersion Forces= weakest IMFmuch easier to “pull” molecules apart
C H
H
HH
H
H
HH
Hydrogen bonding: • strongest IMF• influences physical props a great deal
H-F > H-O > H-N
IMF vs Physical PropertiesIf IMF then:
Boiling point Melting point Heat of Fusion Heat of Vaporization
while: Evaporation Rate
Change from solid to liquid w/o changing temp
Change from liquid to gas w/o changing temp
Rate at which conc. will go from liquid to gas
Why do some substances exist as gases, some as liquids, and some as solids at room temp?
#1 reason = IMF
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 tempParticles free to spread
apart
Why do some substances exist as gases, some as liquids, and some as solids at room temp?
#1 reason = IMF
#2 reason = temperature (avg. KE)
Temp = average KEIf we change T we change KEIncrease KE will help “pull” molecules
apart (overcome IMF)
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