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Intermolecular Forces
Chemistry: Intermolecular Forces
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Chemistry
Intermolecular Forces
Chapter 10
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32 Terms
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1
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interactions within a molecule
intramolecular forces
2
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attractions between molecules and/or ions
- electrostatic
- weaker than intramolecular
- influence physical properties
intermolecular forces
3
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separation of charge in an atom/molecule momentary uneven e- distribution
induced dipoles
4
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intermolecular force between nonpolar molecules caused by presence of temporary dipoles in molecules
London dispersion forces (LDF)
5
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increases strength when surface area, polarizability, or e- # increases
experienced by all atoms to some degree
LDF characteristics
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relative ease of which an e- cloud can be distorted
polarizability
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- way of interaction with other atoms
- over greater distances
induced dipole characteristic
8
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between an ion and a molecule that has permanent dipole moment
ion dipole interaction
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cluster of water molecules surrounding an ion in aqueous solution
sphere of hydration
10
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between polar molecules (permanent dipoles)
dipole dipole interaction
11
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between a polar molecule and opposite charge of induced dipole of another molecule
dipole induced dipole interaction
12
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between hydrogen atom bonded to small, highly electronegative element (O, N, F)
hydrogen bond
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strongest
ion-dipole
hydrogen bond
dipole-dipole
dipole-induced dipole
LDF
weakest
order of intermolecular forces strength
14
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organic compound with general formula R-O-R'
ethers
15
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"water fearing"
- repulsive interaction between solute and water
- non polar molecule
hydrophobic
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"water loving"
- attractive interaction between solute and water
- polar molecule
hydrophilic
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solubility down
temp up
pressure down
solubility of O2 in H2O
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principle that concentration of sparingly soluble, unreactive gas in liquid is proportional to partial pressure of gas
Henry's law
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Cgas = KH Pgas
Henry's law equation
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1) temperature - T up VP up
2) surface area - SA up VP up
3) intermolecular forces - IMF up VP down
rate of vapor pressure factors
21
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pressure exerted by a gas at a given temp in equilibrium with its liquid phase
vapor pressure
22
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temperature at which the vapor pressure of a liquid equals 1 atm
normal boiling point
23
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a relationship between the vapor pressure of a substance at two temps
Clausius-Clapeyron equation
24
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graphical representation of how stabilities of physical states of a substance depend on temperature and pressure
phase diagram
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temperature and pressure at which all three phases coexist
triple point
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specific temperature and pressure at which liquid and gas phases have same density and are indistinguishable
critical point
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hydrogen bonds
cause of unique characteristics of water
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energy needed to separate molecules at surface of liquid
surface tension
29
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concave/convex surface of a liquid in a tube with a small diameter
meniscus
30
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cohesive
- hydrogen bonds between molecules
adhesive
- liquid against glass
two forces of surface tension
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rise of a liquid in a narrow tube as a result of adhesive forces within liquid
capillary action
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resistance to flow of a liquid
- nonpolar - molar mass up viscosity up
- polar - LDF and dipole
viscosity
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