A. IMFs and States of Matter (Section 12.1)
1. At a given temperature, the magnitude of intermolecular forces (IMFs) determines the phase of matter:
a. If the IMFs are too weak to hold the particles together, the substance is a gas. b. If the IMFs are strong enough to hold the particles together, the substance will be a liquid or solid.
Referred to collectively as the
2. There are three IMFs we consider in pure substances:
a.
Present in all compounds.
b.
Present only in polar molecules.
c.
Present only when H is bonded directly to
B.
Review of Lewis Structures, VSEPR, and Polarity
1. To draw a Lewis Structure:
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a. Determine the total number of valence electrons in the molecule.
b. Determine the central atom; place outer atoms around central atom.
c. Draw a single bond between the central and outer atoms.
d. Place remaining electrons, in pairs, around the outer atoms until their octet is satisfied.
Start with highest EN element first.
e. Any remaining electrons go on the central atom.
f.
Check to make sure all atoms have their octets.
If the central atom does not have an octet, use multiple bonds.
2. VSEPR Review
# edomains
# nonbonding domains EDG
MG
Bond
Angles
Hybridization
2
0
Linear
Linear
180°
sp
3
0
Trigonal Planar
Trigonal Planar
120°
sp2
3
1
Trigonal Planar
Bent
<120°
sp2
4
0
Tetrahedral
Tetrahedral
109.5°
sp3
4
1
Tetrahedral
Trigonal
Pyramidal
<109.5°
sp3
4
2
Tetrahedral
Bent
<109.5°
sp3
2
# e- domains
# nonbonding domains EDG
MG
Bond
Angles
Hybridization
5
0
Trigonal
Bipyramidal
Trigonal
Bipyramidal
120°, 90°
sp3d
5
1
Trigonal
Bipyramidal
See-Saw
5
2
Trigonal
Bipyramidal
T-Shape
5
3
Trigonal
Bipyramidal
Linear
6
0
Octahedral
Octahedral
90°
sp3d2
6
1
Octahedral
Square
Pyramidal
6
2
Octahedral
Square Planar
3. Molecules can be either polar or nonpolar:
a.
Polar (dipole):
A polar molecule must have at least one polar bond!
b.
Nonpolar (no dipole):
Molecule with polar bonds can still be nonpolar!
c.
Determine if the center of positive & negative charge are in the same place. Make sure to take the account! into
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C.
Properties of Liquids (Section 12.2)
1. Surface Tension-
a.
Forces that must be overcome to increase the surface area of a liquid.
b.
Due to an unequal pulling of the molecules at the surface of the liquid.
c.
As IMFs increase, surface tension
d.
The attraction of a substance to itself is known as
All forces holding liquid together.
e.
The attraction of a substance to another substance is known as
Forces attracting a liquid to another surface.
2. Capillary Action
a.
For a liquid in a vessel, the relative magnitudes of cohesion and adhesion to the vessel affect its behavior:
If the magnitude of adhesion is greater than cohesion, the liquid is drawn up the walls, forming a meniscus. o This is the basis of capillary action.
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If the magnitude of cohesion is greater than adhesion, the liquid is drawn toward itself, forming a meniscus. b.
Capillary action occurs when a liquid creeps up or down a capillary tube (caused by adhesion between liquid and the glass) until gravity forces eventually stop it.
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3. Viscositya.
As IMFs increase, viscosity.
Viscosity low when molecules can easily slide past one another (weak intermolecular forces). o Oil has
b.
viscosity, gasoline
.
Measured by
, which measures flow time through a capillary tube required for a specific volume of liquid.
Society of Automotive Engineers (SAE) developed viscosity scale for automobile oil. o Higher number oils have higher viscosities.
SAE 40 Oil
SAE 10 Oil
4. Vapor Pressure
a.
Often, molecules in a liquid will have enough energy to vaporize spontaneously. 6
Vaporization o Molecules of liquid have distribution of
o As T increases fraction of molecules with sufficient KE increases, and evaporation rate increases. o Since only high energy molecules are escaping,