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States of Matter
Chapter 13
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Matter
Let’s get to the heart of it…
The particles are in constant motion
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Kinetic-Molecular Theory Describes the motion of individual
molecules Kinetic = “to move” Also called Kinetic Theory
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Forces of Attraction Affect on States of Matter
At room temperature (20oC-25oC, 68oF-77oF) all particles of matter have the same kinetic energy
So why do we have different states of matter for these materials?
There are different strengths of INTERMOLECULAR FORCES
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13.2 Forces of Attraction
Intermolecular ForcesWhat holds molecules together
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Intermolecular Forces
They are what make solid and liquid molecular compounds possible.
The weakest are called van der Waal’s forces - there are two kinds Dispersion forces (London forces) Dipole Interactions
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Dispersion Force
Depends only on the number of electrons in the molecule
Bigger molecules more electrons More electrons stronger forces
F2 is a gas
Br2 is a liquid
I2 is a solid
All are nonpolar but why are they different states of matter?
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Dispersion force
H H H HH H H H
+ -
H H H H
+ - +
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Dispersion Force Occurs between all molecules
Depends only on the number of electrons in the molecule
Result from a temporary shift in density of electrons in electron clouds
Causes nonpolar molecule to become polar
Happens quickly and temporarily for nonpolar molecules
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Dipole interactions
Occur when polar molecules are attracted to each other.
Slightly stronger than dispersion forces.
Opposites attract but not completely hooked like in ionic solids.
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Dipole interactions
Occur when polar molecules are attracted to each other.
Slightly stronger than dispersion forces.
Opposites attract but not completely hooked like in ionic solids.
H F
H F
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Hydrogen bonding
Are the attractive force caused by hydrogen bonded to F, O, or N.
F, O, and N are very electronegative so it is a very strong dipole.
Causes hydrogen to have a large partial positive charge on it
The molecules are small, so they can get close together
The hydrogen partially share with the lone pair of electrons on an atom in a neighboring molecule
The strongest of the intermolecular forces.
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Hydrogen Bonding
HH
O+ -
+
H HO+-
+
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Hydrogen bonding
HH
O H HO
HH
O
H
H
OH
HO
H
HO HH
O
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Hydrogen bonding is the reason why water has unique properties compared to other molecules its same size
Properties: It is a liquid at room temp. It is a good solvent It is less dense as a solid (ice floats)
Just remember Water is not the only molecule that has hydrogen bonds.
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Examples:
What type of intermolecular forces do the following molecules have? NH3
O2
CO2
HBr Which of the following compounds
can form dipole-dipole forces: Cl2, CO, NO, CH4
Hydrogen bonding
Dispersion forces
Dispersion forces
Dipole-dipole forces
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13.4 Phase Changes
What is a phase? The distinct states of matter when they
are in mixtures How is this different from just states
of matter?
Occur due to changes in temperature.
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Phase changes that need energy
Melting
Heat of Fusion
Melting Point
KMT?
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Vaporization
Heat of Vaporization
How is this different from evaporation?
KMT?
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Boiling Point
Normal Boiling Point
KMT?
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Sublimation – Dry Ice Ice in the Freezer
KMT?
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Phase Changes that Release Energy
Condensation
What is this the reverse of?
KMT?
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Freezing
Freezing Point
How do the melting point & freezing points of a substance compare?
KMT?
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Deposition
What is this the reverse of?
KMT?
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Heating Curve
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Vapor Pressure Graphs
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Phase Diagram
For Water
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Phase Diagram
For CO2
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Video lesson Water, a polar molecule, on YouTube:
http://www.youtube.com/watch?v=DVCYlST6mYQ
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ReviewIonic and Covalent Compounds
Practice Quiz and Graphics: http://www.elmhurst.edu/~chm/vchembook/145Areview.html
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Internet resources Molecular polarity:
http://www.elmhurst.edu/~chm/vchembook/210polarity.html
Polar covalent compounds: http://www.elmhurst.edu/~chm/vchembook/152Apolar.html
Nonpolar covalent compounds: http://www.elmhurst.edu/~chm/vchembook/150Anpcovalent.html
Ionic compounds: http://www.elmhurst.edu/~chm/vchembook/143Aioniccpds.html
Compare Ionic, Polar, and Nonpolar Bonds: http://www.elmhurst.edu/~chm/vchembook/153Acompare.html
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Properties of Molecules
Most have LOW melting & boiling points
tend to be gases and liquids at room temperature
Ex: CO2, NH3, H2O
Polar and Nonpolar molecules have a little bit different properties due to the partial charges.
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H - F+ -
H - F
+-H -
F+-
H -
F
+-
H - F +-
H - F+-
H - F
+-
H - F
+-
+-
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Properties of Solid Molecules
Two kinds of crystals: Molecular solids – molecules held together
by attractive forces Ex: BI3, Dry Ice, sugar
Network solids- atoms held together by bonds
One big molecule (diamond, graphite) High melting & boiling points, brittle, extremely hard
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Graphite Diamond