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CH 12: Intermolecular Forces and Liquids and Solids
I. States of Mattera) Kinetic Energy vs. Attractive Forces
II. Intermolecular Forces (Attractive, van der Waal Forces)a) Dipole-Dipole--- (Polar Molecules)
i. Hydrogen Bonding
b) Dispersion (London) Forces--- (NonPolar Molecules)
c) Attractive Forces Involving Ions
Intermolecular Forces and Liquids and Solids
III. Properties of Liquidsa) Viscosityb) Meniscus Formationc) Surface Tensiond) Capillary Action
IV. Phase Changesa) Equilibrium Vapor Pressure
i. Normal boiling point
b) Phase Diagrams
Intermolecular Forces and Liquids and Solids
V. Crystalline Structure of Solidsa) Unit Cells (Simple Cubic, BCC, FCC)
i. Coordination Number
ii. # Lattice Points in a Unit Cell
VI. Radius vs. Unit Cell Edge Length,aa) Density
VII. Types of Crystalline Solidsa) Ionic, Molecular, Covalent, and Metallic
Factors in Determining State of Matter
I. Kinetic Energy
II. Intermolecular Forces; Attractive Forces between different molecules• neglible in gases
• important in solids, liquids
Intermolecular Forces
11.2
Interermolecular forces; attractive forces between diff. Moleculeswhich bring the molecules in contac with eac other
Intraramolecular forces hold atoms together in a molecule.
Intermolecular vs Intramolecular
• 41 kJ to vaporize 1 mole of water (inter)
• 930 kJ to break all O-H bonds in 1 mole of water (intra)
Generally, intermolecular forces are much weaker than intramolecular forces.
“Measure” of intermolecular force
boiling point
melting point
Hvap
Hfus
Hsub
Types of Intermolecular Forces
1. Dipole/ Dipole Forces (Polar Molecules)
• Hydrogen Bonds
2. London/ Dispersion Forces (NonPolar Molecules)
Intermolecular Forces
I. Dipole-Dipole Forces
Attractive forces between polar molecules
Orientation of Polar Molecules in a Solid
11.2
Intermolecular Forces
II. Dispersion Forces
Attractive forces that arise as a result of temporary dipoles induced in atoms or nonpolar molecules
11.2
Polarizability
• Ease at which the electron distribution in an atom or molecule can be distorted and a temporary dipole induced
– More electrons (greater Molar Mass) leads to greater polarizability.
Formation of Temporary Dipoles
1. Random movement of electrons
2. ion-induced dipole interaction
3. dipole-induced dipole interaction
SO
O
What type(s) of intermolecular forces exist between each of the following molecules?
HBrHBr is a polar molecule: dipole-dipole forces. There are also dispersion forces between HBr molecules.
CH4
CH4 is nonpolar: dispersion forces.
SO2
SO2 is a polar molecule: dipole-dipole forces. There are also dispersion forces between SO2 molecules.
11.2
Boiling Point- Temperature at which there is enough Kinetic Energy to Overcome Intermolecular Forces
Liquid
Has Intermolecular Forces
Gas
No Intermolecular Forces
Boiling Point Increases with..
1. Stronger Intermolecular Force
2. If same Intermolecular Force;• increasing Molar Mass, higher boiling point
Explain why the Higher Molar Mass Compound, CF4, has a Lower
Boiling Point than H2Se
CF4
• Boiling Point; -150.0°C• Molar Mass ~ 88 g/mole
H2Se• Boiling Point; -42.0 °C• Molar Mass ~ 81 g/mole
Intermolecular Force; Dispersion Force
Intermolecular Force; Dipole-Dipole Force
Boiling Points of Polar Hydrogen Compounds
Approximate Molar Mass;
g/mole
Boiling Point;
°C
H2O 18 + 100
H2S 34 -60
H2Se 81 -42
H2Te 130 -2
Hydrogen Bond
• Strong Type of Dipole-Dipole Force. This Type of Intermolecular Force Happens When H is directly bonded to O, N, or F.
High Strength of H- bond
1. Large electronegativity difference between H and N, O, or F.
2. Small size of H atom allows it to get close to another molecule
Which of the Two Polar Molecules Has a Higher Boiling Point ?
diethyl ether
C
H
H
H O C
H
H
H
C
H
H
H C
H
H
O H
ethanol
Importance of H-Bonds in H2O
1. Very high boiling point for water (H2O(l)) for its Molar Mass.
2. The solid form of the material is less dense than liquid form
• Ice Floats on liquid water.• Water expands as it freezes
Importance of H-Bonds in H2O
1. Very high boiling point for water (H2O(l)) for its Molar Mass.
2. Ice floats on liquid water. • The solid form of the material is less dense
than liquid form• Water expands as it freezes
3. High specific heat of Water