Score _____ / 10 pts.
Name _____________________________
Class _____ Date ____________________
8.3 Intermolecular Forces
Forces of Attraction within the Structure
1. Draw a model to represent ionic bonding.
2. State some physical properties associated with ionic crystalline structures.
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Do conduct electricity in solution
Highly ordered
Dissolve in water
High boiling & melting points
Solid at room temperature
3. Draw a model to represent covalent bonding.
4. State some physical properties associated with covalent molecules.
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Do not conduct electricity
Soluable in nonpolar substances
Low boiling/melting points
Gas, solid, liquid at room temperature
5. Draw a model to represent metallic bonding.
6. State some physical properties associated with metallic structures or alloys.
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Malleable
Can be pounded into sheets
Ductile (meaning it can be drawn into wires)
Conducts electricity
Intermolecular Forces: Dispersion, Dipole-Dipole, and Hydrogen Bonds
1.
Explain how dispersion forces form and draw a picture.
a.
What type of particles exhibit dispersion forces?
All molecules exhibit dispersion forces
b.
How is the strength of dispersion forces related to mass?
The strength of the dispersion forces is directly proportionate to the mass of the
atoms.
Bigger atoms= Stronger dispersion forces
2.
Describe dipole-dipole attractions and draw a picture to represent how they work?
a.
What type of particles exhibit dipole-dipole attractions?
Polar molecules exhibit dipole-dipole interactions.
b.
What determines the strength of dipole-dipole attractions?
The strength of the polarity is directly proportionate to the strength of the
dipole-dipole attraction.
Stronger polarity= Stronger dipole-dipole attraction
3.
What is hydrogen bonding? Draw a diagram that represents how it works.
a.
What type of particles would engage in hydrogen bonding?
Hydrogen bonding occurs between the lone pairs of Nitrogen, Oxygen, and
Fluorine.
N, O, F
b.
How does hydrogen bonding compare to other forms of intermolecular attractions?
Hydrogen bonding is the strongest form of intermolecular attractions.
c.
4.
How do ions interact with dispersion forces?
a.
5.
Which of the following molecules could form hydrogen bonds? (H 2, H2S, HCl, HF)
How do ions interact with dipole-dipole forces?
Draw a flow chart that summarizes types of intermolecular forces and their characteristics.
6.
Put the following compounds in order from weakest attractions to strongest.
KI, H2O, CCl4, KBr, SF4, CsBr, NH3, Cl2, CaO
7.
What characteristic intermolecular forces would result in a substance taking on the gas phase?
In the gas phases, molecules have weak intermolecular forces—they are not highly attracted to each other, and
thus remain in the gas phase.
8.
What characteristic intermolecular forces would lead to a substance taking on the liquid phase?
In the liquid phase, intermolecular forces are much greater than gases, but are weaker than solids. They are more
tightly compact and attracted to each other.
a.
How would intermolecular forces affect viscosity and surface tension of the liquid?
Viscosity: a measure of the resistance to flow. High viscosity= the liquid doesn’t flow well
Liquids have HIGH VISCOSITY if: LARGE molecules, LOW temperatures, and High Intermolecular Forces (more
attracted to their own particles).
Surface Tension: measure of the inward pull by particles in the interior—OR—particles try to minimize surface area
by being tightly attracted to each other.
9.
What characteristic intermolecular forces would lead to a substance taking on a solid phase?
Substances in the solid phase have high intermolecular foces.