Module 2 Chapter 5 Lesson 4 - Intermolecular Forces
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What are the three types of intermolecular forces?
Hydrogen bonds Permanent Dipole-Dipole London Dispersion Forces (AKA Induced dipole-dipole)
What is the strongest relative intermolecular force?
Hydrogen bonds
When does hydrogen bonding occur?
Between hydrogen and N/O/F
What is a feature of hydrogen bonding?
Very electronegative
What is the medium strength relative intermolecular force?
Permanent dipole-dipole interactions
Where are permanent dipole-dipole interactions present?
Polar molecules
Define permanent dipole-dipole interactions.
Permanent partial charges attracting each other.
What is the weakest relative intermolecular force?
London Dispersion Forces (Induced dipole-dipole forces)
What influences the strength of London Dispersion Forces?
Number of electrons
Where are LDF present?
All molecules
What happens when a combination of ethanol and water is left overnight?
Hydrogen bonding increases. So the atoms are closer together. Causing the volume to decrease.
What are the steps to find out if a molecule is polar or not?
Dot and Cross 3D structure Identify lone pairs Identify difference in dipoles Identify bonding pairs.
What are eight features to find out if a molecule is polar or not?
Lone Pairs = Polar Difference in dipoles = Polar Different bonding pairs = Polar Dipoles don’t cancel out = Polar Non - Symmetrical = Polar Dipoles cancel out = Non - Polar Same bonding pairs = Non - Polar Symmetrical = Non - Polar
What are the rules for drawing hydrogen bonding diagrams?
Dipoles Dashed line for forces between molecules Straight line for intramolecular forces
What does electrons oscillating randomly cause?
Electrons oscillate and randomly move. Uneven distribution of charge. Creates instantaneous dipole. Induces dipole in neighbouring molecules.
What has stronger LDF forces Cl-Cl or Br-Br and why?
Br-Br Larger/Higher molecular mass More electrons High uneven distribution of electrons Higher LDF.