Intermolecular Forces Flashcards
What are the three types of intermolecular forces?
Dipole-dipole, hydrogen bonding, and London dispersion forces.
How do intermolecular forces affect boiling points?
Stronger intermolecular forces lead to higher boiling points.
Why do larger molecules generally have higher boiling points?
They have more electrons, leading to stronger London dispersion forces.
Why do Cl2 and C4H10 have similar boiling points?
Both rely on London dispersion forces, which depend on molecular size.
Which has a lower boiling point: C2H6 or CH3F?
C2H6, because CH3F has dipole-dipole interactions in addition to London forces.
Why does Br2 have a higher boiling point than C3H8?
Br2 is larger, leading to stronger London dispersion forces.
Does C2H5F have a higher or lower boiling point than ethanol (C2H5OH)?
Lower, because ethanol has hydrogen bonding.
How do hydrogen bonds compare to covalent bonds in strength?
Hydrogen bonds are much weaker than covalent bonds but stronger than other intermolecular forces.
What property of water is a result of hydrogen bonding?
High surface tension.
