London Dispersion Forces
What is another name for London Dispersion Forces?
Induced dipole–induced dipole forces.
Give one example of a substance that exhibits dipole–dipole forces.
HCl - Hydrochloric Acid
Which atoms can hydrogen bond with?
Nitrogen (N), Oxygen (O), or Fluorine (F).
Which is stronger: ion–dipole or hydrogen bonding?
Ion–Dipole Forces
What type of molecules exhibit only London Dispersion Forces?
Nonpolar molecules/substances
Between what types of molecules do dipole–dipole forces occur?
Between polar molecules.
Give examples of substances that exhibit hydrogen bonding.
H₂O, NH₃, HF
Give an example of ion–dipole interaction.
Na⁺ ions attracted to the oxygen end of water molecules.
How does molecular size affect London Dispersion Forces?
Larger molecules with more electrons have stronger dispersion forces.
How do dipole–dipole forces compare to London Dispersion Forces in strength?
They are stronger than LDFs.
Why does water (H₂O) have a high boiling point compared to other similar molecules?
Due to the strong hydrogen bonding between water molecules.
Between what types of particles do ion–dipole forces occur?
Between an ion and the partial charge of a polar molecule.
What causes London Dispersion Forces?
Temporary fluctuations in electron distribution that create instantaneous dipoles.
What causes dipole–dipole forces?
Attraction between the positive end of one molecule and the negative end of another.
Why is hydrogen bonding stronger than regular dipole–dipole forces?
Because of the high polarity and small size of hydrogen, leading to strong attraction.
In what situation are ion–dipole forces most common?
When ionic compounds dissolve in polar solvents, like salt in water.
Give one physical property affected by London Dispersion Forces.
Boiling Point
What happens to the strength of dipole–dipole forces when molecular polarity increases?
The forces becomes stronger
What is hydrogen bonding?
A strong dipole–dipole attraction involving hydrogen and highly electronegative atoms.
What is the main difference between ion–dipole and dipole–dipole forces?
Ion–dipole forces involve an ion and a polar molecule, while dipole–dipole forces occur between two polar molecules.