4.2 INTERMOLECULAR FORCES
C-Cl and C-Br both have dipole dipole forces. However, one of them will exhibit stronger dipole dipole forces than the other. Which one is it and why? a. C-Br because there is a larger electronegativity difference b. C-Br because there is a smaller relative electronegativity difference c. C-Cl because there is a smaller relative electronegativity difference d. C-Cl because there is a larger electronegativity difference
C-Cl because there is a larger electronegativity difference
If CH4 and C2H6 both have only London Dispersion Forces, which one would have stronger attraction and why? C2H6 because it can also form hydrogen bonds C2H6 because it has a higher molar mass CH4 because it would have lower vapor pressure
C2H6 because it has a higher molar mass
If CH4 and C2H6 both have only London Dispersion Forces, why does C2H6 have a higher melting point? C2H6 has less LDFs because of its higher molar mass C2H6 has a stronger LDFs because it has a higher molar mass CH4 has a lower molar mass so it would have stronger intermolecular forces
C2H6 has a stronger LDFs because it has a higher molar mass
Comparing the following molecules, CH4, H2S, and HF, which of the following would have the highest vapor pressure? H2S HF CH4
CH4
Comparing the following molecules, CH4, H2S, and HF, which of the following would have the highest melting point? H2S CH4 HF
HF
Which of the following has the highest vapor pressure/volatility? dipole dipole hydrogen bonding LDFs
LDFs
Which of the following is true of London Dispersion Forces/Van der Waals forces? Choose all that apply + LDFs are the weakest intermolecular force + polar molecules contain LDFs + nonpolar molecules contain LDFs + LDFs are the strongest intermolecular force
LDFs are the weakest intermolecular force polar molecules contain LDFs nonpolar molecules contain LDFs
A substance with a higher molar mass has stronger LDFs True False
True: there are more electrons to move around (more electrons allows a higher chance for a temporary dipole to be formed).
Compare H2O vs. CH3OH. Both have hydrogen bonds. Which substance has stronger intermolecular forces and why? a. CH3OH has stronger intermolecular forces because it can create more hydrogen bonds b. H2O has stronger intermolecular forces because it has a lower molar mass c. H2O has stronger intermolecular forces because it can create more Hydrogen bonds d. CH3OH has stronger intermolecular forces because it can create less hydrogen bonds
c. H2O has stronger intermolecular forces because it can create more Hydrogen bonds
intermolecular force
forces of attraction between multiple molecules
intramolecular force
forces of attraction within just one molecule
Which of the following has the highest melting point/boiling points? a. dipole dipole b. hydrogen bonding c. LDFs
hydrogen bonding
What type of molecules form hydrogen bonds? a. all polar molecules b. only polar molecules with O-H, F-H, or N-H bonds c. nonpolar molecules
only polar molecules with O-H, F-H, or N-H bonds