Complete the quiz using ONLY a calculator and your Reference Tables.
London Dispersion Forces
Ion-Dipole Forces
Dipole-Dipole Forces
Hydrogen Bonds
London Dispersion Forces
Ion-Dipole Forces
Dipole-Dipole Forces
Hydrogen Bonds
London Dispersion Forces
Ion-Dipole Forces
Dipole-Dipole Forces
Hydrogen Bonds
London Dispersion Forces
Ion-Dipole Forces
Dipole-Dipole Forces
Hydrogen Bonds
The partial negative end must be touching the Br^- ion, since like charges between partial negative end (O) in water and the negative ion attract.
The partial negative end must be touching the Br^- ion, since opposite charges between partial positive end (O) in water and the negative ion attract.
The partial positive end must be touching the Br^- ion, since opposite charges between partial positive end (H) in water and the negative ion attract.
None of the above
NH3 has a higher boiling point, because it contains London forces.
NH3 has a higher boiling point, because it contains hydrogen bonds.
NH3 has a higher boiling point, because it contains dipole-dipole forces.
NH3 has a higher boiling point, because it contains ion-dipole forces.
HF has a higher boiling point, because it contains London forces.
HF has a higher boiling point, because it contains hydrogen bonds.
HF has a higher boiling point, because it contains dipole-dipole forces.
HF has a higher boiling point, because it contains ion-dipole forces.
The solution of CuO has a higher boiling point than water does.
Water has a higher boiling point than the CuO solution does.
Dipole-Dipole Forces
Hydrogen Bonding
Ion-Dipole Forces
London Dispersion Forces
NaF (aq) < H2S < HF < CF4
H2S < CO2 < HF < NaF (aq)
CO2 < H2S < HF < NaF (aq)
CO2 < HF < H2S < NaF (aq)
CF4 < CH3OH < CH3Cl < Na2O (aq)
CF4 < CH3Cl < CH3OH < Na2O (aq)
CF4 < Na2O (aq) < CH3Cl < CH3OH
CF4 < Na2O (aq) < CH3OH < CH3Cl
Sulfur
Tellurium
Selenium
Oxygen
Substance A
Substance B
Substance C
Substance D
NH3 and HF have higher boiling points, because they contain London Forces.
NH3 and HF have higher boiling points, because they contain hydrogen bonds.
NH3 and HF have higher boiling points, because they contain dipole-dipole forces.
NH3 and HF have higher boiling points, because they contain ion-dipole forces.
H2Se and CO have higher boiling points, because they contain London Forces.
H2Se and CO have higher boiling points, because they contain hydrogen bonds.
H2Se and CO have higher boiling points, because they contain dipole-dipole forces.
H2Se and CO have higher boiling points, because they contain ion-dipole forces.
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