WorksheetsIntermolecular Attractions
Total questions: 10
Worksheet time: 3hrs 30mins
NH3 molecules can form...
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
HF molecules can form...
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
HCl molecules can form...
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
CH4 molecules can form...
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
CH3Cl molecules can form...
London dispersion forces
Dipole-dipole forces
Hydrogen bonds
Which one has the highest boiling point?
CH4
SO2
H2O
Which of the following non-polar molecules has the highest boiling point? (Refer Page 15 - 17 of Intermolecular Forces)
CH4; molar mass = 16.04 g/mol
CCl4; molar mass = 153.82 g/mol
PF5; molar mass = 125.966 g/mol
Rn; molar mass = 222.01758 g/mol
H2O and NH3 are polar molecules that can form the strongest type of intermolecular force (hydrogen bonding). However, the boiling point of H2O is 100.00 °C whereas NH3 is -33.34 °C.
Why is that so? (Refer Page 32 of Intermolecular Forces)
H2O can form more hydrogen bonds than NH3
H2O can form less hydrogen bonds than NH3
O on the H2O is more electronegative than N on the NH3
Between HF and H2O... which one has a higher boiling point? (Refer Page 32 of Intermolecular Forces)
H2O
HF
Factor(s) that influence the strength of London dispersion forces
Molecular size
Molecular shape
Molecular polarity
