Worksheetsvan der Waals forces
Total questions: 15
Worksheet time: 10mins
Which is the correct description about van der Waals' forces?
They are the weakest of the intermolecular forces arising from instantaneous dipole - induced dipole interactions.
They are the strongest of the intermolecular forces arising from dipole - dipole interactions.
Name the type of van der Waals forces exist in I2
London dispersion forces
Dipole-dipole forces
Name the type of van der Waals forces exist in SO2
London dispersion forces
Dipole-dipole forces
Name the type of van der Waals forces exist in CH4
London dispersion forces
Dipole-dipole forces
Which of the following molecules can form London dispersion forces between its molecules?
Sulphur tetrafluoride, SF4
Tetrachloromethane, CCl4
Water, H₂O
Ammonia, NH3
Which of the following compounds can form dipole-dipole forces between its molecule?
CH₄
SF₄
BCl₃
PCl₅
All molecules feel this kind of intermolecular forces
Hydrogen bonding
Dipole-dipole forces
London dispersion forces
Only polar molecules feel this kind of intermolecular forces
Hydrogen bonding
Dipole-dipole forces
London dispersion forces
Only polar molecules with H-F, H-N, or H-O bonds feel this kind of Intermolecular forces
Hydrogen Bonding
Dipole-dipole forces
London dispersion forces
Which type of intermolecular force is the strongest?
Hydrogen bonding
Dipole-dipole forces
London dispersion forces
What is the strongest kind of intermolecular forces that occurs between molecules of NH3?
Hydrogen bonding
Dipole-Dipole forces
London dispersion forces
The boiling point of bromine and chlorine are 58.8 ⁰C and -35 ⁰C respectively. Why?
Bromine is more polar than chlorine.
Bromine has stronger London dispersion forces since its molar mass is greater than chlorine.
Chlorine has stronger London dispersion forces since its molar mass is smaller than bromine.
Bromine is located at a lower period than chlorine.
Why is the boiling point of methane greater than that of neon?
A molecule of methane has a greater mass than a molecule of neon
A molecule of methane has more electrons than a molecule of neon
Molecules of methane have stronger intermolecular forces than those of neon
Molecules of methane from hydrogen bonds, but those of neon do not
The molecule of methane is polar, but that of neon is not
The boiling points of water and ammonia are 373 K and 240 K respectively. The boiling point of water is higher than that of ammonia because
oxygen is less electronegative than nitrogen
the O-H bond in H2O is stronger than the N-H bond in NH3
the hydrogen bonds between water molecules are stronger than the hydrogen bonds between ammonia molecules
a water molecule has a larger size than an ammonia molecule
The boiling point of butanone (CH3CH2COCH3) is higher than that of pentane (CH3CH2CH2CH2CH3) because
the temporary dipole-induced dipole attractions in butanone are stronger than in pentane
the covalent bonds in butanone are stronger than the covalent bonds in pentane
butanone forms intermolecular hydrogen bonds but pentane does not
butanone is polar but pentane is non-polar
