A solute is most likely to be highly soluble in a solvent if the solute is _____ and the solvent is ______.

• non-polar, polar

• ionic or polar, non-polar

• non-polar, ionic

• ionic or polar, polar

Based on the following information:

CF₄, Molecular Weight 87.99, Normal Boiling Point -182°C

CCl₄, Molecular Weight 153.8, Normal Boiling Point -123°C

The intermolecular forces of attraction in the above substances is described by which of the following:

• dipole-dipole forces (permanent dipoles)

• ion-dipole forces

• London dispersion forces

• gravitational forces

The boiling point of CH₄ is much lower than that of HF. This is because:

• of dipole-dipole interactions in CH₄

• HF is more polarizable

• CH₄ is polar

• of hydrogen bonding in HF

Why is the normal boiling point of hydrogen fluoride is so much higher than that of hydrogen chloride, the hydride of the next element in group VIIA?

• the HF molecules have a lower dipole moment.

• HCl molecules are non-polar.

• the HF molecules undergoes a higher degree of hydrogen bonding than HCl.

• the electron cloud in the HF molecule is more easily distorted (i.e. is more polarizable) than that of HCl.

What types of intermolecular forces are acting in the following phases of matter?

N_2(g)

• Ion Ion

• Ion Dipole

• Dipole Dipole

• London Dispersion

What types of intermolecular forces are acting in the following phases of matter?

C6H5OH

• Dispersion forces and Dipole Dipole

• Dispersion forces and Hydrogen Bonding

• Hydrogen Bonding and Dipole Dipole

• Dispersion forces

Which substance in each of the following pairs would have the greater intermolecular force?

• CO2

• OCS

Which substance has the greater intermolecular force?

• SeO2

• SO2

Which substance would have the greater intermolecular forces?

• CH3CH2CH2NH2

• H2NCH2CH2NH2

Which substance would have the greater intermolecular force?

• H2CO

• CH3CH3