Dipole-dipole interactions are the strongest intermolecular force of attraction.

Because methane is a non-polar molecule it is not capable of hydrogen bonding or dipole-dipole intermolecular forces. There are no bond dipoles and no dipole-dipole interactions. Even if the molecule had polar C-H bonds, the symmetry of molecule would cause the bond dipoles to cancel.

The only intermolecular forces in methane are London dispersion forces.

In order from strongest to weakest, the intermolecular forces given in the answer choices are: ion-dipole, hydrogen bonding, dipole-dipole, and Van der Waals forces.

Dipole-Dipole interaction is an intermolecular force that acts between molecules, so it is inherently much weaker than the intramolecular bonds such as ionic, covalent or metallic- so in this context it is weak. Yes, it is a weak interaction but it is not the weakest interaction.

As a result, it is more difficult to deform the surface of water than the surface of ethyl alcohol. Therefore, since water molecules on a liquid surface are harder to push down on the surface tension is higher for water than for ethyl alcohol.

Hydrogen Bonds

dispersion forces

The strongest of those listed s hydrogen bonding. This type of intermolecular force is the attraction that occurs between hydrogen atoms and the lone pairs on atoms of oxygen, nitrogen and/or fluorine. Hydrogen bonds are the strongest while dispersion forces are the weakest.

This type of intermolecular force is called a dipole-dipole interaction or dipole-dipole attraction since it occurs in polar molecules with dipoles. Remember that oxygen is more electronegative than carbon so the carbon-oxygen bonds in this molecule are polar bonds.

The only intermolecular forces existing between oxygen molecules (O2) are: London dispersion.

London Dispersion Forces: These are called London dispersion forces and they are the weakest intermolecular force as the dipoles are only temporary.

Hydrogen bonding of water molecules The plus end of one—a hydrogen atom—associates with the minus end of another—an oxygen atom. These attractions are an example of hydrogen bonds, weak interactions that form between a hydrogen with a partial positive charge and a more electronegative atom, such as oxygen.

O2 … O=O … is not polar, but it can be the recipient of several intermolecular attractions: hydrogen bonding, Debye forces and London dispersion forces. Dissolved O2 can be a hydrogen bond acceptor. There are also Debye forces involved in the attraction between water and dissolved oxygen.

Actually, gravity is the weakest of the four fundamental forces. Ordered from strongest to weakest, the forces are 1) the strong nuclear force, 2) the electromagnetic force, 3) the weak nuclear force, and 4) gravity.

Two inter molecular forces that are active between two molecules of CHCl3 are Dipole Dipole, because it is a polar molecule, and London dispersion, because all molecules use them. CHCl3 does not use Hydrogen bonding because it does no contain the atoms N, O, or F for the Hydrogen to bond to.

The answer is indeed C, because oxygen liquid is the only one of these molecules held together by weak London/van der Waals forces.