Multiple Select QuestionSelect all that applySelect all the compounds that have dipole-dipole interactions.Multiple select question.C2H6CHCl3CH3OCH3CH3FCH4

Dipole-dipole interactions occur between molecules that have permanent net dipoles. This means that one end of the molecule carries a slight positive charge and the other end carries a slight negative charge.

1. C2H6: This is an example of a nonpolar molecule. The electronegativity difference between carbon and hydrogen is very small, so there are no polar bonds in this molecule. Therefore, it does not have dipole-dipole interactions.

2. CHCl3: This molecule is polar because the electronegativity difference between carbon and chlorine is large, creating a polar bond. Therefore, it has dipole-dipole interactions.

3. CH3OCH3: This molecule is also polar. The oxygen atom is more electronegative than the carbon and hydrogen atoms, creating polar bonds and a net dipole. Therefore, it has dipole-dipole interactions.

4. CH3F: This molecule is polar because the electronegativity difference between carbon and fluorine is large, creating a polar bond. Therefore, it has dipole-dipole interactions.

5. CH4: This is a nonpolar molecule. The electronegativity difference between carbon and hydrogen is very small, so there are no polar bonds in this molecule. Therefore, it does not have dipole-dipole interactions.

So, the compounds that have dipole-dipole interactions are CHCl3, CH3OCH3, and CH3F.