The intermolecular forces possible between molecules of propane are ... Question 4Select one:a.Hydrogen Bonding onlyb.London Dispersion Forces and Covalent Bondingc.London Dispersion Forces onlyd.London Dispersion Forces, Dipole - Dipole attraction and Hydrogen Bonding

The correct answer is c. London Dispersion Forces only.

Here's why:

Propane is a nonpolar molecule. Nonpolar molecules do not have positive and negative ends, and therefore, cannot have dipole-dipole attractions or hydrogen bonding.

1. Hydrogen Bonding: This type of intermolecular force occurs when a hydrogen atom bonded to a strongly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons. Propane does not have this type of bonding because it does not contain a hydrogen atom bonded to a strongly electronegative atom.

2. Dipole-Dipole attraction: This type of intermolecular force occurs between the positive end of one polar molecule and the negative end of another polar molecule. Propane cannot have this type of attraction because it is a nonpolar molecule.

3. London Dispersion Forces: These are the weakest intermolecular force and occur between all molecules, whether they are polar or nonpolar. These forces arise due to the temporary random movement of electrons in a molecule which creates a temporary dipole. Other molecules nearby are affected by this temporary polarity, causing attractions between molecules.

4. Covalent Bonding: This is not an intermolecular force, but an intramolecular force, meaning it occurs within a molecule, not between molecules. Propane does have covalent bonds within its molecule, but this is not relevant to the question.

So, the only intermolecular force possible between molecules of propane is London Dispersion Forces.