Here it says we need to identify the major type of intermolecular force between the particles of each of the following. So first we're going to start out with N2. Since it's just a nitrogen connected to each other, they have the same electronegativity and therefore there be no difference in their electronegativity. So this would represent a nonpolar covalent compound and therefore London dispersion or dispersion forces or Vanderwall's forces would be the answer.
For the next one, we have Chapter 30. Here we have hydrogen directly connected to oxygen, which means that this molecule can do hydrogen bonding with other molecules. So here be hydrogen bonding as its major intermolecular force. For the next one we have Chapter 4 and water. We know that water is a polar solvent and chapter 4 is a hydrocarbon, so it's nonpolar. When you have a nonpolar and a polar, that means that this is dipole induced dipole.
Next we have chapter 3 CL. So here we have carbon in the center connected to three hydrogens and one chlorine. Because the central element is connected to different surrounding elements, it's a polar covalent compound and therefore its intermolecular force would be dipole, dipole. And then finally, here we have potassium chloride and chapter 308 which is methanol. So potassium chloride is an ionic compound since it's connected to a metal and nonmetal. And C3O has hydrogen bonding like we said earlier, which means that it's polar because hydrogen bonding is a polar force.
So remember when you have an ionic compound with a polar substance, then the intermolecular force is ion dipole. So that's what we can say in terms of the intermolecular force for each one of these options. So those would be our final answers.