Identify the intermolecular forces present in both a solute and solvent and predict whether a solution will form between the two. So here we have 50 grams of arsenic pentachloride placed into 250 grams of water. All right, so first of all, we know that water is our solvent since it's larger in a mouth. Water we know as a polar solvent because it possesses hydrogen bonding. So we're going to say H bonding.
Now arsenic pentachloride, it's not as obvious what kind of intermolecular force it has, so we're going to draw it out. Arsenic is in Group 5A, so it has five valence electrons and we're going to say here that the chlorines are in Group 7A, so they have 7 valence electrons. And remember, halogens, when they're not in the center, only make single bonds. So each one of these chlorines will single bond to the arsenic and in that way we'll have our molecular shape for arsenic pentachloride.
If we take a look here, we're going to know that this is one of our perfect shapes that we've talked about in our earlier topics dealing with molecular polarity. Because it is a perfect shape. It has the same surrounding elements, it has no lone pairs. It's one of the perfect shapes. It is non polar in nature. So we're going to say here that arsenic pentachloride is nonpolar and therefore it's intermolecular force would be London dispersion forces or Vander Waals forces.
Now London dispersion is a non polar force, hydrogen bonding is a polar force. Their polarities don't match and as a result we cannot form a solution with them. So we've classified with their intermolecular forces are and we've classified their polarity as a result and from that we know that no, a solution will not form between the two.