Based upon the intermolecular forces present, rank the following substances according to the expected boiling point for the substance: MgF2, H2O, HCl, N2

I would rank from low to high as

N2, HCl, H2O, MgF2 but you should confirm that. Look on Google and check the boiling points.

Well, let's see here. MgF2, H2O, HCl, and N2 walk into a bar. The bartender takes one look at them and says, "Hey, I heard you guys are competing in a boiling point contest. So, let me tell you who's going to win."

MgF2, being an ionic compound, has strong ionic bonds. It's like a high school couple who can't keep their hands off each other, always attracted with a force so strong it's hot! So, MgF2 takes the lead, like a teenage love affair, with the highest boiling point.

Next up we have H2O, also known as water. It may not have the sizzling passion of MgF2, but its hydrogen bonds make it a solid contender. Those tiny H-bonds are like tiny little magnets that love to hold hands and stick together, creating a strong attraction. So, H2O is the second in line for the boiling point contest.

Then we have HCl, which is a polar covalent compound. Picture it like two friends, one with a slight positive charge (H) and the other with a slight negative charge (Cl). They're not as strong a bond as MgF2 or H2O, but they're still pretty tight. So, HCl takes the third position.

Finally, we have N2, which is made up of two nitrogen atoms that are not very attracted to each other. They're like two strangers at a party who just happen to be standing next to each other. They don't really care about being close, so their boiling point is the lowest.

So, if we rank these substances according to their expected boiling points, it would go like this: MgF2 -> H2O -> HCl -> N2.

To rank the substances according to their expected boiling points based on intermolecular forces, we need to consider the strength of the intermolecular forces present in each substance. Generally, the stronger the intermolecular forces, the higher the boiling point. Here is the ranking of the substances from highest to lowest boiling point:

1. H2O (water): Water exhibits hydrogen bonding, which is the strongest intermolecular force among the substances listed. Hydrogen bonding results from the attraction between the hydrogen atom of one water molecule and the oxygen atom of another water molecule. Due to the strong hydrogen bonding, water has a higher boiling point.

2. HCl (hydrogen chloride): HCl exhibits dipole-dipole forces. These forces occur between the positive end of one molecule (hydrogen in HCl) and the negative end of another molecule (chlorine in HCl). While dipole-dipole forces are weaker than hydrogen bonding, they are stronger than the forces present in the remaining substances.

3. MgF2 (magnesium fluoride): MgF2 exhibits ionic bonding between magnesium and fluoride ions. Ionic bonds are relatively strong, but they are not as strong as dipole-dipole forces or hydrogen bonding. Therefore, MgF2 has a lower boiling point compared to HCl and H2O.

4. N2 (nitrogen): N2 is a diatomic molecule that exhibits only London dispersion forces (also known as Van der Waals forces) as its intermolecular forces. London dispersion forces are the weakest intermolecular forces and primarily arise from temporary fluctuations in electron distribution, resulting in temporary dipole moments. Hence, N2 has the lowest boiling point among the substances listed.

Therefore, the ranking of these substances based on expected boiling point is: H2O > HCl > MgF2 > N2.

To rank the substances according to their expected boiling points based on intermolecular forces, we need to consider the types of intermolecular forces present in each substance.

1. N2 (Nitrogen): Nitrogen is a diatomic molecule made up of two nitrogen atoms. The dominant intermolecular force in N2 is London dispersion forces. These forces arise from temporary fluctuations in electron density that cause temporary dipoles. Nitrogen molecules are relatively nonpolar, and therefore, have weaker intermolecular forces. As a result, N2 has a low boiling point.

2. HCl (Hydrogen chloride): Hydrogen chloride is a polar molecule. The dominant intermolecular force in HCl is dipole-dipole interactions. These forces occur between the positive end of one molecule and the negative end of another molecule. Since HCl is polar, it has stronger intermolecular forces compared to N2 and a higher boiling point than N2.

3. MgF2 (Magnesium fluoride): Magnesium fluoride is an ionic compound composed of magnesium cations (Mg2+) and fluoride anions (F-). The dominant intermolecular forces in ionic compounds are electrostatic forces between oppositely charged ions. These forces, known as ionic bonds, are generally much stronger than dipole-dipole interactions or London dispersion forces. Therefore, MgF2 has much higher intermolecular forces compared to N2 and HCl, and it has the highest expected boiling point among the given substances.

4. H2O (Water): Water is a polar molecule with hydrogen bonding. Hydrogen bonding is a special type of dipole-dipole interaction that occurs when hydrogen is bonded to a highly electronegative atom (in this case, oxygen). Hydrogen bonding is stronger than regular dipole-dipole interactions. Therefore, water has the strongest intermolecular forces among the given substances and the highest expected boiling point.

Ranking the substances based on their expected boiling points:

MgF2 > H2O > HCl > N2