Given the compounds H2S, NH3, and SO2. Determine the order o boiling points. Rank them from highest to lowest boiling point. Give an explanation for your ranking by the electronegativity data a by type of intermolecular force.

On the basis of molar mass alone, the order would be SO2 highest followed by H2S followed by NH3. (64 for SO2, 34 for H2S and 17 for NH3)

The electronegativity of N is higher than that of S, and it can form hydrogen bonds which will make the boiling point higher. Personally, I think it's a guess as to how far up you move NH3, certainly above H2S but probably not enough to move above SO2.
I think the order will be SO2, NH3, H2S highest to lowest.

To determine the order of boiling points for the compounds H2S, NH3, and SO2, we need to consider both electronegativity data and the type of intermolecular forces present.

1. NH3 (Ammonia):
NH3 has the highest boiling point among the given compounds. This is due to hydrogen bonding, which is a strong intermolecular force present in NH3. Nitrogen is highly electronegative, creating a significant partial positive charge on hydrogen and a partial negative charge on nitrogen. These partial charges allow for strong hydrogen bonding interactions between NH3 molecules.

2. H2S (Hydrogen sulfide):
H2S has a lower boiling point than NH3. Although sulfur is less electronegative than nitrogen, H2S also experiences hydrogen bonding. However, hydrogen bonding in H2S is weaker than in NH3 due to the larger size of sulfur compared to nitrogen. This results in weaker intermolecular forces and a lower boiling point for H2S compared to NH3.

3. SO2 (Sulfur dioxide):
SO2 has the lowest boiling point among the given compounds. Sulfur dioxide exhibits dipole-dipole interactions, which are weaker than hydrogen bonding. Sulfur is less electronegative than oxygen, but the molecule still has a partial positive charge on sulfur and partial negative charges on the oxygen atoms. Yet, these dipole-dipole forces are not as strong as hydrogen bonding present in NH3 and H2S, resulting in a lower boiling point for SO2.

Therefore, the order of boiling points from highest to lowest is:
NH3 > H2S > SO2

To determine the order of boiling points for the compounds H2S, NH3, and SO2, we need to consider their intermolecular forces and the electronegativity data.

1. H2S (Hydrogen sulfide):
H2S is a polar molecule due to the difference in electronegativity between hydrogen (2.20) and sulfur (2.58). It has dipole-dipole interactions. Although H2S is a polar molecule, it is less polar than NH3 and SO2, resulting in weaker intermolecular forces. As a result, H2S has the lowest boiling point among the three compounds.

2. SO2 (Sulfur dioxide):
SO2 is also a polar molecule due to the difference in electronegativity between sulfur (2.58) and oxygen (3.44). It exhibits dipole-dipole interactions similar to H2S. However, in comparison to H2S, SO2 has stronger intermolecular forces because sulfur is more electronegative than hydrogen. Consequently, SO2 has a higher boiling point than H2S but lower than NH3.

3. NH3 (Ammonia):
NH3 is a highly polar molecule due to the difference in electronegativity between nitrogen (3.04) and hydrogen. It exhibits hydrogen bonding, which is a stronger intermolecular force compared to dipole-dipole interactions. Hydrogen bonding occurs between the hydrogen atom of one molecule and the lone pair of electrons on the nitrogen atom of another molecule. Consequently, NH3 has the highest boiling point among the three compounds due to its strong intermolecular forces.

Therefore, the ranking from highest to lowest boiling point is:
1. NH3 (Ammonia)
2. SO2 (Sulfur dioxide)
3. H2S (Hydrogen sulfide)

This ranking is based on the increasing strength of the intermolecular forces present in the compounds, specifically hydrogen bonding in NH3 and dipole-dipole interactions in SO2 and H2S, respectively.