James Pelezo said:Physical, Chemical
The original question was why is water liquid, but H2S is gas (i.e., doesn't demonstrate H-Bonding as does HOH) under the same conditions (i.e., 25oC; 1 atm)? To answer that question one needs to understand how chemical bonds, physical bonds and properties of the elements and molecules interact. You are right, it is a continuum of factoids drawn from each topic listed. Was just trying to make a suggestion of what should be reviewed to answer such questions.Borek said:Not sure what you are referring to, but I am more than sure that whatever you mean by each they are just ends of a bond continuum, and it is possible to give examples that lie exactly in between.
Water is a liquid at room temperature because the hydrogen bonds between its atoms create strong intermolecular forces that hold the molecules together. On the other hand, hydrogen sulphide is a gas at room temperature because the hydrogen bonds between its atoms are much weaker, resulting in a lower boiling point.
The differences in physical states between water and hydrogen sulphide can be attributed to the differences in their molecular structures. While both molecules have the same chemical formula (H2O and H2S), water molecules are arranged in a tetrahedral structure, whereas hydrogen sulphide molecules have a linear structure. This difference in molecular shape affects the strength of intermolecular forces and thus, the boiling points of the two substances.
Yes, hydrogen sulphide can be a liquid under certain conditions. At very low temperatures and high pressures, the intermolecular forces between hydrogen sulphide molecules become stronger, causing it to condense into a liquid state.
As mentioned earlier, water has stronger intermolecular forces due to its tetrahedral molecular structure. This means that more energy is required to overcome these forces and turn water into a gas, resulting in a higher boiling point compared to hydrogen sulphide.
Other factors that can affect the physical states of water and hydrogen sulphide include temperature and pressure. Higher temperatures generally result in weaker intermolecular forces and thus, a lower boiling point. Additionally, increasing the pressure on a substance can also lead to a higher boiling point as it compresses the molecules together, making it more difficult for them to escape into a gas state.