Question

4

Answer 1

What do you think the answer is?

Answer 2

These two questions revolve around bonding think of how each answer choice in each question is bonded and whether these bonds are polar or nonpolar. Dont forget to consider intermolecular forces at hand in question #2

Answer 3

Your choice for question 1 was correct.

Answer 4

For question 2 the substance with the lowest vapor pressure will have the strongest forces acting upon and it will also be the substance with the highest boiling point. So in this case which answer do you think it should be?

Answer 5

either ethanol or water because they have, H-bonding, Dipole, and London Dispersion forces

Answer 6

isn't it weaker IMF = higher Vapor pressure

Answer 7

Yes weaker IMF = higher vapor pressure. That is why substances like methane are a gas at room temperature.

Answer 8

But in this case ethanol and water are not the lowest vapor pressure molecules.

Answer 9

Dont forget the fact that metals have very high boiling points and this is due to the strong metallic bonds between the electrons in the sea of delocalized electrons

Answer 10

hmmmm.... okay. I just didn't think metals had intermolecular forces

Answer 11

Well your kind of right in which there not classified as intermolecular forces. However, there are strong interactions between metal atoms. The question is really just asking which compound has the lowest vapor pressure.

Answer 12

Therefore if you were to look at the boiling point of each compound you would notice Hg's boiling point is roughly three times greater than H2O's boiling point.

Answer 13

okay, thank you

Answer 14

np