1) Which of the following properties of water can be explained using hydrogen bonding arguments?
1. its ability to dissolve most ionic compounds.
2. its high boiling point.
3. its low vapor pressure
a) only 1 or only 2 or only 3
b) 1 and 2 only
c) 1 and 3 only
d) 2 and 3 only
e) 1 and 2 and 3
I think that all three of the statements are correct? Is this right.
I don't know about 1. I think the polar nature of H2O has more to do with dissolving ionic substances.
Ok so would you say just high boiling point and low vapor pressure?
Those would be my answers.
Yes, you are correct. All three statements are correct. The properties of water mentioned can be explained using hydrogen bonding arguments.
To understand why each statement is true, let's break it down:
1. The ability of water to dissolve most ionic compounds can be explained by the polar nature of water molecules due to hydrogen bonding. Water molecules have a partial positive charge on the hydrogen atom and a partial negative charge on the oxygen atom. This allows water to interact with ions, which are also polar in nature, and separate them from the crystal lattice of the ionic compound.
2. The high boiling point of water can also be attributed to hydrogen bonding. Hydrogen bonds are stronger than van der Waals forces and require more energy to break. As a result, water molecules need to be heated to a higher temperature for the hydrogen bonds to be overcome, leading to a higher boiling point.
3. The low vapor pressure of water is also related to hydrogen bonding. The strong hydrogen bonds between water molecules hold them together, leading to lower vaporization rates. Higher temperatures are required to provide enough energy to break these hydrogen bonds and allow water molecules to escape into the gas phase.
So the correct answer to the question is (e) 1 and 2 and 3.