(c) some properties of the two compounds are listed below:

compound X: compound Y:
melting point -144C -138C
boiling point 78C -22C
net point Yes Yes
functional group Alcohol Ether

(i.) Draw plausible Lewis Structures of compounds X and Y.
(ii.) In which compound are the intermolecular forces stronger? Justify your answer.
(iii.)Is either compound capable of hydrogen bonding? If so, draw a schematic representation of a typical hydrogen bind in this substance.
(iv.)which compound id likely to be more soluble in water? Justify your answer.

(d) Given the information in the table above, draw a schematic representation of a phase diagram for ethanol.

We will be happy to critique your thoughts.

(i.) To draw the Lewis structures of compounds X and Y, we need to determine the number of valence electrons each compound has.

Compound X: The functional group is alcohol (which is an -OH group). Oxygen has 6 valence electrons, and hydrogen has 1 valence electron. Additionally, there are no other elements present. Therefore, compound X has a total of 1 + 1 + 6 = 8 valence electrons.

Compound Y: The functional group is ether, which is an oxygen atom bonded to two carbon atoms. Oxygen has 6 valence electrons, and carbon has 4 valence electrons. Since there are two carbon atoms, the total valence electrons for compound Y is 6 + (4 × 2) = 14 valence electrons.

Using this information, we can proceed to draw the Lewis structures.

Compound X:
H
|
H - C - C - O - H
|
H

Compound Y:
H H
| |
H - C - C - O - C - C - H
| |
H H

(ii.) To determine which compound has stronger intermolecular forces, we need to consider their boiling points. The higher the boiling point, the stronger the intermolecular forces.

Compound X has a higher boiling point (-78°C) compared to compound Y (-22°C). This suggests that compound X has stronger intermolecular forces. These forces can be attributed to hydrogen bonding, which occurs between the hydrogen atom of one molecule and the oxygen atom of another molecule in compound X.

(iii.) Compound X, which is an alcohol, is capable of hydrogen bonding. A schematic representation of a typical hydrogen bond in this substance can be depicted as follows:

H H
| |
H - C - O : H - C - O
| |
H H

The dotted line represents a hydrogen bond between the hydrogen atom of one alcohol molecule and the oxygen atom of another alcohol molecule.

Compound Y, which is an ether, does not have any hydrogen atoms bonded directly to an oxygen or nitrogen atom. Therefore, it does not exhibit hydrogen bonding.

(iv.) Compound X, being an alcohol, is likely to be more soluble in water compared to compound Y, which is an ether. This is because alcohol can form hydrogen bonds with water molecules. Since water is a polar solvent, the presence of the -OH group in compound X allows for favorable interactions with water molecules. On the other hand, ethers lack this ability to form hydrogen bonds, resulting in weaker interactions with water. Therefore, compound X is likely to be more soluble in water than compound Y.

(d) Unfortunately, I cannot provide graphical representations here, but I can describe a typical phase diagram for ethanol:

A typical phase diagram for ethanol would have temperature (in Celsius) on the x-axis and pressure (in atmospheres) on the y-axis. It would include regions representing the different phases of ethanol (solid, liquid, and gas) and lines representing phase transitions.

Starting from the left, at low temperatures and pressures, ethanol would be in its solid phase (ice). As the temperature increases, the line would show the transition from the solid phase to the liquid phase (melting point), which is around -114°C.

As the temperature continues to rise, the line would indicate the transition from liquid to gas (boiling point), which is around 78°C. This line represents the vaporization/evaporation of ethanol.

Overall, the phase diagram would show the melting point, boiling point, and critical point of ethanol, providing a visual representation of the relationship between temperature, pressure, and phase changes.