How does the boiling point of ethane (CH3CH3) compare with that of ethanol (CH3CH2OH)?

1. The boiling point of ethane is higher because it has stronger London dispersion forces.
2. The boiling point of ethane is higher because it has stronger dipole-dipole forces.
3. The boiling point of ethane is lower because it lacks hydrogen bonds.
4. The boiling point of ethane is lower because it has weaker covalent bonds.

The boiling point of ethane is lower because it lacks hydrogen bonds. I took the quiz

Option 3 I promise like aliyah windom I took the quiz I can verify

Well, first of all, have you tried inviting both ethane and ethanol to a hot tub party? It's a great way to compare their boiling points.

But in all seriousness, the boiling point of ethane (CH3CH3) is actually lower than that of ethanol (CH3CH2OH). The correct answer is number 3 - the boiling point of ethane is lower because it lacks hydrogen bonds.

Now, I'm no expert on intermolecular forces, but I do know a thing or two about having a good time. Ethanol has the lovely ability to form hydrogen bonds, thanks to the presence of that delightful OH group. These hydrogen bonds give ethanol stronger intermolecular forces and thus a higher boiling point. Ethane, on the other hand, lacks this ability to form hydrogen bonds, so its intermolecular forces are weaker, resulting in a lower boiling point.

So remember, folks, next time you're comparing ethane and ethanol, ask them to show you their hydrogen bonds and see who gets invited to the hot tub party!

To answer this question, we need to first understand the intermolecular forces at play in these compounds.

Ethane (CH3CH3) is a nonpolar molecule, meaning it does not have a permanent dipole moment. The intermolecular forces in ethane are primarily London dispersion forces, which are the weak attractive forces between temporary dipoles formed due to fluctuations in electron distribution.

Ethanol (CH3CH2OH), on the other hand, is a polar molecule due to the presence of an -OH (hydroxyl) group. This polar group creates a permanent dipole moment, resulting in additional intermolecular forces apart from London dispersion forces. Ethanol exhibits both London dispersion forces and hydrogen bonding, which is a strong intermolecular force between the hydrogen atom bonded to an electronegative atom and another electronegative atom (in this case, oxygen).

Now, coming back to the question options:

1. The boiling point of ethane is higher because it has stronger London dispersion forces. This statement is incorrect because ethanol has both London dispersion forces and additional hydrogen bonding, which are stronger than London dispersion forces alone.

2. The boiling point of ethane is higher because it has stronger dipole-dipole forces. This statement is incorrect because ethane does not have a permanent dipole moment and, therefore, does not exhibit dipole-dipole forces. Ethanol, with its -OH group, does have dipole-dipole forces in addition to other intermolecular forces.

3. The boiling point of ethane is lower because it lacks hydrogen bonds. This statement is incorrect because ethane indeed lacks hydrogen bonding, but ethanol has hydrogen bonding. Hydrogen bonding is a stronger intermolecular force compared to London dispersion forces, leading to a higher boiling point for ethanol.

4. The boiling point of ethane is lower because it has weaker covalent bonds. This statement is unrelated to the boiling point comparison of ethane and ethanol. The boiling point is determined by the strength of intermolecular forces, not the strength of covalent bonds within the molecules.

Therefore, the correct answer is option 3. The boiling point of ethane is lower than that of ethanol because it lacks hydrogen bonding.

Hydrogen bonding increases the boiling point of ethanol