The compound with the lower melting point between CH3CH2CH2CH3 (Butane) and CH3COCH3 (Acetone) is Acetone.

Here's why:

1. Butane is a non-polar molecule. It only has London dispersion forces which are the weakest intermolecular forces.

2. Acetone, on the other hand, is a polar molecule. It has dipole-dipole interactions and also hydrogen bonding due to the presence of the oxygen atom.

3. Generally, the stronger the intermolecular forces, the higher the melting and boiling points because more energy is needed to break these forces.

4. Therefore, since Acetone has stronger intermolecular forces (dipole-dipole and hydrogen bonding) than Butane (only London dispersion forces), it would be expected to have a higher melting point.

5. However, in this case, Acetone actually has a lower melting point (-95°C) than Butane (-138°C). This is because the molar mass of Butane is higher than that of Acetone, and molar mass also affects the strength of London dispersion forces. The higher the molar mass, the stronger the London dispersion forces, and the higher the melting point.

6. So, despite having stronger intermolecular forces, Acetone's lower molar mass results in a lower overall melting point than Butane.

Question

The compound with the lower melting point between CH3CH2CH2CH3 (Butane) and CH3COCH3 (Acetone) is Acetone.

Here's why:

1. Butane is a non-polar molecule. It only has London dispersion forces which are the weakest intermolecular forces.

2. Acetone, on the other hand, is a polar molecule. It has dipole-dipole interactions and also hydrogen bonding due to the presence of the oxygen atom.

3. Generally, the stronger the intermolecular forces, the higher the melting and boiling points because more energy is needed to break these forces.

4. Therefore, since Acetone has stronger intermolecular forces (dipole-dipole and hydrogen bonding) than Butane (only London dispersion forces), it would be expected to have a higher melting point.

5. However, in this case, Acetone actually has a lower melting point (-95°C) than Butane (-138°C). This is because the molar mass of Butane is higher than that of Acetone, and molar mass also affects the strength of London dispersion forces. The higher the molar mass, the stronger the London dispersion forces, and the higher the melting point.

6. So, despite having stronger intermolecular forces, Acetone's lower molar mass results in a lower overall melting point than Butane.

Knowee AI · Accepted Answer

The compound with the lower melting point between CH3CH2CH2CH3 (Butane) and CH3COCH3 (Acetone) is Acetone.

Here's why:

1. Butane is a non-polar molecule. It only has London dispersion forces which are the weakest intermolecular forces.

2. Acetone, on the other hand, is a polar molecule. It has dipole-dipole interactions and also hydrogen bonding due to the presence of the oxygen atom.

3. Generally, the stronger the intermolecular forces, the higher the melting and boiling points because more energy is needed to break these forces.

4. Therefore, since Acetone has stronger intermolecular forces (dipole-dipole and hydrogen bonding) than Butane (only London dispersion forces), it would be expected to have a higher melting point.

5. However, in this case, Acetone actually has a lower melting point (-95°C) than Butane (-138°C). This is because the molar mass of Butane is higher than that of Acetone, and molar mass also affects the strength of London dispersion forces. The higher the molar mass, the stronger the London dispersion forces, and the higher the melting point.

6. So, despite having stronger intermolecular forces, Acetone's lower molar mass results in a lower overall melting point than Butane.

Which compound has the lower melting point? CH33CCH2CH2CH3 CH33CCOCH3

Question

Solution

Similar Questions

Upgrade your grade with Knowee