The boiling point of a compound is determined by the strength of the intermolecular forces. The stronger the intermolecular forces, the higher the boiling point.

There are three types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

All of these compounds have London dispersion forces, but the strength of these forces increases with the size and shape of the molecule. Therefore, the larger the molecule, the higher the boiling point.

Compounds I, II, and III also have hydrogen bonding because they contain an OH group. Hydrogen bonding is the strongest type of intermolecular force, so these compounds will have a higher boiling point than compound IV, which only has London dispersion forces.

Among compounds I, II, and III, compound III will have the highest boiling point because it is the largest molecule and therefore has the strongest London dispersion forces. Compound II will have the next highest boiling point because it is larger than compound I.

So, the correct order of increasing boiling point is IV

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The boiling point of a compound is determined by the strength of the intermolecular forces. The stronger the intermolecular forces, the higher the boiling point.

There are three types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

All of these compounds have London dispersion forces, but the strength of these forces increases with the size and shape of the molecule. Therefore, the larger the molecule, the higher the boiling point.

Compounds I, II, and III also have hydrogen bonding because they contain an OH group. Hydrogen bonding is the strongest type of intermolecular force, so these compounds will have a higher boiling point than compound IV, which only has London dispersion forces.

Among compounds I, II, and III, compound III will have the highest boiling point because it is the largest molecule and therefore has the strongest London dispersion forces. Compound II will have the next highest boiling point because it is larger than compound I.

So, the correct order of increasing boiling point is IV < I < II < III. Therefore, the correct answer is option A.

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The boiling point of a compound is determined by the strength of the intermolecular forces. The stronger the intermolecular forces, the higher the boiling point.

There are three types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

All of these compounds have London dispersion forces, but the strength of these forces increases with the size and shape of the molecule. Therefore, the larger the molecule, the higher the boiling point.

Compounds I, II, and III also have hydrogen bonding because they contain an OH group. Hydrogen bonding is the strongest type of intermolecular force, so these compounds will have a higher boiling point than compound IV, which only has London dispersion forces.

Among compounds I, II, and III, compound III will have the highest boiling point because it is the largest molecule and therefore has the strongest London dispersion forces. Compound II will have the next highest boiling point because it is larger than compound I.

So, the correct order of increasing boiling point is IV < I < II < III. Therefore, the correct answer is option A.

Arrange the following compounds in order of increasing boiling pointl.CH 3CH2CH2OHII.CH 3CH 2OHIII.CH3CH2CH2CH2OHIV. CH3CH 2CH2CH 2CH 3A. I < II < IV < IIIB. IV < III < II < IC. I < II < III < IVD. IV < I < II< III

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