Arrange in order of increasing boiling point: \(\mathrm{CO}_{2}, \mathrm{SO}_{2}, \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, \mathrm{Al}\)

Short Answer

Expert verified
The substances in order of increasing boiling points are: \(\mathrm{CO}_{2}\), \(\mathrm{SO}_{2}\), \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\), and \(\mathrm{Al}\).

Step by step solution

01

Identify the molecular structure and intermolecular forces for each substance

1. CO2: Linear molecule, symmetric, non-polar. Its primary intermolecular force is London dispersion forces. 2. SO2: Bent molecule, asymmetrical with sulfur double bonded to 2 oxygens. It has a polar structure, leading to dipole-dipole forces. 3. CH3CH2OH (Ethanol): Ethanol molecule contains a polar O-H group, allowing for hydrogen bonding in addition to dipole-dipole forces. 4. Al: Metallic bonding and as a pure metal, is held together by ion-dipole forces
02

Compare the strength of their intermolecular forces

Rank the strength of the intermolecular forces from weakest to strongest: 1. London dispersion force: CO2 2. Dipole-Dipole force: SO2 3. Hydrogen bonding: CH3CH2OH 4. Ion-Dipole force: Al
03

Arrange the substances in order of increasing boiling points

Since the boiling point depends on the strength of the intermolecular forces, the substances can be arranged using the order of intermolecular forces we determined in step 2: 1. CO2 (London dispersion force) 2. SO2 (Dipole-Dipole force) 3. CH3CH2OH (Hydrogen bonding) 4. Al (Ion-Dipole force) Thus, the substances in order of increasing boiling points are: CO2, SO2, CH3CH2OH, Al

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