Which of the following should have the lowest viscosity at room temperature? Whi

Question

Which of the following should have the lowest viscosity at room temperature? Which should have the greatest? Explain.

---Select--- has the strongest intermolecular forces because its molecules can undergo hydrogen bonding interactions, which are stronger than dipole-dipole interactions and London dispersion forces. These molecules are polar and can also participate in dipole-dipole interactions. London dispersion forces exist in all substances, so these weak forces would be present in this molecule as well.

---Select--- cannot participate in hydrogen bonding interactions, but can participate in dipole-dipole interactions since these molecules are polar. London dispersion forces would also be present.

---Select--- has the weakest intermolecular forces of the three molecules. These molecules are not polar and cannot participate in hydrogen bonding interactions. The only attractive forces between these molecules would be London dispersion forces, which are the weakest of the intermolecular forces.

Since  ---Select--- has the weakest intermolecular forces, it will have the lowest viscosity at room temperature. Since  ---Select--- has the strongest intermolecular forces, it will have the greatest viscosity at room temperature.

Therefore, the ranking from greatest viscosity to lowest viscosity will be:  ---Select--- >  ---Select--- >  ---Select--

Explanation / Answer

Ethylene glycol because of presence two -OH bonds with strucutre (OH-CH2-CH2-OH) has the strongest intermolecular forces

Pentanal will show dipole-dipole interactions

C2F6 has weakest forces because of not polar and cannot participate in hydrogen bonding forces

Correct answer will be Ethylene Glycol > Pentanal > C2F6

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