What type(s) of intermolecular forces allow CO2 to dissolve in water? Do CO2 and H2O have a relatively strong or weak attraction to one another? Explain.

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CO2 can dissolve in water due to a combination of intermolecular forces, specifically dipole-dipole interactions and London dispersion forces.

Dipole-dipole interactions occur between the positively charged hydrogen atoms of water (H2O) molecules and the negatively charged oxygen atom in CO2. These attractions are relatively weak but still contribute to the overall dissolution of CO2 in water.

In addition, CO2 and H2O also experience London dispersion forces. These forces result from temporary fluctuations in electron distribution within molecules and induce temporary dipoles. The temporary dipoles in one molecule can then induce dipoles in neighboring molecules, creating attractive forces between them. The London dispersion forces between CO2 and H2O molecules further enhance their interaction.

Regarding the strength of attraction, the dipole-dipole interactions and London dispersion forces between CO2 and H2O can be considered relatively weak compared to other intermolecular forces. However, they are still sufficient to enable CO2 to dissolve in water.

Overall, the ability of CO2 to dissolve in water is a result of a combination of intermolecular forces, including dipole-dipole interactions and London dispersion forces. Although these forces are relatively weak, they are significant enough to allow for the dissolution of CO2 in water.