Van der Waal's forces
Ionic attraction
dipole attraction
covalent bonding
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The correct answer is: C. dipole attraction
The solubility of CO₂ in water can be accounted for by dipole-dipole interactions between the water molecules and the CO₂ molecules. Water's polarity allows it to dissolve CO₂ through these intermolecular attractions.
@myschool, The solubility of CO₂ in water is best explained by dipole attraction.
CO₂ is a linear molecule, overall nonpolar, but each C=O bond is polar.
Water is strongly polar, with partial negative charge on oxygen and partial positive charges on hydrogen.
When CO₂ dissolves, water molecules interact with the slightly negative oxygen atoms in CO₂ through dipole–induced dipole interactions.
Van der Waal’s forces → weak, play a minor role but not the main factor.
Ionic attraction → CO₂ and water are not ionic species.
Covalent bonding → no new covalent bonds form between CO₂ and water.
The solubility of CO₂ in water is primarily accounted for by C. dipole attraction.
CO₂ is a nonpolar molecule, but water is polar. The oxygen atoms in CO₂ have a slight negative charge, while the carbon atom has a slight positive charge. This allows the polar water molecules to interact with the CO₂ through dipole interactions, particularly via hydrogen bonding with the slightly negatively charged oxygen atoms in CO₂. This dipole attraction is the primary reason CO₂ dissolves in water.
You said:
Are you sure?
ChatGPT said:
ChatGPT
I appreciate the check—let's go over the reasoning again.
CO₂ is indeed a nonpolar molecule overall because of its linear structure, which results in the dipole moments of the C=O bonds canceling each other out. However, when CO₂ dissolves in water, the interaction is largely due to the fact that water is polar and can interact with CO₂ through dipole-induced dipole interactions. The water molecules can induce a temporary dipole in the CO₂ molecule, allowing it to dissolve.
Given the options:
Van der Waal's forces: These are weak intermolecular forces, including dipole-induced dipole interactions, which play a role but are not the strongest factor in the solubility of CO₂ in water.
Ionic attraction: This does not apply, as CO₂ and water are not ionic species.
Dipole attraction: This option suggests interactions between polar molecules, which can be extended to include the interaction between water's dipole and the induced dipole in CO₂.
Covalent bond: No covalent bond forms between CO₂ and water in solution.
The correct answer remains C. dipole attraction, considering the dipole-induced dipole interactions as part of this category. This is the most significant factor in the solubility of CO₂ in water.
