Br₂ is much more soluble in tetrachloromethane (CCl₄) than in water. Explain.

Verified step by step guidance

1. Step 1: Understand the nature of the solute and solvents involved. Bromine (Br₂) is a nonpolar molecule, while tetrachloromethane (CCl₄) is also nonpolar. Water, on the other hand, is a polar solvent.
2. Step 2: Recall the principle 'like dissolves like,' which means that nonpolar solutes tend to dissolve well in nonpolar solvents, and polar solutes dissolve well in polar solvents.
3. Step 3: Analyze the interactions. In a nonpolar solvent like CCl₄, Br₂ molecules can interact through London dispersion forces, which are weak intermolecular forces that occur between nonpolar molecules.
4. Step 4: Consider the interactions in water. Water molecules are polar and can form hydrogen bonds, which are strong intermolecular forces. Br₂, being nonpolar, cannot effectively interact with water molecules, leading to poor solubility.
5. Step 5: Conclude that the solubility of Br₂ in CCl₄ is higher than in water because the nonpolar Br₂ molecules are more compatible with the nonpolar CCl₄, allowing for better solvation through dispersion forces.