To visualize how magnesium chloride (MgCl₂) dissolves in water, imagine a beaker filled with water, where MgCl₂ is added. As the solid dissolves, you can see the Mg²⁺ ions and Cl⁻ ions separate from each other and disperse into the water. The polar water molecules surround the magnesium and chloride ions, stabilizing them and allowing them to move freely throughout the solution.
In the illustration, Mg²⁺ ions, which are positively charged, would be surrounded by water molecules with their oxygen atoms facing the magnesium ion (due to their partial negative charge), while the negatively charged Cl⁻ ions would attract water molecules with their hydrogen ends facing the chloride ions (due to their partial positive charge). This interaction between the polar water molecules and the ions helps to overcome the ionic bonds in solid MgCl₂, leading to its dissolution. As a result, a homogeneous solution of magnesium and chloride ions emerges, emphasizing the effectiveness of water as a solvent for ionic compounds.
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