Question

In each pair, determine which ion would be more strongly hydrated with water and explain why: Na⁺ or Li⁺, Na⁺ or MgF₂, ClO₄⁻ or ClO₂⁻.

Answer 1

Li⁺ would be more strongly hydrated than Na⁺, Na⁺ would be more strongly hydrated than MgF₂, and ClO₄⁻ would be more strongly hydrated than ClO₂⁻.

Step-by-step explanation:

In each pair, the ion that is more strongly hydrated with water is the one that forms stronger attractions with water molecules. This can be determined by looking at the charge and size of the ions.

1. Na⁺ or Li⁺: Li⁺ would be more strongly hydrated because it is smaller in size and has a higher charge than Na⁺.

2. Na⁺ or MgF₂: Na⁺ would be more strongly hydrated because it is smaller in size and has a higher charge than Mg²⁺. Additionally, the fluoride ions in MgF₂ form stronger ion-dipole attractions with water molecules compared to the sodium ions in Na⁺.

3. ClO₄⁻ or ClO₂⁻: ClO₄⁻ would be more strongly hydrated because it is larger in size and has a higher charge than ClO₂⁻.