Questions: 3. Specify which compound in the following pairs of ionic compounds has the higher lattice energy. Explain your choice. ( 6 points) a. KCl or MgO

3. Specify which compound in the following pairs of ionic compounds has the higher lattice energy. Explain your choice. ( 6 points)
a. KCl or MgO
Transcript text: 3. Specify which compound in the following pairs of ionic compounds has the higher lattice energy. Explain your choice. ( 6 points) a. KCl or MgO
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Solution

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Solution Steps

Step 1: Understanding Lattice Energy

Lattice energy is the energy required to separate one mole of an ionic solid into its gaseous ions. It is influenced by two main factors: the charge of the ions and the size of the ions. Higher charges and smaller ionic radii result in higher lattice energies.

Step 2: Analyzing the Charges of the Ions

In the given compounds:

  • KCl consists of \( \text{K}^+ \) and \( \text{Cl}^- \) ions.
  • MgO consists of \( \text{Mg}^{2+} \) and \( \text{O}^{2-} \) ions.

The charges on the ions in MgO are higher (\(2+\) and \(2-\)) compared to those in KCl (\(1+\) and \(1-\)).

Step 3: Considering the Ionic Radii

The ionic radii also play a role in lattice energy. Generally, smaller ions will have a higher lattice energy because they can pack more closely together, increasing the electrostatic attraction.

  • The ionic radius of \( \text{Mg}^{2+} \) is smaller than that of \( \text{K}^+ \).
  • The ionic radius of \( \text{O}^{2-} \) is similar to or slightly smaller than that of \( \text{Cl}^- \).
Step 4: Conclusion Based on Lattice Energy Factors

Given that MgO has ions with higher charges and smaller radii compared to KCl, MgO will have a higher lattice energy.

Final Answer

\(\boxed{\text{MgO has the higher lattice energy.}}\)

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