1. What is Lattice Energy?

Lattice energy (LE) is the energy required to completely separate one mole of a solid ionic compound into gaseous ions. It's a measure of the strength of the ionic bonds in a crystal lattice.

2. How Does the Calculator Work?

The calculator uses the lattice energy equation:

Where:

• \( LE \) — Lattice energy (kJ/mol)
• \( k \) — Proportionality constant (typically 8.988×10⁹ N·m²/C²)
• \( Q_1 \) — Charge of first ion (dimensionless)
• \( Q_2 \) — Charge of second ion (dimensionless)
• \( r \) — Distance between ion centers (pm)

Explanation: The equation shows that lattice energy increases with larger ion charges and decreases with greater distance between ions.

3. Importance of Lattice Energy Calculation

Details: Lattice energy helps predict ionic compound properties like solubility, melting point, and stability. It's crucial in materials science and chemistry.

4. Using the Calculator

Tips: Enter all values with correct units. The default k value is appropriate for most calculations. Distance must be greater than zero.

5. Frequently Asked Questions (FAQ)

Q1: What are typical lattice energy values?
A: Values typically range from 700-4000 kJ/mol. Higher charges and smaller ions result in greater lattice energies.

Q2: How does lattice energy relate to solubility?
A: Compounds with higher lattice energies tend to be less soluble as more energy is required to break the ionic bonds.

Q3: What factors affect lattice energy?
A: Main factors are ion charge (biggest effect), ion size, and crystal structure arrangement.

Q4: Can this equation be used for all ionic compounds?
A: This is a simplified model. More accurate calculations consider crystal structure and additional energy terms.

Q5: Why is distance measured in picometers?
A: Ionic radii are typically in the picometer range (100-200 pm), making this a convenient unit for calculations.