Relate ionic lattice strength to charge and ionic radius.

In the subtopic Ionic bonding, this AQA A-Level Chemistry 7405 learning objective focuses on relate ionic lattice strength to charge and ionic radius. It belongs to Bonding, so revision should stay anchored to this exact subtopic rather than drifting into a generic GCSE-level chemistry summary. Approved keywords to use include lattice, ion. Ionic radius. means the ionic radius is the measure of an ion's size, which affects the distance between ions in an ionic lattice Avoid the mistake of students often confuse the effects of ionic charge and ionic radius on lattice strength, thinking that only one factor influences it; instead, to relate ionic lattice strength to charge and ionic radius, use the rule that higher charges and smaller ionic radii lead to stronger lattices. For example, the lattice energy (U) can be calculated using the formula: U = k * (Q1 * Q2) / r, where Q1 and Q2 are the charges of the ions and r is the distance between them. Substituting values for two ions, such as Na+ and Cl- (Q1 = +1, Q2 = -1, r = 0.227 nm), gives U = k * (1 * -1) / 0.227. This shows that increasing the charge or decreasing the radius increases the lattice strength. Therefore, the conclusion is that ionic compounds with higher charges and smaller ionic radii have stronger lattices For exam answers, to relate ionic lattice strength to charge and ionic radius, remember that higher charges and smaller ionic radii lead to stronger lattices. Use the formula: Lattice Energy ∝ (Charge1 × Charge2) / Distance