What is the smallest whole-number ratio of ions in a crystal lattice?
If I understand the question I suppose 1:1.
A unit cell
The smallest whole-number ratio of ions in a crystal lattice is determined by the ratio between the cations (positively charged ions) and anions (negatively charged ions) that make up the crystal structure. This ratio is known as the empirical formula.
To find the empirical formula, you need to know the charges of the ions involved. Let's assume we have a metal cation (M+) and a non-metal anion (X-) as an example.
1. Determine the charges: Find the charges of the metal cation and non-metal anion. Note that these charges must balance each other out to form a neutral compound. For example, if M+ has a charge of +2, then X- must have a charge of -2.
2. Determine the ratio: Divide the absolute values of the ion charges to find the smallest whole-number ratio. In the example, the ratio would be 2:2, which can be simplified to 1:1.
3. Determine the empirical formula: Use the ratio obtained to write the empirical formula. In this case, the empirical formula would be MX.
It is important to note that different crystal lattices can have different ratios depending on the composition and charges of the ions involved. The above steps outline a general method to determine the smallest whole-number ratio of ions in a crystal lattice.