Final answer:
Without specific data or a figure, we cannot precisely estimate the As-I bond length. We usually rely on adding ionic and atomic radii or similar empirical methods to estimate bond lengths, comparing them to known experimental values, like the 2.55 Å As-I bond length in AsI₃.
Step-by-step explanation:
To estimate the As-I bond length from given data, we would typically look for trends or empirical relationships between known bond lengths and radii of atoms involved in the bond. For instance, a similar approach is the use of covalent atomic radii to predict bond lengths. The given experimental As-I bond length in triiodide (AsI₃) is 2.55 Å. If we were to rely on typical ionic and atomic radii, we could add the radii of the two atoms to estimate the bond length. Unfortunately, without a specific figure or further data provided in the question, we cannot perform a precise estimation.
Thallium(I) iodide, TlI, provides an example where the edge length of its unit cell is 4.20 Å, and given the ionic radius of I- (iodide) as 2.16 Å, we calculate the ionic radius of Tl+ (thallium(I)). Since TlI crystallizes in the same structure as CsCl, where the cation and anion touch each other along the diagonal of the cube, we can apply Pythagorean theorem to the right-angled triangle formed by half the edge length and the body diagonal to find the sum of the radii, and subsequently, the individual radius of Tl+.
We could compare suggested methodologies, such as this use of geometric relationships in crystalline structures or adding covalent atomic radii, to figure out estimates for bond lengths. The desired estimate can be compared to the provided experimental bond length of AsI₃ to assess the accuracy of such an estimation.