Question

XeF₂ is isostructural with

• A. TeF₂
• B. \(ICl^-_2\)
• C. SbCl₃
• D. BaCl₂

Answer 1

The Correct Option is B

The problem at hand is to determine which of the given compounds is isostructural with \(\text{XeF}_2\). To solve this, we need to understand the concept of isostructurality in chemistry, which refers to different compounds that share the same shape or geometric structure.

\(\text{XeF}_2\) has a linear molecular geometry. This can be explained by the VSEPR (Valence Shell Electron Pair Repulsion) theory. In \(\text{XeF}_2\), xenon (Xe) is the central atom with two fluorine (F) atoms attached and three lone pairs of electrons. According to VSEPR theory, this results in a linear structure, as the molecule arranges itself to minimize repulsion between these electron pairs.

Now, let's evaluate the options to determine which is isostructural with \(\text{XeF}_2\):

• TeF₂: Tellurium difluoride (TeF₂) does not have the same linear structure as \(\text{XeF}_2\), because the electron pairs and bonded atoms around tellurium lead to a different geometry.
• SbCl₃: Antimony trichloride (SbCl₃) has a trigonal pyramidal structure due to a different number of lone pairs and bonded atoms compared to \(\text{XeF}_2\).
• BaCl₂: Barium chloride (BaCl₂) is an ionic compound, and its structural arrangement is not molecular like \(\text{XeF}_2\), so it cannot be isostructural.
• \(ICl^-_2\): The iodine chloride ion (\(ICl^-_2\)) is isostructural with \(\text{XeF}_2\). Like \(\text{XeF}_2\), \(ICl^-_2\) also has a linear geometry, as iodine (I) is surrounded by three lone pairs and two bonded chloride atoms, similar to xenon's electron arrangement in \(\text{XeF}_2\).

Thus, the correct answer is that \(\text{XeF}_2\) is isostructural with \(ICl^-_2\).