Question

question 14 (1 point)
the geometry of the icl₂⁻ molecule is best described as:
bent
tetrahedral
t - shaped
linear
triangular planar
you can use this periodic table during the quiz. however, as stated in the course outline, and in the orientation session, this quiz is not open book. you cannot access course material while you write the quiz. nor can you google your answers, work as a group, use a cheat sheet, etc.

Explanation:

1. First, find the central - atom and its valence - electron count: In $ICl_2^-$, the central atom is iodine (I). Iodine has 7 valence electrons, and the ion has an extra electron due to the negative charge, so there are 8 valence electrons around the central I atom.
2. Then, consider the number of bonding and non - bonding pairs: Iodine forms 2 bonds with 2 chlorine (Cl) atoms. So, the number of bonding pairs is 2. The number of non - bonding (lone) pairs is $\frac{8 - 2}{2}=3$.
3. According to VSEPR (Valence - Shell Electron - Pair Repulsion) theory, for a molecule with 2 bonding pairs and 3 lone pairs around the central atom, the molecular geometry is linear. The lone pairs are arranged in a trigonal - bipyramidal electron - pair geometry, and the two bonding pairs are 180° apart to minimize repulsion.

Answer:

linear