Question

the geometry of the icl₂⁻ molecule is best described as: bent tetrahedral t - shaped linear triangular planar

Explanation:

First, calculate the number of valence electrons for ICl₂⁻: I has 7, each Cl has 7, plus 1 for the negative charge, total 7 + 2×7 +1 = 22. The central I atom forms 2 bonds with Cl atoms, using 4 electrons. The remaining 18 electrons are lone pairs: 18/2 =9 lone pairs total. Subtract 2 bonding pairs (4 electrons) from total electron pairs: (22/2)=11 electron pairs, so 11-2=9 lone pairs? Wait no—correct: electron domains around I: bonding pairs (2) + lone pairs. Wait better: steric number = number of bonding pairs + lone pairs. For ICl₂⁻: I has 2 bonding pairs (to Cl) and 3 lone pairs (since 7+1=8 valence electrons for I, minus 2 used in bonding =6, which is 3 lone pairs). So steric number=2+3=5. Electron domain geometry is trigonal bipyramidal. Lone pairs occupy equatorial positions to minimize repulsion, so the two bonding pairs are axial—resulting in linear molecular geometry.

Answer:

linear