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Chapter 10: Problem 8

Predict the geometries of these species: (a) \(\mathrm{AlCl}_{3}\) (b) \(\mathrm{ZnCl}_{2},\) (c) \(\mathrm{ZnCl}_{4}^{2-}\)

Short Answer

Expert verified
The geometries for the given species are: (a)AlCl3 is Trigonal Planar, (b)ZnCl2 is Linear, and (c)\(ZnCl_{4}^{2-}\) is Tetrahedral.

Step by step solution

01

- Determine Geometry of AlCl3

Aluminium trichloride, AlCl3, has 3 bonds and no lone pairs. After determining the number of valence electrons, in cases like these, where there are no lone pairs, the geometry is determined by the number of bonding pairs. Thus, for AlCl3, the geometry will be trigonal planar.
02

- Determine Geometry of ZnCl2

Zinc chloride, ZnCl2, again has two bonding pairs and no lone pairs. This molecule is linear in its molecular geometry due to the arrangement of outer atoms.
03

- Determine Geometry of \(ZnCl_{4}^{2-}\)

Tetrachloro zincate, \(ZnCl_{4}^{2-}\), has 4 chemical bonds and no lone pairs. This makes its geometry tetrahedral.

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