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Chapter 10: Problem 8

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

Short Answer

Expert verified
\(\mathrm{AlCl}_{3}\) is Trigonal Planar, \(\mathrm{ZnCl}_{2}\) is Linear, and \(\mathrm{ZnCl}_{4}^{2-}\) is Tetrahedral.

Step by step solution

01

Predict Geometry of \(\mathrm{AlCl}_{3}\)

Starting with \(\mathrm{AlCl}_{3}\), Aluminium has three valence electrons, each of which form covalent bonds with the Chloride atoms, having 0 lone pairs. The geometry in such molecules with three regions of electron density around a central atom (3 bonding, 0 lone pair) is trigonal planar. Therefore, the geometry of \(\mathrm{AlCl}_{3}\) is Trigonal Planar.
02

Predict Geometry of \(\mathrm{ZnCl}_{2}\)

Moving to \(\mathrm{ZnCl}_{2}\), Zinc has 2 valence electrons which create bonds with two Chloride atoms, leaving 0 lone pairs. In cases with two regions of electron density around the central atom (2 bonding, 0 lone pairs), the geometry is linear. Therefore, the geometry of \(\mathrm{ZnCl}_{2}\) is Linear.
03

Predict Geometry of \(\mathrm{ZnCl}_{4}^{2-}\)

Finally for \(\mathrm{ZnCl}_{4}^{2-}\), Zinc forms bonds with each of the four Chlorine atoms, and has 0 lone pairs. Molecules with four regions of electron density around the central atom (4 bonding, 0 lone pairs) take a tetrahedral geometry. Therefore, the geometry of \(\mathrm{ZnCl}_{4}^{2-}\) is Tetrahedral.

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Most popular questions from this chapter

What is the hybridization of atomic orbitals? Why is it impossible for an isolated atom to exist in the hybridized state?

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line \() .\) What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

What is molecular orbital theory? How does it differ from valence bond theory?

How does a hybrid orbital differ from a pure atomic orbital? Can two \(2 p\) orbitals of an atom hybridize to give two hybridized orbitals?

What is the state of hybridization of the central \(\mathrm{O}\) atom in \(\mathrm{O}_{3} ?\) Describe the bonding in \(\mathrm{O}_{3}\) in terms of delocalized molecular orbitals.
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