Question 12 For the covalent molecule, silicon tetrabromide. a. Draw the Lewis diagram. b. How many total valence electrons are present? c. How many bonding electron pairs? How many lone pairs does the central atom have? d. What is the molecular shape of the molecule? e. Is the molecule polar or nonpolar? f. What is the strongest attraction between molecules of silicon tetrabromide?
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Silicon tetrabromide (SiBr₄) is an interesting molecule! Silicon, with its four valence electrons, shares one with each of the four bromine atoms, which have seven valence electrons each. This sharing results in a total of 32 valence electrons (4 from silicon and 4*7 from bromine). The shape? Imagine tetrahedrons sprouting from a central atom! That's right—it adopts a tetrahedral shape for minimal repulsion between bonding pairs, making it nonpolar overall due to the symmetry of the Br-Si-Br angles. In terms of intermolecular forces, the primary attraction between silicon tetrabromide molecules comes from London dispersion forces, due to the presence of bromine's larger electron cloud. These forces are generally weak compared to polar covalent bonds, but they play a crucial role in the behavior of nonpolar molecules like SiBr₄ in various environments!
