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Perfecting Perbromate Ion: Achieving Zero Formal Charges
Chapter 10, Problem 10.24(choose chapter or problem)
Despite many attempts, the perbromate ion \({\rm{BrO}}_4^ -\) was not prepared in the laboratory until about 1970. (In fact, articles were published explaining theoretically why it could never be prepared!) Draw a Lewis structure for \({\rm{BrO}}_{\rm{4}}^{\rm{ - }}\) in which all atoms have the lowest formal charges.
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QUESTION:
Despite many attempts, the perbromate ion \({\rm{BrO}}_4^ -\) was not prepared in the laboratory until about 1970. (In fact, articles were published explaining theoretically why it could never be prepared!) Draw a Lewis structure for \({\rm{BrO}}_{\rm{4}}^{\rm{ - }}\) in which all atoms have the lowest formal charges.
ANSWER:Step 1 of 3
First, you have Bromine with 7 valence electrons. You also have four Oxygen atoms, each with 6 valence electrons, summing up to 24 for all of them. Because the perbromate ion has a 2- charge, we add two additional electrons. This gives us a total of 33 electrons available to create bonds and fill octets.
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Perfecting Perbromate Ion: Achieving Zero Formal Charges
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Learn how to create a Lewis structure for the perbromate ion, ensuring all atoms achieve zero formal charges. Follow the step-by-step guide to understand the bonding and electron distribution in this chemical compound.