Bromite ion (BrO2)-) is an anion and contains bromine and oxygen atoms. Lewis structure of BrO2)-) contains one Br-O bond and one Br=O bond. Bromine atom has two lone pairs and oxygen atom holds -1 charge. In this tutorial, we will learn how to draw lewis structures of BrO2)- ion.
There is a single bond between center bromine atom and one oxygen atom. As well, a double is located between same bromine atom and other oxygen atom.
Bromine atom has two lone pairs and one oxygen atom also has two lone pairs. Other oxygen atom has three lone pairs and holds a -1 charge.
When we draw a lewis structure, guidelines are given for convenience. Number of steps can be changed according the complexity of the molecule or ion. Because Br2 is an ion, there are several steps to draw the lewis structure carefully. However those all steps are mentioned and explained in detail in this tutorial for your knowledge improvement.
There are only two elements in bromite ion. Oxygen, a VIA group element has six electrons in its last shell. Bromine is a group VIIA element in the periodic table and contains seven electrons in its last shell. Now, we know how many electrons are there in valence shells of bromine and oxygen atoms.
Total valance electrons pairs = σ bonds + π bonds + lone pairs at valence shells
Total electron pairs are determined by dividing the number total valence electrons by two. For, bromite ion, Total pairs of electrons are ten in their valence shells.
After determining the center atom and sketch of BrO2- ion, we can start to mark lone pairs on atoms. Remember that, there are total of ten electron pairs.
There are charges above drawn structure as below (each oxygen atom has -1 charge and bromine atom has +1 charge).
Because, there are charges on every atoms in above structure, that structure is not stable. Therefore, convert lone pairs to bonds as appropriate as below to reduce charges to get the most stable structure.
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