Question 8.8: Draw the Lewis structure for the BrO3^- ion.
Draw the Lewis structure for the BrO^{-}_{3} ion.
Bromine (Group 17) has seven valence electrons, and oxygen (Group 16) has six. We must add one more electron to our sum to account for the 1- charge of the ion. The total number of valence electrons is, therefore, 7 + (3 × 6) + 1 = 26. For oxyanions— SO^{2-}_{4} , NO^{-}_{3} , CO ^{2-}_{3} , and so forth—the oxygen atoms surround the central nonmetal atom. After arranging the O atoms around the Br atom, drawing single bonds, and distributing the unshared electron pairs, we have
\left[\overset{\cdot \cdot }{\underset{\cdot \cdot }{:O}}-\overset{\cdot \cdot }{\underset{\underset{{\underset{\large{}\cdot \cdot }{\large:O:}}}{|} }{Br}} -\overset{\cdot \cdot }{\underset{\cdot \cdot }{O:}}\right]^{-}Notice that the Lewis structure for an ion is written in brackets and the charge is shown outside the brackets at the upper right.
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