Question 6.17: Use VSEPR theory to predict the shape of the polyatomic ion ...

Use VSEPR theory to predict the shape of the polyatomic ion NO3NO_{3}^{-} .

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STEP 1   Draw the Lewis structure. The polyatomic ion NO3NO_{3}^{-} contains three electron groups (two single bonds between the central N atom and O atoms, and one double bond between N and O). Note that the double bond can be drawn to any of the O atoms.

[O — NO=O] \left[ {}_{\bullet }^{\bullet } \overset{\bullet \bullet }{\underset{\bullet \bullet }{O}}  —  \underset{\underset{{}_{\bullet }^{\bullet }\underset{\bullet \bullet }{O_{\bullet }^{\bullet }} }{|} }{N} = \overset{\bullet \bullet }{O_{\bullet }^{\bullet }} \right]

STEP 2   Arrange the electron groups around the central atom to minimize repulsion. To minimize repulsion, three electron groups would have a trigonal planar geometry.

STEP 3   Use the atoms bonded to the central atom to determine the shape. Because NO3NO_{3}^{-} has three bonded atoms, it has a trigonal planar shape.

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