We’re being asked to identify **which has greater O-N-O bond angles**. Since we don’t know the Lewis structure for nitrile ion (NO_{2}^{-}) or the nitrate ion (NO_{3}^{-}), we need to do the following steps:

*Step 1:* Determine the central atom in this molecule.

*Step 2:* Calculate the total number of valence electrons present.

*Step 3:* Draw the Lewis structure for the molecule.

*Step 4:* Determine the number of electron groups around the indicated atom.

*Step 5:* Determine the electron geometry and bond angle using this:

**Electron Regions Electronic Geometry Bond Angles**

2 linear 180˚

3 trigonal planar 120˚

4 tetrahedral 109.5˚

5 trigonal bipyramidal 90˚, 120˚, and 180˚

6 octahedral 90˚ and 180˚

Are the O-N-O bond angles greater in the nitrile ion (NO_{2}^{-}) or the nitrate ion (NO_{3}^{-})?

Please select the answer the best explains your conclusion.

a. Nitrite has the greater bond angle because a trigonal planar bond angle is greater than a tetrahedral bond angle

b. Nitrite has the greater bond angle because a linear bond angle is greater than a trigonal planar bond angle

c. Nitrate has the greater bond angle because nitrite’s lone pairs take up more space than bonds

d. Nitrate has the greater bond angle because double bonds take up more space than single bonds

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Bond Angles concept. You can view video lessons to learn Bond Angles. Or if you need more Bond Angles practice, you can also practice Bond Angles practice problems.