Problem: Explain why the following ions have different bond angles: CLO2- and NO2-. Predict the bond angle in each case.

FREE Expert Solution

We’re being asked to predict the bond angles for ClO2and NO2- and explain why they have different bond angles


We need to do the following steps to predict and compare the bond angles for ClO2and NO2- 


Step 1: Determine the central atom for each ion.

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

Step 3: Draw the Lewis structure for each ion.

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˚


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Problem Details

Explain why the following ions have different bond angles: CLO2- and NO2-. Predict the bond angle in each case.

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Pelton's class at UMN.