We’re being asked to predict the bond angles for ClO2- and NO2- and explain why they have different bond angles
We need to do the following steps to predict and compare the bond angles for ClO2- and 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˚
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.