🤓 Based on our data, we think this question is relevant for Professor Pelton's class at UMN.
Explain why the following ions have different bond angles: CLO2- and NO2-. Predict the bond angle in each case.
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˚