We’re being asked to identify the bond angle in ICl4+. Since we don’t know the Lewis structure for ICl4+, 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˚
What are the expected bond angles in ICl4+?
d. 180 °
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Our expert Chemistry tutor, Dasha took 3 minutes and 52 seconds to solve this problem. You can follow their steps in the video explanation above.
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Based on our data, we think this problem is relevant for Professor Guerra's class at RUTGERS.