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Predict whether each of the following mo...

Predict whether each of the following molecule has a dipole momnet
(a) `BF_(3)` (b) `IB r` (c ) `CH_(2)CI_(2)` .

Text Solution

AI Generated Solution

To determine whether each of the given molecules has a dipole moment, we need to analyze their molecular structures, electronegativity differences, and symmetry. Let's go through each molecule step by step: ### Step 1: Analyze BF₃ (Boron Trifluoride) 1. **Structure**: BF₃ has a trigonal planar structure, with Boron (B) at the center and three Fluorine (F) atoms at the corners of an equilateral triangle. 2. **Electronegativity**: Fluorine is more electronegative than Boron. Therefore, each B-F bond is polar, with the dipole moment directed towards the Fluorine atoms. 3. **Symmetry**: The molecule is symmetrical. The three dipole moments from each B-F bond point towards the Fluorine atoms and are equal in magnitude but opposite in direction. 4. **Conclusion**: The dipole moments cancel each other out due to symmetry, resulting in a net dipole moment of zero. ...
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