Problem: Draw Lewis structures for BF3 and (CH3)2BF. (The formal charges should be minimized in each.)The B-F distance in both molecules is the same (130 pm). Does this observation support the argument that all the boron-fluorine bonds in BF3 are single bonds?a. Yesb. Noc. Cannot be determined

FREE Expert Solution

We are going to do the following steps to draw the Lewis structure:

Step 1: Calculate the total number of valence electrons present.

Step 2: Draw the Lewis structure for the molecule.


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Problem Details

Draw Lewis structures for BF3 and (CH3)2BF. (The formal charges should be minimized in each.)


The B-F distance in both molecules is the same (130 pm). Does this observation support the argument that all the boron-fluorine bonds in BF3 are single bonds?

a. Yes

b. No

c. Cannot be determined

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