(Polar molecules, Non-polar molecules, etc.)
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4.81 is asking for the Lewis structure of the borazine (B3N3H6). the boron and nitrogen molecules alternate to form a hexagon core where each one is also attached to one hydrogen. In the solutions manual it has a double bond for every other bond in the hexagon. However, this means the nitrogen have a formal charge of +1 and the borons have a formal charge of -1. Why are all the bonds not single bonds with lone pairs on the nitrogen. This would mean no atoms have a formal charge. I am aware boron would not have a full octet, but I though they were an exception to this rule.
The wording of the question gives you the hint that borazine will have an alternating single and double bond structure like benzene. This arrangement leads to the phenomenon of "aromaticity" which, like in benzene, makes the molecule significantly more stable than if it had all single bonds.
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