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Lewis structure of acids and bases

Posted: Sat Dec 07, 2019 8:42 pm
by Hannah_1G
When figuring out the lewis structure of an acid or base, should you stay away from double or triple bonds even if it stabilizes the molecule? Do the bonds make it have less acid/base characteristic. In all of the examples I've seen of finding if a molecule is an acid or base from the lewis structure, double bonds are hardly used even though the molecule is more stable with one, e.g., SO3 and B(OH)3.

Re: Lewis structure of acids and bases

Posted: Sat Dec 07, 2019 8:57 pm
by Manav Govil 1B
The filling of the octets is the most important aspect - double and triple bonds come in later. Double bonds should be used when both the central and attached atom has an extra lone pair each, and if the formal charge conditions are most favorable. I am not sure what you are talking about regarding SO3, but SO3 has three double bonds - making it very stable.

Re: Lewis structure of acids and bases

Posted: Sat Dec 07, 2019 9:03 pm
by Hannah_1G
Manav Govil 4A wrote:The filling of the octets is the most important aspect - double and triple bonds come in later. Double bonds should be used when both the central and attached atom has an extra lone pair each, and if the formal charge conditions are most favorable. I am not sure what you are talking about regarding SO3, but SO3 has three double bonds - making it very stable.

In hw. 6.5 SO3 is drawn in the book with one double bond and two single bonds which is less stable than three double bonds, but it's acting as an acid.