Open study

is now brainly

With Brainly you can:

  • Get homework help from millions of students and moderators
  • Learn how to solve problems with step-by-step explanations
  • Share your knowledge and earn points by helping other students
  • Learn anywhere, anytime with the Brainly app!

A community for students.

Why is it so that covalent bonds don't have formal charges?

Chemistry
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

Get this expert

answer on brainly

SEE EXPERT ANSWER

Get your free account and access expert answers to this and thousands of other questions

hmm...a bunch of covalently bonded organic molecules can be represented by lewis structures with formally charged atoms. i believe ozone is an example.
Yes, but how does it (O3) attain formal charge as it is a covalent bond and covalent bond has equal sharing.
I think, it will include coordinate bond.

Not the answer you are looking for?

Search for more explanations.

Ask your own question

Other answers:

Please check the attachment. I have included the "coordinate bond" there.
1 Attachment
i don't understand your concern...formal charges are assigned by a set of rules that humans (not mother nature) made up. sometimes they can be completely wrong, as in they give us a wrong idea of what the electronic distribution actually looks like. btw, i think your idea of "coordinately bonded" O3 is highly controversial. but that's beside the point.
Well, @gsoda can you draw the structure without the coordinate bond Do you accept that O3 has a covalent bonding?
of course, i can draw one lewis structure of O3 with regular covalent bonds, and it's going to have formal charges. conventionally speaking, there's also going to be resonance and so on, but it's not the point. yes, i accept that O3 has covalent bonding, but I am not going to say your picture is incorrect just because it looks a little funny to me. why do we fixate on O3 though? what about azide and other example? are you going to say they are all coordinately bonded?
NO @gsoda , I am not against you but I just want to clear my doubt. Well, why is it funny to you? Anything wrong?
Please let me know the mistake.

Not the answer you are looking for?

Search for more explanations.

Ask your own question