-2
$\begingroup$

Basically, my concepts regarding Resonance are not totally clear. I just need some help, on how to find the no. of resonating structures, given a molecule, and how do I draw those structures. Some examples would be pretty helpful. Thanks 🙂

$\endgroup$

closed as too broad by Jan, Zhe, Todd Minehardt, ron, paracetamol Jan 20 '17 at 3:47

Please edit the question to limit it to a specific problem with enough detail to identify an adequate answer. Avoid asking multiple distinct questions at once. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.

-1
$\begingroup$

Essentially, resonance structures are explained by Resonance Theory. Resonance theory looks to answer the question: How do we reconcile the differences between Lewis Structures of species and their observed characteristics? There are a few rules that must be followed when determining resonance of compound.

  1. Resonance occurs in species for which there are two or more valid Lewis structures.

For a species, each valid Lewis structure is called a Resonance Structure or Resonance Contributor. In these cases, you are simply moving an electron or pair of electrons to another location in a molecule. An example is HCO2-.There are two possible resonance contributors in this molecule. As shown in the example, resonance structures differ only in the placement of their valence electrons, not their atoms.

  1. Resonance structures are imaginary; the one, true species is represented by the resonance hybrid.

The Resonance Hyrbid is the weighted average of all resonance structures. An example of the resonance hybrid occurs in either of these molecules.

  1. The resonance hybrid looks most like the lowest energy (most stable) resonance structure. Essentially, the least formal charges on the molecule, or most evenly distributed charges.

A few tips I have for drawing resonance structures based on Lewis structures for different molecules include:

  1. Move away from a negative charge. If presented with a negative charge on a specific atom, it means that there is an excess of electrons on that atom. Either take electrons away from the atom, or move a bond that it is involved in.

  2. Move towards a positive charge. A positive charge represents a lack of electrons, this means that you should move electrons to the atom with the charge, or move a double/triple bond to allow it to become involved in another bond.

  3. Move away from a radical. A radical does not represent a charge, as it is only a single electron, but you should (in most cases) move electrons away from the radical.

Also, always remember that electrons are the only things that move in resonance structures. They can also not be added or subtracted, but only moved. Make sure not to move/add/remove any atoms, and you cannot move electrons to an atom that is already saturated with bonds for example, an sp3 hybridized Carbon as it is already saturated with Hydrogens.

Best of luck!

$\endgroup$
  • 1
    $\begingroup$ Wow. Thanks. That should hopefully clear some facts for me 🙂 $\endgroup$ – Bhavya Jan 20 '17 at 0:56
  • $\begingroup$ Yeah for sure, let me know if there are any other questions that I can help with! :D $\endgroup$ – BrendynStLouis Jan 20 '17 at 0:56
  • 1
    $\begingroup$ 1. There are more than two resonance contributors in $\ce{HCO2-}$. 2. There is no most stable resonance structure! 3. "Essentially, the least formal charges on the molecule, or most evenly distributed charges." This might be purely based on experience and is not at all true. The prime counter example is CO. $\endgroup$ – Martin - マーチン Jan 20 '17 at 7:02

Not the answer you're looking for? Browse other questions tagged or ask your own question.