Draw as many resonance structures as you can for the following species, adding appropriate forma

Draw as many resonance structures as you can for the...

Key Concepts

Stability of Resonance Structures

The stability of resonance structures is assessed by factors such as the minimization of formal charges, the use of full octets where possible, and the placement of negative and positive charges on electronegative and electropositive atoms, respectively. These criteria help determine which resonance forms make the greatest contribution to the resonance hybrid.

Lewis Structures

Lewis structures are drawings that represent the bonding between atoms of a molecule and the lone pairs of electrons. They provide the foundation for constructing resonance structures and evaluating electron distribution, making them a key component in understanding molecular structure and reactivity.

Resonance Structures

Resonance structures are different valid Lewis representations of a molecule that illustrate the possible delocalization of electrons. They depict variations in electron distribution while the positions of the atoms remain unchanged, providing insight into electron delocalization and contributing to a better understanding of the molecule's stability.

Formal Charge

Formal charge is a tool used to assign charges to individual atoms in a molecule based on the difference between an atom's valence electrons and the electrons assigned to it in a Lewis structure. It is crucial for determining the most stable resonance form, as structures with minimized formal charges are generally favored.

Electron Delocalization

Electron delocalization refers to the spreading of electron density over multiple atoms rather than being confined to a single pair of atoms. This phenomenon, explained by resonance, allows for greater molecular stability by distributing charge and lowering electron-electron repulsion in the molecule.

Transcript

00:01 They want us to draw as many resident structures as we can for the following species and making sure we add appropriate formal charges.

00:09 So let's go ahead and start with nitromethane here.

00:14 Now the most natural resonant structure, i would think, to start with, is going to be, well, we could move one of these lone pairs from this oxygen towards the nitrogen.

00:26 And then between this nitrogen and this double bonded oxygen, we could break that bond and move one of the lone pairs up like that.

00:38 And in doing that, we would have...

00:43 So now up top here, this oxygen would have three lone pairs because i had two before and accepted one.

00:49 So it was neutrally charged, but it accepted an electron.

00:52 So it's essentially negatively charged now.

00:54 And then over here, this oxygen went to go form that double bond and it should have two lobe pairs since it donated one and it should go from negative to neutrally charged.

01:11 And now our nitrogen here accepted a bond and lost a bond, so it would be positively charged still.

01:17 So the charge wouldn't change on it.

01:21 Now maybe i should probably say, so like this nitrogen, or this carbon over here, just has three hydrogens attached to it.

01:29 There is no loan pairs or anything like that, and it can't take care.

01:33 Accept any bonds.

01:34 So for the residents, this carbon is just kind of coming along for the ride.

01:38 We can't do anything to that one.

01:41 All right.

01:41 So now that's the most natural resident structure.

01:45 But we could do another one, one that probably isn't very likely, but still a resident structure, nonetheless.

01:51 Well, what if we just moved this lone pair, or this double bond to form a loan pair there and we didn't move anything else.

02:00 So now that oxygen up top, nothing changed for it.

02:05 It would still have that negative charge.

02:07 But now this other one would also have a negative charge on it.

02:11 So then this nitrogen lost a bond.

02:16 So that means it would gain a plus charge.

02:21 So now it should be two plus instead of just plus one.

02:26 Now this one isn't very likely at all.

02:28 Because having that plus two charge on pretty much any of the non -metals is very unlikely, but i mean, we can still draw this out.

02:40 All right.

02:42 Now what about for ozone here? well, we could do the more obvious one to start, kind of like what we did before.

02:53 We would first move one of the lone pairs from the oxygen on the right to form a double.

03:00 Bond with oxygen in the middle, but now that oxygen is going to have too many electrons in its octet, because it would have 10.

03:07 So then that would mean we would move the double bond over here to that one.

03:14 So that's going to give us.

03:16 So the oxygen on the end now should have, or on the left end, should have three lone pairs, but it was neutral.

03:23 It gained an electron, so now it's negatively charged...

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