Draw a Lewis structure for each of the following species: a. CH3 N2 b. CH2 N2 c. N3^- d. N2 O (a

step 1 So here we are asked to draw different Lewis structures. Our first compend is CH3 and 2. So basi

Draw a Lewis structure for each of the following species: a....

Key Concepts

Resonance Structures

Resonance structures are alternate Lewis structures for a single molecule that depict different possible distributions of electrons, especially in systems where electrons are delocalized. These structures are used to represent molecules or ions that cannot be adequately described by a single static structure, providing insight into areas of electron density that contribute to the overall stability and reactivity of the species.

Formal Charge Calculation

Formal charge calculation involves assigning electrons in a Lewis structure to individual atoms based on bonding and non-bonding pairs, then comparing this number to the atom's standard valence electron count. The goal is to minimize formal charges across the molecule, as structures with lower formal charges are generally more stable and more representative of the actual electron distribution.

Octet Rule

The octet rule is a guideline that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, similar to the electron configuration of noble gases. Although there are exceptions—such as molecules with an odd number of electrons or elements in higher periods that can expand their octet—this rule provides a useful benchmark for arranging electrons and determining the structure of molecules.

Valence Electron Counting

Valence electron counting is the process of summing all electrons available for bonding from each atom in a molecule, including any additional electrons from negative charges or subtracting those due to positive charges. This concept is fundamental in constructing Lewis structures because it ensures that all electrons are accounted for when forming bonds and lone pairs, establishing the basis for predicting molecular structure.

Transcript

00:01 So here we are asked to draw different lewis structures.

00:04 Our first compend is ch3 and 2.

00:07 So basically, first we can count up the number of valance electrons, so 2 times 5, plus 4 for carbon, plus 3 times 1 for hydrogen.

00:18 So this is 17.

00:19 So since it's an odd number, this likely implies that there's going to be some type of a free radical somewhere.

00:30 Although we could check basically if there's a structure without a free radical, that would likely be more stable.

00:36 So we can first try by drawing our structure out.

00:40 So c, h with three hydrogens.

00:46 Then we can have our nitrogen.

00:49 So now we have to decide whether or not we need two or three bonds on nitrogen.

00:54 So here we have 2, 4, 6, 8, 10, 12.

00:58 So we have 5 more possible electrons remaining.

01:02 So the only way that this would be satisfied would be some form like this.

01:08 But this also has many different contributing resin structures that we could also possibly draw, but this is one possible lewis structure for this species.

01:20 And so for part b, we're asked to draw ch2n2.

01:25 And this we have an even number of electrons.

01:30 Since we have one less hydrogen atom, this would be 16 valence electrons.

01:36 So this would become ch2.

01:38 So we have to make sure that we satisfy essentially the number, the correct number of everything.

01:48 So here, this would be 246, 8, 10, 12, 14, then this would be 16.

01:58 But that would leave a carbocat ion here.

02:02 So that's not relatively stable, so we would likely try to look for something more stable than a carbocat ion.

02:09 So we could possibly have this type of structure.

02:11 So this would become c double bond to n, double bond to n, and this is another possible resin structure.

02:28 Generally, carbon ions are relatively unstable, so anything other than carbon ions are more strongly favored.

02:35 So in this case, we can check again.

02:36 We have four valance electrons here, and total charge is zero, which satisfies our initial compound.

02:42 So four plus eight here, 12, and 12, 14, 16.

02:47 So this is satisfied.

02:49 So for part c, we're asked to draw n3 minus...

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