Draw a picture of 2 NO2 molecules colliding with the proper orientation to produce 1 N2 O4 mole

step 1 Alright, to this question, we're drawing low structures. So first off, we have C2H4. Now, the fi

Draw a picture of 2 NO2 molecules colliding with the proper...

Key Concepts

Dimerization Reaction

A dimerization reaction involves the combination of two identical molecules to form a single, larger molecule. This concept is key in understanding how individual molecular units can bond to create more complex structures through a process that is sensitive to molecular orientation and energy.

Reaction Mechanism

The reaction mechanism is the step-by-step description of the process by which reactants transform into products. It includes details about the intermediate states, transition states, and the specific orientation of colliding molecules, which are all critical for predicting and visualizing the course of the reaction.

Collision Theory

Collision theory explains that chemical reactions occur when reactant molecules collide with sufficient energy and the correct orientation. It emphasizes that not all collisions result in chemical reactions, as only those with the proper conditions can overcome the activation energy barrier.

Molecular Orientation

Molecular orientation refers to the spatial arrangement of molecules as they approach one another during a collision. Correct orientation is crucial for effective collisions, ensuring that the reactive sites of the molecules are properly aligned to facilitate bond formation or breaking.

Transcript

00:01 Alright, to this question, we're drawing low structures.

00:03 So first off, we have c2h4.

00:06 Now, the first step to drawing a low structure is to calculate how many valence electrons you're working with.

00:11 So for carbon, carbon has four valence electrons because it's in group 4a.

00:17 So we have four electrons for each of the carbons, and we have two carbons.

00:23 And then for hydrogen, we have one electron for each hydrogen, and we have four of them.

00:28 So that's four electrons.

00:30 Well, to be consistent, i'll put 1 times 4.

00:35 That equals a total of 12 electrons that we need to distribute.

00:39 So let's first start by drawing a carbon.

00:43 We know from this equation that, or we can at least infer, that the two carbons are bonded, and we have four hydrogens.

00:52 So i'm going to put two hydrogens on each of the carbons.

00:58 So we're fairly certain that this is the very base structure of our compound that we'll probably have to add some electrons to or double bonds to.

01:09 But let's just start by saying where we are at.

01:12 So each bond, remember, contains two electrons.

01:17 And we have five bonds in this compound so far.

01:21 So two times five, that means that's 10 electrons out of the 12 we've used up.

01:28 Now where do we put these last two electrons? we could try putting them on one of the carbons, but that leaves the other carbon with only six electrons.

01:44 So we try splitting them like this.

01:46 Well, let's count the electrons.

01:48 This carbon has three bonds, so six electrons in those bonds, plus a single electron.

01:55 So this carbon has seven electrons.

01:57 That's not enough.

01:59 So the answer is we could draw another bond between the two carbon atoms.

02:06 This way, this carbon has eight electrons because that has four bonds, two electrons per bond, and so does this carbon.

02:18 And that bond uses up the last two electrons.

02:22 So this is the lewis structure for c2h4.

02:29 Our next molecule that we're asked to draw is n2h4.

02:38 So let's start by drawing out, well, let's start by adding...