For each of the following compounds and ions,
1. Draw a...

Question

For each of the following compounds and ions,

1. Draw a Lewis structure.

2. Show the kinds of orbitals that overlap to form each bond.

3. Give approximate bond angles around each atom except hydrogen.

b. [CH₂OH]⁺

Accepted Answer

Welcome back everyone to another video. What is the Louis structure for the CH three cohh with a positive charge ion? What are the orbitals that cause the overlap in each of its bonds? What are the bond angles around each of its atoms except hydrogen? Now, first of all, we want to draw the Louis structure of the given ion. And for simplicity, we want to recall the valency of each atom involved val is the number of bonds that an atom makes in a specific compound. So let's suppose that we choose carbon, right? Because it is in our, in our structure, hydrogen and oxygen carbon has the eval of four. There are four bombs. Hygen has the avail of one and oxygen has the eval of two. It has two L pairs which essentially compensate for the teal. And now to draw the result of iron, we can just read it from left to right. First of all, we have CH three and what we're going to do is just draw carbon with three hydrogen atoms bonded, set each hygen forms a single bond. So we are good and our carbon has three bonds, meaning it needs an additional bond, this carbon is bonded to the other carbon in our structure when we read it from left to right. So we're essentially adding the next carbon. And in parenthesis, we indicate that the oh group is bonded to that previous carbon. Meaning we simply want to indicate that alcohol group, we are firstly adding oxygen and then hydrogen oxygen forms two bonds and therefore, it must have two long pairs. So we are done with the part and parentis and the next atom that we have is hydrogen, meaning it's bonded to the previous carbon, we are going to add that hydrogen. And now we can consider our structure. Let's first of all understand if everything is correct. So the carbon atom in question actually has we bonds. So we can see that it gets the positive charge within our ion, but carbon does not have an octet. And we, we can essentially draw a resonant stabilized form where the long pair of oxygen is used in the formation of a P bond. So what we're going to do is just remove one of the two lone pairs of oxygen and use it in the formation of a pi bond between carbon and oxygen, which provides that carbon with an octet. So now that carbon has an octet and oxygen gets a formal positive charge because instead of having two bonds and two lump pairs, it has three bonds and one lump pair. And this will be the structure of our iron. Now, what we want to do from here is identify the orbitals involved in each bond. First of all, let's remember that hydrogen, whenever it bonds to an atom utilizes its s orbital, when we think about carbon, we want to find its hybridization. So carbon number one or the left carbon, let's suppose that we call it carbon left has four electron regions or basically four single bonds. And that means it is sp three hybridized carbon on the right has three electron regions. In particular, it has two single bonds and one double bond. And this makes it sp two hybrids. Finally, oxygen has three election regions. It has one single bond, one double bond and one lone pair. Therefore, it is also sp two hybridized. So now we can utilize this information to state what orbitals are involved in each bond formation. First of all, we noticed that our three carbon hydrogen bombs, we can label them, all of them are obtained by the overlap of the s orbital of hydrogen and the sp three orbitals of carbon. So we can say that the overlap represents the SP three S overlap where all of the three carbon hygen bonds. When it comes to our carbon carbon bond, we have to understand that the left carbon is sp three hybridized and the right one is sp two hybridized. So we have an overlap in the form of SB two SB three. Now, when we consider our carbon hydrogen bond. We already said that hydrogen will use its s orbital and the carbon in question is sp two hybridized. So we're going to say that we have an SP two S overlap. In addition to that, when we consider our oxygen hydrogen bond, we can say that this is an SP two S overlap because oxygen is sp two hybridized and we have hydrogen which uses its S orbital. And finally, we actually want to consider our double bond. Let's remember that double bonds consist of one sigma and one pi bond. The pi bond is obtained by the overlap of the P orbitals. And for the sigma bond, we will use the same strategy as before carbon oxygen sigma bond is obtained by the overlap of the SP two orbitals. So we're going to say that we have our SP two sp two overlap. And in addition to that, we have our pp overlap because we are also forming a pi bond. And not just sigma. Finally, we will find the bond angles around the two carbon atoms and oxygen. And for that purpose, we want to recall the vs er theory according to the electronic geometry, if an atom is sp three hybridized, it will form a tetrahedral electronic geometry with a bond angle of 109.5 degrees. NSB two hybridized atom will form trigonal planar geometry with a bond angle of 120 degrees. So we can say that the bond angles around the left carbon, which is sp three hybridized will be 109.5 degrees. For the white carbon, we can essentially say that the bond angles will be 120 degrees because it's, it is sp two hybridized. And for the oxygen, which actually forms a bond structure because it's sp two hybridized, the bond angle will be approximately 120 degrees. So we can say that oxygen will also form a bond angle of about 120 degrees. Now, we are going to label our final answer with the bond angles, our loose structure and the orbitals involved in the bond formation. That's be our final answer. And thank you for watching.

For each of the following compounds and ions,
1. Draw a Lewis structure.
2. Show the kinds of orbitals that overlap to form each bond.
3. Give approximate bond angles around each atom except hydrogen.
b. [CH₂OH]⁺

Key Concepts

Lewis Structure

Orbital Overlap

Bond Angles

Watch next