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

h. Lewis structure of a compound showing bond formation and approximate bond angles around atoms.

Accepted Answer

Welcome back, everyone draw the Lewis structure of the given molecule and label the orbitals that overlap to form each bond and the bond angle around each atom except hydrogen. We're given a scalar structure. And essentially, we want to recall that at each corner and each vertex, we are going to observe an implicit carbon atom. So essentially, let's label those implicit carbon atoms to understand that we have a six number ring to begin with carbon is bonded to oxygen, then it is bonded to another oxygen within the ring. And we're going to add the remaining carbons to form a six number ring 123456, right? And what we notice is that our carbon atoms have a double bond within the rank. So we're also going to include that double bond carbon number 123, right. So carbons two and three form that double bond. Now, we want to introduce the missing hydrogens. Every carbon atom must have four bonds. So if our carbon does not have four bonds, we must include two, we we must include an appropriate number of hydrogens to make sure that each carbon has four bonds. So the bottom carbon has two bonds. And therefore, we need to add two hydrogens. Similarly, we're going to add one hydrogen for each double bonded carbon, which gives each double bonded carbon a total of four bonds. And we also have two additional hydrogens for the lost carbon because the top carbon already has four bonds. And now oxygen must have two bonds and two long pairs of electrons based on the octet rule. So we have the required Louis structure well done. And now we're going to consider the orbital overlap for the orb for the orbital overlap. We want to recall that carbons with four electron regions will be s sp three hybridized. So let's label our carbon atoms or basically all carbon and oxygen atoms. So 123, 456 and seven. So we have a total of seven atoms to consider except hydrogen, right? And we're going to say that the first carbon is sp three sp two hybridized because it contains three electron regions, two single bonds and one double bond carbons two and three are also SB two hybridized. So we can say that carbons 12 and three, they are all SB two hybridized based on the presence of a double bond. Meanwhile, we also have sp three hybridized atoms which are these, well, carbon 45. So four and five, right, essentially because they have four election regions. What about oxygens? Six and seven? Well, they are SB two hybridized oxygen seven has a one double bond and two L pairs. So that's SB two oxygen six, even though it appears to have four electron regions, it's actually its L pairs are conjugated within the system of the P system. Right. So essentially, we have our L pair that can be delocalized into resonance because it is an ether. So instead of having SB three oxygen, it's actually SB two. So now that we have our hybridization, we also want to recall that each hydrogen will have an un hybridized orbital for bonding. So let's answer color coding. First of all, we're going to consider our SP to you s overlap. So those would be all of the SP two carbon hydrogen bonds. For example, the bond between carbon number two and hy hydrogen would be our SB two S overlap because each carbon is SP two hybridized and Hygen uses its s orbital for bonding. Well done. So now let's consider P three S overlap in blue, which essentially means that we are observing SP three hybridized carbons bonded to hydrogens and we have 12, we four of those. Now we are done with all of our hydrogens, we essentially want to consider the bonding between our carbon atoms. So for carbons, we're going to observe, first of all SP two SP two carbon bonds, right? So let's consider SB two SB two overlap. We know that we have one of them, two of them, right? So there will be an SB two SB two overlap between Carbonis carbon and the neighboring carbon as well as an additional one between the double bonded carbon atoms. Now, in addition to that, we will also have an SB two SB two overlap between oxygen and carbon and also our sigma bond within the double bond. So those would be in green. Now, it is important to understand that we will also have the PP overlap. This is the pi bond. So within each double bond, we're going to observe the PP overlap given to us in pink. And finally, we also want to consider the SP three SP two overlap, right? So let's consider SP three SB two overlap. Those would be in red. And of course, we have one of them and that would be the overlap between we hybridize carbon and SB two oxygen. So we have one bond. And now if we consider the remaining carbons, we have an SP three sp three overlap, right? So for this one, we can use a different color, but we can also notice that if we move on, there's an SP two carbon that overlaps with an SP three carbon. So there's an additional one and the very final bond is a bond between an SP three carbon and another SP three carbon. So we can simply use a different color to illustrate that let's say that we use yellow, it's not really visible. So let's change it. Let's go with brown. And let's illustrate the SP three sp three overlap. That would be the bond between our sp three hybridized carbons. Well, then, so we have illustrated all of the orbital overlaps. And I would just want to consider the bond angles. So for the bond angles, we are just going to once again take our structure and consider the VSE pr theory. So let's essentially start with our SP two hybridized carbon from the carbonel. We know that SP two hybridized carbon would have the trigonal planar molecular geometry. So it would have a bond angle around carbon of 120 degrees. Similarly, each double bonded carbon will have the same bond angle 120 120 right now, when we are considering our SP two auction as well, right, we want to do, we are going to essentially say that the bond angle that we are observing would be 120 degrees approximately. What about the SP three carbons? Well, we know that they will have tetrahedral geometry. So we're expecting to observe bond angles of around 109.5 degrees for each 109.5 degrees. And that's it. We have the required bond angles around central carbons and oxygens. Well, then let's label our answer for this part. And if we look back at the previous parts, we also have our Louis structure and the Lewis structure that also illustrates the orbital overlap. We have our legend or each overlap. 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
h.

Key Concepts

Lewis Structures

Orbital Overlap and Bond Formation

Bond Angles and Molecular Geometry

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