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Rice University

Drexel University

University of Maryland - University College

Numerade Educator

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so like before we see that we can combine the atomic orbital's to make molecular orbital's specifically for our last example. We've seen how we can combine the S orbital to make the Sigma and Sigma stock. And so if we go back thio our introduction, we know that we can combine the P atomic orbital's to create Thesiger Mama single star as well as the pie and pie star Molecular Orbital's. And so let's look at a few examples where we see die atomic molecules with P orbital's that can be combined to make thes type of or bills. And so, for example, let's look at B two. And so for B two we have as orbital's as well as Thebe or rules. And so let's recall that energy is increasing and we have the two p for the other one. And so again, when we combine these orbital's the case of us, we have the Sigma and single star and since we have three for the PS for each atom, we can have a total of six for the P orbital's, and so the energies would be why, which is specific between boron through nitrogen. But we'll see that the energy changes once we go into the M O diagrams for option and flooring us well as yeah, and so we have. Why star as well, a single star. And so this is the general diagram that you'll see for BP Orbital's. So let's just quickly show well, using the fewer rules. We can make different types of M O or rules, and so it's important to label these all right? And so this is the general, um, well, that will be using for the following examples. And so first, let's look at be to so this is essentially two bronze. And so let's recall that the electron configuration is one is to to us to and to be one. And so for this one, we actually just need to look at the highest energy levels. And so we don't need to look at the ones, too, because it's basically the same thing. That's to us, too. And so we'll be drawing the M O diagram specifically for the second energy level. And so again we need Thio Ad de Valence electrons for each one. And so when we draw the about diagram, we should expect to see six electrons in the and so now we just need to fill up the electrons based on energy level and so we can fill the M O orbital's for the acids, and now we can add the electrons. And so this would be your M O diagram for B two, because we have three that can participate in the overlap of the atomic orbital's. And so we basically again full of the electrons from Lois largest energy, and so we can see that the electrons and the P orbital will participate in the pie orbital's. And so these are the orbital's that are involved with mixing, and so we'll see the significance of that as we go into a few more. And so let's look at a case where we are looking at the bond between carbon and carbon. And so let's recall that the electron configuration is one us to to us to and to p two. And so this has one extra electron boron, and so we can stop us up in a similar way and so we can fill in the sigma and sing the star. And then, from there we can fill in all of the atomic orbital's. And so this would be our I'm a diagram for Carbon. And now let's look at the M O diagram for nitrogen. And so Nitrogen has a pretty similar diagram as well. Accept it now has an extra electron in the atomic orbital's. And so let's recall that the electron configuration is want us to to us two and tp three. And so we have to end the US and we have three p, and we can draw the same thing on the other side and save ranting. We can fill this up like before, except in this case. Now we have electrons in the single and so this makes sense because we have five electrons for the atomic orbital's for each one. And so we should see 10 in the m O diagram, which we see. And so this would be the M O diagram for unto