If we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9

If we assume that the energy-level diagrams for homonuclear...

Key Concepts

Magnetic Behavior

The magnetic behavior of a molecule depends on the presence or absence of unpaired electrons in its molecular orbitals. Molecules with unpaired electrons exhibit paramagnetism and are attracted to magnetic fields, whereas molecules with all electrons paired are diamagnetic and are weakly repelled by magnetic fields.

Molecular Orbital Theory

This theory describes the formation of molecular orbitals by the linear combination of atomic orbitals. It explains how electrons are distributed in molecules across bonding and antibonding orbitals, which in turn determines a molecule's chemical bonding, bond order, and magnetic properties. Understanding the ordering and energy levels of these orbitals is essential for predicting molecular behavior.

Bond Order

Bond order is a measure of the strength and stability of a bond within a molecule. It is calculated by taking the difference between the number of electrons in bonding orbitals and antibonding orbitals and dividing by two. A higher bond order indicates a stronger bond, while a bond order of zero implies instability or a nonexistent bond.

Transcript

00:01 All right, guys, we're doing problem 80 of chapter 9 in chemistry, central science.

00:06 So if we assume the energy level diagrams for homonuclear diatomic ion shown a figure, 9 .43 can be applied to heteronuclear diatomic molecules and ions.

00:16 We predict the bond or magnetic behavior of these molecules.

00:20 So let's go here.

00:22 So we're going to start with co plus.

00:31 So we first have to look at the electron configuration of carbon, which is helium, 2s2, 2p2, and oxygen 2s2, 2p4.

00:44 Now, we're going to have one of our, since we have a positively charged ion, one of our atoms is going to lose an electron.

00:54 In terms of like what we draw on our diagram, it doesn't particularly matter.

00:59 So i chose oxygen is going to lose that atom.

01:04 So now we have our non -bonding, our electrons in our non -bonding orbitals.

01:10 So we're going to put that into our bonding orbitals.

01:15 So we fill up, so we have five electrons in total.

01:18 So we have two in our sigma bond, two in our sigma orbital, two in our pi orbital.

01:27 Oh, and one in our other pi orbital.

01:35 So then, so you can see that we have one unpaired, electron.

01:42 So that means that we are going to be paramagnetic.

01:54 Now we're going to look at our bond order.

02:03 So if we look at our bond order, we have filled up electrons in one, in our sigma orbital, and also in one of our pi orbitals.

02:13 And we are half filled in the other pi orbital.

02:16 So our bond order is going to be somewhere between two and three.

02:25 So let's approximate it and say 2 .5.

02:34 Now, let's look at no.

02:36 So we have our nitrogen with three electrons, and we have our oxygen, and we have our oxygen with four electrons into p orbital.

02:49 And then we have another electron because we have no minus.

02:53 So now we, as i just gave that to my nitrogen.

02:59 So now we take our electrons in our non -bonding orbital.

03:01 We're going to put them in our bonding orbital.

03:03 So we're going to have a fill up our sigma, both our pi.

03:07 Orbitals and then put an electron each of our antipi orbitals.

03:14 So it looks like that, it looks like the bond.

03:21 Well, first of all, our substance is going to be paramagnetic because we have unpaired electrons in our antipy orbital.

03:38 And our substance is going as and our bond order, we have filled out the orbitals for single, double and triple bonds.

03:51 We have two electrons in our anti -pie orbital.

03:54 So these two electrons are going to weaken our bonding.

03:58 So you can approximately you can think of each bond, each electron anti -pi orbital as dropping our bond order down by 0 .5...

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