Make a set of molecular orbitals very much like the ones you made for linear HHH in Problem 1.64

Make a set of molecular orbitals very much like the ones you...

Key Concepts

Molecular Orbital Theory

This concept explains how atomic orbitals combine to form molecular orbitals that extend over an entire molecule, rather than being localized on one atom. It is based on quantum mechanics and is used to predict the spatial distribution and energy levels of electrons within molecules.

Linear Combination of Atomic Orbitals (LCAO)

The LCAO method is a procedure for constructing molecular orbitals by taking weighted sums of atomic orbitals. This method allows one to build orbitals that are either bonding (lower in energy) or antibonding (higher in energy), dependent on the phase relationships and the symmetry of the overlapping atomic orbitals.

Bonding and Antibonding Orbitals

When atomic orbitals combine, their interactions can be constructive, leading to bonding orbitals that are more stable and lower in energy, or destructive, resulting in antibonding orbitals that are less stable and higher in energy. Understanding these terms is crucial to predicting the stability and reactivity of molecular species.

Orbital Symmetry and Overlap

Proper combination of atomic orbitals requires that they have compatible symmetries, ensuring effective overlap. This concept is essential in determining which atomic orbitals can mix, how they split into different energy levels, and how their resulting spatial distributions influence molecular bonding.

Energy Ordering of Molecular Orbitals

Once the molecular orbitals are constructed, it is important to arrange them in order of increasing energy. This ordering provides insight into the electron configuration, chemical reactivity, and properties of the molecule, as lower energy orbitals are typically occupied before higher energy ones.

Transcript

00:01 We are going to find right here the hybridization about the central atom.

00:09 So basically, which orbitals are we're going to use to help those molecules to hybridize? so first thing that we're going to do is that we are going to draw the lewis substructure for this to find how many domains.

00:26 And according to the domains, how many orbitals are being used.

00:30 So we know that selenium has six valence electrons and chlorine has seven valence electrons, but since we have two atoms, they're 14.

00:42 So in here, i am looking at a total of 20 electrons.

00:48 So now what i'm going to do is that i'm going to draw the structure of this.

00:59 Okay, so i'm trying to do as symmetrical as possible.

01:03 And these electrons right here are telling me that i need 20 electrons around this oil atoms.

01:12 Remember that you always begin putting electrons in the outer atoms, and then if you have leftovers, you're going to complete to the center.

01:21 So i already have two and two, so there's four, meaning that i need 60 more.

01:27 So four, six, eight, and ten, twelve, four, four, four, four, four, six, eight, and ten, twelve, 12, 14, 16, 18, and 20.

01:40 Now i'm going to check that each one of them have eight electrons around.

01:46 I always said, let's check if they are happy because remember that they are extremely happy if they have eight electrons around.

01:54 So if you count the electrons around this chlorine, you see that it has eight, this chlorine has eight and this selenium has eight.

02:06 So now everybody's happy.

02:08 Now i'm going to count how many electron domains this selenium has around.

02:14 So this selenium has one, two, three, and four.

02:19 So there are four electron domains.

02:24 So if selenium has four electron domains, it means that it will have four electron domains, orbitals.

02:39 I'm going to represent those orbitals with lines.

02:42 One, two, three, and four, and then i'm going to label those lines.

02:49 Remember that we have orbitals, s, p, and f.

02:54 So, s can only have, or only have one orbital.

03:02 Then the next one in energy is p, and p has three.

03:06 So these three are going to be labeled p.

03:08 Meaning that the hybridization in here or the orbitals that that atom is using to make hybrid orbitals r1s, 1, 2, and 3ps.

03:29 Now, let's follow the same procedure for the h3o plus molecule.

03:37 H has one valence electron, but i have three atoms, so that's three.

03:45 Oxygen has six.

03:48 And in this case, i have a positive charge in here, meaning that this whole molecule is losing one electron.

03:54 So i'm going to subtract one.

03:57 And i have eight electrons in total.

04:05 Now i'm going to put my oxygen in the center.

04:09 I'm going to put three hydrogens.

04:16 And now i need to put eight electrons around.

04:20 I already have six.

04:21 Remember that hydrogen cannot have more than two, so i'm not going to touch these outer atoms.

04:29 And my leftovers is going to the center that is o.

04:34 And now everybody's happy...

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