What orbitals are used to form each bond in the following molecules? a. CH3BeH b, (CH3)3B c. CH3

What orbitals are used to form each bond in the following...

Key Concepts

Atomic Orbitals

Atomic orbitals are the basic regions in an atom where electrons are found, such as s and p orbitals. They describe the electron density and come with specific shapes and orientations, which serve as the starting point for bonding interactions.

Hybridization

Hybridization is the process of mixing atomic orbitals (like s and p) to form new, equivalent hybrid orbitals that better accommodate bonding with other atoms. This concept is used to explain molecular geometries and the directional nature of bonds, such as sp, sp², and sp³ hybridization.

Sigma (?) Bond Formation

Sigma bonds are a type of covalent bond resulting from the head-on overlap of orbitals. Whether the overlaps occur between hybrid orbitals or between a hybrid and an unhybridized orbital, sigma bonds are typically the strongest and primary bonds in a molecule.

Orbital Overlap

Orbital overlap refers to the way atomic or hybrid orbitals come together to form molecular orbitals. Effective overlap is crucial for bond formation, as it influences the strength and stability of the resulting bond by enabling the sharing of electron density between atoms.

Transcript

00:01 This problem asks you to determine which orbitals are overlapping in order to form a bond, for instance, between carbon and beryllium, or between carbon and hydrogen for each of these three molecules.

00:11 The way to go about this problem is first to determine which orbitals are being used by which atoms.

00:18 So you want to figure out the hybridization.

00:21 Well, hydrogen only ever can contribute an s -orbital to orbital overlap.

00:27 Carbon in this case has four groups attached to it, meaning it's sp3 hybridized.

00:33 And borrelium in this case only has two bonds, therefore it's sp hybridized.

00:38 Then when you're looking at each individual bond, you can figure out what is actually overlapping, and that's your answer.

00:45 So, for instance, just to show you what the overlap looks like, are made of lobes coming off of each center of the carbon to make a tetrahedral.

00:52 That gets the four groups as far apart as possible, making it the most.

00:56 Stable and lowest in energy.

00:59 We can do the same thing for the other hydrogens, as well as for the beryllium carbon bond.

01:04 And i've just drawn that in green just because it's a different hybridized orbital.

01:09 So the carbon hydrogen bonds, all of them, all three of them, are made up of an s hydrogen orbital overlapping with a carbon sp3 orbital.

01:19 So the answer for say this bond is carbon sp3 overlap with hydrogen s.

01:26 You could also write that as well, hydrogen s overlapping with carbon and sp3.

01:30 But this is typically how we draw it.

01:33 If we look at the carbon beryllium bond, well, we have a carbon sp3 hybridized orbital overlapping with a beryllium sp hybridized orbital...

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