Describe the hybrid orbitals used by the central atom(s) and the type(s) of bonds formed in (a)

Describe the hybrid orbitals used by the central atom(s) and...

Key Concepts

Hybridization

Hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that are better oriented for bonding. This concept explains how atoms combine their orbitals (such as s and p orbitals) to form orbitals like sp, sp², or sp³, which then overlap with orbitals on other atoms to form bonds. The type of hybridization influences molecular geometry and bond angles, and it is fundamental in rationalizing the bonding patterns in many molecules.

Sigma Bonds

Sigma bonds are the primary bonds formed from the head-on overlap of hybrid orbitals or an overlap between an sp hybrid orbital and an unhybridized p orbital. These bonds are characterized by their cylindrical symmetry along the bond axis and are generally stronger than other bond types. In many molecules, every bond, whether part of a single, double, or triple bond, includes one sigma bond which contributes significantly to the structural rigidity of the molecule.

Pi Bonds

Pi bonds are additional bonds that form in the presence of multiple bonding (double or triple bonds) and result from the side-on overlap of unhybridized p orbitals. These bonds, which lie above and below the plane of the atoms involved, are generally weaker than sigma bonds and contribute to the formation of double and triple bonds. The presence of pi bonds restricts rotational freedom around the bond, impacting the overall molecular conformation.

Transcript

00:01 This program is asking us to find the hybrid orbitals used by the central atom in addition to the types of bones form.

00:13 So let's begin with the first molecule.

00:17 So the first thing that you need to do is that you need to draw the lewis dot structure to be able to find the hybridization of the central atom.

00:26 And in addition to find the type of bonds, sigma and pi bonds.

00:31 So you know that fluorine has seven electrons, nitrogen has five valence electrons, and then oxygen has six valence electrons.

00:47 So we are looking at a total of 18 valence electrons in our molecule.

00:53 So what we're going to do is that we're going to place nitrogen in the center, oxygen, and fluorine.

01:01 Now that we have the skeletal formula, we're going to start putting electrons.

01:06 Around the outer atoms and remember once those are filled with eight then you can move to the center so you already have two four six eight ten twelve fourteen sixteen and eighteen oh no but what happened nitrogen is not happy but you know that oxygen can form double box so what you're going to do is that you're going to move these two electrons that i just erase and you're going to make a double bond and now everybody's happy.

01:51 So now let's count.

01:54 Nitrogen is the central atom.

01:56 Nitrogen has one, two, and three domains around.

02:03 So nitrogen has one, two, and three domains.

02:09 The first equals to the s orbital, the second one equals to the p orbital.

02:17 So this nitrogen in this molecule has an sp2, hybridization, and now let's count sigma and pi bonds.

02:32 So you have one sigma, two sigma bonds, and then you have one pi bond.

02:46 Now let's move to this molecule.

02:49 Carbon is 4, has 4 valence electrons, so you have 2.

02:53 That means that this is 8 valence electrons.

02:56 Florine has 7 electrons, but you have 4 of them, so this is 28 electrons, meaning, okay, that we're going to have a total of 36 electrons.

03:16 So how we're going to do this? i have a c and i have another c and this c is going to have one f.

03:24 This c is going to have another f.

03:27 This c is going to have another f and this c is going to have another f.

03:34 And now we need to put 36 electrons around and we already have 2, 4, 6, 8 and 10, 12, 14, 16, 18, 20, 22, 24, 26, 28, 30, 32, 34, 30, 32, 34...

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