Write the Lewis structures for the following, and include...

Key Concepts

Bond Order

Bond order is a concept that quantifies the number of chemical bonds between a pair of atoms. It is calculated by taking into account bonding and antibonding interactions, especially in cases involving resonance where multiple structures contribute. A higher bond order generally correlates with a stronger, shorter bond, and it is an important factor when comparing bond strengths in different molecules.

Lewis Structures

Lewis structures are diagrams that represent the arrangement of valence electrons around atoms in a molecule. They use dots to denote valence electrons and lines to indicate bonds between atoms. This approach helps in visualizing how atoms share electrons to form molecules and is fundamental in understanding molecular geometry and reactivity.

Resonance Structures

Resonance structures are multiple valid Lewis representations of a molecule that cannot be accurately depicted by a single structure. They show how electrons may be delocalized within the molecule, contributing to an overall resonance hybrid that better describes the true electron distribution and can influence properties like bond lengths and stability.

Bond Strength

Bond strength refers to the energy required to break a bond between two atoms. It is closely related to the bond order and electron distribution in a molecule. Stronger bonds, which typically have higher bond orders and more effective electron sharing or delocalization, require more energy to break. Understanding bond strength is crucial when comparing molecules, such as determining which molecule has a stronger carbon-oxygen bond.

Transcript

00:01 Good day.

00:02 In this video, we are going to write down the lewis structures and the resonance forms of the following molecules.

00:08 And we're also going to determine which of the two molecules has the strongest carbon -oxygen bonds.

00:14 So we will start off with carbon dioxide.

00:22 So we need to calculate the total number of valence electrons to do that.

00:26 We add four valence electrons for carbon and six valence electrons for oxygen times the number of.

00:34 Of oxygen atoms in the molecule and this gives us a total of 16.

00:39 Then we write down the least electronegative atom in the center, which is carbon and then oxygen on the outside.

00:48 Then we write down the pairing electrons.

00:51 That is four in total and that leaves us with 12, which we then distribute on the outer electrons forming full octates.

01:01 Now in doing so, we notice that the oxygens have full octates, but carbon does not.

01:07 Therefore, we need to remove that set of electrons and we form a double bond there and a double bond there as well.

01:20 And that gives us a four octet for oxygen, for carbon, and as well as with the other oxygen.

01:26 Then now to write down the resonance forms.

01:28 So for the resonance forms, we move the loan pay electrons, or pairs of electrons that are in double bonds or triple bonds.

01:43 So we have our carbon and oxygen atom set d.

01:50 Now for our first resonance form, what we can do is we'll move one pair of bonding electrons and place it on this oxygen.

02:10 That will give us one single one and then we will move one pair of electrons from that oxygen to form a triple bond on this end.

02:23 That would be our second form.

02:25 And then the third, we write down our oxygens, right down our oxygens over there...

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