Cyclopropane forms a ring structure that can be seen between the three carbon atoms to the left. Forming an equilateral triangle will form bond angles within the carbon ring that are less than any ideal angle degree of 109.5. Having an acute bond angle of 60 degrees puts strain on the other atoms involved. Each atom in the molecule would like to be as far away from one another but close enough to share electrons. This happy medium is sought after by all molecules but is different with cyclopropane due to its ring structure.
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![Picture](/uploads/4/9/0/9/49092885/6760844.jpg?249)
The picture to the right shows a Lewis structure of cyclopropane. The bond angles between the carbons are 60 degrees while the bond angles between the hydrogen are 115 degrees. This picture shows the individual atoms and their bonds where the picture below shows the bond angle measurements more clearly.
The small dashed lines leading off the carbon atom to the hydrogen are used to represent a hydrogen atom that is beneath the solid line leading to the first hydrogen.
Cyclopropane does not take a traditional AXe form like many other molecules. Cyclopropane does not have a central atom which eliminates that type of classification. Due to its strange bonding, Cyclopropane can be classified under the "Common points group" as a D3H which is similar to the VSEPR tables.
Intermolecular forces
Intermolecular forces are forces that act upon two different molecules or atoms when they begin to interact.
The three intermolecular forces are...
- Dipole- dipole- When molecules get close enough to one another, depending on their polarity, they will be attracted to one another. If a molecule has a positive and a negative side to it and the other molecule it is combining with has a similar make up, then the positive side of the molecule will bond with the negative side of the other molecule and vise versa.
- Hydrogen bonding- When a molecule contains a hydrogen atom, the hydrogen is attracted to another molecule if the other molecule has either one of the following; nitrogen, oxygen and florine. Hydrogen bonding is very similar to dipole dipole forces due to the hydrogen high level of positive polarity.
- Dispersion- Any atoms adjacent to another will be attracted to one another.
We can see an example of these forces by putting cyclopropane next to NH3.
If these molecules were to interact, the intermolecular forces acting on them can be discussed.
When two or more atoms or molecules interact, the force of dispersion will always be present. When looking at C3H6 alone, it can be determined as a non polar molecule, but when looking at NH3 it is a polar molecule. This difference in polarity will result in a dipole dipole bond. Finally, the last of the forces, hydrogen bonding, is still applied to these molecules where C3H6 has many hydrogen atoms which are naturally attracted to the nitrogen on the NH3.
Between these two molecules, the three intermolecular forces are at work.
When two or more atoms or molecules interact, the force of dispersion will always be present. When looking at C3H6 alone, it can be determined as a non polar molecule, but when looking at NH3 it is a polar molecule. This difference in polarity will result in a dipole dipole bond. Finally, the last of the forces, hydrogen bonding, is still applied to these molecules where C3H6 has many hydrogen atoms which are naturally attracted to the nitrogen on the NH3.
Between these two molecules, the three intermolecular forces are at work.