# Chem 2: # of pi bonds in a molecule

• Chemistry
• CausativeAgent
In summary, the formula for finding the number of pi bonds in a molecule is (6nPi+2-total # of electrons)/2. For a molecule with the empirical formula C12H18, the maximum number of pi bonds can be determined by substituting 12 for n in the formula, resulting in a total of 4 pi bonds. This assumes that the molecule is acyclic, and for cyclic structures, the number of pi bonds may be different.

## Homework Statement

How many pi bonds are in the molecule C12H18?

## Homework Equations

I have in my notes the formula (6nPi+2-total # of electrons)/2.

## The Attempt at a Solution

Unfortunately I can't find an explination for this formula in the book and I don't remember what was shown in lecture. I do know that there are 66 valence electrons total in this molecule. I also understand the basic definitions of pi and sigma bonds.

As I remember it,
For every single bond, you have one “sigma” bond.
If you have a double bond, you have one “sigma” bond and one “pi” bond.
If you have a triple bond, you have 1 sigma bond and two pi bonds.

So to find the total number of pi bonds in the molecule, you need to identify the number of double and triple bonds in the molecule.
# of pi bonds = (# double bonds) + (2 * # of triple bonds)

It would help to draw out the structure with the appropriate bonds between the atoms.

Thanks for the reply. But I'm almost positive there is a quicker way to do it using that formula. This would be one of many questions on a one hour test and drawing the lewis structure for something that big would take me forever. One thing to add for clarification is I think technically that formula is for the maximum number of pi bonds. Also, it is not 100% accurate and may be off by one or two.

The empirical formula (C12H18) doesn't have enough information to tell you that without making at least one assumption. That assumption would be that the compound contains either a known number of cyclic structures or no cyclic structures. For acyclic compounds, the empirical formula should be CnH2n+2. You can prove this to yourself by inspection (try ethane, propane, etc...).

So, for a C12 molecule, the hydrogens should equal to 2(12)+2=26. We have 18 and at least 2 hydrogens must be removed to form each pi bond or cyclic structure. For example C6H12 could be cyclohexane (no pi bonds) or hexene (any of 3 isomers with 1 pi bond). If we assume that the molecule is acyclic, C12H18 has 8 fewer hydrogens that would be predicted for a saturated compound and therefore has 4 pi bonds.

For the answer to the question regarding the maximum number of pi bonds, assume that the molecule is acyclic.

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I finally just decided to ask my teacher. Your method does yield the correct answer but it shows a greater depth of understanding than we're required to have at this point. It turns out that formula just means six multiplied by the number of atoms that can potentially form pi bonds plus two minus the total # of valence electrons, all divided by two. So for C12H18 it would be:

(6x12+2-66)/2 = 4

## 1. How do you determine the number of pi bonds in a molecule?

The number of pi bonds in a molecule can be determined by counting the number of double or triple bonds present in the molecule. Each double bond has one pi bond and each triple bond has two pi bonds.

## 2. What is the difference between a pi bond and a sigma bond?

A pi bond is formed by the overlap of two atomic orbitals that are parallel to each other. A sigma bond, on the other hand, is formed by the overlap of two atomic orbitals that are directly in line with each other.

## 3. Can a molecule have both pi and sigma bonds?

Yes, most molecules have both pi and sigma bonds. However, the number of each type of bond may vary depending on the structure of the molecule.

## 4. How does the number of pi bonds affect the properties of a molecule?

The number of pi bonds in a molecule can affect its shape, reactivity, and stability. Generally, molecules with more pi bonds tend to be more reactive and less stable due to the increased delocalization of electrons.

## 5. Can a molecule have an odd number of pi bonds?

Yes, a molecule can have an odd number of pi bonds. This typically occurs when there is an odd number of double or triple bonds present in the molecule.