How to Draw the Lewis Structure of 2-Chloropropene

10/18/2023

In this article, we will learn how to draw the Lewis structure of 2-chloropropene(CAS557-98-2), also known as 2-chloropropylene or isopropyl chloride. The Lewis structure is a way of representing the valence electrons of a molecule, which are the electrons that participate in chemical bonding. The Lewis structure can help us predict the shape, polarity, and reactivity of a molecule.

What is 2-Chloropropene?

2-Chloropropene(CAS557-98-2) is an organochlorine compound with the formula CH2=C(Cl)CH3. It is a colorless gas that condenses just below room temperature. Unlike the closely related vinyl chloride, which is a major industrial chemical, 2-chloropropene(CAS557-98-2) has no commercial applications and is a lightly studied compound. In the research laboratory, it is used as a source of the 2-propenyl group.

Steps to Draw the Lewis Structure of 2-Chloropropene

To draw the Lewis structure of 2-chloropropene, we need to follow these steps:

Count the total number of valence electrons in the molecule. Each hydrogen atom has 1 valence electron, each carbon atom has 4 valence electrons, and each chlorine atom has 7 valence electrons. The total number of valence electrons is 1 x 4 + 4 x 2 + 7 x 1 = 18.
Draw the skeletal structure of the molecule, connecting the atoms with single bonds. The central atom is usually the one with the lowest electronegativity, which in this case is carbon. We can arrange the atoms as CH2=C(Cl)CH3, where the double bond between the two carbon atoms indicates that they share two pairs of electrons.
Distribute the remaining valence electrons around the atoms to complete their octets (or duets for hydrogen). Each atom should have 8 valence electrons (except hydrogen, which should have 2) around it, including the ones in the bonds. We can place 6 electrons around chlorine, 4 electrons around each terminal carbon, and 2 electrons around each hydrogen. We have used up all 18 valence electrons.
Check the formal charges of each atom to see if the structure is stable. The formal charge is calculated by subtracting the number of valence electrons in the free atom from the number of valence electrons in the bonded atom. A stable structure should have formal charges as close to zero as possible, and preferably no negative charges on more electronegative atoms than positive charges on less electronegative atoms. In this case, all atoms have a formal charge of zero, which means that the structure is stable.

The final Lewis structure of 2-chloropropene is shown below:

H H
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H–C=C–C–Cl
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H H

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