Do we see any separation of any electronic charge in this compound, which led the molecule to have both positive and negative ends?

We will explain how the molecule from the periodic table changes because of molecular geometry and electronegativity.

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First, let us describe the chemical formula CH2Cl2, also known as Dichloromethane. 

It is a clear, colorless, volatile liquid with a slightly sweet odor that commonly originates from macroalgae, volcanoes, oceanic sources, and wetlands. 

This would be associated with electricity, magnetism, and electronegativity when talking about polarity in a usual scenario. 

This is not one of the usual scenarios, though. Still, Dichloromethane, also known as Methyl Chloride, develops a net dipole moment across C-Cl and C-H bonds. 

The chemical bond results in a net 1.67 D dipole moment, thus making it a polar compound.

CH2Cl2 Molecular Structure

We look at the Lewis Structure of Dichloromethane or CH2Cl2 to determine if chemical reactions change its structure. 

Lewis structure will help us understand, based on the octet rule, the structure of a specific compound with eight electrons in its outer shell to be stable or inert. 

In the compound Dichloromethane, you will find Carbon atoms with 4 electrons, and Hydrogen atoms have 2 electrons in their neutral form. 

The two atoms need additional electrons to complete the bond formation. 

Chlorine atoms, on the other hand, have 17(seventeen) electrons distributed around their nucleus.


However, only 7 of those are valence electrons that are on the outer shell. 

Therefore, there are a total of 20 valence electrons. Out of 20 valence electrons, 8 electrons took part in the bond formation.

How to Determine CH2Cl2 Polarity



You can also determine the polarity of a compound with its shape. If the dipole moment on each molecule does not cancel out, then that is a polar compound. 

However, a nonpolar molecule can have polar bonds within it, but the dipoles of these valence electrons get canceled by each other due to the symmetric shape of the molecules. 


The one with the partial negative charge in a polar covalent bond is the more electronegative atom. The electron distribution is more polarized, and the partial charges of these atoms become more prominent. Some electrons have lower electronegativity(1), such as the Hydrogen atom, compared to the electrons found on the chlorine atom.

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Dipole Moment

What made us say CH2Cl2 is a polar compound?

In the case of Dichloromethane, the distribution of positive and negative charges of the molecules of all the bonding atoms are as follows, Hydrogen=2.2, carbon atom =2.5, and chlorine=3.1.

Electronegativity has an unequal distribution, partly because of Hydrogen molecules, which are lower than the two bonds.

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There is symmetry in the compound despite Hydrogen being less electronegative than a carbon atom, causing it not to cancel out; hence there are dipole moments in the compound.