Lewis Structure of CH3OCH3 (In 4 Simple Steps)

Lewis structure of CH3OCH3

Ready to learn how to draw the lewis structure of CH3OCH3?


Here, I have explained 4 simple steps to draw the lewis dot structure of CH3OCH3 (along with images).

So, if you are ready to go with these 4 simple steps, then let’s dive right into it!

Lewis structure of CH3OCH3 contains single bonds between Carbon-Oxygen atoms as well as between Carbon-Hydrogen atoms. The Oxygen atom (O) has 2 lone pairs.

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of CH3OCH3).

4 Steps to Draw the Lewis Structure of CH3OCH3

Step #1: Calculate the total number of valence electrons

Here, the given molecule is CH3OCH3. In order to draw the lewis structure of CH3OCH3, first of all you have to find the total number of valence electrons present in the CH3OCH3 molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in CH3OCH3

  • For Carbon:

Carbon is a group 14 element on the periodic table. [1]

Hence, the valence electrons present in carbon is 4 (see below image).

  • For Hydrogen: 

Hydrogen is a group 1 element on the periodic table. [2]

Hence, the valence electron present in hydrogen is 1 (see below image).

  • For Oxygen:

Oxygen is a group 16 element on the periodic table. [3]

Hence, the valence electron present in oxygen is 6 (see below image).

Hence in a CH3OCH3 molecule,
Valence electrons given by each Carbon (C) atom = 4
Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by Oxygen (O) atom = 6
So, total number of Valence electrons in CH3OCH3 = 4 + 1(3) + 6 + 4 + 1(3) = 20

Step #2: Make the rough sketch

From the chemical formula itself, you can get the idea that an oxygen atom is at the center which is surrounded by CH3 on both sides.

So let’s draw a rough sketch for the CH3OCH3 molecule.

step 1

Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of CH3OCH3 molecule, put the two electrons (i.e electron pair) between the carbon atom, oxygen atom and hydrogen atom to represent a chemical bond between them.

step 2

These pairs of electrons present between the Carbon (C), Oxygen (O) and Hydrogen (H) atoms form a chemical bond, which bonds these atoms with each other in a CH3OCH3 molecule.

Step #4: Put the remaining electron pair/s on the central atom

In the above sketch of CH3OCH3, the outer atoms are hydrogen atoms, and these hydrogen atoms are forming a duplet and they are stable (because hydrogen requires only 2 electrons to have a complete outer shell).

Now, only 16 valence electrons of CH3OCH3 molecule are used in the above structure.

But there are total 20 valence electrons in CH3OCH3 molecule (as calculated in step #1).

So the number of electrons left to be kept on the central atom = 20 – 16 = 4.

So let’s keep these four electrons (i.e 2 electron pairs) on the central atom.

step 3

You can see in the above image that all the atoms are stable. Because the hydrogen atoms are forming a stable duplet and the carbon & oxygen atoms are forming a stable octet.

And hence, the above lewis structure of CH3OCH3 is the final stable structure only.

Each electron pair (:) in the lewis dot structure of CH3OCH3 represents the single bond ( | ). So the above lewis dot structure of CH3OCH3 can also be represented as shown below.

CH3OCH3 Lewis structure

Related lewis structures for your practice:
Lewis Structure of HCOOH (Formic acid)
Lewis Structure of IF3
Lewis Structure of XeO4
Lewis Structure of SF3+
Lewis Structure of XeO3 

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Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online learning platform that provides students with easily understandable explanations.

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