Lewis structure of CH3NO2

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The Lewis structure of CH₃NO₂ contains five single bonds and one double bond, with carbon and nitrogen in the center. The carbon is attached with three hydrogens, and nitrogen is attached with two oxygens. The top oxygen has three lone pairs, right oxygen has two lone pairs, and nitrogen atom, carbon atom, and hydrogen atom do not have any lone pair.

Contents

Steps

By using the following steps, you can easily draw the Lewis structure of CH₃NO₂.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Complete octet on atoms
#5 Calculate formal charge and check stability

Let’s one by one discuss each step in detail.

#1 Draw skeleton

In this step, first calculate the total number of valence electrons. And then, decide the central atom.

Let’s calculate the total number of valence electrons

We know that… carbon is a group 14 element, hydrogen is a group 1 element, nitrogen is a group 15 element, and oxygen is a group 16 element. Hence, carbon has four valence electrons, hydrogen has one valence electron, nitrogen has five valence electrons, and oxygen has six valence electrons.

Now CH₃NO₂ has one carbon atom, three hydrogen atoms, one nitrogen atom, and two oxygen atoms.

So the total number of valence electrons = valence electrons of carbon atom + (valence electrons of hydrogen atom × 3) + valence electrons of nitrogen atom + (valence electrons of oxygen atom × 2)

Therefore, the total number of valence electrons = 4 + 3 + 5 + 12 = 24

Now decide the central atom

We can not assume hydrogen as the central atom, because the central atom is bonded with at least two other atoms. And hydrogen has only one electron in its last shell, so it can not make more than one bond.

Therefore, choose the central atom from carbon, nitrogen, and oxygen.

The atom with the least electronegative value is placed at the center. By looking at the periodic table, we get the electronegativity values for carbon, nitrogen, and oxygen as follows:

Electronegativity value of carbon = 2.55
Electronegativity value of nitrogen = 3.04
Electronegativity value of oxygen = 3.44

Obviously, carbon is less electronegative than nitrogen and oxygen. Hence, assume that carbon is the central atom.

So now, put carbon in the center and nitrogen, two oxygens, and three hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of CH₃NO₂ something like this:

Skeleton structure for Lewis structure of CH₃NO₂ | Image: Root Memory

Also read: How to draw Lewis structure of AsF₃ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since carbon is surrounded by nitrogen, two oxygens, and three hydrogens, use twelve electrons to show six chemical bonds as follows:

Six chemical bonds shown between atoms | Image: Root Memory

#3 Mark lone pairs

As calculated earlier, we have a total of 24 valence electrons. And in the above structure, we have already used twelve valence electrons. Hence, twelve valence electrons are remaining.

Two valence electrons represent one lone pair. So twelve valence electrons = six lone pairs.

Note that all (carbon, nitrogen, and oxygen) are the period 2 elements, so they can not keep more than 8 electrons in their last shell. And hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell.

Also, make sure that you start marking these lone pairs on outside atoms first. And then, on the central atom.

The outside atoms are hydrogens, oxygens, and nitrogen. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So each oxygen will get three lone pairs. And nitrogen and the central atom (carbon) will not get any lone pair, because all six lone pairs are used.

Now draw the Lewis structure of CH₃NO₂ something like this:

Lone pairs marked on Lewis structure of CH₃NO₂ | Image: Root Memory

In the above structure, you can see that the octet is completed on the central atom (carbon), and also on the outside atoms (except nitrogen).

So in the next step, we have to complete the octet on nitrogen.

Also read: How to draw Lewis structure of NO₂Cl (5 steps)

#4 Complete octet on atoms

Remember that nitrogen is a period 2 element, so it can not keep more than 8 electrons in its last shell.

Now nitrogen already has six valence electrons. Hence, nitrogen needs two more valence electrons to complete its octet.

So convert one lone pair from the oxygen atom to make a new bond with the nitrogen atom. And then, the Lewis structure of CH₃NO₂ looks something like this:

Lone pair of right oxygen is converted, and octet is completed on atoms | Image: Root Memory

In the above structure, you can see that the octet is completed on the central atom (carbon), and also on the outside atoms. Therefore, the octet rule is satisfied.

After completing the octet, one last thing we need to do is, calculate the formal charge and check the stability of the above structure.

Also read: How to draw Lewis structure of BeCl₂ (4 steps)

#5 Calculate formal charge and check stability

The following formula is used to calculate the formal charges on atoms:

Formal charge = valence electrons – nonbonding electrons – ½ bonding electrons

Collect the data from the above structure and then, write it down below as follows:

For carbon atom

Valence electrons = 4
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 4 – 0 – ½ (8) = 0

For each hydrogen atom

Valence electrons = 1
Nonbonding electrons = 0
Bonding electrons = 2

Formal charge = 1 – 0 – ½ (2) = 0

For nitrogen atom

Valence electrons = 5
Nonbonding electrons = 0
Bonding electrons = 8

Formal charge = 5 – 0 – ½ (8) = +1

For top oxygen atom

Valence electrons = 6
Nonbonding electrons = 6
Bonding electrons = 2

Formal charge = 6 – 6 – ½ (2) = -1

For right oxygen atom

Valence electrons = 6
Nonbonding electrons = 4
Bonding electrons = 4

Formal charge = 6 – 4 – ½ (4) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of CH₃NO₂ looks something like this:

Formal charges are calculated, and got the most stable Lewis structure of CH₃NO₂ | Image: Root Memory

In the above structure, you can see that the formal charges of atoms are closer to zero. Therefore, this is the most stable Lewis structure of CH₃NO₂.

And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.

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External links

Chemical Bonding: CH3NO2 Lewis Structure – The Geoexchange
CH3NO2 Lewis Structure & Characteristics (15 Helpful Facts) – Lambda Geeks
CH3NO2 Lewis Structure in 6 Steps (With Images) – Pediabay

CH3NO2 Lewis structure, molecular geometry, bond angles, resonance – Topblogtenz
CH3NO2 Lewis Structure, Molecular Geometry, Hybridization, and Polarity – Techiescientist
CH3NO2 Lewis Structure (Nitromethane) – Pinterest

Draw and explain the Lewis diagram for nitromethane, CH₃NO₂ – Homework.Study.com
Draw the best Lewis structure of CH3NO2, a neutral compound – Brainly
Draw the Lewis structure (including all resonance structures) for nitromethane (CH3NO2) – Chegg

Compare and contrast the Lewis structures of nitromethane, CH3NO2, and methyl nitrite, CH3ONO – Quizlet
Draw the Lewis structure (including resonance structures) for nitromethane (CH3NO2) – Bartleby
Hybridization of N in CH3NO2? – Chemical Forums

Deep

Rootmemory.com was founded by Deep Rana, who is a mechanical engineer by profession and a blogger by passion. He has a good conceptual knowledge on different educational topics and he provides the same on this website. He loves to learn something new everyday and believes that the best utilization of free time is developing a new skill.