Lewis structure of CH3CH2NH2

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The Lewis structure of CH₃CH₂NH₂ contains nine single bonds, with two carbons in the center, and nitrogen and seven hydrogens on either side. There is one lone pair on the nitrogen atom, and carbon atom and hydrogen atom do not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of CH₃CH₂NH₂.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Calculate formal charge and check stability (if octet is already completed on central atom)

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, and nitrogen is a group 15 element. Hence, carbon has four valence electrons, hydrogen has one valence electron, and nitrogen has five valence electrons.

Now CH₃CH₂NH₂ has two carbon atoms, seven hydrogen atoms, and one nitrogen atom.

So the total number of valence electrons = (valence electrons of carbon atom × 2) + (valence electrons of hydrogen atom × 7) + valence electrons of nitrogen atom

Therefore, the total number of valence electrons = 8 + 7 + 5 = 20

• 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 and nitrogen.

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 and nitrogen as follows:

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

Obviously, carbon is less electronegative than nitrogen. Hence, assume that left carbon is the central atom (as there are two carbons).

So now, put two carbons in the center and nitrogen and seven hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of CH₃CH₂NH₂ something like this:

Also read: How to draw Lewis structure of NF₂^– (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since two carbons are surrounded by nitrogen and seven hydrogens, use eighteen electrons to show nine chemical bonds as follows:

Also read: How to draw Lewis structure of CH₃CH₂Cl (4 steps)

#3 Mark lone pairs

As calculated earlier, we have a total of 20 valence electrons. And in the above structure, we have already used eighteen valence electrons. Hence, two valence electrons are remaining.

And two valence electrons represent one lone pair.

Note that both (carbon and nitrogen) 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, nitrogen, and right carbon. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So nitrogen will get one lone pair. And right carbon and central atom (left carbon) will not get any lone pair, because all lone pairs are used.

Now draw the Lewis structure of CH₃CH₂NH₂ something like this:

In the above structure, you can see that the octet is completed on the central atom (left 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 C₂F₂ (5 steps)

#4 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 each 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 = 2
Bonding electrons = 6

Formal charge = 5 – 2 – ½ (6) = 0

Mention the formal charges of atoms on the structure. So the Lewis structure of CH₃CH₂NH₂ looks something like this:

In the above structure, you can see that the formal charges of all atoms are zero. Therefore, this is the stable Lewis structure of CH₃CH₂NH₂.

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

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Related

• Lewis structure of NF₂^–
• Lewis structure of CH₃CH₂Cl
• Lewis structure of C₂F₂
• Lewis structure of C₂H₃Cl
• Lewis structure of CH₂Br₂

External video

• How to Draw the Lewis Dot Structure for CH3CH2NH2: Ethylamine – Wayne Breslyn

External links

• Draw the Lewis structure for ethylamine (CH3CH2NH2). Assign lone pairs where appropriate – Homework.Study.com
• draw ch3ch2nh2 lewis structure – Brainly
• what is the lewis structure for ethylamine ch3ch2nh2 – Chegg
• lewis structure for ch3ch2nh2 – Quizlet
• Ethylamine | C2H5NH2 | CID 6341 – National Institutes of Health (.gov)
• what is the lewis structure for ethylamine ch3ch2nh2 – OneClass
• CH3CH2NH2 (Dimethylamine) Oxidation Number – ChemicalAid
• Ethylamine | C2H7N – ChemSpider