The Lewis structure of CH3CH2Cl contains seven single bonds, with two carbons in the center. The left carbon is attached with three hydrogens, and right carbon is attached with one chlorine and two hydrogens. There are three lone pairs on the chlorine 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 CH3CH2Cl.
#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 chlorine is a group 17 element. Hence, carbon has four valence electrons, hydrogen has one valence electron, and chlorine has seven valence electrons.
Now CH3CH2Cl has two carbon atoms, five hydrogen atoms, and one chlorine atom.
So the total number of valence electrons = (valence electrons of carbon atom × 2) + (valence electrons of hydrogen atom × 5) + valence electrons of chlorine atom
Therefore, the total number of valence electrons = 8 + 5 + 7 = 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 chlorine.
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 chlorine as follows:
Electronegativity value of carbon = 2.55
Electronegativity value of chlorine = 3.16
Obviously, carbon is less electronegative than chlorine. Hence, assume that left carbon is the central atom (as there are two carbons).
So now, put two carbons in the center and chlorine and five hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of CH3CH2Cl something like this:
Also read: How to draw Lewis structure of C2F2 (5 steps)
#2 Show chemical bond
Place two electrons between the atoms to show a chemical bond. Since two carbons are surrounded by chlorine and five hydrogens, use fourteen electrons to show seven chemical bonds as follows:
Also read: How to draw Lewis structure of C2H3Cl (5 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 fourteen valence electrons. Hence, six valence electrons are remaining.
Two valence electrons represent one lone pair. So six valence electrons = three lone pairs.
Note that carbon is a period 2 element, so it can not keep more than 8 electrons in its last shell. Hydrogen is a period 1 element, so it can not keep more than 2 electrons in its last shell. And chlorine is a period 3 element, so it can keep more than 8 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, chlorine, 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 chlorine will get three lone pairs. And right carbon and central atom (left carbon) will not get any lone pair, because all three lone pairs are used.
Now draw the Lewis structure of CH3CH2Cl 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 CH2Br2 (4 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 chlorine atom
Valence electrons = 7
Nonbonding electrons = 6
Bonding electrons = 2
Formal charge = 7 – 6 – ½ (2) = 0
Mention the formal charges of atoms on the structure. So the Lewis structure of CH3CH2Cl 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 CH3CH2Cl.
And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.
Related
- Lewis structure of C2F2
- Lewis structure of C2H3Cl
- Lewis structure of CH2Br2
- Lewis structure of NHF2
- Lewis structure of Cr2O72-
External links
- Draw the Lewis structure for CH3CH2Cl – Homework.Study.com
- Draw the complete Lewis structure for CH3CH2Cl – Chegg
- There are __________ valence electrons in the lewis structure of ch3ch2cl – Brainly
- Draw the complete Lewis structure for CH3CH2Cl – Numerade
- There are ______ covalent bonds in the lewis structure of ch3ch2cl – Brainly
- Chloroethane | C2H5Cl | CID 6337 – National Institutes of Health (.gov)
- CH3CH2Cl (Chloroethane) Oxidation Number – ChemicalAid
- There are ______ valence electrons in the lewis structure of ch3ch2cl – Quizlet
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.