The Lewis structure of CH3SH contains five single bonds, with carbon in the center, and four hydrogens and sulfur on either side. There are two lone pairs on the sulfur 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 CH3SH.
#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 sulfur is a group 16 element. Hence, carbon has four valence electrons, hydrogen has one valence electron, and sulfur has six valence electrons.
Now CH3SH has one carbon atom, four hydrogen atoms, and one sulfur atom.
So the total number of valence electrons = valence electrons of carbon atom + (valence electrons of hydrogen atom × 4) + valence electrons of sulfur atom
Therefore, the total number of valence electrons = 4 + 4 + 6 = 14
- 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 sulfur.
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 sulfur as follows:
Electronegativity value of carbon = 2.55
Electronegativity value of sulfur = 2.58
Obviously, carbon is less electronegative than sulfur. Hence, assume that carbon is the central atom.
So now, put carbon in the center and hydrogens and sulfur on either side. And draw the rough skeleton structure for the Lewis structure of CH3SH something like this:
Also read: How to draw Lewis structure of C2H2Br2 (5 steps)
#2 Show chemical bond
Place two electrons between the atoms to show a chemical bond. Since carbon is surrounded by four hydrogens and sulfur, use ten electrons to show five chemical bonds as follows:
Also read: How to draw Lewis structure of N2O3 (5 steps)
#3 Mark lone pairs
As calculated earlier, we have a total of 14 valence electrons. And in the above structure, we have already used ten valence electrons. Hence, four valence electrons are remaining.
Two valence electrons represent one lone pair. So four valence electrons = two 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 sulfur 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 and sulfur. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.
So sulfur will get two lone pairs. And the central atom (carbon) will not get any lone pair, because all two lone pairs are used.
Now draw the Lewis structure of CH3SH something like this:
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 H2PO4– (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 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 sulfur 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 CH3SH 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 CH3SH.
And each horizontal line drawn in the above structure represents a pair of bonding valence electrons.
Related
- Lewis structure of C2H2Br2
- Lewis structure of N2O3
- Lewis structure of H2PO4–
- Lewis structure of C2H2O
- Lewis structure of HPO42-
External links
- CH3SH Lewis Structure in 6 Steps (With Images) – Pediabay
- CH3SH lewis structure, molecular geometry, hybridization, polarity – Topblogtenz
- Draw the Lewis structure for the compound methanethiol (CH3SH) – Chegg
- What is the Lewis structure of methanethiol, CH3SH? – Brainly
- Methanethiol | CH3SH | CID 878 – National Institutes of Health (.gov)
- What is the Lewis structure of methanethiol, CH3SH? – Numerade
- how many lone pairs are in lewis structure of CH3SH? – Bartleby
- CH3SH (Methyl Mercaptan) Oxidation Number – ChemicalAid
- What is the Lewis structure of methanethiol, CH3SH? – OneClass
- What is the lewis structure of methanethiol CH3SH – Course Hero
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.