Lewis structure of C6H6

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The Lewis structure of C₆H₆ contains three double bonds and nine single bonds, with six carbons in the center, and each carbon is attached with one hydrogen. Both hydrogen atom and carbon atom do not have any lone pair.

Steps

By using the following steps, you can easily draw the Lewis structure of C₆H₆.

#1 Draw skeleton
#2 Show chemical bond
#3 Mark lone pairs
#4 Complete octet on central atom
#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 and hydrogen is a group 1 element. Hence, carbon has four valence electrons and hydrogen has one valence electron.

Now C₆H₆ has six carbon atoms and six hydrogen atoms.

So the total number of valence electrons = (valence electrons of carbon atom × 6) + (valence electrons of hydrogen atom × 6)

Therefore, the total number of valence electrons = 24 + 6 = 30

• 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 carbon as the central atom.

But there are six carbon atoms in C₆H₆. Hence, we can assume any one as the central atom. Let’s assume that top carbon is the central atom.

So now, put six carbons in the center and six hydrogens on either side. And draw the rough skeleton structure for the Lewis structure of C₆H₆ something like this:

Also read: How to draw Lewis structure of SBr₂ (4 steps)

#2 Show chemical bond

Place two electrons between the atoms to show a chemical bond. Since six carbons are surrounded by six hydrogens, use twenty-four electrons to show twelve chemical bonds as follows:

#3 Mark lone pairs

As calculated earlier, we have a total of 30 valence electrons. And in the above structure, we have already used twenty-four 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. 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, left carbons, right carbons, and bottom carbon. But hydrogen can not keep more than 2 electrons in its last shell. Hence, don’t mark the lone pairs on hydrogen.

So two left carbons and one right carbon will get one lone pair. And the remaining carbon atoms will not get any lone pair, because all three lone pairs are used.

Now draw the Lewis structure of C₆H₆ something like this:

In the above structure, you can see that the octet is completed on outside atoms. But, the central atom (top carbon) doesn’t form an octet.

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

Also read: How to draw Lewis structure of NBr₃ (4 steps)

#4 Complete octet on central atom

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

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

So convert one lone pair from each left carbon atom and top right carbon atom to make a new bond with the adjacent carbon atoms. And then, the Lewis structure of C₆H₆ looks something like this:

In the above structure, you can see that the octet is completed on the central atom (top 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 HOCl (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 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

Mention the formal charges of atoms on the structure. So the Lewis structure of C₆H₆ looks something like this:

In the above structure, you can see that the formal charges of both (carbon and hydrogen) are zero. Therefore, this is the stable Lewis structure of C₆H₆.

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

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Related

• Lewis structure of SBr₂
• Lewis structure of NBr₃
• Lewis structure of HOCl
• Lewis structure of SeF₄
• Lewis structure of NH₂Cl

External links

• Chemical Bonding: C6H6 Lewis Structure – The Geoexchange
• What is the Lewis structure of benzene? – Quora
• C6H6 (Benzene) Lewis Structure in 4 Steps (With Images) – Pediabay
• C6H6 lewis structure, molecular geometry, bond angle, hybridization – Topblogtenz
• Draw the Lewis structure for C6H6. Include any resonance forms – Homework.Study.com
• C6H6 (Benzene): Lewis Dot Structure and Polarity – Science Struck
• Draw a Lewis structure and any resonance forms of benzene, C6H6 – Chegg
• How to Draw the Lewis Structure for C6H6 (Benzene) – VoiceTube
• What is the resonance structure for C6H6? – Socratic
• Benzene Lewis Structure, Molecular Geometry, Hybridization, Polarity, and MO Diagram – Techiescientist
• how the c6h6 lewis structure? – Brainly
• Draw the Lewis structure for C6H6 – Quizlet
• C6H6 (Benzene) Oxidation Number – ChemicalAid