# Lewis Structure of HCOOH (Formic acid) (In 6 Simple Steps)

I’m super excited to teach you the lewis structure of HCOOH molecule in just 6 simple steps.

Infact, I’ve also given the step-by-step images for drawing the lewis dot structure of HCOOH molecule.

So, if you are ready to go with these 6 simple steps, then let’s dive right into it!

Lewis structure of HCOOH (or CH2O2 or Formic acid) is a simple lewis structure that contains a Hydrogen atom (H) attached with a COOH functional group. The Oxygen atoms (O) present in this lewis structure have 2 lone pairs.

Let’s draw and understand this lewis dot structure step by step.

(Note: Take a pen and paper with you and try to draw this lewis structure along with me. I am sure you will definitely learn how to draw lewis structure of HCOOH).

## 6 Steps to Draw the Lewis Structure of HCOOH

### Step #1: Calculate the total number of valence electrons

Here, the given molecule is HCOOH (also known as formic acid). In order to draw the lewis structure of HCOOH, first of all you have to find the total number of valence electrons present in the HCOOH molecule.
(Valence electrons are the number of electrons present in the outermost shell of an atom).

So, let’s calculate this first.

Calculation of valence electrons in HCOOH

• For Hydrogen:

Hydrogen is a group 1 element on the periodic table. [1]

Hence, the valence electron present in hydrogen is 1 (see below image).

• For Carbon:

Carbon is a group 14 element on the periodic table. [2]

Hence, the valence electrons present in carbon is 4 (see below image).

• For Oxygen:

Oxygen is a group 16 element on the periodic table. [3]

Hence, the valence electron present in oxygen is 6 (see below image).

Hence in a HCOOH molecule,
Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by each Carbon (C) atom = 4
Valence electrons given by each Oxygen (O) atom = 6
So, total number of Valence electrons in HCOOH molecule = 1 +4 + 6 + 6 + 1 = 18

### Step #2: Select the center atom (H is always outside)

While selecting the center atom, always put the least electronegative atom at the center.

(Remember: Fluorine is the most electronegative element on the periodic table and the electronegativity decreases as we move right to left in the periodic table as well as top to bottom in the periodic table). [4]

Here in the HCOOH molecule, if we compare the carbon atom (C), oxygen atom (O) and hydrogen atom (H), then hydrogen is less electronegative than oxygen and carbon. But as per the rule, we have to keep hydrogen outside.

So, carbon (which is less electronegative than oxygen) should be placed in the center and the remaining oxygen and hydrogen atoms will surround it.

In a simple way, you can also draw a Hydrogen atom (H) attached with a COOH functional group.

### Step #3: Put two electrons between the atoms to represent a chemical bond

Now in the above sketch of HCOOH molecule, put the two electrons (i.e electron pair) between the carbon atom, oxygen atom and hydrogen atom to represent a chemical bond between them.

These pairs of electrons present between the Carbon (C), Oxygen (O) and Hydrogen (H) atoms form a chemical bond, which bonds these atoms with each other in a HCOOH molecule.

### Step #4: Complete the octet (or duplet) on outside atoms

Don’t worry, I’ll explain!

In the Lewis structure of HCOOH, the outer atoms are hydrogen atoms as well as oxygen atom.

Hydrogen already has a duplet (see below image).

So now, you have to complete the octet on oxygen atom (because oxygen requires 8 electrons to have a complete outer shell).

Now, you can see in the above image that the oxygen atom forms an octet.

Also, all the 18 valence electrons of HCOOH molecule (as calculated in step #1) are used in the above structure. So there are no remaining electron pairs.

Hence there is no change in the above sketch of HCOOH.

Let’s move to the next step.

### Step #5: Check whether the central atom has octet or not. If it does not have an octet, then move the electron pair from the outer atom to form a double bond or triple bond

In this step, we have to check whether the central atom (i.e carbon) has an octet or not.

In simple words, we have to check whether the central Carbon (C) atom has 8 electrons or not.

As you can see from the above image, the central atom (i.e carbon) has only 6 electrons. So it does not fulfill the octet rule.

Now, in order to fulfill the octet of carbon atom, we have to move the electron pair from the outer atom (i.e oxygen atom) to form a double bond.

Now you can see from the above image that the carbon atom is having 8 electrons. So it fulfills the octet rule.

### Step #6: Final step – Check the stability of lewis structure by calculating the formal charge on each atom

Now, you have come to the final step and here you have to check the formal charge on carbon atom (C), oxygen atom (O) as well as each hydrogen atom (H).

For that, you need to remember the formula of formal charge;

Formal charge = Valence electrons – Nonbonding electrons – (Bonding electrons)/2

• For Carbon:
Valence electrons = 4 (as it is in group 14)
Nonbonding electrons = 0
Bonding electrons = 8
• For Hydrogen:
Valence electron = 1 (as it is in group 1)
Nonbonding electrons = 0
Bonding electrons = 2
• For Oxygen:
Valence electron = 6 (as it is in group 16)
Nonbonding electrons = 4
Bonding electrons = 4

So you can see above that the formal charges on carbon, hydrogen as well as oxygen are “zero”.

Hence, there will not be any change in the above structure and the above lewis structure of HCOOH is the final stable structure only.

Each electron pair (:) in the lewis dot structure of HCOOH represents the single bond ( | ). So the above lewis dot structure of HCOOH (formic acid) can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of IF3
Lewis Structure of XeO4
Lewis Structure of SF3+
Lewis Structure of XeO3
Lewis Structure of H2CO3

Article by;

Author
##### Jay Rana

Jay is an educator and has helped more than 100,000 students in their studies by providing simple and easy explanations on different science-related topics. With a desire to make learning accessible for everyone, he founded Knords Learning, an online learning platform that provides students with easily understandable explanations.