# Lewis Structure of C2H3F (With 6 Simple Steps to Draw!)

Ready to learn how to draw the lewis structure of C2H3F?

Awesome!

Here, I have explained 6 simple steps to draw the lewis dot structure of C2H3F (along with images).

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

Lewis structure of C2H3F contains a double bond between the two Carbon (C) atoms and a single bonds between Carbon-Hydrogen atoms and Carbon-Fluorine atoms. The Fluorine atom has 3 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 C2H3F).

## 6 Steps to Draw the Lewis Structure of C2H3F

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

Here, the given molecule is C2H3F. In order to draw the lewis structure of C2H3F, first of all you have to find the total number of valence electrons present in the C2H3F 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 C2H3F

• For Carbon:

Carbon is a group 14 element on the periodic table.

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

• For Hydrogen:

Hydrogen is a group 1 element on the periodic table.

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

• For Fluorine:

Fluorine is a group 17 element on the periodic table.

Hence, the valence electrons present in fluorine is 7 (see below image).

Hence in a C2H3F molecule,

Valence electrons given by each Carbon (C) atom = 4
Valence electron given by each Hydrogen (H) atom = 1
Valence electrons given by Fluorine (F) atom = 7
So, total number of Valence electrons in C2H3F molecule = 4(2) + 1(3) + 7 = 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).

Here in the C2H3F molecule, if we compare the carbon atom (C) and fluorine atom (F), then the carbon is less electronegative than fluorine.

So, carbon should be placed in the center and the fluorine atom will surround it.

Also as per the rule, we have to keep hydrogen outside.

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

Now in the above sketch of C2H3F molecule, put the two electrons (i.e electron pair) between the carbon-hydrogen atoms and carbon-fluorine atoms to represent a chemical bond between them.

These pairs of electrons present between the Carbon & Hydrogen atoms as well as between the Carbon & Fluorine atoms form a chemical bond, which bonds these atoms with each other in a C2H3F molecule.

### Step #4: Complete the octet (or duplet) on outside atoms. If the valence electrons are left, then put the valence electrons pair on the central atom

Don’t worry, I’ll explain!

In the Lewis structure of C2H3F, the outer atoms are hydrogen atoms and fluorine atom.

So now, you have to check whether these hydrogen atoms are forming a duplet or not! (because hydrogen requires only 2 electrons to have a complete outer shell).

You also have to see whether the fluorine atom is forming an octet or not! (because fluorine requires 8 electrons to have a complete outer shell).

You can see in the above image that both the hydrogen atoms form a duplet. And the fluorine atom also forms an octet.

Also, only 16 valence electrons of C2H3F molecule are used in the above structure.

But there are total 18 valence electrons in C2H3F molecule (as calculated in step #1).

So the number of electrons left to be kept on the carbon atom = 18 – 16 = 2.

So let’s keep these two electrons (i.e electron pair) on one of the central carbon atoms.

Now, 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 convert the lone pair into double bond or triple bond

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

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

As you can see from the above image, one carbon atom has 8 electrons, while the other carbon atom has only 6 electrons. So this carbon atom does not fulfill the octet rule.

Now, in order to fulfill the octet of this carbon atom, we have to convert the lone pair into a double bond.

Now you can see from the above image that both the central carbon atoms are having 8 electrons. So they fulfill the octet rule and both the carbon atoms are stable.

### 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 atoms (C), fluorine atom (F) as well as hydrogen atoms (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 Fluorine:
Valence electrons = 7 (as it is in group 17)
Nonbonding electrons = 6
Bonding electrons = 2

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

Hence, there will not be any change in the above structure and the above lewis structure of C2H3F is the final stable structure only.

Each electron pair (:) in the lewis dot structure of C2H3F represents the single bond ( | ). So the above lewis dot structure of C2H3F can also be represented as shown below.

Related lewis structures for your practice:
Lewis Structure of NH2F
Lewis Structure of SeI2
Lewis Structure of H2Te
Lewis Structure of TeCl2
Lewis Structure of CH2I2