How do I draw the lewis dot structure for C2H3F

How do I draw the lewis dot structure for C2H3F?

The correct answer and explanation is :

To draw the Lewis dot structure for C2H3F (fluoroethene), we need to follow a few steps systematically to ensure the correct bonding and electron distribution. Below is a step-by-step guide and explanation:

Step 1: Determine the total number of valence electrons

Each atom has a specific number of valence electrons:

• Carbon (C) is in group 14, so it has 4 valence electrons.
• Hydrogen (H) is in group 1, so it has 1 valence electron.
• Fluorine (F) is in group 17, so it has 7 valence electrons.

Now, calculate the total number of valence electrons:

• 2 Carbon atoms × 4 electrons = 8 electrons
• 3 Hydrogen atoms × 1 electron = 3 electrons
• 1 Fluorine atom × 7 electrons = 7 electrons

Total valence electrons = 8 (C) + 3 (H) + 7 (F) = 18 valence electrons.

Step 2: Choose a central atom

Carbon atoms will be the central atoms since they can form more bonds. Fluorine will be placed on the periphery, as it is highly electronegative and typically only forms one bond. Hydrogens will be placed around the carbon atoms, as hydrogen can only form one bond.

Step 3: Form single bonds

Place a single bond (represented by a line) between the two carbon atoms and between the carbon atoms and the hydrogen and fluorine atoms. Each single bond uses 2 electrons.

• 1 bond between the two carbon atoms = 2 electrons
• 3 bonds between carbon and hydrogen atoms = 6 electrons
• 1 bond between carbon and fluorine = 2 electrons

Step 4: Distribute remaining electrons

After placing the single bonds, you will have used 10 electrons, leaving 8 electrons remaining. These remaining electrons will be placed as lone pairs.

• Fluorine will take 3 lone pairs (6 electrons) to complete its octet.
• The remaining 2 electrons will be placed as lone pairs on the second carbon atom.

Step 5: Double bond formation

In the current structure, carbon atoms do not yet have a full octet. To satisfy the octet rule for carbon, we will form a double bond between the two carbon atoms. This uses 2 additional electrons, resulting in 12 electrons used.

Step 6: Final structure

• Each carbon atom has 8 electrons in its valence shell.
• Fluorine has 8 electrons in its valence shell (via the single bond with carbon and 3 lone pairs).
• Each hydrogen atom has 2 electrons (from the single bond).

Lewis Dot Structure:

    H   H
     |   |
H - C = C - F
     |   
    H

Explanation:

• The two carbon atoms are bonded with a double bond (C=C), which ensures each carbon gets 8 electrons.
• Each hydrogen atom is bonded to a carbon atom via a single bond (C-H).
• Fluorine is attached to one carbon atom via a single bond (C-F) and has three lone pairs of electrons to complete its octet.
• The structure satisfies the octet rule for all atoms, and the total number of electrons is correctly accounted for.

Image:

Here is the Lewis dot structure for C2H3F (fluoroethene). As you can see, the two carbon atoms are bonded by a double bond, with hydrogen atoms attached to one of the carbons and a fluorine atom attached to the other. The fluorine has three lone pairs of electrons to complete its octet, and each carbon atom satisfies the octet rule.