Create the Lewis structure of CF4

Create the Lewis structure of CF4. NOTE: do only the step asked for in each part and then click Check–don’t work ahead to solve the final structure.

The Correct Answer and Explanation is :

To draw the Lewis structure of carbon tetrafluoride (CF₄), follow these steps:

1. Determine the Total Number of Valence Electrons:

• Carbon (C) is in group 14 of the periodic table, so it has 4 valence electrons.
• Fluorine (F) is in group 17, contributing 7 valence electrons per atom.
• With four fluorine atoms, the total valence electrons from fluorine are 7 × 4 = 28.
• Adding these together, the total number of valence electrons is 4 (from C) + 28 (from F) = 32 electrons.

1. Arrange the Atoms:

• Place the carbon atom in the center, as it is less electronegative than fluorine.
• Position the four fluorine atoms around the carbon atom.

1. Form Single Bonds:

• Connect each fluorine atom to the carbon atom with a single bond.
• Each single bond consists of two electrons, so four bonds use 4 × 2 = 8 electrons.

1. Distribute Remaining Electrons as Lone Pairs:

• After forming the bonds, 32 total electrons minus 8 electrons used in bonds leaves 24 electrons.
• Distribute these 24 electrons as lone pairs on the fluorine atoms.
• Each fluorine atom needs three lone pairs to complete its octet, using 3 × 4 = 12 electrons.
• The remaining 12 electrons are placed as lone pairs on the carbon atom.

1. Verify the Octet Rule:

• Each fluorine atom has 8 electrons (2 from the bond and 6 from lone pairs), satisfying the octet rule.
• The carbon atom has 8 electrons (4 from bonds), also satisfying the octet rule.

The final Lewis structure shows a central carbon atom bonded to four fluorine atoms, each with three lone pairs, forming a tetrahedral geometry.

For a visual demonstration, you might find this video helpful:

videoHow to Draw The Lewis Structure for CF4 (Carbon Tetrafluoride)turn0search0