Identify the correct Lewis structure of CCl4. Ensure that all charges and lone pairs are shown.Group of answer choices

The Lewis structure for CCl4 (Carbon Tetrachloride) is a simple process to draw, but it is important to follow the steps:

1. Count the total number of valence electrons. Carbon has 4 valence electrons and each Chlorine atom has 7 valence electrons. Since there are 4 Chlorine atoms, the total number of valence electrons is 4+(4*7)=32.

2. Draw a skeleton structure of the molecule. Carbon is the central atom and the Chlorine atoms are surrounding it.

3. Connect the central atom to the surrounding atoms with a single bond (a line). Each line represents 2 electrons, so now we have used 8 out of 32 electrons.

4. Complete the octets on the surrounding atoms. Each Chlorine atom needs 6 more electrons to complete its octet. So, we add 6 more electrons (3 pairs) to each Chlorine atom. This uses up 24 more electrons, for a total of 32.

5. Check to make sure each atom has a full octet. Carbon has 8 electrons (4 bonds * 2 electrons/bond = 8 electrons) and each Chlorine atom also has 8 electrons (1 bond * 2 electrons/bond + 6 lone pair electrons = 8 electrons).

So, the Lewis structure of CCl4 is a Carbon atom connected to 4 Chlorine atoms, each Chlorine atom has 3 lone pairs of electrons, and there are no charges because all atoms have a full octet.