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

To determine the correct Lewis structure of carbon tetrachloride (CCl₄), follow these steps:

1. Break Down the Problem

• Identify the elements involved: Carbon (C) and Chlorine (Cl).
• Determine the number of bonds and lone pairs present based on valence electrons.

2. Relevant Concepts

• Carbon is in group 14 and has 4 valence electrons.
• Chlorine is in group 17 and has 7 valence electrons.
• The total number of valence electrons in CCl₄ = 4 (from C) + 4 × 7 (from 4 Cl) = 4 + 28 = 32 electrons.

3. Analysis and Detail

• Carbon will be the central atom since it can form four bonds.

• Each chlorine will form a single bond with carbon. Thus, C will have 4 Cl atoms each forming a single bond:

  $\text{C - Cl} \quad \text{C - Cl} \quad \text{C - Cl} \quad \text{C - Cl}$

• After forming four single bonds, Carbon will have 0 lone pairs, and each Chlorine will have 3 lone pairs:

  • For each Cl:
    • 1 bond (shared with C)
    • 3 lone pairs (6 electrons remaining for each Cl)

4. Verify and Summarize

• Verify that all atoms achieve a stable electron configuration:
  • Carbon has 8 electrons (4 bonds).
  • Each chlorine has 8 electrons (1 bond + 6 from lone pairs).

This confirms a stable structure with all atoms fulfilling the octet rule.

Final Answer

The Lewis structure of CCl₄ is represented as follows:

     Cl
      |
  Cl - C - Cl
      |
     Cl

Where each chlorine (Cl) atom has three lone pairs around it, while carbon (C) is at the center with four single bonds to each chlorine atom.