Which of the following Lewis dot structures correctly represents the electron arrangement in a neutral molecule of CCl_4?

• A. A central carbon atom with one triple bond to a chlorine atom and three single bonds to the other chlorine atoms.
• B. A central carbon atom with four single bonds to four chlorine atoms, each chlorine atom having two lone pairs.
• C. A central carbon atom with two double bonds to two chlorine atoms and two single bonds to the other two chlorine atoms.
• D. A central carbon atom with four single bonds to four chlorine atoms, each chlorine atom having three lone pairs.

Answer: (D)

Verified step by step guidance

1. Recall that carbon (C) has 4 valence electrons and chlorine (Cl) has 7 valence electrons each.
2. Determine the total number of valence electrons in CCl_4 by adding the valence electrons of one carbon atom and four chlorine atoms: \$4 + 4 \times 7$.
3. Understand that carbon typically forms four single covalent bonds to complete its octet, and chlorine atoms typically form one single bond and have three lone pairs to complete their octets.
4. Analyze each proposed Lewis structure to check if all atoms satisfy the octet rule: carbon should have 8 electrons around it (from bonds), and each chlorine should have 8 electrons (from bonds plus lone pairs).
5. Identify that the correct Lewis structure for CCl_4 is the one where the central carbon atom forms four single bonds to four chlorine atoms, and each chlorine atom has three lone pairs, ensuring all atoms have complete octets.