How can a Lewis structure be drawn for carbon tetrachloride?

To draw a Lewis structure for carbon tetrachloride ($CC{l}_4$), you can follow a systematic process based on the octet rule developed by the American chemist Gilbert N. Lewis.12

Steps to Construct the Structure

1. Count Valence Electrons: First, determine the total number of valence electrons available for bonding. For $CC{l}_4$, carbon provides 4 electrons and each of the four chlorine atoms provides 7, resulting in a total of $4+(4\times 7)=32$ electrons.12
2. Arrange Atoms: Place the chemical symbols in an arrangement that reflects their connectivity, with carbon typically acting as the central atom surrounded by the four chlorine atoms.12
3. Add Bonding Pairs: Place one bonding pair (represented as a single line) between the central carbon atom and each of the four chlorine atoms.12
4. Distribute Remaining Electrons: Distribute the remaining electrons as lone pairs around the atoms until each atom achieves a share in an octet of electrons.12
5. Finalize Representation: Ensure each bonding pair is represented by a dash. In the final structure, the carbon atom is connected to four chlorine atoms, each of which retains three lone pairs to complete its octet.12

Note that Lewis structures represent the topological pattern of bonds rather than the actual three-dimensional shape of the molecule.12