To draw the Lewis structure for CCl4, follow these steps:

1. Count the total number of valence electrons for CCl4, where C contributes 4 valence electrons and each Cl contributes 7 valence electrons. The total is 4 + (4 × 7) = 32 valence electrons.

2. Place the least electronegative atom, carbon (C), in the center. Connect the carbon atom to each chlorine atom (Cl) using a single bond.

Cl Cl
\ /
C
/ \
Cl Cl

3. Distribute the remaining electrons around the atoms to fulfill the octet rule (except for hydrogen, which only needs 2 electrons). Start with the chlorine atoms. Place 6 electrons (3 lone pairs) around each of the chlorine atoms to satisfy their octets.

Cl Cl
\ /
C
/ \
Cl Cl
| |

4. Place the remaining electrons on the central carbon atom. Since each chlorine atom already has 3 lone pairs, carbon needs 8 electrons (4 lone pairs) to complete its octet. Place these lone pairs on the carbon atom.

Cl Cl
\ /
C
/ \
Cl Cl
| |
: : : :

5. Check if all atoms have a complete octet. In this case, carbon and chlorine have complete octets.

6. If there are any remaining electrons, try forming double or triple bonds to see if you can eliminate any formal charges. However, in the case of CCl4, all the formal charges are zero and the octets are complete, so there is no need for double or triple bonds.

The final Lewis structure for CCl4 is:

Cl Cl
\ /
C
/ \
Cl Cl

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