You're asking about the electron configuration of the molecule CCl₄ (carbon tetrachloride), not a single atom. Here's how to approach it:

1. Focus on Bonding:

* CCl₄ is a covalent molecule. The carbon atom forms four single bonds with four chlorine atoms.

* To determine the electron configuration, we need to consider the sharing of electrons in these bonds.

2. Lewis Structure:

* Carbon (C): Has 4 valence electrons (2s²2p²). It needs to share 4 electrons to complete its octet.

* Chlorine (Cl): Has 7 valence electrons (3s²3p⁵). Each chlorine needs to share 1 electron to complete its octet.

The Lewis structure for CCl₄ shows carbon at the center with four chlorine atoms surrounding it, each connected by a single bond.

3. Simplified Electron Configuration:

* Since we're dealing with a molecule, we can simply say that each atom in CCl₄ has a filled outer shell after bonding.

* Carbon effectively has 8 valence electrons (due to sharing), fulfilling the octet rule.

* Each chlorine also has 8 valence electrons (due to sharing), fulfilling the octet rule.

Important Note: You won't see a specific "electron configuration" like you would for an atom. In molecules, the electrons are delocalized in bonding orbitals.