Solid carbon tetrachloride, CCl4(s), is represented by the diagram above [VISUAL]. The attractions b — Bonding Chemistry Question

STEPS:

1. Distinguish between intramolecular and intermolecular forces:
The question asks for the attractions *between* separate $\text{CCl}_4$ molecules that hold them together in the solid state. These are intermolecular forces. In contrast, chemical bonds (such as covalent bonds) are intramolecular forces that hold the carbon and chlorine atoms together *within* a single molecule.

2. Analyze the chemical bonds and symmetry within a single $\text{CCl}_4$ molecule:
Each carbon-chlorine ($\text{C-Cl}$) bond inside a carbon tetrachloride molecule is a polar covalent bond because of the difference in electronegativity between carbon and chlorine. However, the $\text{CCl}_4$ molecule features four of these equivalent polar bonds symmetrically arranged in a tetrahedral geometry around the central carbon atom.

3. Determine the overall molecular polarity:
Because of this highly symmetric tetrahedral arrangement, the individual $\text{C-Cl}$ bond dipoles point in opposite directions and cancel each other out completely. As a result, the $\text{CCl}_4$ molecule is entirely nonpolar.

4. Identify the type of intermolecular forces (IMFs) present:
Because $\text{CCl}_4$ molecules are nonpolar, they lack a permanent molecular dipole and cannot experience dipole-dipole attractions. Therefore, the only intermolecular forces capable of holding $\text{CCl}_4$ molecules together are London dispersion forces.

5. Relate London dispersion forces to temporary dipoles:
London dispersion forces are weak intermolecular attractions that arise from the constant motion of electrons within a molecule's electron cloud. This motion leads to momentary, uneven distributions of charge, producing temporary dipoles. These temporary dipoles then induce matching temporary dipoles in adjacent molecules, creating the attractions that hold $\text{CCl}_4(s)$ together in the solid state. This identifies Option C as the correct answer.

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WHY_OTHERS_WRONG:

• Options A and B are incorrect: Both polar covalent bonds (Option A) and nonpolar covalent bonds (Option B) are intramolecular forces that hold atoms together within a molecule. They do not represent the attractions acting between discrete covalent molecules in a molecular solid. Furthermore, the $\text{C-Cl}$ bonds themselves are polar, not nonpolar.
• Option D is incorrect: Attractions resulting from permanent dipoles (dipole-dipole forces) can only occur between polar molecules. Because $\text{CCl}_4$ is a symmetric, nonpolar molecule, it does not possess a permanent dipole.