The correct answer is **B**: \[ \text{CCl}_4 \] is a nonpolar compound with \[ \text{C - Cl} \] bonds oriented in all directions.
### Explanation:
1. **Molecular Structure of \[ \text{CCl}_4 \]:**
- \[ \text{CCl}_4 \] (carbon tetrachloride) has a tetrahedral structure where the carbon atom is at the center and the four chlorine atoms are at the corners of the tetrahedron.
- The bond angles in \[ \text{CCl}_4 \] are approximately 109.5°, which is typical for a tetrahedral geometry.
2. **Polarity of \[ \text{CCl}_4 \]:**
- Although \[ \text{C - Cl} \] bonds are polar due to the difference in electronegativity between carbon and chlorine, the tetrahedral symmetry of \[ \text{CCl}_4 \] causes the dipole moments of the individual \[ \text{C - Cl} \] bonds to cancel each other out.
- This cancellation results in a nonpolar overall molecule.
3. **Electrical Conductivity:**
- For a substance to conduct electricity, it needs to have free-moving charged particles (such as ions or electrons).
- In \[ \text{CCl}_4 \], there are no free ions or electrons in the liquid or solid state.
- It is a covalent compound with no mobile charge carriers, so it cannot conduct electricity.
Thus, \[ \text{CCl}_4 \] does not conduct electricity because it is a nonpolar molecule and lacks mobile charge carriers.
