Which of the following molecules will have zero dipole moment:
`SiCl_(4), H_(2)O, CO_(2), BF_(3), NH_(3)`?

Explanation

To determine which of the given molecules has a zero dipole moment, we need to analyze the molecular geometry and the distribution of electron density in each molecule. The molecules in question are SiCl4, H2O, CO2, BF3, and NH3.

### Step-by-Step Solution:

1. **SiCl4 (Silicon Tetrachloride)**:
- **Hybridization**: Silicon (Si) has 4 valence electrons and forms 4 bonds with chlorine (Cl). The hybridization is sp³.
- **Molecular Geometry**: The shape is tetrahedral.
- **Dipole Moment**: The individual dipole moments of the Si-Cl bonds point towards the chlorine atoms. However, due to the symmetrical tetrahedral shape, these dipole moments cancel each other out, resulting in a net dipole moment of zero.
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