Questions: Draw the Lewis structure of SiCl4. What is the geometry? What are the bond angles? Is this molecule polar or non-polar?

Transcript text: Draw the Lewis structure of $\mathrm{SiCl}_{4}$. What is the geometry? What are the bond angles? Is this molecule polar or non-polar?

Solution

Solution Steps

Step 1: Draw the Lewis Structure of SiCl₄

Silicon (Si) is the central atom.
Silicon has 4 valence electrons, and each Chlorine (Cl) has 7 valence electrons.
Each Cl forms a single bond with Si, using one of Si's valence electrons.
The Lewis structure shows Si in the center with four Cl atoms bonded to it, each with three lone pairs of electrons.

Step 2: Determine the Geometry

SiCl₄ has four regions of electron density (four Si-Cl bonds) around the central Si atom.
According to VSEPR theory, four regions of electron density arrange themselves in a tetrahedral geometry to minimize repulsion.

Step 3: Identify the Bond Angles