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

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?
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Solution

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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
  • In a tetrahedral geometry, the bond angles between the bonds are 109.5 degrees.

Final Answer

  • Geometry: Tetrahedral
  • Bond Angles: 109.5 degrees
  • Polarity: Non-polar (since the molecule is symmetrical and the dipoles cancel out)
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