Is SiCl₄ square planar or tetrahedral?

Silicon tetrachloride (SiCl₄) has a tetrahedral molecular geometry. This shape arises because the silicon atom is at the center, surrounded by four chlorine atoms at the corners of a tetrahedron.

Key Characteristics of SiCl₄

• Tetrahedral Shape: The bond angles in SiCl₄ are approximately 109.5 degrees.
• Bonding: Each silicon-chlorine bond is formed through single covalent bonds.
• Polarity: SiCl₄ is a nonpolar molecule due to its symmetrical shape.

Why Not Square Planar?

A square planar geometry typically occurs in molecules with a central atom bonded to four other atoms in a flat arrangement, often seen in transition metals with d-orbitals. Since SiCl₄ has no lone pairs on the silicon atom and all four bonds are equivalent, it adopts the tetrahedral configuration instead.