Which of following compounds shows octahedral geometry? 

CONCEPT:

Octahedral Geometry

• The octahedral geometry corresponds to a molecular structure in which six atoms, groups, or ligands are symmetrically arranged around a central atom, forming an octahedron.
• Octahedral geometry arises when the central atom has six regions of electron density, which can be bonding pairs or lone pairs. Examples include molecules like SF₆, where six fluorine atoms are symmetrically arranged around sulfur.
• The bond angles in octahedral geometry are typically 90°.

EXPLANATION:

• 1) XeF₂: Xenon difluoride has a linear geometry due to the presence of three lone pairs and two bonding pairs around xenon.
  
• 2) XeF₄: Xenon tetrafluoride has a square planar geometry due to two lone pairs and four bonding pairs around xenon.
  
• 3) XeO₃: Xenon trioxide has a pyramidal geometry due to one lone pair and three bonding pairs around xenon.
  
• 4) SF₆: Sulfur hexafluoride has an octahedral geometry because there are six bonding pairs and no lone pairs around sulfur.
  
• Thus, among the given compounds, SF₆ exhibits octahedral geometry.

Therefore, the correct answer is SF₆.