What is the molecular shape of OCl
? bent square planar linear see-saw tetrahedral
The Correct Answer and Explanation is:
The molecular shape of OCl₂ (oxygen dichloride) is bent.
Here’s a detailed explanation:
To determine the molecular shape of OCl₂, we use the VSEPR (Valence Shell Electron Pair Repulsion) theory. VSEPR theory states that the electron pairs around a central atom will arrange themselves in a way that minimizes the repulsion between them. This arrangement determines the molecular geometry.
Step-by-step analysis:
- Electron Configuration:
Oxygen (O) has six valence electrons, and each chlorine (Cl) atom has seven valence electrons, making a total of 20 valence electrons for OCl₂. - Lewis Structure:
In the Lewis structure of OCl₂, oxygen is the central atom, and it is bonded to two chlorine atoms through single bonds. The oxygen atom will have two lone pairs of electrons remaining after forming the bonds. - Electron Pair Geometry:
The central oxygen atom has two bonding pairs (from the two chlorine atoms) and two lone pairs. According to VSEPR theory, the arrangement of these four electron pairs around oxygen would result in a tetrahedral electron geometry. - Molecular Shape:
However, the molecular shape is determined by the positions of the atoms, not the electron pairs. Since the lone pairs are not visible in the molecular structure, they are ignored when determining the shape. The two bonding pairs and two lone pairs around oxygen cause the molecule to adopt a bent shape, similar to the molecular geometry of water (H₂O).
Therefore, the molecular shape of OCl₂ is bent due to the lone pairs on the oxygen atom pushing the bonding pairs closer together, creating a bond angle of about 110 degrees. This results in the bent shape observed in the molecule.
Thus, the correct answer to the question is bent.
