The molecular shape of OCl2 A. None of the above B tetrahedral C. Bent D. Triagonal planar e. Linear
The Correct Answer and Explanation is:
The correct answer is C. Bent.
Explanation:
OCl₂ (oxygen dichloride) is a molecule that consists of an oxygen (O) atom bonded to two chlorine (Cl) atoms. To determine its molecular shape, we need to consider the electron pairs around the central atom (oxygen) and apply the VSEPR (Valence Shell Electron Pair Repulsion) theory.
- Electron Groups around Oxygen:
The oxygen atom in OCl₂ has two bonding pairs of electrons (from the two chlorine atoms) and two lone pairs of electrons. This gives a total of 4 electron pairs around the oxygen atom. - Electron Geometry:
With 4 electron pairs, the electron geometry is tetrahedral, which is the basic arrangement of these electron pairs around the central atom. However, the molecular shape is determined by the positions of the atoms, not the lone pairs. - Molecular Geometry:
The lone pairs of electrons occupy space, and they repel the bonding pairs. Because lone pairs are not visible in the molecular shape, they cause the bonding pairs to be pushed closer together, resulting in a bent geometry. This shape is similar to that of water (H₂O), where there are two lone pairs on the oxygen atom. - Bond Angles:
In a perfect tetrahedral structure, the bond angles are 109.5°. However, due to the repulsion from the lone pairs, the bond angle in OCl₂ will be slightly less, around 104.5°.
Conclusion:
Given the electron geometry is tetrahedral, but the molecular shape is influenced by the presence of lone pairs, the shape of OCl₂ is bent rather than tetrahedral. Hence, the correct answer is C. Bent.
