Choose the hybridization for the carbon atom in CO2.
sp³d
sp2
sp³
sp
The correct answer and explanation is :
The correct hybridization for the carbon atom in carbon dioxide (CO₂) is sp.
Explanation:
In the CO₂ molecule, carbon is at the center, bonded to two oxygen atoms through double bonds. To determine the hybridization of carbon, we need to consider the following factors:
- Valence Shell Electron Pair Repulsion (VSEPR) Theory: According to VSEPR theory, the carbon atom in CO₂ forms two regions of electron density, each associated with a double bond to an oxygen atom. The electron density is arranged linearly to minimize repulsion, meaning the geometry is linear, with an angle of 180° between the bonds. This linear shape indicates that the carbon atom must have two regions of electron density, corresponding to sp hybridization.
- Bonding and Hybridization:
- In sp hybridization, one 2s orbital combines with one 2p orbital to form two sp hybrid orbitals.
- These two sp hybrid orbitals are oriented linearly (180° apart), which allows for the formation of two σ (sigma) bonds, one with each oxygen atom.
- The remaining unhybridized p orbitals on the carbon atom overlap with unhybridized p orbitals on the oxygen atoms to form two π (pi) bonds, which are responsible for the double bonds in CO₂.
- Electron Configuration:
- The carbon atom in its ground state has the electron configuration 1s² 2s² 2p². In CO₂, it undergoes hybridization where the 2s and one of the 2p orbitals combine to form two sp hybrid orbitals. The other two 2p orbitals remain unhybridized and are used for the formation of the π bonds.
Thus, the carbon atom in CO₂ adopts sp hybridization, which corresponds to a linear molecular shape.
Image of CO₂ Structure with Hybridization:
Let me generate an image to illustrate the structure and hybridization of CO₂.
Here is an illustration of the CO₂ molecule with the sp hybridization of the carbon atom, showing the linear structure and bond angles. The carbon atom forms sigma bonds with oxygen using sp hybrid orbitals and pi bonds using unhybridized p orbitals.