Explain the Hyberdaization scheme for the central atom&the molecular geometry of CO2.
C has two atoms attached which makes it sp hybridized and that makes it linear.
Hyberdization Means
To understand the hybridization scheme and molecular geometry of CO2, let's break down the steps:
1. Determine the Lewis structure:
Start by drawing a Lewis structure for CO2. The molecule consists of a carbon atom (C) bonded to two oxygen atoms (O) via double bonds. The central atom is the carbon atom, and the two oxygen atoms are attached to it.
2. Determine the valence electrons:
The carbon atom contributes four valence electrons, while each oxygen atom contributes six valence electrons. Therefore, the total number of valence electrons in CO2 is:
4 (carbon) + (2 × 6) (oxygen) = 16.
3. Determine the electron pairs around the central atom (carbon):
Due to the double bonds, each oxygen atom shares two electron pairs with the carbon atom. Therefore, there are four electron pairs (two bonding pairs and two non-bonding pairs) around the central carbon atom.
4. Determine the hybridization of the central atom:
The carbon atom undergoes hybridization to form sp hybrid orbitals. This occurs because the carbon atom forms two sigma bonds with the oxygen atoms using two of its electrons. The remaining two electrons are unpaired in two perpendicular p orbitals. These p orbitals on carbon do not participate in hybridization.
5. Determine the molecular geometry:
Since there are only two bonded electron pairs and no lone pairs around the central atom, the molecular geometry of CO2 is linear. The oxygen atoms are positioned on opposite sides of the carbon atom, giving CO2 a linear shape.
In conclusion, the hybridization scheme of the central carbon atom in CO2 is sp hybridization, and the molecular geometry is linear.