Identify the hybridization of the central atom in CO2.

Identify the hybridization of the central atom in CO2.

Step 1: Identify the central atom in CO2. The central atom is carbon (C).
Step 2: Count the number of valence electrons for carbon. Carbon has 4 valence electrons.
Step 3: Determine how many bonds carbon needs to form to satisfy the octet rule. Carbon needs 4 more electrons to have 8.
Step 4: Identify the surrounding atoms. In CO2, there are two oxygen (O) atoms.
Step 5: Each oxygen atom can form a double bond with carbon. This means carbon will form 2 double bonds.
Step 6: Determine the hybridization based on the number of bonds. Carbon forms 2 double bonds, which corresponds to sp hybridization.
Step 7: Conclude that the hybridization of the central atom (carbon) in CO2 is sp.

Hybridization – The concept of hybridization involves the mixing of atomic orbitals to form new hybrid orbitals that can accommodate bonding.
Molecular Geometry – Understanding the molecular geometry helps in determining the hybridization state of the central atom.
Bonding Types – Recognizing the types of bonds (single, double, triple) formed by the central atom is crucial for determining hybridization.