Identify the hybridization of the central atom in CO2.

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Question: Identify the hybridization of the central atom in CO2.

Options:

Correct Answer: sp

Solution:

Carbon in CO2 is sp hybridized, forming two double bonds with oxygen.

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.