The carbon atom requires additional electrons to form four bonds with hydrogen and other carbon atoms in the synthesis of C2H2.
What is the Hybridization of Ethyne?
- Ethyne molecules are essentially 2 CH molecules when broken down. However, we'll first draw the orbital diagrams of the carbon and hydrogen molecules individually.
- When we do this, we will see that hydrogen has one electron and carbon has six.
- Now, if we look at the electronic structure of carbon in its ground state, we can see that it is represented as 1s2 2s2 2p2. The electrical configuration will change to 1s2 2s1 2px12py1 2pz1 when it enters an excited state.
- One of the electrons from the 2s orbital will transfer or jump to the 2pz orbital. The 2s1 and 2pz1 orbitals get hybridized as a result of the CH molecule's single hydrogen atom.
- As a result, four sp hybridized orbitals are formed, with two of them being formed by each CH molecule.
- When two sp orbitals from each carbon overlap with the hydrogen's 1s orbital during hybridization, two C-H bonds are generated, forming a C-C sigma bond when each carbon's second sp orbital overlaps with the hydrogen's s orbital.
- There will be two partially filled 2p orbitals on the carbon atom in this scenario.
- As a result of the formation of two pi bonds rather than participating in the hybridization, these two pairs of p orbitals create a triple bond.
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