Скачать или смотреть sp² Hybridization Explained Using Ethylene (Ethene) | Sigma and Pi Bonds Made Easy

sp² Hybridization Explained Using Ethylene (Ethene) | Sigma and Pi Bonds Made Easy

We explore sp² orbital hybridization using ethylene (ethene) as a classic and important example from Organic Chemistry. This concept is essential for understanding alkenes, double bonds, molecular geometry, and reactivity.

We begin by reviewing the atomic orbitals of carbon (2s and 2p) and explain how one s orbital mixes with two p orbitals to form three equivalent sp² hybrid orbitals. These hybrid orbitals lie in the same plane, arranged at 120°, giving ethylene its trigonal planar geometry around each carbon atom.

Next, we analyze bond formation in ethylene:
Each carbon uses its three sp² hybrid orbitals to form sigma (σ) bonds
One unhybridized p orbital remains on each carbon
These unhybridized p orbitals overlap side-by-side to form a pi (π) bond
Bonding Summary in Ethylene (C₂H₄):

✔️ 5 sigma (σ) bonds

4 C–H σ bonds

1 C–C σ bond

✔️ 1 pi (π) bond

Formed from sideways overlap of unhybridized p orbitals

✔️ Total bonds: 6

The C=C double bond consists of 1 sigma + 1 pi bond

This step-by-step explanation helps students visualize orbital overlap, bond types, and molecular structure, making sp² hybridization easier to understand and apply in exams and reaction mechanisms.

links: https://www.youtube.com/live/en7ISH9a...

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