Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in valence bond theory. Hybrid orbitals are useful in the explanation of the shape and bonding properties of molecules. For example, carbon atoms form four bonds, but carbon's electron configuration is $2s^2 2p^2$. Hybridization theory explains how carbon forms four equivalent bonds by mixing the $2s$ and $2p$ orbitals to create four $sp^3$ hybrid orbitals.
This worksheet will test your knowledge of these concepts. Let's begin!
Match the following terms with their correct definitions:
| Term | Definition |
|---|---|
| 1. $sp^3$ | A. The mixing of one s and two p atomic orbitals |
| 2. $sp^2$ | B. The mixing of one s and three p atomic orbitals |
| 3. $sp$ | C. The mixing of one s and one p atomic orbitals |
| 4. Sigma Bond ($\sigma$) | D. A covalent bond resulting from the end-to-end overlap of atomic orbitals |
| 5. Pi Bond ($\pi$) | E. A covalent bond resulting from the side-by-side overlap of atomic orbitals |
(Match the numbers to the letters)
Complete the following paragraph with the correct words:
In methane ($CH_4$), carbon undergoes $_______$ hybridization. This results in four $_______$ orbitals that are arranged in a $_______$ geometry. Each hybrid orbital forms a $_______$ bond with a hydrogen atom. The bond angle between each $C-H$ bond is approximately $_______$ degrees.
Explain how hybridization affects the shape and properties of molecules. Provide an example to illustrate your answer.
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