Complete the table below for the composition of hybrid orbitals. Linear Trigonal Planar Tetrahedral Trigonal Bipyramidal Octahedral Atomic orbitals mixed Hybrid orbitals formed Unhybridized orbitals remaining s s s s s p p p p p d d sp s
s
s
d s
d
p p p d d
The Correct Answer and Explanation is:
Here’s the completed table for the composition of hybrid orbitals:
| Molecular Geometry | Atomic Orbitals Mixed | Hybrid Orbitals Formed | Unhybridized Orbitals Remaining |
|---|---|---|---|
| Linear | 1 s, 1 p | sp | 2 p |
| Trigonal Planar | 1 s, 2 p | sp² | 1 p |
| Tetrahedral | 1 s, 3 p | sp³ | 0 |
| Trigonal Bipyramidal | 1 s, 3 p, 1 d | sp³d | 4 d |
| Octahedral | 1 s, 3 p, 2 d | sp³d² | 3 d |
Explanation
Hybridization is a concept in valence bond theory where atomic orbitals mix to form new, equivalent hybrid orbitals. These hybrids explain molecular shapes more accurately, aligning with VSEPR (Valence Shell Electron Pair Repulsion) theory predictions.
- Linear Geometry (sp hybridization): This involves the mixing of one s and one p orbital, forming two sp hybrid orbitals that arrange linearly at 180°. The two remaining unhybridized p orbitals can be used in forming π bonds, as seen in molecules like BeCl₂ or CO₂.
- Trigonal Planar Geometry (sp² hybridization): One s and two p orbitals mix to form three sp² hybrid orbitals arranged in a trigonal planar shape (120° bond angles). One p orbital remains unhybridized, available for π bonding, as in BF₃ or ethene (C₂H₄).
- Tetrahedral Geometry (sp³ hybridization): One s and three p orbitals combine to form four sp³ orbitals, oriented at 109.5° to each other. This accounts for molecules like CH₄ and NH₃. All valence orbitals are hybridized, so no unhybridized p orbitals remain.
- Trigonal Bipyramidal Geometry (sp³d hybridization): One s, three p, and one d orbital mix to create five sp³d hybrid orbitals, giving rise to a trigonal bipyramidal shape (e.g., PCl₅). Four d orbitals remain unhybridized.
- Octahedral Geometry (sp³d² hybridization): One s, three p, and two d orbitals combine to form six sp³d² hybrid orbitals, yielding an octahedral geometry (e.g., SF₆). Three d orbitals remain unhybridized.
These hybridizations help explain the observed bond angles, molecular shapes, and bonding behaviors of covalently bonded molecules.
