What is the Difference Between Hybrid and Degenerate Orbitals?
🆚 Go to Comparative Table 🆚The main difference between hybrid and degenerate orbitals lies in their formation and energy levels. Here are the key differences:
- Formation: Hybrid orbitals are formed by the combination of two or more atomic orbitals, a process known as hybridization. In contrast, degenerate orbitals already exist in an atom and do not need to be formed through hybridization.
- Energy Levels: Hybrid orbitals have the same energy, while degenerate orbitals in an atom have the same energy levels as well. However, hybrid orbitals are molecular orbitals, whereas degenerate orbitals are atomic orbitals.
In summary, hybrid orbitals are created through the mixing of atomic orbitals and have the same energy level, while degenerate orbitals are atomic orbitals with the same energy level that already exist in an atom before hybridization.
Comparative Table: Hybrid vs Degenerate Orbitals
Hybrid orbitals and degenerate orbitals are related concepts in quantum mechanics and chemistry. Here is a table summarizing the differences between them:
| Feature | Hybrid Orbitals | Degenerate Orbitals |
|---|---|---|
| Definition | Hybrid orbitals are formed by the combination of two or more atomic orbitals, creating new orbitals with the same energy. | Degenerate orbitals are atomic orbitals that have the same energy, such as the three p orbitals in a p subshell. |
| Formation | Hybrid orbitals are created through a process called hybridization. | Degenerate orbitals are a result of their atomic structure and energy levels. |
| Energy | All hybrid orbitals in a molecule have the same energy. | Degenerate orbitals in an atom have the same energy. |
| Geometry | Hybrid orbitals can have different geometries depending on the shape of the molecule and the number of hybrid orbitals formed. | The arrangement of degenerate orbitals depends on their energy levels and the atomic structure. |
| Examples | In BeH2, two equivalent sp hybrid orbitals are formed by combining the 2s orbital of beryllium and any one of the three degenerate 2p orbitals. | In a p orbital subshell, there are three atomic orbitals (px, py, pz) that differ in spatial arrangement but have the same energy. |
It is important to note that hybrid orbitals are molecular orbitals, while degenerate orbitals are atomic orbitals. Hybrid orbitals are used to explain the bonding patterns observed in most real molecules, while degenerate orbitals are a result of their atomic structure and energy levels.
- Pure vs Hybrid Orbitals
- Hybridized vs Unhybridized Orbitals
- Atomic Orbital vs Hybrid Orbital
- Molecular Orbital Theory vs Hybridization Theory
- Molecular Orbital vs Atomic Orbital
- Bonding vs Antibonding Molecular Orbitals
- Molecular Orbital Theory vs Valence Bond Theory
- Orbit vs Orbital
- Sigma vs Pi Molecular Orbitals
- Wobble vs Degeneracy
- Orbital Diagram vs Electron Configuration
- Degenerate vs Non-degenerate Semiconductor
- Molecular Geometry vs Electron Geometry
- sp3d2 vs d2sp3 Hybridization
- Spin vs Orbital Angular Momentum
- Px Py vs Pz Orbitals
- Hybridization vs Cloning
- Localized vs Delocalized Electrons
- 1s vs 2s Orbital