What is the Difference Between Orbit and Orbital?
🆚 Go to Comparative Table 🆚The terms "orbit" and "orbital" are often used in the context of atomic structure, but they have distinct meanings:
- Orbit: An orbit refers to the fixed path along which electrons revolve around the atom's nucleus. It is a simple planar representation, meaning it is two-dimensional. An orbit is non-directional in nature, which means the shape of an atom cannot be described by an orbit.
- Orbital: An orbital, on the other hand, is a three-dimensional (3-D) space surrounding the nucleus of an atom, representing the probable area where an electron can be found with maximum density. Orbitals can describe the shape of an atom, as they are directional by nature.
In summary:
- Orbits are fixed paths for electrons to revolve around the nucleus, while orbitals are probabilistic areas where electrons are most likely to be found.
- Orbits are 2-dimensional, whereas orbitals are 3-dimensional.
- Orbits are non-directional and cannot describe the shape of an atom, while orbitals are directional and can describe the shape of an atom.
Comparative Table: Orbit vs Orbital
Here is a table comparing the differences between an orbit and an orbital:
| Feature | Orbit | Orbital |
|---|---|---|
| Definition | An orbit is the simple planar representation of an electron or the circular or elliptical path followed by the electrons around the nucleus. | An orbital refers to the dimensional motion of an electron around the nucleus in a three-dimensional motion or the possible area where an electron can be found. |
| Nature | Orbits are fixed paths with a well-defined radius and circumference. | Orbitals are probabilistic regions where electrons are most likely to be found. |
| Shape | Orbits can be circular or elliptical. | Orbitals can have various shapes, such as s, p, d, and f orbitals. |
| Quantization | Orbits are quantized, meaning they have specific energy levels. | Orbitals are not quantized and can have continuous energy levels. |
| Heisenberg's Uncertainty Principle | Orbits violate Heisenberg's Uncertainty Principle, as they do not allow for the simultaneous determination of position and momentum of a subatomic particle. | Orbitals adhere to Heisenberg's Uncertainty Principle, as they deal with probabilities rather than exact positions. |
In summary, an orbit is a fixed path where electrons revolve around the nucleus, while an orbital is a three-dimensional region where electrons are most likely to be found. Orbits are quantized and violate Heisenberg's Uncertainty Principle, whereas orbitals are probabilistic and adhere to the principle.
Read more:
- Escape Velocity vs Orbital Velocity
- Molecular Orbital vs Atomic Orbital
- Atomic Orbital vs Hybrid Orbital
- Spin vs Orbital Angular Momentum
- Geosynchronous vs Geostationary Orbit
- Orbital Diagram vs Electron Configuration
- 1s vs 2s Orbital
- Rotation vs Revolution
- Circle vs Sphere
- Planet vs Moon
- Pure vs Hybrid Orbitals
- Ball vs Sphere
- Gravity vs Gravitation
- Atmosphere vs Space
- Circle vs Ellipse
- Star vs Planet
- Hybridized vs Unhybridized Orbitals
- Hyperbola vs Ellipse
- Hybrid vs Degenerate Orbitals