What Is the Main Difference Between Orbit and Orbital in Science?
The Difference Between Orbit And Orbital is a fundamental topic in atomic structure, often asked in competitive and board exams. Understanding their distinction helps students accurately explain how electrons are arranged around the nucleus, which is essential for mastering chemistry concepts.
Definition of Orbit
An orbit is a fixed two-dimensional path around the nucleus where, according to Bohr’s model, an electron revolves with a definite energy.
Each orbit corresponds to a specific energy level, denoted as K, L, M, N, etc., and shows where electrons are likely to be found in classical atomic models. Related atomic structure comparisons include Difference Between Mass And Weight.
Definition of Orbital
An orbital is a three-dimensional region around the nucleus where the probability of finding an electron is maximum, described by quantum mechanical models.
Orbitals have various shapes (spherical, dumbbell, etc.) like s, p, d, and f, and are defined by four quantum numbers, representing the probable location and energy of electrons.
Difference Table
| Orbit | Orbital |
|---|---|
| Fixed circular path in Bohr's atomic model | Three-dimensional region in quantum mechanical model |
| Two-dimensional representation | Three-dimensional space |
| Described by principal quantum number (n) only | Defined by four quantum numbers (n, l, m, s) |
| Visualized as concentric circles | Visualized as electron clouds or shapes |
| Classical concept from Bohr’s theory | Modern concept from quantum mechanics |
| Specifies definite path of electron | Specifies probable location of electron |
| No sub-types | Types like s, p, d, and f orbitals |
| Can accommodate 2n2 electrons per shell | Holds maximum two electrons with opposite spins |
| Does not consider Pauli Exclusion Principle | Obeys Pauli Exclusion Principle |
| Does not account for uncertainty principle | Accounts for Heisenberg's uncertainty principle |
| Does not indicate probability of electron presence | Indicates high probability area for electron presence |
| Movement of electron is certain in a path | Movement of electron is probabilistic |
| Explains hydrogen atom structure only | Explains structures for all atoms |
| No nodal planes in orbits | Presence of nodal planes in orbitals |
| Energy level differences between orbits are fixed | Energy within orbitals varies within the same shell |
| Path can be depicted exactly | Path cannot be depicted exactly |
| Based on early atomic models | Based on quantum and wave mechanical models |
| No specific shape for orbits except circular | Orbitals have specific shapes (s, p, d, f) |
| Mainly theoretical now | Widely accepted and used in modern chemistry |
| Used for simple atomic structure explanation | Used for detailed electron configuration and chemical bonding |
Key Differences
- Orbit is a fixed path; orbital is a region of probability
- Orbits are two-dimensional, while orbitals are three-dimensional
- Orbit concept belongs to Bohr’s model; orbital comes from quantum theory
- Orbitals have specific shapes; orbits are only circular
- Each orbital holds two electrons; a shell (orbit) holds up to 2n2 electrons
Examples
In a hydrogen atom, the electron in n=2 is said to be in the second orbit in Bohr’s model, while quantum mechanics states it is in a 2s or 2p orbital, depending on quantum numbers as discussed in Difference Between Electric Field And Magnetic Field.
A 1s orbital is spherical in shape and holds a maximum of two electrons, while the first Bohr orbit is a shell around the nucleus with a fixed radius.
Applications
- Orbits are useful for basic atomic structure explanation
- Orbitals determine electron configuration of elements
- Orbitals are key in explaining chemical bonding
- Orbitals are essential in molecular geometry prediction
- Used in spectroscopy for transition prediction
- Helps explain periodic trends and properties
One-Line Summary
In simple words, Orbit is a fixed circular path prescribed by Bohr, whereas Orbital is a quantum mechanical region with the highest probability of finding an electron.
FAQs on Understanding the Difference Between Orbit and Orbital
1. What is the difference between an orbit and an orbital?
An orbit is the fixed circular or elliptical path that an electron follows around the nucleus, while an orbital is a 3-dimensional region in space where there is a high probability of finding an electron.
Key differences:
- Orbit: Defined path, based on Bohr’s model, classical in nature
- Orbital: Region of high electron probability (quantum mechanical), does not have a fixed path
- Orbit deals with fixed energy levels, orbital deals with shapes (s, p, d, f)
2. Define orbit in chemistry.
Orbit in chemistry describes the circular or elliptical path traced by an electron as it revolves around an atom's nucleus, according to Bohr’s atomic model.
- Represents a definite fixed path
- Electrons have a precise energy and distance from the nucleus
- Concept is classical and less accurate for modern atomic theory
3. What do you mean by an orbital?
An orbital is the region in an atom where the probability of finding an electron is maximum. It is described by quantum mechanics.
- Does not specify a fixed path, but a probability region
- Each orbital has a specific shape (e.g. spherical for s, dumbbell-shaped for p)
- Orbitals are denoted as s, p, d, f
4. How do orbits and orbitals differ in terms of electron position?
Orbits represent exactly where an electron moves, while orbitals give a probability region where electrons are likely to be found.
- Orbit: Precise position and path
- Orbital: Uncertainty in exact position, described statistically
5. What are the types of atomic orbitals?
Atomic orbitals are of four main types: s, p, d, and f.
- s orbital: Spherical shape
- p orbital: Dumbbell shape
- d orbital: Cloverleaf shape
- f orbital: Complex shapes
6. What are the main similarities between an orbit and an orbital?
Both orbit and orbital refer to concepts related to the position of electrons in an atom.
- Both concepts describe locations associated with electrons
- Both are connected to energy levels within an atom
- Used to explain the arrangement and behavior of electrons
7. Differentiate between orbit and orbital with examples.
An orbit is like the path a planet takes around the sun, while an orbital is like a cloud where you’re most likely to find an electron.
- Orbit (e.g. Bohr’s second shell): Electron travels in a fixed ring
- Orbital (e.g. 2p orbital): Probability cloud shaped like a dumbbell in the second energy level
8. Are orbitals real paths like orbits?
Orbitals are not real, fixed paths; they are regions defined by the likelihood of finding an electron at any time.
- Orbitals are probability zones, not set pathways
- Based on quantum mechanical principles, not classic paths
9. Why did the concept of orbitals replace orbits in modern atomic theory?
The concept of orbitals replaced orbits because quantum mechanical models showed that electrons do not move in fixed paths, but rather exist in regions of high probability.
- Orbitals give a more accurate description of electron arrangement
- Heisenberg’s uncertainty principle disproved the possibility of knowing exact electron paths and positions
10. Explain with points why orbitals are important in the study of atoms.
Orbitals are crucial in atomic theory because they:
- Define where electrons are most likely to be found
- Determine chemical bonding and properties of elements
- Explain the shapes and structures of molecules
- Help predict the arrangement of electrons in multi-electron atoms
11. What are the key differences between orbit and orbital for CBSE Class 11?
For CBSE Class 11 chemistry, key differences are:
- Orbit: Fixed circular/elliptical path, classical concept
- Orbital: Probability region, quantum mechanical concept
- Orbit describes energy levels; orbital describes sub-levels and shapes
12. Can two electrons occupy the same orbital? If yes, how?
Yes, two electrons can occupy the same orbital, provided they have opposite spins, as per the Pauli Exclusion Principle.
- Maximum of 2 electrons per orbital
- Each electron must have opposite spin quantum numbers
