Comparing Orbits and Orbitals: Similarities and Differences Explained

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Orbits and orbitals both describe the movement of electrons around an atom, with orbits representing a two-dimensional circular path and orbitals indicating a three-dimensional volume where electrons are likely to be found. The key difference lies in their dimensionality, as orbits are flat and defined by Bohr's model, while orbitals encompass a range of probable locations for electrons. Additionally, orbitals can represent complex shapes based on quantum mechanics, unlike the simpler circular nature of orbits. Both concepts are essential for understanding atomic structure and electron behavior. This distinction is crucial for grasping the fundamentals of quantum chemistry.
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Homework Statement


describe one way in which orbits are similar and two ways in which they are different


Homework Equations


N/A

The Attempt at a Solution


the differences:
first, the orbital is a 3-dimensional volume of space where the probability of finding some electron is very probable
The orbit, on the other hand, is 2-dimensional (a circle) and comes from Bohr's model.
the similarity:
an orbit is a path an electron takes around an atom and the orbital is shape resulting in the combination of all probable orbits
 
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is this correct or anything that should be changed?
 
Hi,
i think in general you are correct.
Orbit: revolving path of electron around nucleus.
Orbital: may be a 3D space (surface, or volume).
 
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