Rules for Filling Electrons in Orbitals An orbital is a region of space surrounding the nucleus where the probability of finding an electron is highest. Elec...
An orbital is a region of space surrounding the nucleus where the probability of finding an electron is highest. Electrons are negatively charged particles with a half-integer spin, which means they can exist in orbitals that are either symmetric or asymmetrical.
Filling Orbitals:
Electrons are first filled into orbitals with spherical shapes before occupying orbitals with more complex shapes.
Each orbital can hold 2 electrons in a spherical orbital.
The order of filling orbitals follows increasing energy levels and decreasing angular momentum quantum numbers (l).
The s orbitals are spherical and have l = 0.
The p orbitals have l = 1 and are dumbbell-shaped.
The d orbitals have l = 2 and have four lobes with increasing distance from the nucleus.
Important Points:
Electrons can only occupy orbitals that intersect the region of space where the probability of finding them is highest.
The angular momentum quantum number (l) describes the orientation of the orbital in space.
The l = 0 orbitals are symmetric, while the l = 1 orbitals are dumbbell-shaped.
The l = 2 orbitals have four lobes with increasing distance from the nucleus.
Examples:
The 1s orbital is spherical and has l = 0.
The 2s orbital is spherical and has l = 0.
The 2p orbital has three lobes with increasing distance from the nucleus.
The 3d orbital has four lobes with increasing distance from the nucleus