Introduction to Atomic Orbitals

Study Notes

Orbitals are the areas around the nucleus of an atom where there is a high probability of finding electrons.
They describe the likely locations and energies of electrons in atoms.

s Orbitals
- Have a spherical shape.
- The nucleus is situated at the center.
- The size of the s orbital increases as the principal quantum number (n) increases.
- Each s orbital can accommodate a maximum of two electrons.
- S orbitals have the lowest energy level among all orbitals.
p Orbitals
- Have a dumbbell shape.
- There are three types of p orbitals (2px, 2py, 2pz), each oriented along one of the three axes (x, y, z).
- They have a nodal plane at the nucleus, where the probability of finding an electron is zero.
- Their size increases as the principal quantum number (n) increases.
- Each p orbital can accommodate a maximum of two electrons.
d Orbitals
- Have complex, cloverleaf-like or dumbbell shapes with a ring around the nucleus.
- There are five types of d orbitals (dxy, dyz, dzx, dx2-y2, dz2).
- They also increase in size with the principal quantum number (n).
- Important in the chemistry of transition metals, particularly in bonding and electron distribution.
- Each d orbital can accommodate a maximum of two electrons.

Orbitals are regions around the nucleus where there's a high probability of finding electrons.
The shape of an orbital describes the electron's probable location.
Orbitals are filled in order of increasing energy level.

D orbitals are more complex in shape, often resembling cloverleaves.
There are five D orbitals (dxy, dyz, dzx, dx2-y2, dz2).
D orbitals are found in energy levels starting from the third (n = 3).
They increase in size with increasing principal quantum number (n).
They are important for the chemistry of transition metals involved in bonding and electron distribution.
They can each hold up to 2 electrons.