5.13: Orbitals

The flight path of a commercial airliner is carefully regulated by the Federal Aviation Administration. Each airplane must maintain a distance of five miles from another plane flying at the same altitude and 2,000 feet above and below another aircraft (1,000 feet if the altitude is less than 29,000 feet). So, each aircraft only has certain positions it is allowed to maintain while it flies. As we explore quantum mechanics, we see that electrons have similar restrictions on their locations.

We can apply our knowledge of quantum numbers to describe the arrangement of electrons for a given atom. We do this with something called electron configurations. They are effectively a map of the electrons for a given atom. We look at the four quantum numbers for a given electron and then assign that electron to a specific orbital in the next Module.

\(s\) Orbitals

For any value of \(n\), a value of \(l=0\) places that electron in an \(s\) orbital. This orbital is spherical in shape:

Figure \(\PageIndex{1}\): \(s\) orbitals have no orientational preference and resemble spheres.

\(p\) Orbitals

Fro the table below, we see that we can have three possible orbitals when \(l=1\). These are designated as \(p\) orbitals and have dumbbell shapes. Each of the \(p\) orbitals has a different orientation in three-dimensional space.

Figure \(\PageIndex{2}\): \(p\) orbitals have an orientational preference and resemble dumbells.

\(d\) Orbitals

When \(l=2\), \(m_l\) values can be \(-2, \: -1, \: 0, \: +1, \: +2\) for a total of five \(d\) orbitals. Note that all five of the orbitals have specific three-dimensional orientations.

Figure \(\PageIndex{3}\): \(d\) orbitals have an orientational preference and exhibit complex structures.

\(f\) Orbitals

The most complex set of orbitals are the \(f\) orbitals. When \(l=3\), \(m_l\) values can be \(-3, \: -2, \: -1, \: 0, \: +1, \: +2, \: +3\) for a total of seven different orbital shapes. Again, note the specific orientations of the different \(f\) orbitals.

Figure \(\PageIndex{4}\): \(d\) orbitals have an orientational preference and exhibit quite complex structures.

Orbitals that have the same value of the principal quantum number form a shell. Orbitals within a shell are divided into subshells that have the same value of the angular quantum number. Some of the allowed combinations of quantum numbers are compared in Table\(\PageIndex{1}\).

Table \(\PageIndex{1}\): Electron Arrangement Within Energy Levels

Principal Quantum Number \(\left( n \right)\)	Allowable Sublevels	Number of Orbitals per Sublevel	Number of Orbitals per Principal Energy Level	Number of Electrons per Sublevel	Number of Electrons per Principal Energy Level
1	\(s\)	1	1	2	2
2	\(s\)	1	4	2	8
	\(p\)	3		6
3	\(s\)	1	9	2	18
	\(p\)	3		6
	\(d\)	5		10
4	\(s\)	1	16	2	32
	\(p\)	3		6
	\(d\)	5		10
	\(f\)	7		14

Summary

There are four different classes of electron orbitals. These orbitals are determined by the value of the angular momentum quantum number \(l\).

Contributors

• CK-12 Foundation by Sharon Bewick, Richard Parsons, Therese Forsythe, Shonna Robinson, and Jean Dupon.