# General Chemistry/Shells and Orbitals

## Electron shells[edit]

Each **shell** is subdivided into **subshells**, which are made up of **orbitals**, each of which has electrons with different angular momentum. Each orbital in a shell has a characteristic shape, and is named by a letter. They are: **s**, **p**, **d**, and **f**. In a one-electron atom (e.g. H, He^{+}, Li^{+2}, etc.) the energy of each orbital within a particular shell is identical. However, when there are multiple electrons, they interact and split the orbitals into slightly different energies. Within any particular shell, the energy of the orbitals depend on the angular momentum of orbitals s, p, d, and f in order of lowest to highest energy. No two orbitals have the same energy level.

This image shows the orbitals (along with hybrid orbitals for bonding and a sample electron configuration, explained later).

## The s orbital[edit]

The simplest orbital in the atom is the 1s orbital. It has no radial or angular *nodes*: the 1s orbital is simply a sphere of electron density. A node is a point where the electron probability is zero. As with all orbitals the number of radial nodes increases with the principle quantum number (i.e. the 2s orbital has one radial node, the 3s has two etc.). Because the angular momentum quantum number is 0, there is only one choice for the magnetic quantum number - there is only one s orbital per shell. The s orbital can hold two electrons, as long as they have different spin quantum numbers.

## The p orbitals[edit]

Starting from the 2nd shell, there is a set of p orbitals. The angular momentum quantum number of the electrons confined to p orbitals is 1, so each orbital has one **angular node**. There are 3 choices for the magnetic quantum number, which indicates 3 differently oriented p orbitals. Finally, each orbital can accommodate two electrons (with opposite spins), giving the p orbitals a total capacity of 6 electrons.

The p orbitals all have two lobes of electron density pointing along each of the axes. Each one is symmetrical along its axis. The notation for the p orbitals indicate which axis it points down, i.e. p_{x} points along the x axis, p_{y} on the y axis and p_{z} up and down the z axis. The p orbitals are **degenerate** — they all have the same energy. P orbitals are very often involved in **bonding**.

2p_{x} |
2p_{y} |
2p_{z} |
---|---|---|

## The d orbitals[edit]

The first set of d orbitals is the 3d set. The angular momentum quantum number is 2, so each orbital has two **angular nodes**. There are 5 choices for the magnetic quantum number, which gives rise to 5 different d orbitals. Each orbital can hold two electrons (with opposite spins), giving the d orbitals a total capacity of 10 electrons.

Note that all the d orbitals have four lobes of electron density, except for the d_{z2} orbital, which has two opposing lobes and a doughnut of electron density around the middle. The d orbitals can be further subdivided into two smaller sets. The d_{x2-y2} and d_{z2} all point directly along the x, y, and z axes. They form an **e _{g}** set. On the other hand, the lobes of the d

_{xy}, d

_{xz}and d

_{yz}all line up in the quadrants, with no electron density on the axes. These three orbitals form the

**t**set. In most cases, the d orbitals are

_{2g}**degenerate**, but sometimes they can split, with the e

_{g}and t

_{2g}subsets having different energy.

**Crystal Field Theory**predicts and accounts for this. D orbitals are sometimes involved in bonding, especially in inorganic chemistry.

## The f orbitals[edit]

The first set of f orbitals is the 4f subshell. There are 7 possible magnetic quantum numbers, so there are 7 f orbitals. Their shapes are fairly complicated, and they rarely come up when studying chemistry. There are 14 f electrons because each orbital can hold two electrons (with opposite spins).