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Electron Orbitals & Orbital Shapes

What is an Electron Orbital?

Electron orbitals are the three-dimensional areas around the nucleus of an atom where a particular electron resides. Each orbital can hold two electrons. They are also known as atomic orbitals. Atomic orbitals come in different shapes, depending on the number of electrons the atom has. We will learn about the s orbital, p orbital, d orbital and f orbital. We will also learn their orbital shapes.

The precise definition of an orbital, is a mathematical function that describes the location of an electron in an atom, based on probability. “Atomic orbital” generally refers to the region of space where an electron could possibly be present, based on the mathematical function for that orbital.

Degenerate orbitals are orbitals in the same main energy level and sublevel that have different orientations. For example, the 5 orientations of d-orbitals on the 3D-plane are degenerate orbitals.

atomic orbitals electron orbitals

Basic Review of the Quantum Numbers

For more details on the quantum numbers, check out our quantum numbers article! There are four quantum numbers that tell the energy level, shape, orientation, and electron spin of orbitals.

  1. Principal Quantum Number (n): indicates main energy level of an electron. The higher the principal quantum number is, the higher the energy level, and therefore the more the distance is between the nucleus and the particular electron.
  2. Angular Momentum Quantum Number (l): indicates the shape of an orbital. Different values of l correspond to specific shapes of electron orbitals. This will be discussed more in detail later.
  3. Magnetic Quantum Number (m): indicates the orientation of an orbital around the nucleus. Because different orbitals have different shapes, they can be rotated around the a 3D-coordinate plane many orientations.
  4. Spin Quantum Number: indicates the direction in which an electron in an orbital is spinning. There are only two possible values of the spin quantum number: -1/2 and +1/2. There are a maximum of two electrons per orbital, and if they both reside in the orbital, they must be spinning the opposite directions (meaning they have the opposite spin quantum number).

Angular Momentum Quantum Number & Orbital Shapes

The angular momentum quantum number has integer values from 0 to (n-1). So, if the principal quantum number (n) = 4, the angular momentum quantum numbers are 0, 1, 2, and 3.

Each angular momentum quantum number represents a letter, which corresponds to a specific shape of an orbital. As you can see, the higher the principal quantum number, the higher the angular momentum quantum number, and the more complex the orbital shape becomes. Mostly, you will only need to know the s orbital, p orbital, d orbital, and f orbitals — after the f orbital, the shapes become too complicated.

Principal Quantum # (n)Angular Momentum Quantum # (l)LetterOrbital Shape Diagram
10sFile:S Orbital.png - Wikimedia Commons
21pFile:Diagram of Px orbital at the origin.png - Wikimedia Commons
32d
43f

How Do Electrons Occupy the Orbital Space?

S Orbital

At the first main energy level, when n = 1, the only sublevel, or orbital, possible is the s-orbital, which has a sphere shape.

P Orbital

When n = 2, two sublevels are possible: these are the s-orbital and p-orbitals. If you recall, the magnetic quantum number shows the orientations of an orbital, with the values –l to +l. So an s-orbital has only one magnetic quantum number which is 1, meaning it only has one possible orientation. This makes sense because a sphere has the same shape no matter how it is rotated. Thus, a p-orbital has three possible orientations (-1, 0, 1 magnetic quantum numbers).

Shape of p-orbitals in 3D

Neon, the last element in the main second energy level, has 10 electrons. How are these electrons distributed and located? The first 2 electrons go in the 1s-orbital, or the s-orbital in the first main energy level. Then, the next 2 electrons occupy in the 2s-orbital, or the s-orbital in the second main energy level. Remember, because there is only one orientation of an s-orbital, there is only one s-orbital per energy level. Finally, the last 6 electrons are divided evenly into the 2p-orbitals. Since there are three orientations of a p-orbital, there are three p-orbitals per energy level.

s orbital p orbital d orbital

As shown in the example above, electrons can be identified by the orbitals in which they reside. Electron configurations show how electrons are organized in orbitals in an atom.

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