# 8.4: An Electron Has an Intrinsic Spin Angular Momentum

Imagine doing a hypothetical experiment that would lead to the discovery of electron spin. Your laboratory has just purchased a microwave spectrometer with variable magnetic field capacity. We try the new instrument with hydrogen atoms using a magnetic field of 10^{4} Gauss and look for the absorption of microwave radiation as we scan the frequency of our microwave generator (Figure \(\PageIndex{1}\)).

**Figure \(\PageIndex{1}\): **Schematic diagram of a microwave spectrometer transmission Electron Spin Resonance (ESR) spectrometer with the sample in a magnetic field. (left) EPR spectrometer Faculty of Biochemistry, Biophysics and Biotechnology Jagiellonian University. (right) Schematic of the ESR instrument. The strength of the magnetic field is set, and the sample’s absorption of microwave photons is measured for a range of microwave photon energies (or frequencies). Images used with permission (CC BY 3.0)

Finally we see absorption at a microwave photon frequency of 28 × l0^{9} Hz (28 gigahertz). This result is really surprising from several perspectives. Each hydrogen atom is in its ground state, with the electron in a 1s orbital. The lowest energy electronic transition that we predict based on existing theory (the electronic transition from the ground state (\(\psi _{100}\) to \(\psi _{21m}\)) requires an energy that lies in the vacuum ultraviolet (the lower Lyman line at 121 nm), not the microwave, region of the spectrum. Furthermore, when we vary the magnetic field we note that the frequency at which the absorption occurs varies in proportion to the magnetic field.

### The Zeeman Effect: Breaking Degeneracy

Magnetism results from the circular motion of charged particles. This property is demonstrated on a macroscopic scale by making an electromagnet from a coil of wire and a battery. Electrons moving through the coil produce a magnetic field, which can be thought of as originating from a magnetic dipole or a bar magnet. Electrons in atoms also are moving charges with angular momentum so they too produce a magnetic dipole, which is why some materials are magnetic. A* magnetic dipole* interacts with a magnetic field, and the energy of this interaction is given by the scalar product of the magnetic dipole moment, and the magnetic field, \(B\).

\[E_B = -\vec{\mu}_m \cdot \vec{B} \label {8.4.0}\]

Pieter Zeeman was one of the first to observe the splittings of spectral lines in a magnetic field caused by this interaction. Consequently such splittings are known as the Zeeman effect. (Figure \(\PageIndex{2}\)). The \(m_l\) quantum number degeneracy of the hydrogen atom is removed by the magnetic field. For example, the three hydrogen atom eigenstates \(|\psi _{211} \rangle\), \(|\psi _{21-1} \rangle\), and \(|\psi _{210} \rangle \) are degenerate in zero magnetic field, but have different energies in an externally applied magnetic field (Figure \(\PageIndex{2}\)).

**Figure \(\PageIndex{2}\): **The Zeeman effect for the \(2s \rightarrow 1s\) transition. Emission when an electron switches from a 2p orbital to a 1s orbital occurs at only one energy in the absence of a magnetic field, but can occur at three different energies in the presence of a magnetic field.

The \(m_l = 0\) state, for which the component of angular momentum and hence also the magnetic moment in the external field direction is zero, experiences no interaction with the magnetic field. The \(m_l = +1\) state, for which the angular momentum in the z-direction is +ħ and the magnetic moment is in the opposite direction, against the field, experiences a raising of energy in the presence of a field. Maintaining the magnetic dipole against the external field direction is like holding a small bar magnet with its poles aligned exactly opposite to the poles of a large magnet. It is a higher energy situation than when the magnetic moments are aligned with each other.

### Electron Spin and the Stern-Gerlach Experiment

To discover new things, experimentalists sometimes must explore new areas in spite of contrary theoretical predictions. Our theory of the hydrogen atom at this point gives no reason to look for absorption in the microwave region of the spectrum. By doing the crazy experiment outlines above, we discovered that when an electron is in the \(|1s \rangle\) orbital of the hydrogen atom, there are two different states that have the same energy. When a magnetic field is applied, this degeneracy is removed, and microwave radiation can cause transitions between the two states. In the rest of this section, we see what can be deduced from this experimental observation. This experiment actually could be done with electron spin resonance spectrometers available today (Figure \(\PageIndex{1}\)).

To explain our observations, a new model for the hydrogen atom. Our original model for the hydrogen atom accounted for the motion of the electron and proton in our three-dimensional world; the new model needs something else that can give rise to an additional Zeeman-like effect. We need a charged particle with angular momentum to produce a magnetic moment, just like that obtained by the orbital motion of the electron. We can postulate that our observation results from a motion of the electron that was not considered in the last section - electron spin. We have a charged particle spinning on its axis. We then have charge moving in a circle, angular momentum, and a magnetic moment, which interacts with the magnetic field and gives us the Zeeman-like effect that we observed (Figure \(\PageIndex{3}\)).

**Figure \(\PageIndex{3}\)**: Electron Spin. In a magnetic field, an electron has two possible orientations with different energies, one with spin up, aligned with the magnetic field, and one with spin down, aligned against it. All other orientations are forbidden.

In 1920, Otto Stern and Walter Gerlach designed an experiment, which unintentionally led to the discovery that electrons have their own individual, continuous spin even as they move along their orbital of an atom. Today, this electron spin is indicated by the fourth quantum number, also known as the **Electron Spin Quantum Number** and denoted by \(m_s\). In 1925, Samuel Goudsmit and George Uhlenbeck made the claim that features of the hydrogen spectrum that were unexamined might by explained by assuming electrons act as if it has a spin, which can be denoted by an arrow pointing up, which is +1/2, or an arrow pointing down, which is -1/2. The Stern and Gerlach experiment which demonstrated this was done with a beam of vaporized silver atoms that split into two beams after passing through a magnetic field (Figure \(\PageIndex{4}\)).

**Figure \(\PageIndex{4}\)**: Stern–Gerlach experiment: silver atoms travel through an inhomogeneous magnetic field and are deflected up or down depending on their spin. Figure used with permission from Wikipedia.

An explanation of this is that an electron has a magnetic field due to its spin. When electrons that have opposite spins are put together, there is no net magnetic field because the positive and negative spins cancel each other out. The silver atom used in the experiment has a total of 47 electrons, 23 of one spin type, and 24 of the opposite. Because electrons of the same spin cancel each other out, the *one unpaired electron* in the atom will determine the spin.

Electron "spin" does not originate from electrons Spinning

Electron's hypothetical surface would have to be moving** ***faster* than the speed of light for it to rotate quickly enough to produce the observed angular momentum. Hence, an electron is not simply a spinning ball or ring and electron spin appears to be an *intrinsic angular moment* of the particle rather than a consequence of the rotation of a charge particle like Figure \(\PageIndex{3}\) suggests. Despite this, the term "spin" is persists in quantum vernacular.

### Spin Eigenstates and Eigenvalues

To describe electron spin from a quantum mechanical perspective, we must have spin wavefunctions and spin operators. The properties of the spin states are deduced from experimental observations and by analogy with our treatment of the states arising from the orbital angular momentum of the electron. The important feature of the spinning electron is the spin angular momentum vector, which we label \(S\) by analogy with the orbital angular momentum \(L\). We define spin angular momentum operators with the same properties that we found for the rotational and orbital angular momentum operators. After all, angular momentum is angular momentum, no matter if it is *orbital* or *spin* in nature.

We found that

\[ \hat {L}^2 | Y^{m_l} _l \rangle = l(l + 1) \hbar^2 | Y^{m_l}_l \rangle \label {8.4.1}\]

so by analogy for the spin states, we must have

\[ \hat {S}^2 | \sigma ^{m_s} _s \rangle = s( s + 1) \hbar ^2 | \sigma ^{m_s}_s \rangle \label {8.4.2}\]

where \(\sigma\) is a spin wavefunction with quantum numbers \(s\) and \(m_s\) that obey the same rules as the quantum numbers \(l\) and \(m_l\) associated with the spherical harmonic wavefunction \(Y\). We also found the project of the orbital angular momentum on the z-axis is

\[ \hat {L}_z | Y^{m_l}_l \rangle = m_l \hbar | Y^{m_l}_l \rangle \label {8.4.3}\]

so by analogy, we must have a similar projection for the spin angular momentum:

\[ \hat {S}_z | \sigma ^{m_s}_s \rangle = m_s \hbar | \sigma ^{m_s}_s \rangle \label {8.4.4}\]

Since \(m_l\) ranges in integer steps from \(-l\) to \(+l\), also by analogy \(m_s\) ranges in integer steps from \(-s\) to \(+s\). In our hypothetical experiment, we observed one absorption transition, which means there are two spin states. Consequently, the two values of \(m_s\) must be \(+s\) and \(-s\), and the difference in \(m_s\) for the two states, labeled f and i below, must be the smallest integer step, i.e., 1. The result of this logic is that

\[\begin{align} m_{s,f} - m_{s,i} &= 1 \nonumber\\[5pt] (+s) - (-s) &= 1 \nonumber\\[5pt] 2s &= 1 \nonumber\\[5pt] s &= \dfrac {1}{2} \label {8.4.5} \end{align}\]

Therefore our conclusion is that the magnitude of the spin quantum number is 1/2 and the values for \(m_s\) are +1/2 and -1/2. The two spin states correspond to spinning clockwise and counter-clockwise with positive and negative projections of the spin angular momentum onto the z-axis. The state with a positive projection, \(m_s\) = +1/2, is called \(\alpha\); the other is called \(\beta\). These spin states are arbitrarily labeled \(\alpha\) and \(\beta\), and the associated spin wavefunctions also are designated by \(|\alpha \rangle \) and \(| \beta \rangle\).

From Equation \(\ref{8.4.4}\), the magnitude of the z-component of spin angular momentum, \(S_z\), is given by

\[S_z = m_s \hbar \label {8.4.6}\]

so the value of \(S_z\) is \(+ħ/2\) for spin state \(\alpha\) and \(-ħ/2\) for spin state \(\beta\). Hence, we conclude that the \(\alpha\) spin state, where the magnetic moment is aligned against the external field direction, has a **higher energy** than the \(\beta\) spin state.

Even though we do not know their functional forms, the spin wavefunctions are taken to be normalized and orthogonal to each other.

\[ \int \alpha ^* \alpha \,d \tau _s = \int \beta ^* \beta \,d \tau _s = 1 \label {8.4.7a}\]

or in braket notation

\[ \langle \alpha | \alpha \rangle = \langle \beta | \beta \rangle =1 \label{8.4.7b}\]

and

\[ \int \alpha ^* \beta\, d \tau _s = \int \beta ^* \alpha\, d \tau _s = 0 \label {8.4.8a}\]

or in braket notation

\[ \langle \alpha | \beta \rangle = \langle \alpha | \beta \rangle = 0 \label{8.4.8b}\]

where the integral is over the spin variable \(\tau _s\).

### Contributors

Adapted from "Quantum States of Atoms and Molecules" by David M. Hanson, Erica Harvey, Robert Sweeney, Theresa Julia Zielinski