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# Photoelectric effect

Explaining the experiments on the photoelectric effect. How these experiments led to the idea of light behaving as a particle of energy called a photon.

## Key points

• Based on the wave model of light, physicists predicted that increasing light amplitude would increase the kinetic energy of emitted photoelectrons, while increasing the frequency would increase measured current.
• Contrary to the predictions, experiments showed that increasing the light frequency increased the kinetic energy of the photoelectrons, and increasing the light amplitude increased the current.
• Based on these findings, Einstein proposed that light behaved like a stream of particles called photons with an energy of $\text{E}=h\nu$.
• The work function, $\mathrm{\Phi }$, is the minimum amount of energy required to induce photoemission of electrons from a metal surface, and the value of $\mathrm{\Phi }$ depends on the metal.
• The energy of the incident photon must be equal to the sum of the metal's work function and the photoelectron kinetic energy: ${\text{E}}_{\text{photon}}={\text{KE}}_{\text{electron}}+\mathrm{\Phi }$

## Introduction: What is the photoelectric effect?

When light shines on a metal, electrons can be ejected from the surface of the metal in a phenomenon known as the photoelectric effect. This process is also often referred to as photoemission, and the electrons that are ejected from the metal are called photoelectrons. In terms of their behavior and their properties, photoelectrons are no different from other electrons. The prefix, photo-, simply tells us that the electrons have been ejected from a metal surface by incident light.
In this article, we will discuss how 19th century physicists attempted (but failed!) to explain the photoelectric effect using classical physics. This ultimately led to the development of the modern description of electromagnetic radiation, which has both wave-like and particle-like properties.

## Predictions based on light as a wave

To explain the photoelectric effect, 19th-century physicists theorized that the oscillating electric field of the incoming light wave was heating the electrons and causing them to vibrate, eventually freeing them from the metal surface. This hypothesis was based on the assumption that light traveled purely as a wave through space. (See this article for more information about the basic properties of light.) Scientists also believed that the energy of the light wave was proportional to its brightness, which is related to the wave's amplitude. In order to test their hypotheses, they performed experiments to look at the effect of light amplitude and frequency on the rate of electron ejection, as well as the kinetic energy of the photoelectrons.
Based on the classical description of light as a wave, they made the following predictions:
• The kinetic energy of emitted photoelectrons should increase with the light amplitude.
• The rate of electron emission, which is proportional to the measured electric current, should increase as the light frequency is increased.
To help us understand why they made these predictions, we can compare a light wave to a water wave. Imagine some beach balls sitting on a dock that extends out into the ocean. The dock represents a metal surface, the beach balls represent electrons, and the ocean waves represent light waves.
If a single large wave were to shake the dock, we would expect the energy from the big wave would send the beach balls flying off the dock with much more kinetic energy compared to a single, small wave. This is also what physicists believed would happen if the light intensity was increased. Light amplitude was expected to be proportional to the light energy, so higher amplitude light was predicted to result in photoelectrons with more kinetic energy.
Classical physicists also predicted that increasing the frequency of light waves (at a constant amplitude) would increase the rate of electrons being ejected, and thus increase the measured electric current. Using our beach ball analogy, we would expect waves hitting the dock more frequently would result in more beach balls being knocked off the dock compared to the same sized waves hitting the dock less often.
Now that we know what physicists thought would happen, let's look at what they actually observed experimentally!

## When intuition fails: photons to the rescue!

When experiments were performed to look at the effect of light amplitude and frequency, the following results were observed:
• The kinetic energy of photoelectrons increases with light frequency.
• Electric current remains constant as light frequency increases.
• Electric current increases with light amplitude.
• The kinetic energy of photoelectrons remains constant as light amplitude increases.
These results were completely at odds with the predictions based on the classical description of light as a wave! In order to explain what was happening, it turned out that an entirely new model of light was needed. That model was developed by Albert Einstein, who proposed that light sometimes behaved as particles of electromagnetic energy which we now call photons. The energy of a photon could be calculated using Planck's equation:
${\text{E}}_{\text{photon}}=h\nu$
where ${\text{E}}_{\text{photon}}$ is the energy of a photon in joules ($\text{J}$), $h$ is Planck's constant , and $\nu$ is the frequency of the light in $\text{Hz}$. According to Planck's equation, the energy of a photon is proportional to the frequency of the light, $\nu$. The amplitude of the light is then proportional to the number of photons with a given frequency.
Concept check: As the wavelength of a photon increases, what happens to the photon's energy?

## Light frequency and the threshold frequency ${\nu }_{0}$‍

We can think of the incident light as a stream of photons with an energy determined by the light frequency. When a photon hits the metal surface, the photon's energy is absorbed by an electron in the metal. The graphic below illustrates the relationship between light frequency and the kinetic energy of ejected electrons.
The scientists observed that if the incident light had a frequency less than a minimum frequency ${\nu }_{0}$, then no electrons were ejected regardless of the light amplitude. This minimum frequency is also called the threshold frequency, and the value of ${\nu }_{0}$ depends on the metal. For frequencies greater than ${\nu }_{0}$, electrons would be ejected from the metal. Furthermore, the kinetic energy of the photoelectrons was proportional to the light frequency. The relationship between photoelectron kinetic energy and light frequency is shown in graph (a) below.
Because the light amplitude was kept constant as the light frequency increased, the number of photons being absorbed by the metal remained constant. Thus, the rate at which electrons were ejected from the metal (or the electric current) remained constant as well. The relationship between electron current and light frequency is illustrated in graph (b) above.

## Isn't there more math somewhere?

We can analyze the frequency relationship using the law of conservation of energy. The total energy of the incoming photon, ${\text{E}}_{\text{photon}}$, must be equal to the kinetic energy of the ejected electron, ${\text{KE}}_{\text{electron}}$, plus the energy required to eject the electron from the metal. The energy required to free the electron from a particular metal is also called the metal's work function, which is represented by the symbol $\mathrm{\Phi }$ (in units of $\text{J}$):
${\text{E}}_{\text{photon}}={\text{KE}}_{\text{electron}}+\mathrm{\Phi }$
Like the threshold frequency ${\nu }_{0}$, the value of $\mathrm{\Phi }$ also changes depending on the metal. We can now write the energy of the photon in terms of the light frequency using Planck's equation:
${\text{E}}_{\text{photon}}=h\nu ={\text{KE}}_{\text{electron}}+\mathrm{\Phi }$
Rearranging this equation in terms of the electron's kinetic energy, we get:
${\text{KE}}_{\text{electron}}=h\nu -\mathrm{\Phi }$
We can see that kinetic energy of the photoelectron increases linearly with $\nu$ as long as the photon energy is greater than the work function $\mathrm{\Phi }$, which is exactly the relationship shown in graph (a) above. We can also use this equation to find the photoelectron velocity $\text{v}$, which is related to ${\text{KE}}_{\text{electron}}$ as follows:
${\text{KE}}_{\text{electron}}=h\nu -\mathrm{\Phi }=\frac{1}{2}{m}_{e}{\text{v}}^{2}$
where ${m}_{e}$ is the rest mass of an electron, $9.1094×{10}^{-31}\phantom{\rule{0.167em}{0ex}}\text{kg}$.

## Exploring the wave amplitude trends

In terms of photons, higher amplitude light means more photons hitting the metal surface. This results in more electrons ejected over a given time period. As long as the light frequency is greater than ${\nu }_{0}$, increasing the light amplitude will cause the electron current to increase proportionally as shown in graph (a) below.
Since increasing the light amplitude has no effect on the energy of the incoming photon, the photoelectron kinetic energy remains constant as the light amplitude is increased (see graph (b) above).
If we try to explain this result using our dock-and-beach-balls analogy, the relationship in graph (b) indicates that no matter the height of the wave hitting the dock$-$whether it's a tiny swell, or a huge tsunami$-$the individual beach balls would be launched off the dock with the exact same speed! Thus, our intuition and analogy don't do a very good job of explaining these particular experiments.

## Example $1$‍ : The photoelectric effect for copper

The work function of copper metal is . If we shine light with a frequency of on copper metal, will the photoelectric effect be observed?
In order to eject electrons, we need the energy of the photons to be greater than the work function of copper. We can use Planck's equation to calculate the energy of the photon, ${\text{E}}_{\text{photon}}$:
If we compare our calculated photon energy, ${\text{E}}_{\text{photon}}$, to copper's work function, we see that the photon energy is greater than $\mathrm{\Phi }$:

Thus, we would expect to see photoelectrons ejected from the copper. Next, we will calculate the kinetic energy of the photoelectrons.

## Example $2$‍ : Calculating the kinetic energy of a photoelectron

What is the kinetic energy of the photoelectrons ejected from the copper by the light with a frequency of ?
We can calculate the kinetic energy of the photoelectron using the equation that relates ${\text{KE}}_{\text{electron}}$ to the energy of the photon, ${\text{E}}_{\text{photon}}$, and the work function, $\mathrm{\Phi }$:
${\text{E}}_{\text{photon}}={\text{KE}}_{\text{electron}}+\mathrm{\Phi }$
Since we want to know ${\text{KE}}_{\text{electron}}$, we can start by rearranging the equation so that we will be solving for the kinetic energy of the electron:
${\text{KE}}_{\text{electron}}={\text{E}}_{\text{photon}}-\mathrm{\Phi }$
Now we can insert our known values for ${\text{E}}_{\text{photon}}$ and $\mathrm{\Phi }$ from Example 1:
Therefore, each photoelectron has a kinetic energy of .

## Summary

• Based on the wave model of light, physicists predicted that increasing light amplitude would increase the kinetic energy of emitted photoelectrons, while increasing the frequency would increase measured current.
• Experiments showed that increasing the light frequency increased the kinetic energy of the photoelectrons, and increasing the light amplitude increased the current.
• Based on these findings, Einstein proposed that light behaved like a stream of photons with an energy of $\text{E}=h\nu$.
• The work function, $\mathrm{\Phi }$, is the minimum amount of energy required to induce photoemission of electrons from a specific metal surface.
• The energy of the incident photon must be equal to the sum of the work function and the kinetic energy of a photoelectron: ${\text{E}}_{\text{photon}}={\text{KE}}_{\text{electron}}+\mathrm{\Phi }$

## Try it!

When we shine light with a frequency of $6.20×{10}^{14}\phantom{\rule{0.167em}{0ex}}\text{Hz}$ on a mystery metal, we observe the ejected electrons have a kinetic energy of $3.28×{10}^{-20}\phantom{\rule{0.167em}{0ex}}\text{J}$. Some possible candidates for the mystery metal are shown in the table below:
MetalWork function $\mathrm{\Phi }$ (Joules, $\text{J}$)
Calcium, $\text{Ca}$$4.60×{10}^{-19}$
Tin, $\text{Sn}$$7.08×{10}^{-19}$
Sodium, $\text{Na}$$3.78×{10}^{-19}$
Hafnium, $\text{Hf}$$6.25×{10}^{-19}$
Samarium, $\text{Sm}$$4.33×{10}^{-19}$
Based on this information, what is the most likely identity of our mystery metal?