# If 6000 angstrom light is shined onto a metal work a certain work function, what is the wavelength in "m" of the fastest photoelectron that can be emitted?

Jun 30, 2017

Here's what I got.

#### Explanation:

The idea here is that the metal has something called a work function, which basically represents the amount of energy needed in order to remove an electron from the surface of the metal.

Now, it's important to realize that not all the electrons emitted from the surface will have the same kinetic energy.

That happens because not all the energy carried by a photon will be transferred to the surface electrons. Some of this energy will actually be transferred to the bulk of the metal instead, i.e. to electrons that are not located near the surface.

This means that the fastest electrons emitted from the metal will absorb all the energy of an incoming photon that is not needed to remove the electron from the surface and that is not transferred to the bulk of the metal.

In other words, the maximum kinetic energy of an emitted electron is given by

${K}_{\text{E max" = E_"photon}} - W$

Here

• ${E}_{\text{photon}}$ represents the energy of the incoming photon
• $W$ is the work function of the metal

It's worth mentioning that if $W > {E}_{\text{photon}}$, then the incoming photon does not have enough energy to overcome the work function $\to$ the electrons are not being emitted from the surface of the metal, i.e. the photoelectric effect does not take place! Also, notice that the slowest electron emitted from the surface of the metal has

${K}_{\text{E min" ~~ "0 J}}$

because, for all intended purposes, all the energy of the incoming photon is used up to overcome the work function, i.e. ${E}_{\text{photon}} = W$.

Now, the energy of the photon is calculated by using the Planck - Einstein equation, which looks like this

$\textcolor{b l u e}{\underline{\textcolor{b l a c k}{E = h \cdot \frac{c}{l a m \mathrm{da}}}}}$

Here

• $E$ is the energy of the photon
• $l a m \mathrm{da}$ is the wavelength of the photon
• $c$ is the speed of light in a vacuum, usually given as $3 \cdot {10}^{8} {\text{m s}}^{- 1}$
• $h$ is Planck's constant, equal to $6.626 \cdot {10}^{- 34} \text{J s}$

In your case, the wavelength is given in angstrom, so convert it to meters by using

$1 \textcolor{w h i t e}{.} \stackrel{\circ}{\text{A}} = 1 \cdot {10}^{- 10}$ $\text{m}$

You will end up with

6000 color(red)(cancel(color(black)(stackrel(@)("A")))) * (1 * 10^(-10)color(white)(.)"m")/(1color(red)(cancel(color(black)(stackrel(@)("A"))))) = 6.0 * 10^(-7) $\text{m}$

Plug this into the Planck - Einstein equation and find the energy of the incoming photon

E = 6.626 * 10^(-34)"J"color(red)(cancel(color(black)("s"))) * (3 * 10^8 color(red)(cancel(color(black)("m"))) color(red)(cancel(color(black)("s"^(-1)))))/(6.0 * 10^(-7)color(red)(cancel(color(black)("m"))))

$E = 3.313 \cdot {10}^{- 19}$ $\text{J}$

Now, assuming that the work function of the metal is equal to $W$ $\text{J}$, you can say that the maximum kinetic energy of an emitted electron is equal to

${K}_{\text{E max" = 3.313 * 10^(-19)color(white)(.)"J" - Wcolor(white)(.)"J}}$

${K}_{\text{E max}} = \left(3.313 \cdot {10}^{- 19} - W\right)$ $\text{J}$

color(red)(!) Keep in mind that the work function must be expressed in joules per electron in order for the above equation to work, so if the problems provides the work function in kilojoules per mole, make sure to convert it before using it!

So, you now know that the fastest electron emitted from the surface of the metal has a kinetic energy equal to ${K}_{\text{E max}}$.

To find the de Broglie wavelength, you must use the following equation

$\textcolor{b l u e}{\underline{\textcolor{b l a c k}{l a m {\mathrm{da}}_{\text{matter}} = \frac{h}{p}}}} \to$ the de Broglie wavelength

Here

• $p$ is the momentum of the electron
• $l a m {\mathrm{da}}_{\text{matter}}$ is its de Broglie wavelength

As you know, the momentum of the electron depends on its velocity, $v$, and on its mass, $m$.

$\textcolor{b l u e}{\underline{\textcolor{b l a c k}{p = m \cdot v}}}$

This means that the de Broglie wavelength is equal to

$l a m {\mathrm{da}}_{\text{matter}} = \frac{h}{m \cdot v}$

Now, the kinetic energy of the fastest electron is defined as

${K}_{\text{E max}} = \frac{1}{2} \cdot m \cdot {v}^{2}$

Rearrange to find the velocity of the electron

$v = \sqrt{\frac{2 \cdot {K}_{\text{E max}}}{m}}$

Use this expression for the velocity of the electron to find its de Broglie wavelength

lamda_ "matter" = h/(m * sqrt( (2 * K_ "E max")/m))

If you take the mass of the electron to be approximately equal to

${m}_{{\text{e}}^{-}} \approx 9.10938 \cdot {10}^{- 31}$ $\text{kg}$

and use the fact that

$\text{1 J} = 1$ ${\text{kg m"^2"s}}^{- 2}$

you can say that the de Broglie wavelength will be equal to

lamda_ "matter" = (6.626 * 10^(-34) color(blue)(cancel(color(black)("kg"))) "m"^color(purple)(cancel(color(black)(2)))color(green)(cancel(color(black)("s"^(-2)))) * color(green)(cancel(color(black)("s"))))/(9.10938 * 10^(-31)color(blue)(cancel(color(black)("kg"))) * sqrt( (2 * (3.313 * 10^(-19) - W) color(red)(cancel(color(black)("kg"))) color(purple)(cancel(color(black)("m"^2)))color(green)(cancel(color(black)("s"^(-2)))))/(9.10938 * 10^(-31)color(red)(cancel(color(black)("kg")))))

which gets you

lamda_ "matter" = (7.2738 * 10^(-4))/(1.4817 * 10^(15) * sqrt((3.313 * 10^(-19) - W)) $\text{m}$

lamda_"matter" = (4.91 * 10^(-19))/(sqrt((3.313 * 10^(-19)-W)) $\text{m}$

At this point, all you have to do is plug in the value you have for the work function in joules per electron and find the value of $l a m {\mathrm{da}}_{\text{matter}}$.
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