We’re being asked to determine the wavelength of radiation (light) that must be used to eject electrons from a chromium metal.

When photons with enough energy hit the surface of a metal, electrons are emitted. This phenomenon is known as the **Photoelectric Effect**.

**Total energy (****ΔE)** in photoelectric effect can be calculated using the following equation:

$\overline{){\mathbf{\u2206}}{\mathbf{E}}{\mathbf{=}}{{\mathbf{E}}}_{\mathbf{w}\mathbf{o}\mathbf{r}\mathbf{k}\mathbf{}\mathbf{f}\mathbf{u}\mathbf{n}\mathbf{c}\mathbf{t}\mathbf{i}\mathbf{o}\mathbf{n}}{\mathbf{+}}{{\mathbf{E}}}_{\mathbf{K}\mathbf{E}\mathbf{}\mathbf{o}\mathbf{f}\mathbf{}\mathbf{e}\mathbf{l}\mathbf{e}\mathbf{c}\mathbf{t}\mathbf{r}\mathbf{o}\mathbf{n}}}$

**Where:**

• **Δ****E **is* the** total energy or the energy of the light/photon/radiation* and can be calculated using the equation:

$\overline{){\mathbf{\u2206}}{\mathbf{E}}{\mathbf{=}}{\mathbf{h}}{\mathbf{\nu}}}$

E_{total energy} = J

h = Planck’s constant = 6.626x10^{-34} J∙s

ν = frequency = Hz or s^{-1}

• **E _{work function} **is

The work function for chromium metal is 4.37 eV. What wavelength of radiation must be used to eject electrons with a velocity of 2500 km/s?

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