🤓 Based on our data, we think this question is relevant for Professor Poehlmann & Waymouth's class at STANFORD.

**Calculate the energy required to remove 1 electron:**

$\mathbf{E}\mathbf{=}\frac{\mathbf{208}\mathbf{.}\mathbf{4}\mathbf{}\overline{)\mathbf{kJ}}}{\overline{)\mathbf{mol}\mathbf{}\mathbf{electron}}}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\mathbf{J}}{\mathbf{1}\mathbf{}\overline{)\mathbf{kJ}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}\mathbf{electro}}\mathbf{n}}{\mathbf{6}\mathbf{.}\mathbf{022}\mathbf{\times}{\mathbf{10}}^{\mathbf{23}}\mathbf{}\mathbf{electron}}$

**E = 3.461****×****10 ^{‒19} J/electron**

**3.461****×****10 ^{‒19} J of **energy is required to remove a single electron from an atom on the surface of solid rubidium.

$\overline{)\mathbf{E}\mathbf{=}\mathbf{h\nu}}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{c}}{\mathbf{\lambda}}\mathbf{=}\frac{\overline{)\mathbf{\lambda}}\mathbf{\xb7}\mathbf{\nu}}{\overline{)\mathbf{\lambda}}}\phantom{\rule{0ex}{0ex}}\mathbf{\nu}\mathbf{=}\frac{\mathbf{c}}{\mathbf{\lambda}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{E}\mathbf{=}\frac{\mathbf{hc}}{\mathbf{\lambda}}}$

It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium metal. (1 mol electrons = 6.022 x 10^{23} electrons.) How much energy does it take to remove a single electron from an atom on the surface of solid rubidium? What is the maximum wavelength of light capable of doing this?

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Based on our data, we think this problem is relevant for Professor Poehlmann & Waymouth's class at STANFORD.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.