We are asked to calculate the maximum wavelength of light that takes takes 7.21 x 10 ^{-19} J of energy to remove an electron from an iron atom

**Calculate the wavelength from the total energy (****Δ****E).**

• ΔE = 7.21 x 10 ^{-19} J

• h = 6.626x10^{-34} J∙s

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

*In the equation, the frequency of the light is used but we need wavelength. **We can relate frequency and wavelength using the speed of light:*

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

▪* c = speed of light = 3.0x10 ^{8} m/s*▪ λ = wavelength, m

It takes 7.21 x 10 ^{-19} J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.