## Chemistry: The Central Science (13th Edition)

Published by Prentice Hall

# Chapter 6 - Electronic Structure of Atoms - Exercises: 6.33b

#### Answer

The wavelength of radiation that will provide a photon of that energy is $275nm$.

#### Work Step by Step

The wavelength of radiation could be calculated using this formula: $$c=\nu\times\lambda$$ We already have: - Speed of light in a vacuum: $c\approx2.998\times10^8m/s$ - Frequency of radiation that will provide a photon of that energy: $\nu=\nu_{min}=1.09\times10^{15}s^{-1}$ Therefore, the wavelength of radiation that will provide a photon of that energy is: $\lambda=\frac{c}{\nu}=\frac{2.998\times10^8}{1.09\times10^{15}}\approx2.75\times10^{-7}m\approx275nm$

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