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

Published by Prentice Hall

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

#### Answer

The minimum energy needed to eject an electron is $7.222\times10^{-19}J$.

#### Work Step by Step

*Strategy: The minimum energy needed to eject an electron is the energy of a photon of radiation with a minimum frequency of $1.09\times10^{15}s^{-1}$ which can be acquired by this formula: $$E_{min}=h\times\nu_{min}$$ $E_{min}$ : minimum energy of a photon of radiation needed to eject an electron off its surface $h$ : Planck's constant ($h\approx6.626\times10^{-34}J.s$) $\nu_{min}$ : minimum frequency of radiation needed to eject an electron off its surface ($\nu_{min}=1.09\times10^{15}s^{-1})$ Therefore, the minimum energy needed to eject an electron is: $E_{min}=h\times\nu_{min}=(6.626\times10^{-34})\times(1.09\times10^{15})\approx7.222\times10^{-19}J$

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