If the energy required to remove an electron from sodium is #8.23xx10^-19 J#, what frequency of light will cause sodium to ionize?

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1 Answer
Aug 10, 2017

#1.24xx10^15# #"s"^-1#

Explanation:

What we need to do here is convert from energy of a photon to its corresponding wavelength.

To do this, we can use the formula

#ul(E = hf#

where

  • #E# is the energy of the photon (given as #8.23xx10^-19# #"J"#)

  • #h# is Planck's constant, equal to #6.626xx10^-34# #"J"*"s"#

  • #f# is the frequency of the light

We can rearrange the equation to solve for the frequency, #f#:

#f = E/h#

Plugging in known values:

#f = (8.23xx10^-19cancel("J"))/(6.626xx10^-34cancel("J")*"s") = color(red)(ulbar(|stackrel(" ")(" "1.24xx10^15color(white)(l)"s"^-1" ")|)#