If the energy required to remove an electron from sodium is #8.23xx10^-19 J#, what frequency of light will cause sodium to ionize?
1 Answer
Aug 10, 2017
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 = 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" ")|)#
