The first ionization energy of a nitrogen atom is 2.32 aJ (attojoules). What is the frequency and wavelength, in nanometers, of photons capable of just ionizing nitrogen atoms?

Respuesta :

Explanation:

It is given that,

The ionization energy of a nitrogen atom, [tex]E=2.32\ aJ[/tex]

aJ is attpjoules. [tex]1\ aJ=10^{-18}\ J[/tex]

[tex]E=2.32\times 10^{-18}\ J[/tex]

The energy of an atom is given by :

[tex]E=h\times f[/tex]

f is the frequency of the photons

[tex]f=\dfrac{E}{h}[/tex]

[tex]f=\dfrac{2.32\times 10^{-18}}{6.67\times 10^{-34}}[/tex]

[tex]f=3.47\times 10^{15}\ Hz[/tex]

Also, [tex]E=\dfrac{hc}{\lambda}[/tex]

[tex]\lambda=\dfrac{hc}{E}[/tex]

[tex]\lambda=\dfrac{6.67\times 10^{-34}\times 3\times 10^8}{2.32\times 10^{-18}}[/tex]

[tex]\lambda=8.62\times 10^{-8}\ m[/tex]

Hence, this is the required solution.

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