Question

An energy of 13.6 eV is needed to ionize an electron from the ground state of a hydrogen atom. Selecting the longest wavelength that will work from the those given below, what wavelength is needed if a photon accomplishes this task

Answer 1

Answer:

The  wavelength is  $\lambda = 91nm$  

Explanation:

From the question we are told that

    The energy required is  $E = 13.6 \ eV$

     

This energy needed in form of a photon  can be mathematically represented as

         $E = \frac{h * c }{\lambda }$

where h is the Planck constant with a value  $h = 4.1357 * 10{-15} eV \cdot sec$

and  c is the speed of light which is  

 substituting values      

         $13.6 eV = \frac{ 4.1357 * 10^{-15} eV * 3.0*10^8 }{\lambda }$

= >   $\lambda = 9.1*10^{-8}$    

      $\lambda = 91nm$