Based on the equation $\Delta E = - 2.0 \times 10^{-18} \, J \left( \frac{1}{n_2^2} - \frac{1}{n_1^2} \right)$,the wavelength of the light that must be absorbed to excite a hydrogen electron from level $n = 1$ to level $n = 2$ will be: $(h = 6.625 \times 10^{-34} \, J \, s, c = 3 \times 10^8 \, m \, s^{-1})$

• A
  $1.325 \times 10^{-7} \, m$
• B
  $1.325 \times 10^{-10} \, m$
• C
  $2.650 \times 10^{-7} \, m$
• D
  $5.300 \times 10^{-10} \, m$