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 hydrogen electron from level n = 1 to level \[n=2\] will be: (\[h=6.625\times {{10}^{-34}}Js\],\[C=3\times {{10}^{8}}m{{s}^{-1}}\])

• A. \[1.325\times {{10}^{-7}}m\]
• B. \[1.325\times {{10}^{-10}}m\]
• C. \[2.650\times {{10}^{-7}}m\]
• D. \[5.300\times {{10}^{-10}}m\]