Chemistry

Problem

Based on the equation:

\Delta E = -2.0 \times 10^{-18} \text{ 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} \text{ Js}

c = 3 \times 10^8 \text{ ms}^{-1}

) (a)

1.325 \times 10^{-7} \text{ m}

(b)

1.325 \times 10^{-10} \text{ m}

(c)

2.650 \times 10^{-7} \text{ m}

(d)

5.300 \times 10^{-10} \text{ m}