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Question: The energy difference between the ground state of an atom and its excited state is \(3 \times 10^{- ...

The energy difference between the ground state of an atom and its excited state is 3×10−193 \times 10^{- 19}J. What is the wavelength of the photon required for this transition?

A

6.6×10−34m6.6 \times 10^{- 34}m

B

3×10−8m3 \times 10^{- 8}m

C

1.8×10−7m1.8 \times 10^{- 7}m

D

6.6×10−7m6.6 \times 10^{- 7}m

Answer

6.6×10−7m6.6 \times 10^{- 7}m

Explanation

Solution

: ΔE=hcλ\Delta E = \frac{hc}{\lambda}

λ=6.6×10−34Js×3×108ms−13×10−19J=6.6×10−7m\lambda = \frac{6.6 \times 10^{- 34}Js \times 3 \times 10^{8}ms^{- 1}}{3 \times 10^{- 19}J} = 6.6 \times 10^{- 7}m