The energies of four levels of the hydrogen atom are: level P, -13.60 eV; level Q, -3.40 eV; level R, -1.50 eV; level S, -0.85 eV. Taking Planck's constant as 6.63 × 1 0 − 34 J s , the electron c

Question

The energies of four levels of the hydrogen atom are: level P, -13.60 eV; level Q, -3.40 eV; level R, -1.50 eV; level S, -0.85 eV. Taking Planck's constant as $6.63 \times 1 0^{- 34} J s$ , the electron charge as $- 1.60 \times 1 0^{- 19} C$ and the speed of light as $3.00 \times 1 0^{8} ms^{- 1}$ , a spectral line of 488 nm could result from an electron transition between levels

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Answer:

D

Solution:

$Δ E = \frac{1240}{488} \approx 2.55 eV . E_{S} - E_{Q} = - 0.85 - (- 3.40) = 2.55 eV$ , so the transition is S → Q.

TestHub · Accepted Answer

Δ E = 488 1240 ​ ≈ 2.55 eV . E S ​ − E Q ​ = − 0.85 − ( − 3.40 ) = 2.55 eV , so the transition is S → Q.

Physics - Modern Physics Question with Solution | TestHub

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