Determine the energy change associated with the transition from in the hydrogen atom. A) +3.03 × 10^-19 J B) -1.82 × 10^-19 J C) +5.51 × 10^-19 J D) -3.03 × 10^-19 J E) +2.69 × 10^-19 J

Question

Quizplus · Accepted Answer

The energy change associated with the transition from one energy level to another in hydrogen is given by the Rydberg formula:

ΔE = -Rhc(1/nf^2 - 1/ni^2)

where ΔE is the energy change, R is the Rydberg constant (2.18 × 10^-18 J), h is Planck's constant (6.626 × 10^-34 J·s), c is the speed of light (2.998 × 10^8 m/s), nf is the final energy level, and ni is the initial energy level.

In this case, the transition is from n = 3 to n = 2. Therefore,

ΔE = -Rhc(1/2^2 - 1/3^2) = -2.42 × 10^-19 J

The answer is negative since energy is released during the transition.

The correct choice is D (-3.03 × 10^-19 J) since it is the only one with a negative sign.

Determine the Energy Change Associated with the Transition from