Question

a red photon in the bright line spectrum of hydrogen gas has an energy of 3.02*10^-19 joule what energy level transition does an electron in a hydrogen atom undergo to produce this photon

Answer 1

The energy level transition that an electron in a hydrogen atom undergoes to produce a red photon in the bright line spectrum can be determined using the equation E = ΔE = hf, where E is the energy, ΔE is the energy difference between initial and final states, h is Planck's constant, and f is the frequency of the photon.

Step-by-step explanation:

The energy of a red photon in the bright line spectrum of hydrogen gas is given as 3.02*10^-19 joule. To determine the energy level transition that an electron in a hydrogen atom undergoes to produce this photon, we can use the equation E = ΔE = hf, where E is the energy, ΔE is the energy difference between initial and final states, h is Planck's constant, and f is the frequency of the photon.

In this case, we know the energy of the photon, so we can equate it to the energy difference between two energy levels. By rearranging the equation, we can solve for the frequency of the photon:

f = E / h = 3.02*10^-19 joule / 6.63*10^-34 joule·second = 4.56*10^14 Hz.

Therefore, the electron in the hydrogen atom undergoes an energy level transition that produces a photon with a frequency of 4.56*10^14 Hz.

Answer 2

The electron in a hydrogen atom undergoes a transition from energy level 3 to energy level 2 to produce a red photon in the bright line spectrum of hydrogen gas.

Step-by-step explanation:

The energy of a red photon in the bright line spectrum of hydrogen gas is 3.02*10^-19 joule. To determine the energy level transition that an electron in a hydrogen atom undergoes to produce this photon, we can use the formula:

E = -13.6 eV / n^2

where E is the energy of the transition and n is the energy level. Rearranging the formula to solve for n, we have:

n = sqrt(-13.6 eV/E)

Plugging in the given energy of the photon, we can calculate the energy level transition:

n = sqrt(-13.6 eV / (3.02*10^-19 J))

n = 3

Therefore, the electron in the hydrogen atom undergoes a transition from energy level 3 to energy level 2 to produce the red photon.