Answer:
B) True. It is the photon is emitted the wavelength is correct
Explanation:
For this exercise let's use the Bohr model for the hydrogen atom
Eₙ = -13.606 / n2
This gives the energy of the levels in eV. let's look for the energy
n = 1
E₁ = -13,606
n = 3
E₃ = -13.606 / 3²
E₃ = -1.512 eV
The transition occurs when moving from one level to another
ΔE = E₃ -E₁
ΔE = -1.512 + 13.606
ΔE = 12.094 eV
Now let's use the Planck equation and the speed of light for the energy of the transition
E = h F
c = λ f
E = h c / λ
E = 6.63 10⁻³⁴ 3 10⁸ / λ
E = 19.89 10⁻²⁶ /λ
λ = 19.89 10⁻²⁶ / E
Let's reduce energy to July
E = 12,094 eV (1.6 10⁻¹⁹ J / 1 eV) = 19.35 10⁻¹⁹ J
λ = 19.89 10⁻²⁶ / 19.35 10⁻¹⁹
λ = 1.0279 10⁻⁷ m
Let's reduce to nm
λ = 1.0279 10⁻⁷ m (10⁹ nm / 1 m)
λ = 102.79 nm
Let's examine the answers
A) False is another wavelength and the photon emitted
B) True. It is the photon is emitted the wavelength is correct
C) False. Wavelength is different
D) False the photon is emitted
E) False wavelength is different
