Question

The electron in a hydrogen atom can undergo a transition from n = 4 to n = 3, emitting a photon with energy 1.06 × 10 –19J. Use this transition to answer the following questions.

i. What is the wavelength of this transition?
ii. How does this transition show that the position of the electron is quantized?

Answer 1

Wavelength (λ) = 1.875 × 10⁻⁶ m

Step-by-step explanation:

Given:

Energy (e) = 1.06 × 10⁻¹⁹ J

Find:

Wavelength (λ) = ?

Computation:

e = hc / λ

λ = hc / e

where c = 3 × 10⁸

Planck's constant (h) = 6.625 × 10⁻³⁴

So,

Wavelength (λ) = (6.625 × 10⁻³⁴)(3 × 10⁸) / (1.06 × 10⁻¹⁹)

1. Wavelength (λ) = 1.875 × 10⁻⁶ m

2. Given n = 4 to n = 3 both are integer not fraction so, electron is quantize