Question

A ground-state H atom absorbs a photon of wavelength 94.91 nm, and its electron attains a higher energy level. The atom then emits two photons: one of wavelength 1281 nm to reach an intermediate energy level, and a second to return to the ground state.
(b) What intermediate level did the electron reach?

Answer 1

The intermediate energy level that the electron reached from the ground state is; n= 3.

What are energy levels in an atom?

The fixed distances from an atom's nucleus where electrons may be found are referred to as energy levels (also known as electron shells). Higher energy electrons have greater energy as you move out from the nucleus.

A region of space within an energy level known as an orbital is where an electron is most likely to be found.

The formula to get the higher level is Rydberg's formula;

1/λ = R(1/n₁² - 1/n₂²)

where;

R is rydberg constant = 1.097 × 10⁷ m⁻¹

We want to find the intermediate level where wavelength = 1281 nm = 1281 × 10⁻⁹ m

Thus;

$\frac{1}{1280(10^{-9})} = 1.097*10^{7}(\frac{1}{n_{2}^{2}}-\frac{1}{5^{2}}) \\0.0712=\frac{1}{n_{2}^{2}}-\frac{1}{25} \\\frac{1}{n_{2}^{2}}=0.0712+\frac{1}{25}\\\frac{1}{n_{2}^{2}}=0.1112$

n₂ = √(1/0.1112)

n₂ ≈ 3

To know more about energy levels, visit: brainly.com/question/10763798

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