Question

What is the energy of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 5?

Answer 1

Answer:

The energy absorbed by a hydrogen atom is 1.549 X10⁻¹⁹ J

Explanation:

Using Bohr's equation; the energy absorbed by the hydrogen atom can be calculated as follows:

$\delta E = (\frac{1}{n_2{^2}} -\frac{1}{n_1^{2}})13.6eV$

When an electron moves from a lower energy level to a higher energy level, energy is absorbed by the atom.

Lower energy level (n₂) = 3

Higher energy level (n₁) = 5

1 eV = 1.602X10⁻¹⁹ C

$\delta E = (\frac{1}{3{^2}} -\frac{1}{5^{2}})13.6X1.602X10^{-19}$

ΔE = 1.549 X10⁻¹⁹J

The energy absorbed by a hydrogen atom  to transition an electron from n = 3 to n = 5 is 1.549 X10⁻¹⁹ J

Answer 2

We have that for the Question,it can be said that  the energy of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 5 is

dE=1.54*10^{-19}J

From the question we are told

What is the energy of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 5?

Generally the equation for the energy  is mathematically given as

dE=\frac{1}{n_2^2}-\frac{1}{n_1^2})13.6eV

Where

e=1.602*10^{-19}

Therefore

dE=\frac{1}{3^2}-\frac{1}{5^2})13.6*1.602*10^{-19}

dE=1.54*10^{-19}J

Therefore

the energy of light that must be absorbed by a hydrogen atom to transition an electron from n = 3 to n = 5 is

dE=1.54*10^{-19}J

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