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:
[tex]\delta E = (\frac{1}{n_2{^2}} -\frac{1}{n_1^{2}})13.6eV[/tex]
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
[tex]\delta E = (\frac{1}{3{^2}} -\frac{1}{5^{2}})13.6X1.602X10^{-19}[/tex]
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
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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