Chemistry, asked by danny41, 3 months ago

Calculate the energy in joules required to shift the electron of the hydrogen atom from the

first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted

when the electron returns to the ground state. The ground state electron energy is -

2.18x10-11 ergs.

Answers

Answered by Vinitvinayak
1

Answer:

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Explanation:

Answer

Grand state, n=1, energy is given by,

E

1

=−2.18×10

−11

ergs

Now, energy of the n=S (5

th

orbit} is given by,

E

s

=

(S)

2

E

1

=

2S

−2.18×10

−11

ergs

=−0.0872×10

−11

ergs

Energy required to go to the 5

th

orbit

=E

S

−E

1

=−0.0872−(−2.18)×10

−11

ergs

=2.0928×10

−11

ergs

Now, 1erg=10

−7

J

⇒2.0928×10

−11

ergs=2.0928×10

−18

J

For wavelength,

λ

1

=R[

(1)

2

1

=

(S)

2

1

]

where, R=1.0973×10

5

cm

−1

λ

1

=1.0973×10

5

[1−

2S

1

]

⇒λ=9.49×10

−5

cm

or, ≃9.5×10

−7

m

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