Question

what is the energy in joules required to shift the electron of the hydrogen atom from the first bohr Orbit to V bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state the ground state energy is -2.8 18 into 10 to the power minus 11 kgswhat is the energy in joules required to shift the electron of the hydrogen atom from the first bohr Orbit to V bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state the ground state energy is -2.18 into 10 to the power minus 11 ergs.

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Answer 1

What is 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 –2.18 × 10–11 ergs.

4 years ago

Answers : (1)

Answer 2

[ -2.18 * 10^-11 ergs = - 2.8 * 10^-11 * 10^-7 that is - 2.8 * 10^-18 J ]

So,

Here it is Excited from Ground state to 5th state...

So We Will Get n1 = 1 and n2 = 5

And By Using Formula

E = $2.18 * 10^{-18} [\frac{1}{n1^{2}} - \frac{1}{n2^{2}}]$

So We Will Get

E = $(2.18 * 10^{-18}) [\frac{1}{1^{2}} - \frac{1}{5^{2}}]$

E = $(2.18*10^-18) [\frac{24}{25}]$

E = 2.0928 * 10^-18 J

Now Wavelength of Emitted Light = $\frac{hc}{E}$

So h = 6.6 * 10^-34

c = 3 * 10^8

and E = 2.0928 * 10^-18

So Wavelength will be,

= $\frac{(6.6 * 10^{-34})(3*10^8)}{2.0928 * 10^-18}$

On solving we will get

Wavelength = 9.498 * 10^-8 m