Question

A sample of H-atoms having electrons in the
ground state is exposed to high energy rays of
quantum energy 13.3875 eV. The H-atoms absorb
the energy and get excited. When the electron
drops from excited state to the ground state, how
many lines are seen in the emission spectrum of
hydrogen?​

Answer 1

Answer:

The electrons were initially present in third orbital and they were excited to higher level by absorption of radiation. In the emission spectrum, two lines corresponding to transitions have higher wavelengths than the light used for the absorption. Other lines have longer wavelengths

Answer 2

28 lines are seen in the emission spectrum of hydrogen.

Explanation:

A sample of H-atoms having electrons in the ground state is exposed to high energy rays of quantum energy 13.3875 eV

The energy of the electron which is found in the ground state of hydrogen atom is -13.6 eV.

The H-atoms absorb the energy and get excited.

ΔE= Z²($\frac{1}{1^{2} } -\frac{1}{2^{2} }$

$13.3875 eV$=$-13.6$  ($1^{2}$){${\frac{1}{1^{2}} -\frac{1}{n2^{2} } }$)

$0.98375=($$1-\frac{1}{n2^{2} }$)

$\frac{1}{n2^{2}} =0.015625$  When the electron drops from excited state to the ground state

$n2^{2} =64$

$n2=8$

number of possible lines produced when electron jumps from n2 to 1st orbit = $\frac{n(n-1)}{2}$

=$\frac{8(8-1)}{2}$

$=\frac{56}{2}$

$=28$

28 lines are seen in the emission spectrum of hydrogen.

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