If each hydrogen atom is excited by giving 8. | vedclass

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(A) The energy required to excite a hydrogen atom from the ground state $(n=1)$ to an excited state $(n)$ is given by the formula:$\Delta E = 13.6 \le

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(A) The energy required to excite a hydrogen atom from the ground state $(n=1)$ to an excited state $(n)$ is given by the formula:$\Delta E = 13.6 \left( 1 - \frac{1}{n^2} ight) \ eV$For $n=2$,$\Delta E = 13.6 \left( 1 - \frac{1}{4} ight) = 13.6 	imes 0.75 = 10.2 \ eV$.For $n=3$,$\Delta E = 13.6 \left( 1 - \frac{1}{9} ight) = 13.6 	imes 0.888 = 12.09 \ eV$.Since $8.4 \ eV$ does not correspond to any transition energy from the ground state $(n=1)$ to any higher energy level $(n > 1)$,the hydrogen atom cannot absorb this energy.Therefore,no electronic excitation occurs,and consequently,no spectral lines are emitted.

If each hydrogen atom is excited by giving $8.4 \ eV$ of energy,then the number of spectral lines emitted is equal to :

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