An electron with kinetic energy E collides wi | vedclass

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(B) The first excitation energy of a hydrogen atom in the ground state $(n=1)$ to the first excited state $(n=2)$ is $E_2 - E_1 = -3.4 \,eV - (-13.6 \

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for $E < 10.2 \,eV$

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(B) The first excitation energy of a hydrogen atom in the ground state $(n=1)$ to the first excited state $(n=2)$ is $E_2 - E_1 = -3.4 \,eV - (-13.6 \,eV) = 10.2 \,eV$.If the kinetic energy $E$ of the incident electron is less than $10.2 \,eV$,the hydrogen atom cannot absorb any energy because there are no energy levels available between $n=1$ and $n=2$. Consequently,no internal energy change occurs,and the collision is elastic.If the kinetic energy $E$ is greater than or equal to $10.2 \,eV$,the hydrogen atom can absorb $10.2 \,eV$ of energy to transition to the $n=2$ state. In this case,the collision is inelastic.Therefore,the collision is elastic for $E < 10.2 \,eV$.

An electron with kinetic energy $E$ collides with a hydrogen atom in the ground state. The collision will be elastic

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