If $n$ is the orbit number of the electron in a hydrogen atom,the correct statement among the following is
- Aelectron energy varies as $n^{2}$
- Belectron energy increases as $n$ increases
- Chydrogen emits infrared rays for the electron transition from $n=\infty$ to $n=1$
- Delectron energy is zero for $n=1$
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The energy of a hydrogen atom in its ground state is $-13.6 \ eV$. The energy of the level corresponding to the quantum number $n = 2$ (first excited state) in the hydrogen atom is......$eV$.
The first excited state of a hydrogen atom is $10.2 \, eV$ above its ground state. The temperature needed to excite hydrogen atoms to the first excited level is
Medium
View SolutionThe total energy of an electron revolving in the second orbit of a hydrogen atom is
If the ionisation energy for the hydrogen atom is $13.6 \ eV$,then the energy required to excite it from the ground state to the next higher state is nearly: (in $eV$)
The energy of a hydrogen atom in its ground state is $-13.6 \,eV$. The energy of the level corresponding to $n=7$ is ...... $eV$.
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