The energy of an electron in the first Bohr orbit of the $H$ atom is $-13.6 \, eV$. The energy value of an electron in the first excited state of the $H$ atom is ............ $eV$.

Which of the following transitions emits a photon with the maximum frequency?

For a $H$ atom,the wavelength for the highest energy transition is $91.2 \ nm$. Calculate the corresponding wavelength for $He^{+}$ in $nm$.

What is the number of photons of light with a wavelength of $4000 \ pm$ that provide $1 \ J$ of energy?

For a hydrogen atom,the energy of an electron in the first excited state is $-3.4 \ eV$. The kinetic energy $(KE)$ of the same electron in the hydrogen atom is $x \ eV$. The value of $x$ is . . . . . . $\times 10^{-1} \ eV$. (Nearest integer)

What is the angular momentum of an electron in the orbit of an $H$ atom where the energy of the electron is $-3.4 \ eV$?