Which of the following correctly relates the kinetic energy (K), potential energy (U), and total energy (E) of an electron in a Bohr orbit?

The de-Broglie wavelength of an electron in the ground state of the hydrogen atom is

Energy of an electron in an excited hydrogen atom is $- 3.4\,\,eV$. Its angular momentum will be $\left( {h = 6.626\,\, imes \,\,{{10}^{ - 34}}\,\,J - s} \right)$

Hydrogen atom emits blue light when it changes from $n = 4$ energy level to the $n = 2$ level. Which colour of light would the atom emit when it changes from the $n = 5$ level to the $n = 2$ level

The ratio of ionization energy of Bohr’s hydrogen atom and Bohr’s hydrogen like lithium atom is

Given the Rydberg constant is $10^7 m^{-1}$, calculate the wavelength of the last line of the Balmer series in the hydrogen spectrum.

How much work must be done to pull apart the electron and the proton that make up the Hydrogen atom, if the atom is initially in the state with $n = 2$

The de-Broglie wavelength of an electron in the first Bohr orbit is

An electron in an atom has a kinetic energy of $6.8$ eV. If its total energy is $-3.4$ eV, what is its potential energy?

The ratio of kinetic energy (K) to the potential energy (U) of an electron in a Bohr orbit of the hydrogen atom is:

The time of revolution of an electron around a nucleus of charge $Ze$ in ${n^{{\rm{th}}}}$ Bohr orbit is directly proportional to