The radius of the first orbit in a hydrogen atom is $5.3 \times 10^{-11} \text{ m}$. The kinetic energy $E_K$, potential energy $E_P$, and total energy $E_T$ of the electron in the first orbit are:
- A$E_K = - 13.6 \text{ eV}, E_P = 27.2 \text{ eV}, E_T = 13.6 \text{ eV}$
- B$E_K = 13.6 \text{ eV}, E_P = - 27.2 \text{ eV}, E_T = - 13.6 \text{ eV}$
- C$E_K = - 27.2 \text{ eV}, E_P = - 13.6 \text{ eV}, E_T = 13.6 \text{ eV}$
- D$E_K = 13.6 \text{ eV}, E_P = - 6.8 \text{ eV}, E_T = - 13.6 \text{ eV}$
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View SolutionIf $m$ is the mass of an electron,$v$ is its velocity,$r$ is the radius of a stationary circular orbit around a nucleus with charge $Ze$,then from Bohr's first postulate,the kinetic energy of the electron is (where $K = 1 / 4 \pi \epsilon_0$):
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