Bohr's Atomic Model

According to the Bohr Theory, among the following, which transition in the hydrogen atom will give rise to the least energetic photon?

The energy of the second Bohr orbit of the hydrogen atom is $-328 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Hence, the energy of the fourth Bohr orbit would be

The radius of hydrogen atom in the ground state is  $0.53\mathrm{\AA }.$  The radius of  ${\mathrm{Li}}^{2+}$ ion (Atomic number = $3$) in first orbit is

In the Balmer series of atomic spectra of hydrogen, there is spectral line having wavelength $434.4 \mathrm{nm}$. Calculate the number of higher orbit from which the electron drops to generate this line. $\left(\mathrm{R}=10.97\times {10}^6 {\mathrm{m}}^{-1}\right)$

Which of the following is the correct value of most probable radius for locating the electron in ${\mathrm{He}}^{+}$?

Assertion : The spectrum of ${\mathrm{He}}^{+}$ is expected to be similar to that of hydrogen.

Reason : ${\mathrm{He}}^{+}$ is also one electron system.

The first orbit is called the ground state in hydrogen like atoms.

Discuss the ground state of hydrogen like atoms.

Is the Bohr's model consistent with the Heisenberg's uncertainty principle?

Bohr's model of an atom is contradicted by

The series of lines present in the visible region of the hydrogen spectrum is

In the Balmer series of atomic spectra of hydrogen, there is spectral line having wavelength $434.4 \mathrm{nm}$. Calculate the number of higher orbit from which the electron drops to generate this line. $\left(\mathrm{R}=10.97\times {10}^6 {\mathrm{m}}^{-1}\right)$

What transition in the ${\mathrm{He}}^{+}$ spectrum would have the same wavelength as the first Lyman transition of hydrogen $({\mathrm{n}}_2=2 \mathrm{to} {\mathrm{n}}_1=1)$?

When electrons from higher orbits of hydrogen atom jump to the $\mathrm{L}$-shell, to which series of the hydrogen spectrum will the emitted light belong?(Lyman/Balmer)

When the electron of a hydrogen atom jumps from $\mathrm{n}=4$ to $\mathrm{n}=1$ state, the number of spectral lines emitted is $6$.

The series of lines present in the visible region of the hydrogen spectrum is _____ (Lyman/Balmer).

In a certain electronic transition in the hydrogen atoms from an initial state $\left(1\right)$ to the final state $\left(2\right)$, the difference in the orbital radius $({\mathrm{r}}_1-{\mathrm{r}}_2)$ is $24$ times the first Bohr radius. Identify the transition.

Which is the correct relation between energies of one electron species?

${\mathrm{E}}_1=$Energy of electron in the first Bohr orbit, ${\mathrm{E}}_2=$Energy of electron in the second Bohr orbit, ${\mathrm{E}}_3=$Energy of electron in the third Bohr orbit, ${\mathrm{E}}_4=$Energy of electron in the fourth Bohr orbit.

The radii of two of the first four Bohr orbits of the hydrogen atom are in the ratio $1:4.$ The energy difference between them may be