Bohr's Model for the Hydrogen Atom

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 Bohr orbit radius for the hydrogen atom (n = 1) is approximately  $0.530\AA .$  The radius for the first excited state (n = 2) orbit is  $(in\AA )$

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 Bohr's model of hydrogen atom, the radius of the first electron orbit is $0.53{\mathrm{A}}^{\mathrm{o}}$. What will be the radius of the third orbit? 

The electron in the ${\mathrm{n}}^{\mathrm{th} }$ orbit of ${\mathrm{Li}}^{2+}$  is excited to $(\mathrm{n}+1)$ orbit using the radiation of energy $1.47\times {10}^{-17} \mathrm{J}$ (as shown in the diagram). The value of $\mathrm{n}$ is ___________

Given : ${\mathrm{R}}_{\mathrm{H}}=2.18\times {10}^{-18} \mathrm{J}$

The energy of an electron in the first Bohr orbit of hydrogen atom is $-2.18\times {10}^{-18} \mathrm{J}$ Its energy in the third Bohr orbit is$\_\_\_\_\_\_\_.$

Given below are two statements

Statement I : According to Bohr’s model of hydrogen atom, the angular momentum of an electron in a given stationary state is quantised.

Statement II : The concept of electron in Bohr’s orbit, violates the Heisenberg uncertainty principle. In the light of the above statements, choose the most appropriate answer from the options given below

Statement-1: According to Bohr's model, angular momentum is Quantised for stationary orbits.

Statement-2: Bohr's Model doesn't follow Heisenberg's Uncertainty principle.

The ratio of radii of second and third Bohr orbits of hydrogen atoms is : 

Radius of second orbit of ${\mathrm{He}}^{+}$ is ${\mathrm{r}}_{\circ }$. Radius of fourth orbit of ${\mathrm{Be}}^{3+}$ is ${\mathrm{xr}}_{\circ }$. Find $\mathrm{x}$ ?

Shortest wavelength will be for which of the following transition.

If radius of ground state hydrogen is $51 \mathrm{pm}$, find out the radius of $5^{\mathrm{th}}$ orbit of ${\mathrm{Li}}^{2+}$ ions in $\mathrm{pm}$.

If the kinetic energy of electron for ${\mathrm{Li}}^{2+}$ in $4^{\mathrm{th}}$ orbit is $\mathrm{Y} \mathrm{eV}$, then the potential energy of electron in the third excited state of ${\mathrm{He}}^{+} (\mathrm{in} \mathrm{eV})$ is

Which of the following electronic transition occurs in H-spectrum having same wavelength as in ${\mathrm{He}}^{+}$ ion spectrum when electron jumps from third excited state to first excited state.

How many maximum line are observed in emission spectrum, if only two hydrogen atoms are present in the sample and electron in both atoms makes electronic transition from $\mathrm{n}=4 \mathrm{to} \mathrm{n}=1$?(Both electrons must follow different path)

Which electronic transition in a hydrogen atom, starting from the orbit $\mathrm{n}=7$, will produce infrared light of wave length $2170 \mathrm{nm}$? (Given: ${\mathrm{R}}_{\mathrm{H}}=1.09677\times {10}^7 {\mathrm{m}}^{-1}$)