List of top Chemistry Questions on Bohr's model of hydrogen atom

X\(^{a+}\) and Y\(^{b+}\) are hydrogen-like species. The wavelength of light absorbed during the transition between the states with principal quantum numbers \(n = 1\) and \(n = 2\) of X\(^{a+}\) is \(\lambda\). The wavelength of light absorbed during the transition between the states with principal quantum numbers \(n = 2\) and \(n = 4\) of Y\(^{b+}\) is \(9\lambda\). The lowest possible value of \((a+b)\) is _______.

According to Bohr's model, the angular momentum of an electron in a stable orbit is an integral multiple of

According to Bohr's model of the hydrogen atom, the ratio of the kinetic energy to the total energy of an electron in \(3^{\text{rd}}\) excited state is?

Ionisation energy of H-atom is \(13.6 \text{ eV}\). The wavelength of the spectral line emitted when an electron in \(\text{Be}^{3+}\) comes from \(5^{\text{th}}\) energy level to \(2^{\text{nd}}\) energy level is:

The degeneracy of a hydrogen atom whose energy equals \(-R_H/16\) is:

The frequency of photon which is emitted during a transition of electron of $\text{He}^+$ ion from fifth energy level to third energy level will be:

A hydrogen atom absorbs energy and rises to the $n = 3$ state from its ground state $n = 1$. If the potential energy of the atom at its ground state is $-22\text{ eV}$, find the wavelength emitted by it when it returns to its ground state: (Take Planck's constant $= 6 \times 10^{-34}\text{ J s}$, speed of light $= 3 \times 10^8\text{ m s}^{-1}$)}

The wavelength of the radiation emitted, when an electron falls from infinity to stationary state 1, would be (Rydberg constant = 1.097 × 10⁷ m⁻¹)

The angular momentum and the energy of the electron in the second Bohr’s orbit are respectively

The transition energy of the electron from higher to lower level is $3.0\times10^{-19},J$. The wavelength of the emitted light is about ($h=6.625\times10^{-34},Js,\ c=3\times10^8,ms^{-1}$)

The energy of the electron in third excited state of the hydrogen atom is

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)

Velocity of \( \text{I}^{\text{st}} \) orbit of hydrogen according to Bohr theory is \( v \), then what is the velocity of \( 3^{\text{rd}} \) orbit of hydrogen?

Which of the following statement is NOT true with Bohr's model of atom?

The ratio of the difference between the radii of \( 3^{rd} \) and \( 4^{th} \) orbits of the \( He^+ \) and those of \( Li^{2+} \) is:

Which of the following is correct in the case of the Bohr model of atoms?
A. Predicts continuous emission spectra for all atoms
B. Assumes that the angular momentum of electrons is quantised
C. Predicts same emission spectrum for singly ionised neon atom and hydrogen atom
D. Predicts same emission spectrum for singly ionised neon atom and singly ionised helium atom

What is the frequency \( \nu \) of the electron in Bohr's first orbit of radius \( r \) of the hydrogen atom?

Ionization potential of hydrogen atom is 13.6 eV. Hydrogen atom in the ground state initially is excited by monochromatic radiation of photon energy 12.75 eV. The number of spectral lines emitted by the hydrogen atom, according to Bohr’s theory will be

What is the radius of first orbit of monopositive helium ion?

If an electron in \(n=4\) orbit of hydrogen atom jumps to \(n=3\), the energy released and wavelength emitted are:

Given below are two statements:
Statement-I: The orbitals having same energy are called as degenerate orbitals.
Statement-II: In hydrogen atom, 3p and 3d orbitals are not degenerate orbitals.
In the light of the above statements, choose the most appropriate answer from the options given

Calculate the wavenumber of the photon emitted during transition from the orbit of $n=2$ to $n=1$ in hydrogen atom. [ $R_{H}=109677\text{ cm}^{-1}$]

If radius of second Bohr orbit of the He⁺ ion is 105.8pm, What is the radius of third Bohr Orbit of Li²⁺ ion?

The correct decreasing order of energy for the orbitals having, following set of quantum numbers:
(A) n = 3, l = 0, m = 0
(B) n = 4, l = 0, m = 0
(C) n = 3, l = 1, m = 0
(D) n = 3, l = 2, m = 1

If the radius of the 3^rd Bohr’s orbit of hydrogen atom is r₃ and the radius of 4^th Bohr’s orbit is r₄. Then