NCERT Exemplar solutions for Physics [English] Class 12 chapter 12 - Atoms [Latest edition]

Taking the Bohr radius as a₀ = 53 pm, the radius of Li⁺⁺ ion in its ground state, on the basis of Bohr’s model, will be about ______.

The binding energy of a H-atom, considering an electron moving around a fixed nuclei (proton), is B = ${\displaystyle -\frac{M{e}^4}{8n^2{\epsilon }_0^2{h}^2}}$. (m = electron mass). If one decides to work in a frame of reference where the electron is at rest, the proton would be moving around it. By similar arguments, the binding energy would be

B = ${\displaystyle -\frac{M{e}^4}{8n^2{\epsilon }_0^2{h}^2}}$ (M = proton mass)

This last expression is not correct because ______.

The simple Bohr model cannot be directly applied to calculate the energy levels of an atom with many electrons. This is because ______.

For the ground state, the electron in the H-atom has an angular momentum = h, according to the simple Bohr model. Angular momentum is a vector and hence there will be infinitely many orbits with the vector pointing in all possible directions. In actuality, this is not true ______.

O₂ molecule consists of two oxygen atoms. In the molecule, nuclear force between the nuclei of the two atoms ______.

Two H atoms in the ground state collide inelastically. The maximum amount by which their combined kinetic energy is reduced is ______.

A set of atoms in an excited state decays ______.

An ionised H-molecule consists of an electron and two protons. The protons are separated by a small distance of the order of angstrom. In the ground state ______.

1. the electron would not move in circular orbits.
2. the energy would be (2)⁴ times that of a H-atom.
3. the electrons, orbit would go around the protons.
4. the molecule will soon decay in a proton and a H-atom.

Consider aiming a beam of free electrons towards free protons. When they scatter, an electron and a proton cannot combine to produce a H-atom ______.

1. because of energy conservation.
2. without simultaneously releasing energy in the from of radiation.
3. because of momentum conservation.
4. because of angular momentum conservation.

The Bohr model for the spectra of a H-atom ______.

1. will not be applicable to hydrogen in the molecular from.
2. will not be applicable as it is for a He-atom.
3. is valid only at room temperature.
4. predicts continuous as well as discrete spectral lines.

The Balmer series for the H-atom can be observed ______.

1. if we measure the frequencies of light emitted when an excited atom falls to the ground state.
2. if we measure the frequencies of light emitted due to transitions between excited states and the first excited state.
3. in any transition in a H-atom.
4. as a sequence of frequencies with the higher frequencies getting closely packed.

Let E_n = ${\displaystyle \frac{-1}{8{\epsilon }_0^2}\frac{m{e}^4}{n^2{h}^2}}$ be the energy of the nth level of H-atom. If all the H-atoms are in the ground state and radiation of frequency (E₂ - E₁)/h falls on it ______.

1. it will not be absorbed at all.
2. some of atoms will move to the first excited state.
3. all atoms will be excited to the n = 2 state.
4. no atoms will make a transition to the n = 3 state.

The simple Bohr model is not applicable to He 4 atom because ______.

1. He⁴ is an inert gas.
2. He⁴ has neutrons in the nucleus.
3. He⁴ has one more electron.
4. electrons are not subject to central forces.

The mass of a H-atom is less than the sum of the masses of a proton and electron. Why is this?

Imagine removing one electron from He⁴ and He³. Their energy levels, as worked out on the basis of Bohr model will be very close. Explain why.

When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the form of electromagnetic radiation. Why cannot it be emitted as other forms of energy?

Would the Bohr formula for the H-atom remain unchanged if proton had a charge (+4/3)e and electron a charge (−3/4)e, where e = 1.6 × 10^–19C. Give reasons for your answer.

Consider two different hydrogen atoms. The electron in each atom is in an excited state. Is it possible for the electrons to have different energies but same orbital angular momentum according to the Bohr model? Justify your answer.

Positronium is just like a H-atom with the proton replaced by the positively charged anti-particle of the electron (called the positron which is as massive as the electron). What would be the ground state energy of positronium?

Assume that there is no repulsive force between the electrons in an atom but the force between positive and negative charges is given by Coulomb’s law as usual. Under such circumstances, calculate the ground state energy of a He-atom.

Using Bohr model, calculate the electric current created by the electron when the H-atom is in the ground state.

Show that the first few frequencies of light that is emitted when electrons fall to the n^th level from levels higher than n, are approximate harmonics (i.e. in the ratio 1 : 2 : 3...) when n >> 1.

What is the minimum energy that must be given to a H atom in ground state so that it can emit an H_γ line in Balmer series. If the angular momentum of the system is conserved, what would be the angular momentum of such H_γ photon?

The first four spectral lines in the Lyman series of a H-atom are λ = 1218 Å, 1028Å, 974.3 Å and 951.4 Å. If instead of Hydrogen, we consider Deuterium, calculate the shift in the wavelength of these lines.

Deutrium was discovered in 1932 by Harold Urey by measuring the small change in wavelength for a particular transition in ¹H and ²H. This is because, the wavelength of transition depend to a certain extent on the nuclear mass. If nuclear motion is taken into account then the electrons and nucleus revolve around their common centre of mass. Such a system is equivalent to a single particle with a reduced mass µ, revolving around the nucleus at a distance equal to the electron-nucleus separation. Here µ = m_eM/(m_e + M) where M is the nuclear mass and m e is the electronic mass. Estimate the percentage difference in wavelength for the 1st line of the Lyman series in ¹H and ²H. (Mass of ¹H nucleus is 1.6725 × 10^–27 kg, Mass of ²H nucleus is 3.3374 × 10^–27 kg, Mass of electron = 9.109 × 10^–31 kg.)

If a proton had a radius R and the charge was uniformly distributed, calculate using Bohr theory, the ground state energy of a H-atom when (i) R = 0.1 Å, and (ii) R = 10 Å.

In the Auger process an atom makes a transition to a lower state without emitting a photon. The excess energy is transferred to an outer electron which may be ejected by the atom. (This is called an Auger electron). Assuming the nucleus to be massive, calculate the kinetic energy of an n = 4 Auger electron emitted by Chromium by absorbing the energy from a n = 2 to n = 1 transition.

The inverse square law in electrostatics is |F| = ${\displaystyle \frac{e^2}{(4\pi {\epsilon }_0).r^2}}$ for the force between an electron and a proton. The ${\displaystyle \left(\frac{1}{r}\right)}$ dependence of |F| can be understood in quantum theory as being due to the fact that the ‘particle’ of light (photon) is massless. If photons had a mass m_p, force would be modified to |F| = ${\displaystyle \frac{e^2}{(4\pi {\epsilon }_0)r^2}[\frac{1}{r^2}+\frac{\lambda }{r}]}$, exp (– λr) where λ = m_pc/h and h = ${\displaystyle \frac{h}{2\pi }}$. Estimate the change in the ground state energy of a H-atom if m_p were 10^-6 times the mass of an electron.

The Bohr model for the H-atom relies on the Coulomb’s law of electrostatics. Coulomb’s law has not directly been verified for very short distances of the order of angstroms. Supposing Coulomb’s law between two opposite charge + q₁, –q₂ is modified to |F| = ${\displaystyle \frac{q_1{q}_2}{(4\pi {\epsilon }_0)}\frac{1}{r^2},r\ge R_0=\frac{q_1{q}_2}{4\pi {\epsilon }_0}\frac{1}{R_0^2}{\left(\frac{R_0}{r}\right)}^{\epsilon },r\le R_0}$ Calculate in such a case, the ground state energy of a H-atom, if ε = 0.1, R₀ = 1Å.