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Energy of H-atom in the ground state is -13.6 eV, hence energy in the second excited state is
1. -6.8 eV 
2. -3.4 eV
3. -1.51 eV 
4. -4.53 eV

Which of the following ions has the maximum magnetic moment?
1. Mn²⁺ 
2. Fe²⁺
3. Ti²⁺
4. Cr²⁺

Which of the following sets of quantum numbers is correct for an electron in 4f orbital?
1. n = 4, l = 3, m = +4, s = + ½
2. n = 4, l = 4, m = -4, s = - ½
3. n = 4, l = 3, m = +1, s = + ½
4. n = 3, l = 2, m = -2, s = + ½

Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l =1 and 2 are, respectively:
1. 12 and 4 
2. 12 and 5
3. 16 and 4 
4. 16 and 5

The wavelength of the radiation emitted, when in a hydrogen atom electron falls from infinity to stationary state 1, would be (Rydberg constant = 1.097 x 10⁷ m^-1):
1. 91 nm 
2. 192 nm
3. 406 nm 
4. 9.1 x 10^-8 nm

Which of the following statements in relation to the hydrogen atom is correct?
1. 3s and 3p orbitals are of lower energy than 3d orbital
2. 3p orbital is lower in energy than 3d orbital
3. 3s orbital is lower in energy than 3p orbital
4. 3s, 3p and 3d orbitals all have the same energy

Of the following sets which one does NOT contain isoelectronic species?
1. ${\mathrm{PO}}_{{}^4}^{3-},{\mathrm{SO}}_4^{2-}, {\mathrm{ClO}}_4^{-}$
2.${\mathrm{CN}}^{-},{\mathrm{N}}_2,{\mathrm{C}}_2^{2-}$
3. ${\mathrm{SO}}_3^{2-}, {\mathrm{CO}}_3^{2-}, {\mathrm{NO}}_3^{-}$ 
4. ${\mathrm{BO}}_3^{3-},{\mathrm{CO}}_3^{2-},{\mathrm{NO}}_3^{-}$

The angular momentum  of 2s and 2p electrons, in units of h / 2π, are respectively  
1. 1, 2                   
2. 2, 2
3 0, √2                 
4. 0, 1

A monoenergetic electron beam with a de Broglie wavelength of x Å is accelerated till its wavelength is halved. By what factor is its kinetic energy changed?
1. 10 
2. 6
3. 4 
4. 2

According to the Bohr theory for the hydrogen atom, the number of revolutions of the electron per second in the orbit of quantum number, n is proportional to
1. n² 
2. 1/n
3. 1 / n² 
4. 1 / n³

If the nitrogen atom has electronic configuration 1s⁷, it would have energy lower than that of the normal ground state configuration 1s² 2s² 2p³ , because the electrons would be closer to the nucleus. Yet 1s⁷ is not observed because it violates.
1. Heisenberg uncertainty principle 
2. Hund’s rule
3. Pauli’s exclusion principle
4. Bohr postulates of stationary orbits.

The electrons, identified by quantum numbers n and l (i) n = 4, l = 1 (ii) n = 4, l = 0 (iii) n = 3, l = 2 (iv) n = 3, l = 1 can be placed in order of increasing energy from the lowest to highest as:
1. (iv) < (ii) < (iii) < (i)
2. (ii) < (iv) < (i) < (iii)
3. (i) < (iii) < (ii) < (iv)
4. (iii) < (i) < (iv) < (ii)

Bohr model can explain: 
1. the solar spectrum
2. the spectrum of the hydrogen molecule
3. the spectrum of hydrogen atoms only
4. spectrum of an atom or ion containing one electron only

Which electronic level would allow the hydrogen atom to absorb a photon but not to emit a photon?
1. 1s 
2. 2s
3. 2p 
4. 3s

Correct set of four quantum numbers for the valence (outermost) electron of rubidium (Z = 37) is
1. 5, 0, 0 , ± ½ 
2. 6, 0, 0 , + ½
3. 5, 1,1, ± ½ 
4. 5, 1, 0, ± ½

The increasing order (lowest first) for the values of e/m (charge / mass) for electron (e), proton (p), neutron (n) and alpha particle (a) is:
1. n, p, a , e 
2. n, p, e, a
3. n, a, p, e 
4. e, p, n, a

Rutherford’s scattering experiment is related to the size of the: 
1. atom 
2. nucleus
3. neutron 
4. electron

The principal quantum number of an atom is related to the
1. orientation of the orbital in space 
2. spin angular momentum
3. orbital angular momentum
4. size of the orbital

Any p-orbital can accommodate upto
1. six electrons
2. four electrons
3. two electrons with opposite spins
4. two electrons with parallel spins

When the electron of a hydrogen atom jumps from n = 4 to n = 1 state, the number of spectral lines emitted is
1. 9 
2. 3
3. 6 
4. 15