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The Balmer series for the H-atom can be observed

(a) If we measure the frequencies of light emitted when an excited atom falls to the ground state

(b) If we measure the frequencies of light emitted due to transitions between excited states and the first excited state

(c) In any transition in a H-atom .

(d) As a sequence of frequencies with the higher frequencies getting closely

The period number in the long form of the periodic table is equal to

(i) Magnetic quantum number of any element of the period.

(ii) Atomic number of any element of the period.

(iii) Maximum Principal quantum number of any element of the period.

(iv) Maximum Azimuthal quantum number of any element of the period.

The Bohr model for the spectra of a H-atom
(a) Will not be applicable to hydrogen in the molecular form
(b) Will not be applicable as it is for a He-atom
(c) Is valid only at room temperature
(d) Predicts continuous as well as discrete spectral lines

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.
(a) Because of energy conservation
(b) Without simultaneously releasing energy in the form of radiation
(c) Because of momentum conservation
(d) Because of angular momentum conservation

Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is:

(i) F > Cl > Br > I

(ii) F < Cl < Br < I

(iii) F < Cl > Br > I

(iv) F < Cl < Br < I

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

The statement that is not correct for periodic classification of elements is:

(i) The properties of elements are periodic function of their atomic numbers.

(ii) Non metallic elements are less in number than metallic elements.

(iii) For transition elements, the 3d-orbitals are filled with electrons after 3p-orbitals and before 4s-orbitals.

(iv) The first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.

A set of atoms in an excited state decays
(a) In general to any of the states with lower energy
(b) Into a lower state only when excited by an external electric field
(c) All together simultaneously into a lower state
(d) To emit photons only when they collide.

Two H atoms in the ground state collide inelastically. The maximum amount by which their combined kinetic energy is reduced is
(a) 10.20 eV  

(b) 20.40eV    

(c) 13.6 eV

The electronic configuration of gadolinium (Atomic number 64) is 

(i) [Xe] 4f ³ 5d⁵ 6s²

(ii) [Xe] 4f⁷ 5d² 6s¹

(iii) [Xe] 4f⁷ 5d¹ 6s²

(iv) [Xe] 4f⁸ 5d⁶ 6s²

0₂ molecule consists of two oxygen atoms. In the molecule, nuclear force between the nuclei of the two atoms
(a) Is not important because nuclear forces are short-ranged
(b) Is as important as electrostatic force for binding the two atoms
(c) Cancels the repulsive electrostatic force between the nuclei
(d) Is not important because oxygen nucleus have equal number of neutrons and protons

The first ionisation enthalpies of Na, Mg, Al and Si are in the order:

(i)   Na < Mg > Al < Si

(ii)  Na > Mg > Al > Si

(iii) Na < Mg < Al < Si

(iv) Na > Mg > Al < Si

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,
(a) Because Bohr model gives incorrect values of angular momentum
(b) Because only one of these Would Have a minimum energy
(c) Angular momentum must be in the direction of spin of electron
(d) Because electrons go around only in horizontal orbits

The first ionisation enthalpies of Na, Mg, Al and Si are in the order:

(i)   Na < Mg > Al < Si

(ii)  Na > Mg > Al > Si

(iii) Na < Mg < Al < Si

(iv) Na > Mg > Al < Si

The simple Bohr model cannot be directly applied to calculate the energy levels of an atom with man electrons. This is because
(a) Of the electrons not being subject to a central force
(b) Of the electrons colliding with each other
(c) Of screening effects
(d) The force between the nucleus and an electron will no longer be given by Coulomb’s law

The order of screening effect of electrons of s, p, d and f orbitals of a given shell of an atom on its outer shell electrons is:

(i) s > p > d > f

(ii) f > d > p > s

(iii) p < d < s > f

(iv) f > p > s > d

The binding energy of a H-atom, considering an electron moving around a fixed nuclei (proton), is B= .

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= (M=proton mass)

This last expression is not correct.

(a) N would not be integral

(b) Bohr-quantisation applies only two electron

(c) The frame in which the electron is at rest is not inertial

(d) The motion of the proton would not be in circular orbits, even approximately.