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Which of the following sets of quantum numbers represent an impossible arrangement?
 

How many unpaired electrons are present in Ni²⁺ cation (atomic number = 28)
1. 0
2. 2
3. 4
4. 6

How many unpaired electrons present in the electronic configuration 1s² 2s² 2p³ ?
1. 2
2. 0
3. 3
4. 1

The quantum number of the most energetic electron in an Ne atom in the first excited state is

The total number of orbitals having l = 3  is - 
1. 3
2. 7
3. 5
4. 9

The total spin resulting for a 3d⁷ configuration is 
1. 3/2
2. 1/2
3. 2
4. 1

 3p orbital has -
1. Two spherical nodes
2. Two non-spherical nodes
3. One spherical and one non-spherical node
4. One spherical and two non-spherical nodes

The number of orbitals that are possible at the L-energy level is
1. 2
2. 4
3. 6
4. 1

The maximum number of electrons in a subshell with l = 3 and n = 4 is
1. 14
2. 16
3. 10
4. 12

The correct set of four quantum numbers for the valence electron of rubidium atom (Z =37) is
1. 5, 1, 1, +1/2               
2. 6, 0, 0, +1/2
3. 5, 0, 0, +1/2               
4. 5, 1, 0, +1/2

Consider the following sets of quantum numbers:
              n         l         m         s
(i)         3         0         0          +1/2
(ii)        2         2         1          +1/2
(iii)       4         3        -2           -1/2
(iv)       1         0        -1           -1/2
(v)        3         2         3           +1/2
Which of the following sets of quantum numbers is not possible?
1. ii, iii and iv                             
2. i, ii, iii and iv
3. ii, iv and v                               
4. i and iii

An electronic configuration representing an atom in the excited state is: 
$1.$ $1{\mathrm{s}}^2,2{\mathrm{s}}^{2}2{\mathrm{p}}^1$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$
$2.$ $1{\mathrm{s}}^2,2{\mathrm{s}}^{2}2{\mathrm{p}}^2$
$3.$ $1{\mathrm{s}}^2,2{\mathrm{s}}^{2}2{\mathrm{p}}^2,3{\mathrm{s}}^1$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$ $$
$4.$ $1{\mathrm{s}}^2,2{\mathrm{s}}^{2}2{\mathrm{p}}^5$

A pair of d-orbitals having electron density along the axes is: 
1. $d_{z^2},$ $d_{xz}$
2. $d_{xz},$ $d_{zy}$
3. $d_{z^2},$ $d_{x^2-y^2}$
4. $d_{xy},$ $d_{x^2-y^2}$

The angular momentum of an electron in d orbital is equal to
1. $\sqrt{6}<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>\sout{\mathrm{h}}$
2. $\sqrt{2}<mspace\; width="1em"></mspace>\mathrm{h}$
3. $2\sqrt{3}<mspace\; width="1em"></mspace>\mathrm{h}$
4. 0 h

If the electronic structure of oxygen atom is written as $1{\mathrm{s}}^2,<mspace\; width="1em"></mspace>2{\mathrm{s}}^2$  it would violate:
1.  Hund's rule
2.  Paulis exclusion principle
3.  Both Hund's and Pauli's principles
4.  None of the above

The correct order of the total number of nodes of atomic orbitals is: 
1.  4f > 6s > 5d
2.  6s > 5d > 4f
3.  4f > 5d > 6s
4.  5d > 4f > 6s

Orbitals having two spherical nodes are: 

The quantum number not obtained from Schrodinger’s wave equation is:

The number of electrons with the azimuthal quantum number l = 1 and 2 for Cr ₂₄ in ground state is
1. 16 and 5
2. 12 and 5
3. 16 and 4
4. 12 and 4

An ion with a mass number of 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. The symbol of the ion is :
$1.$ ${}_{26}{}^{56}\mathrm{Fe}^{+3}$
$2.$ ${}_{26}{}^{57}\mathrm{Fe}^{+3}$
$3.$ ${}_{27}{}^{58}\mathrm{Fe}^{+3}$
$4.$ ${}_{25}{}^{56}\mathrm{Fe}^{+3}$