Iodine molecule dissociates into atoms after absorbing light of 4500 $\stackrel{\circ }{A}$. If one quantum of radiation is absorbed by each molecule, calculate the kinetic energy of iodine atoms:
[Given: Bond energy of I₂ is 240 kJ mol^-1 ]

1. $2.16\times {10}^{-20}<mspace\; width="1em"></mspace>J$

2. $0.16\times {10}^{-20}<mspace\; width="1em"></mspace>J$

3. $5.03\times {10}^{-20}<mspace\; width="1em"></mspace>J$

4. $8.32\times {10}^{-20}<mspace\; width="1em"></mspace>J$

How many electrons can fit in the subshell for which n = 3 and l = 1?

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 incorrect statement among the following is:

1.	Total orbital angular momentum of an electron in 's' orbital is equal to zero.
2.	An orbital is designated by three quantum numbers, while an electron in an atom is designated by four quantum numbers.
3.	The electronic configuration of N atom is
4.	The value of m for dz2 is zero.

The number of d -electrons in Fe²⁺ (atomic number  Z = 26)  is different from the number of:
1. s-electrons in Mg (Z = 12)
2. p-electrons in Cl (Z = 17)
3. d-electrons in Fe (Z = 26)
4. p-electrons in Ne (Z = 10)

The angular momentum of electrons in d orbital is equal to:
1. $\sqrt{6}$ $\sout{h}$
2. $\sqrt{2}$$\sout{h}$
3. $2\sqrt{3}$ $\sout{h}$
4. 0 $\sout{h}$

What is the maximum number of orbitals that can be identified with the following quantum numbers?
n = 3, l = 1, m = 0

Maximum number of electrons in a subshell with l = 3 and n = 4 is:

1. 14

2. 16

3. 10

4. 12