Consider the following sets of quantum numbers: 
 
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 element X has the following isotopic composition: 
²⁰⁰X: 90% 
¹⁹⁹X: 8.0% 
²⁰²X: 2.0% 
The weighted average atomic mass of the naturally-occurring element X is closest to:

1. 200 amu
2. 201 amu
3. 202 amu
4. 199 amu

If the mass of electron is 9.11×10^-31 kg  and the planck's constant is 6.626 ×10^-34 Js, then the uncertainty involved in the measurement of velocity within a distance of 0.1 Å is:

1. $5.79\times {10}^6$ $m{s}^{-1}$

2. $5.79\times {10}^7$ $m{s}^{-1}$

3. $5.79\times {10}^8$ $m{s}^{-1}$

4. $5.79\times {10}^5$ $m{s}^{-1}$

The orientation of an atomic orbital is governed by:

1. azimuthal quantum number

2. spin quantum number

3. magnetic quantum number

4. principal quantum number

If uncertainty in position and momentum are equal, then the uncertainty in velocity is:

1. $\frac{1}{2\mathrm{m}}\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

2. $\sqrt{\frac{\mathrm{h}}{2\mathrm{\pi }}}$

3. $\frac{1}{\mathrm{m}}\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

4. $\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

The incorrect set of quantum numbers among the following is:

1. n= 4, l= 0, m= 0, s= -1/2
2. n= 5, l= 3, m= 0, s= +1/2
3. n= 3, l= 2, m= -3, s= -1/2
4. n= 3, l= 2, m= 2, s= -1/2

The rule used to determine the maximum number of electrons in a subshell of an atom is:

If n = 6, the correct sequence for the filling of electrons will be: 

1. $\mathrm{ns}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-1\right)$ $\mathrm{d}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-2\right)$ $\mathrm{f}$ $\stackrel{}{\to }$ $\mathrm{np}$

2. $\mathrm{ns}$ $-$ $\left(\mathrm{n}-2\right)$ $\mathrm{f}$ $\stackrel{}{\to }$ $\mathrm{np}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-1\right)$ $\mathrm{d}$

3. $\mathrm{ns}$ $-$ $\mathrm{np}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-1\right)\mathrm{d}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-2\right)$ $\mathrm{f}$

4. $\mathrm{ns}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-2\right)$ $\mathrm{f}$ $\stackrel{}{\to }$ $\left(\mathrm{n}-1\right)$ $\mathrm{d}$ $\stackrel{}{\to }$ $\mathrm{np}$

The energies E₁ and E₂ of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths i.e., ${\mathrm{\lambda }}_1$ and ${\mathrm{\lambda }}_2$ will be:

1.  ${\mathrm{\lambda }}_1=2{\mathrm{\lambda }}_2$

2.  ${\mathrm{\lambda }}_1=4{\mathrm{\lambda }}_2$

3.  ${\mathrm{\lambda }}_1=\frac{1}{2}{\mathrm{\lambda }}_2$

4.  ${\mathrm{\lambda }}_1={\mathrm{\lambda }}_2$