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

According to the Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?
1. n = 5 to n = 3
2. n = 6 to n = 1
3. n = 5 to n = 4
4. n = 6 to n = 5

If the energy value is E = 3.03 × 10^–19 Joules, (h = 6.6×10^–34 J x sec., C = 3×10⁸ m/sec), then the value of the corresponding wavelength is:

Uncertainty in position of a $e^{-}$ and He is similar. If uncertainty in momentum of $e^{-}$ is $\mathrm{32 }\times {10}^5$, then uncertainty in momentum of He will be:

Which of the following options does not represent ground state electronic configuration of an atom?

1. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{8}4{\mathrm{s}}^2$

2. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{9}4{\mathrm{s}}^2$

3. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{10}4{\mathrm{s}}^1$

4. $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^{6}3{\mathrm{d}}^{5}4{\mathrm{s}}^1$

Match the ensuing rules with the corresponding statements:
 

The radii of the first bohr orbit of H(r_H), He⁺ (r_He⁺) and Li2+(r_Li²⁺) are in the order:

1.  r_H = r_He⁺ = r_Li⁺²

2.  r_H < r_He⁺ < r_Li²⁺

3.  r_H > r_He⁺ > r_Li²⁺

4.  r_He⁺ < r_H < r_Li²⁺

A 100-watt bulb emits monochromatic light of wavelength 400 nm. The number of photons emitted per second by the bulb is :

1. 4$0.12 \times {10}^{20} {\mathrm{s}}^{-1}$

2. $2.012 \times {10}^{21} {\mathrm{s}}^{-1}$

3. $2.012 \times {10}^{20} {\mathrm{s}}^{-1}$

4. 2$0.12 \times {10}^{21} {\mathrm{s}}^{-1}$