Given below are two statements.

Statement I: According to Bohr’s model of an atom, qualitatively the magnitude of velocity of electron increases with decrease in positive charge on the nucleus as there is no strong hold on the electron by the nucleus.

Statement II: According to Bohr’s model of an atom, qualitatively the magnitude of velocity of electron increases with decrease in principal quantum number.

In the light of the above statements, choose the most appropriate answer from the options given below.

Orbital angular momentum = $\frac{nh}{2\pi }$ $\frac{}{}$

= $\frac{3h}{2\pi }\left(?n=3\right)$

Radius of Bohr’s orbit $R_n=0.529\stackrel{o}{A}\times \frac{n^2}{z}$  

Radius of Bohr’s orbit for hydrogen,   $R_n=0.529\stackrel{o}{A}\times n^2$

For third orbit (R₃) = $0.529\stackrel{o}{A}\times 9$ = r₃ and

Fourth orbit (R₄) = $0.59\stackrel{o}{A}\times 16=r_4$

$\therefore r_4=\frac{16r_3}{9}$  

For irreversible expansion of an ideal gas under isothermal condition
ΔU = 0, ΔS (Total) ≠ 0

105.8 × (2/4) = 52.9 pm ⇒ r_Li+ + r_X- = 52.9 × (3²/3) = 158.7 pm

Bohr's theory accounts for the line spectrum of single electron species but Li? has two electrons. Bohr's theory fails to explain splitting of spectral lines in presence of magnetic field i.e. Zeeman effect.