Bohr's Model of Hydrogen Atom

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

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

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

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

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

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

$\therefore r_4=\frac{16r_3}{9}$  

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.

ΔR? = (a? /3) (16 – 9)
ΔR? = (a? /2) (16 – 9)
∴ ΔR? /ΔR? = 2/3

Bohr's model solved the instability problem by proving about stationary states. In such stats, the electrons move in fixed orbits. They do not emit energy. This contradicted classical electromagnetic theory of Maxwell, which says accelerating charges should emit radiation and collapse into the nucleus. Bohr simply assumed Maxwell's laws don't apply to these special orbits.