Class 12th

Magnetic energy stored in an inductor $=\frac{1}{2}{\mathrm{L}\mathrm{I}}^2$

$\begin{array}{rr}& =\frac{1}{2}*4*{10}^{-6}*(2{)}^2\\ & =8\mu \mathrm{J}\end{array}$

${\text{?}\mathrm{}}_{\mathrm{s}}\stackrel{?}{\mathrm{B}}\cdot \mathrm{d}\stackrel{?}{\mathrm{A}}=0\mathrm{}$ (No monopole exist)

A total refractive prism is also known as a total internal reflection prism. It is an optical prism that is designed for reflecting 100% of the incident light. This happens since this prism uses the principle of total internal reflection. These prisms are oriented and shaped in a specific way so that the light that enters at a specific angle is completely reflected inside the prism. A right-angle prism, porro prism, dove prism and roof prism are some of the examples of total reflective prism. 

Total deviation in a prism is the total angle by which the light ray gets bent as it passes through the prism. It is an angle between incident ray and emergent ray of the prism. When a light enters the prism, it will bend towards the normal. After that, it will travel through the prism and bend away from the normal as it exits. Total deviation is the sum of these two from which the apex angle is subtracted.

The formula for total deviation for a prism is as follows:

$\delta = i_1 + e_2 - A$

• $i_1$ : angle of incidence at first surface
• $e_2$ : angle of emergence at second surface
• A: apex angle of the prism 

Hydrogen shows many spectral lines because of the following reasons. 

• Its electron can occupy many levels (n = 1, 2, 3.). 

• Each line in the hydrogen spectrum actually represents the transition from higher to lower energy levels. 

• These lines are grouped by the final energy level (Lyman n'=1, Balmer n'=2, etc.) 

• Higher energy levels are closer together. They tend to create more possible transitions.

Hydrogen produces a line spectrum because electrons exist only in discrete, quantised energy levels. When electrons jump between these fixed energy states, they emit photons with specific energies (E = h? ). This creates distinct spectral lines instead of continuous wavelengths. Bohr's model explains this through quantised orbits. Classical physics, on the other hand, would predict a continuous spectrum.

The hydrogen emission spectrum contains several spectral series, each named after its discoverer.

• Lyman series (n' = 1): To ground state, visible only in ultraviolet region
• Balmer series (n' = 2): Transitions to second level, appearing in visible region
• Paschen series (n' = 3): Moved to third level, visible in the infrared region
• Brackett series (n' = 4): Transitions to fourth level, appearing in the far infrared region
• Pfund series (n' = 5): Transitions to fifth level, showing in the infrared region
• Humphreys series (n' = 6): Transitions to sixth level, appearing in the infrared region

$\mathrm{R}=22*{10}^3\pm 5\mathrm{\%}$

First band = = Red

2nd band = Red

3rd band = Orange (Multiplier)

4th band  Gold (Tolerance)

$3\mu \mathrm{F}$ and $3\mu \mathrm{F}$  in parallel