Explain hydrogen spectrum by Bohr's model

Explanation

Line spectrum observed in case of hydrogen atom can be explained quantiatively using Both.s model
Emitted energy in the spectrum `(Delta E ) ` : According if the electron moves from the orbit
The energy gap between the two orbits is given by equation
but `E_(n ) = R_(H) (1)/( n^(2))` where n= 1,2,3,
put value of `E_(n ) `
`Delta E = (R )/( n ) = (R )/(n )`
`delta E = R_(H) .(1)/( n_(f ) ) - (1)/(n_(f ))`
Frequency of line spectrum ( v) :
`Delta E = hv ` and `V = (Delta E)/(h )`
Put this value in equation 2.27
`V= (Delta E )/( h )`
`=(2.18 xx 10^(-18))/( 6.626 xx 10^(34)) (1)/( n_(1)^(2)) - (1)/( n_(f ) )`
Wave number of spectrum line ( v)
`v= (c )/(lambda) ` but `vec( v) = (1)/(lambda)`
`vec( v ) 1.09677 xx 10^(7) ((1)/( n^(2)) - (1)/( n^(2))) m^(-1)`
with the help equation 2.29 no of spectral line for hydrogen can be calculate.
in case of emissiion spectrum `n_(1) lt n_(i )` and the term in the parenthetic negative and energy is released
The brightness or intensity of spectral lines depends upon the number of photons of same wavelength of freequency absorbed or emitted.