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Explainhydrogenspectrumby Bohr'smodel |
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Answer» Solution :Linespectrumobserved incase of hydrogenatomcan beexplainedquantiativelyusingBoth.smodel Emitted energyin THESPECTRUM `(Delta E ) ` :Accordingif the electronmovesfrom the orbit The energygapbetweenthe twoorbitsis GIVENBY equation but `E_(N )= R_(H)(1)/( n^(2))` wheren= 1,2,3, putvalueof `E_(n ) ` `Delta E= (R )/(n )= (R )/(n )` `deltaE =R_(H).(1)/( n_(f ) ) - (1)/(n_(f ))` Frequencyof linespectrum ( v) : `DeltaE = hv ` and`V = (Delta E)/(h )` Putthisvaluein equation2.27 `V= (Delta E )/( h )` `=(2.18 xx 10^(-18))/( 6.626 xx 10^(34))(1)/( n_(1)^(2)) - (1)/( n_(f ) )` Wavenumberof spectrumline ( v) `v= (c )/(lambda) ` but`VEC( v) = (1)/(lambda)` `vec( v )1.09677 xx10^(7)((1)/( n^(2)) - (1)/( n^(2)))m^(-1)` withthe helpequation2.29no ofspectralline forhydrogencan becalculate. in caseofemissiionspectrum `n_(1) lt n_(i )`and thetermin theparentheticnegativeand energyisreleased Thebrightness or intensityof spectral linesdependsupon thenumberof photonsofsamewavelength of freequencyabsorbed oremitted. |
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