WAVE NATURE OF ELECTROMAGNETIC RADIATION

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WAVE NATURE OF ELECTROMAGNETIC RADIATION:

Continuous Spectrum: This spectrum is due to dispersion of white light.Dispersion of white light gives "VIBGYOR" colors on photographic plate without any gap between each color.This type of spreading colors is called continuousspectrum.
White light produced from sun light, incandescentfilament lamp and solids (or) liquids at high temperaturegives incandescence. VIBGYOR - means Violet, Indigo, Blue, Green, Yellow, Orange and Red.Emission & Absorpationspectrum: Based on white light emission & absorption by gas (or) vapor, spectra can be divided into 2 types.

01. Emission spectrum.

02. Absorption spectrum.
EMISSION SPECTURUM: Specturum due to emission of white light by gas (or) vapour at high temperature.It consists of bright lines on dark back ground.It is due to emission of energy by electrons.
ABSORPTION SPECTURUM: Spectrum due to absorption of white light by gas and transmitted white light.It consists of dark lines on bright back ground.It is due to absorption of energy by electrons.
LINE &BOND SPECTURUM: Based on spectral lines, spectra can be divided into 2 types.01.Line spectrum or Atomic spectrum.02.Bond spectrum.
LINE SPECTRUM or ATOMIC SPECTRUM or DISCONTINUOUS SPECTRUM:It is characteristic of atoms. E.g. Hydrogen atom.It consists of distinct lines.It is due to excitation & de-excitation of electron in an atom.Emission & absorption spectra shows the line spectrum.
BAND SPECTRUM:Characteristic of molecules. E.g. H2 moleculeIt consists of closely spaced lines called bands.It is due to vibration & rotation of atoms in the molecule. E.g.H2 molecule.
HYDROGEN SPECTRUM:The spectrum of hydrogen is the simplest of all spectra.Hydrogen atom exhibits both emission as well as absorption spectra.In 1885, Balmer first observed a series of bright lines in the visible region of hydrogen spectrum and these are called "lines of balmerseries".Later other series of lines were identified.The lines of Balmer series of hydrogen spectrum are designed as Hα , Hβ , H gamma, Hf.For Hα: n =3, For Hβ: n =4, For H gamma: n=5 and For Hf: n=6.The wave number of the spectral line of hydrogen spectrum for any series is given by Rydberg's equation.
new bar = 1 by lambda = R into 1 by n12 minus 1 by n22 Where: R - Rydberg Constant 109677.8 cm inverse. n1and n2 are whole numbers.Hydrogen spectrum consists of 5 series: You can see the table for the details of each series like year of discovery, spectral series, values of n1 and n2, spectral region and wave number formula.Lyman Series: Electron jumps from n2 = 2, 3, 4...to n1 =1.Balmer Series: Electron jumps from n2 = 3, 4, 5...to n1 =2.Paschen Series: Electron jumps from n2 = 4, 5, 6...to n1 =3.Brackett Series: Electron jumps from n2 = 5, 6, 7...to n1 =4.
PfundSeries: Electron jumps from n2 = 6, 7, 8...to n1 =5.
See the above illustration to clearly understand the 5 series.