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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The Lyman series of spectral lines for the H atom, in the ultraviolet region, arises from transitions from higher levels to n = 1. Calculate the frequency and wavelength of the least energetic line in this series.

Interpretation Introduction

Interpretation:

The frequency and wavelength of least energetic line in Lyman series of the excited H atom has to be calculated.

Concept introduction:

  • The energy difference between two states is calculated by using following formula,

  EnergybetweenthestatesΔE=EfinalEinitial=Rhc(1nfinal21ninitial2)where,R=Rydbergconstanth=Planck'sconstantc=speedoflightn=Principalquantumnumber

  • Planck’s equation,

    E=where, E=energyh=Planck'sconstantν=frequency

The energy increases as the wavelength of the light decrease. Also the energy increases as the frequency of the light increases.

  • The frequency of the light is inversely proportional to its wavelength.

  ν=cλwhere, c=speedoflightν=frequencyλ=wavelength

Electronic transitions that take place in excited H atom is,

  1. 1. Lyman series: electronic transitions take place to the n=1 level and it is in ultraviolet region.
  2. 2. Balmer series: electronic transitions take place from n>2 to the n=2 level and it is in visible region.
  3. 3. Ritz-Paschen series: electronic transitions take place from n>3 to the n=3 level and it is in infrared region.
  4. 4. Brackett series: electronic transitions take place from n>4 to the n=4 level.
  5. 5. Pfund series: electronic transitions take place from n>5 to the n=5 level
Explanation

The frequency and wavelength of least energetic line in Lyman series of the excited H atom is calculated.

Given,

The least energetic line in Lyman series of the excited H atom, if the transition of electron is from n=2 to n=1

  R=1.097×107m1h=6.626×10-34J.sc=2.998×108m/sninitial=2nfinal=1

The energy difference between states while emitting photons is calculated by the equation,

EnergybetweenthestatesΔE=EfinalEinitial=Rhc(1nfinal21ninitial2)

Substituting the values

ΔE=(1.097×107m1)×(6.626×1034J.s)×(2.998×108m/s)(112122)=1.6343×1018J/atom

  • The frequency of least energetic line in Lyman series of the excited H atom is calculated,

According to Planck’s equation

  Ephoton=

Rearranging the equation,

    ν=Ephotonh=1

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