The wavelength and frequency of the least energetic in Pfund series of the excited H atom is to be calculated. Concept introduction: Electronic transitions that take place in excited H atom is, 1. Lyman series: electronic transitions take place to the n = 1 level and it is in ultraviolet region. 2. Balmer series: electronic transitions take place from n > 2 to the n = 2 level and it is in visible region. 3. Ritz-Paschen series: electronic transitions take place from n > 3 to the n = 3 level and it is in infrared region. 4. Brackett series: electronic transitions take place from n > 4 to the n = 4 level. 5. Pfund series: electronic transitions take place from n > 5 to the n = 5 level Energy between the states ΔE = E final − E initial = − Rhc ( 1 n final 2 − 1 n initial 2 ) where, R = Rydberg constant h = Planck's constant c = speed of light n = Principal quantum number As the energy gap between two transition states increases the wavelength of the radiation emitted decreases Planck’s equation, E = hν = hc λ where, E = energy h = Planck's constant ν = 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 = c λ where, c = speed of light ν = frequency λ = wavelength

BuyFind

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
BuyFind

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

Solutions

Chapter 6, Problem 54GQ
Interpretation Introduction

Interpretation: The wavelength and frequency of the least energetic in Pfund series of the excited H atom is to be calculated.

Concept introduction:

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

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

As the energy gap between two transition states increases the wavelength of the radiation emitted decreases

  • Planck’s equation,

    E==hcλwhere, 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

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