1) An energetically excited hydrogen atom has its electron ina 5f sublevel. The

Question

1) An energetically excited hydrogen atom has its electron ina 5f sublevel. The electron drops down to the 3d sublevel,releasing a photon in the process. Given the values:     R =1.097*107m-1      h = 6.626*10-34J.s     c =2.998*108m/s (a) What wavelength of light is emittted by the process? (b) The hydrogen atom now has a single electron in the 3dsublevel. What is the energy in kJ/mol required to remove thiselectron?      Use the constants given above 1) An energetically excited hydrogen atom has its electron ina 5f sublevel. The electron drops down to the 3d sublevel,releasing a photon in the process. Given the values:     R =1.097*107m-1      h = 6.626*10-34J.s     c =2.998*108m/s (a) What wavelength of light is emittted by the process? (b) The hydrogen atom now has a single electron in the 3dsublevel. What is the energy in kJ/mol required to remove thiselectron?      Use the constants given above

Explanation / Answer

   An energetically excited hydrogen atom hasits electron in a 5f sublevel. The electron drops down to the 3dsublevel, releasing a photon in the process. Given the values:     R =1.097*107m-1      h = 6.626*10-34J.s     c =2.998*108m/s Given the values:     R =1.097*107m-1      h = 6.626*10-34J.s     c =2.998*108m/s    a)wavelength of light is emittted by theprocess:       The specific data isni= 5    nf=3       E=  2.179*10-18j(1/52-1/32)            = 2.179*10-18 J *-0.0711            =-0.1549269*10-18 J        When a photon is emittedni> nf concequently the term in parenthises is negative andE is negative .Energy is lost to surroundings .           = ch/ E              =( 2.998*108m/s* 6.626*10-34J.s  ) /0.1549269*10-18 J                =(19.864748 *10-26m*J) /  0.1549269*10-18 J               =128.220* 10-8 m               =  128.220* 10-8 m*(1nm/10-9m)               =1282nm      b)   The energies that canelectron in the hydrogen atom is            En = -RH (1/n2)                 = 2.18*10-18 J (1/32)                 = 0.2422*10-18 J/mol                  =0.2422*10-15 kJ/mol of energy required to removethis electron                 When a photon is emittedni> nf concequently the term in parenthises is negative andE is negative .Energy is lost to surroundings .           = ch/ E              =( 2.998*108m/s* 6.626*10-34J.s  ) /0.1549269*10-18 J                =(19.864748 *10-26m*J) /  0.1549269*10-18 J               =128.220* 10-8 m               =  128.220* 10-8 m*(1nm/10-9m)               =1282nm      b)   The energies that canelectron in the hydrogen atom is            En = -RH (1/n2)                 = 2.18*10-18 J (1/32)                 = 0.2422*10-18 J/mol                  =0.2422*10-15 kJ/mol of energy required to removethis electron         

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