Question

a

Suppose hydrogen atoms absorb energy so that electrons are excited to the  n = 7 energy level. Electrons then undergo these transitions, among others: (a)  n = 7 to  n =1 (b)  n = 7 to  n = 6 (c)  n = 2 to  n = 1 Enter the letter (a, b, or c) for each. the smallest energy? the highest frequency? the shortest wavelength?

b	What is the frequency of a photon resulting from the transition n=6 → n=1? h = 6.62 × 10-34 J·s s-1

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Answer 1

a) the smallest energy = b

    The highest frequency = a

    The shortest wavelength = a

note: by increasing no of energy levels,the energy of each level increases and the energy gap between the levels decreases.so that, smallest energy is n=7 to n=1.

weknowthat,

            E = hv

           v = frequency , (frequency is directly proportional to energy)

          E = hc/l

      l = wavelength. (wavelength is inversely proportional to energy)

b)

wavenumber = 1/wavelength = 109677(1/n1^2-1/n2^2) cm-1

     n1 = 1 , n2 = 6

   1/wavelength = 109677(1/1^2-1/6^2)

             1/l   = 1.07*10^5 cm-1

c = vl

v =frequency = c/l

c = 3*10^10 cm/s

1/l = 1.07*10^5 cm-1

v = (3*10^10)*(1.07*10^5)

   = 3.21*10^15 s-1