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Question

Consider a hypothetical hydrogen like atom (Ground state energy = 0). The wavelength in ˚A for the spectral lines for transition from n=p to n=1 are given by:
λ=1500 p2p21 where p=2,3,4,...

(Take hc=12400 eV˚A)

A
The wavelength of the least energetic and the most energetic photons in this series is 2000 ˚A,1500˚A.
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B
Difference between energies of fourth and third orbit is 0.40 eV
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C
Energy of second orbit 6.2 eV
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D
The ionization of this element is 8.27 eV
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Solution

The correct option is D The ionization of this element is 8.27 eV
Given that,

λ=1500 p2p21=150011p2

(A) The least energetic photon corresponds to the transition from n=2n=1.

So, substituting p=2 ,

λmax=15001122=43×1500˚A

λmax=2000˚A

The most energetic photon corresponds to the transition from n=n=1. So, p=,

λmin=1500112=1500˚A

Now,

λ21=1500114=2000˚A

ΔE21=hcλ21=124002000eV=6.2 eV

λ31=1500119=98×1500˚A

ΔE31=1240098×1500eV=7.35 eV

Simlarly,

ΔE41=124001615×1500eV=7.75 eV

Given that E1=0, From the above data,

E2=6.2 eV
E3=7.35 eV
E4=7.75 eV

E4E3=0.40 eV

So, option B and C are correct.

The ionization energy is the energy required to take an electron from n=1n=

Eion=hcλmin=124001500 eV=8.27 eV

Hence, all the given options are correct.

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