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PhysicsModern PhysicsAtomic structureEasy2 minPYQ_2020

PhysicsEasysingle choice

The energy required for transition in a Hydrogen atom from $1^{s t}$ energy level to the $2^{n d}$ energy level is $E .$ Then, which of the following transitions is possible for the same energy in Helium atom?

Options:

Answer:

Solution:

For Hydrogen: $E = 13.6 (\frac{1}{1^{1}} - \frac{1}{2^{2}}) eV$ ….(i)
For Helium: $E = 13.6 {(2)}^{2} (\frac{1}{n_{1}^{2}} - \frac{1}{n_{2}^{2}}) eV$ …(ii)
From eq (i) & (ii)
$13.6 (\frac{3}{4}) = 13.6 (4) (\frac{1}{n_{1}^{2}} - \frac{1}{n_{2}^{2}})$
$\frac{1}{n_{1}^{2}} - \frac{1}{n_{2}^{2}} = \frac{3}{16}$
Thus, $n_{1} = 2$ & $n_{2} = 4$ are satisfying the equation.

Stream:NTA_ABHYAS_NEETSubject:PhysicsTopic:Modern PhysicsSubtopic:Atomic structure

⏱ 2mℹ️ Source: PYQ_2020

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