Chemistry - Atomic Structure Question with Solution | TestHub

ChemistryAtomic StructureSpectrumMedium2 minPYQ_2014

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Based on the equation: $Δ E = - 2.0 \times 1 0^{- 18} J (\frac{1}{n _{2}^{2}} - \frac{1}{n _{1}^{2}})$ the wavelength of the light that must be absorbed to excite hydrogen electron from level $n = 1$ to level $n = 2$ will be: $(h = 6.625 \times 1 0^{- 34} Js, C = 3 \times 1 0^{8} ms^{- 1})$

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Answer:

Solution:

$Δ E = - 2.0 \times 1 0^{- 18} \times (\frac{1}{2 ^{2}} - \frac{1}{1 ^{2}}) = - 2.0 \times 1 0^{- 18} \times \frac{- 3}{4} = 1.5 \times 1 0^{- 18} Δ E = \frac{h c}{λ} λ = \frac{h c}{Δ E} = \frac{6.6 \times 1 0 ^{- 34} \times 3 \times 1 0 ^{8}}{1.5 \times 1 0 ^{- 18}} = 1.325 \times 1 0^{- 7} m$

Stream:JEESubject:ChemistryTopic:Atomic StructureSubtopic:Spectrum

⏱ 2mℹ️ Source: PYQ_2014

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