A monochromatic radiation of wavelength 975 Å excites the hydrogen atom from its ground state to a higher state. How many different spectral lines are possible in the resulting spectrum? Which transition corresponds to the longest wavelength amongst them?
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Wavelength = 975 Å = 975 × 10⁻¹⁰ m.
From the Ground state to the excited state, this means, n₁ = 1
∴ 1/λ = R(1/n₁² - 1/n₂²)
∴ 1/975 × 10⁻¹⁰ = R(1/1 - 1/n²)
10¹⁰ = 975R(n² - 1)/n²
10¹⁰n² = 975Rn² - 975R
10¹⁰n² = 1.09 × 10⁷(975n² - 975)
1000n² = 1.09 × 975n² - 975 × 1.09
1000n² = 1062.75n² - 1062.75
1062.75n² - 1000n² = 1062.75
62.75n² = 1062.75
n² = 16.94
∴ n = 4.12
∴ n ≈ 4
This means, electrons jumps from the ground state to the 4th level.
Now, Using the Formula,
No. of Spectral lines = (n₂ - n₁ + 1)(n₂ - n₁)/2
= (4 - 0 + 1)(4 - 0)/2
= 5 × 4/2
= 5 × 2
= 10
Therefore, no. of spectral lines is 10.
Longest Transition is from n=1 to n = 4.
Hope it helps.
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