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In the spectrum of singly ionized helium...

In the spectrum of singly ionized helium , the wavelength of a line abserved is almost the same as the first line of Balmer series of hydrogen . It is due to transition of electron from `n_(1) = 6 to n_(2) = ^(''**'')`. What is the value of `(''**'')`.

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To solve the problem, we need to find the value of \( n_2 \) for the transition of an electron in singly ionized helium that produces a wavelength similar to the first line of the Balmer series of hydrogen. ### Step-by-Step Solution: 1. **Understand the Balmer Series for Hydrogen:** The first line of the Balmer series corresponds to the transition from \( n_2 = 3 \) to \( n_1 = 2 \). The formula for the wavelength in the Balmer series is given by: \[ \frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \] where \( R \) is the Rydberg constant. 2. **Calculate the Wavelength for the First Line of Balmer Series:** For the first line (transition from \( n_2 = 3 \) to \( n_1 = 2 \)): \[ \frac{1}{\lambda} = R \left( \frac{1}{2^2} - \frac{1}{3^2} \right) \] Simplifying this: \[ \frac{1}{\lambda} = R \left( \frac{1}{4} - \frac{1}{9} \right) = R \left( \frac{9 - 4}{36} \right) = R \left( \frac{5}{36} \right) \] Thus, we have: \[ \lambda = \frac{36}{5R} \] 3. **Apply the Formula for Singly Ionized Helium:** For singly ionized helium, the atomic number \( Z = 2 \). The formula for the wavelength in this case is: \[ \frac{1}{\lambda} = RZ^2 \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) \] Here, \( n_1 = 6 \) (as given) and \( Z = 2 \): \[ \frac{1}{\lambda} = R \cdot 2^2 \left( \frac{1}{6^2} - \frac{1}{n_2^2} \right) = 4R \left( \frac{1}{36} - \frac{1}{n_2^2} \right) \] 4. **Set the Two Wavelength Equations Equal:** Since the wavelengths are almost the same: \[ \frac{5}{36}R = 4R \left( \frac{1}{36} - \frac{1}{n_2^2} \right) \] Cancel \( R \) from both sides: \[ \frac{5}{36} = 4 \left( \frac{1}{36} - \frac{1}{n_2^2} \right) \] 5. **Simplify and Solve for \( n_2^2 \):** Multiply both sides by 36: \[ 5 = 4 \left( 1 - \frac{36}{n_2^2} \right) \] Expanding gives: \[ 5 = 4 - \frac{144}{n_2^2} \] Rearranging gives: \[ 1 = -\frac{144}{n_2^2} \implies \frac{144}{n_2^2} = 1 \implies n_2^2 = 144 \] Therefore: \[ n_2 = 12 \] ### Final Answer: The value of \( n_2 \) is **12**.

To solve the problem, we need to find the value of \( n_2 \) for the transition of an electron in singly ionized helium that produces a wavelength similar to the first line of the Balmer series of hydrogen. ### Step-by-Step Solution: 1. **Understand the Balmer Series for Hydrogen:** The first line of the Balmer series corresponds to the transition from \( n_2 = 3 \) to \( n_1 = 2 \). The formula for the wavelength in the Balmer series is given by: \[ \frac{1}{\lambda} = R \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right) ...
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Calculate the wavelength of the first line in the Balmer series of hydrogen spectrum

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Knowledge Check

  • The third line of the Balmer series, in the emission spectrum of the hydrogen atom, is due to the transition from the

    A
    fourth Bohr orbit to the first Bohr orbit
    B
    fifth Bohr orbit to the second Bohr orbit
    C
    sixth Bohr orbit to the third Bohr orbit
    D
    seventh Bohr orbit to the third Bohr orbit.
  • If the wavelength of the first line of the Balmer series of hydrogen is 6561 Å , the wavelngth of the second line of the series should be

    A
    `13122 Å`
    B
    `3280 Å`
    C
    `4860 Å`
    D
    `2187 Å`
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