The colour of the second line of the Balmer s | vedclass

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(A) The Balmer series corresponds to transitions where the electron jumps to the $n=2$ orbit.The first line corresponds to the transition from $n=3$ t

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Blue

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(A) The Balmer series corresponds to transitions where the electron jumps to the $n=2$ orbit.The first line corresponds to the transition from $n=3$ to $n=2$.The second line corresponds to the transition from $n=4$ to $n=2$.The wavelength $\lambda$ is calculated using the Rydberg formula: $\frac{1}{\lambda} = R \left( \frac{1}{2^2} - \frac{1}{4^2} \right) = R \left( \frac{1}{4} - \frac{1}{16} \right) = R \left( \frac{3}{16} \right)$.Calculating this gives $\lambda \approx 486.1 \ nm$.This wavelength falls in the blue-green region of the visible spectrum,which is commonly identified as blue.

The colour of the second line of the Balmer series is

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