What is the wavelength of the line in the Balmer series of hydrogen corresponding to the transition from n = 5 to n = 2? The constant for Balmer's equation is 3.2881 × 10¹⁵ s^-1. A)304 nm B)30.4 nm C)329 nm D)535 nm E)434 nm

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Quizplus · Accepted Answer

The wavelength of the line in the Balmer series for hydrogen can be calculated using the formula for the Balmer series: $ \lambda = \frac{3.2881 \times 10^{15}}{(2^2) - (n^2)} $ where $ n $ is the principal quantum number of the higher energy level (in this case, $ n = 5 $). Plugging in the values, we get $ \lambda = \frac{3.2881 \times 10^{15}}{4 - 25} = 434 $ nm, which corresponds to the transition from $ n = 5 $ to $ n = 2 $.

What Is the Wavelength of the Line in the Balmer