### Electron Transitions for the Hydrogen AtomThe diagram shows the electron transitions in a hydrogen atom for different series. Each colored line represents electron transitions from higher energy levels (n) to a specific lower energy level.- **Lyman Series (Ultraviolet Region):** - Transitions from n ≥ 2 to n = 1 - Represented by orange lines.- **Balmer Series (Visible Region):** - Transitions from n ≥ 3 to n = 2 - Represented by green lines.- **Paschen Series (Infrared Region):** - Transitions from n ≥ 4 to n = 3 - Represented by teal lines.- **Brackett Series (Infrared Region):** - Transitions from n ≥ 5 to n = 4 - Represented by blue lines.### Problem StatementThe series limit wavelength of the Balmer series is emitted as the electron in the hydrogen atom falls from \( n = \infty \) to \( n = 2 \). What would be the specific wavelength of such a line?### Hint\[\frac{1}{\lambda} = R_H\left(\frac{1}{n_{\text{final}}^2} - \frac{1}{n_{\text{initial}}^2}\right)\]where \( R_H \) (Rydberg constant) = \( 1.097 \times 10^7 \, \text{m}^{-1} \).### CalculationFor series limit of the Balmer series:- \( n_{\text{initial}} = \infty \)- \( n_{\text{final}} = 2 \)\[\frac{1}{\lambda} = R_H\left(\frac{1}{2^2} - \frac{1}{\infty^2}\right) = R_H\left(\frac{1}{4} - 0 \right) = \frac{R_H}{4}\]\[\lambda = \frac{4}{R_H} = \frac{4}{1.097 \times 10^7 \, \text{m}^{-1}}\]\[\lambda \approx 364.6 \, \text{nm}\]### Multiple Choice QuestionSelect the correct specific wavelength for the Balmer series limit.

Electron transitions for the Hydrogen atom n=7 n=6 n=5 n=4 n=3 Paschen series E(n) to E(n=3) n=2 Balmer series Ein) to E(n=2) n=1 Lyman series E(n) to E(n=1) The series limit wavelength of the Balmer series is emitted as the electron in the hydrogen atom falls from n = ∞ to n = 2. What would be the specific wavelength of such a line? [Hint :1/λ = RH(1/n² - 1/n;²), R₁ being Rydberg constant = 1.097 x 107 /m] 560 nm 365 nm 400 nm 600 nm Brackett series E(n) to E(n=4)

Electron transitions for the Hydrogen atom n=7 n=6 n=5 n=4 n=3 Paschen series E(n) to E(n=3) n=2 Balmer series Ein) to E(n=2) n=1 Lyman series E(n) to E(n=1) The series limit wavelength of the Balmer series is emitted as the electron in the hydrogen atom falls from n = ∞ to n = 2. What would be the specific wavelength of such a line? [Hint :1/λ = RH(1/n² - 1/n;²), R₁ being Rydberg constant = 1.097 x 107 /m] 560 nm 365 nm 400 nm 600 nm Brackett series E(n) to E(n=4)