The Balmer series of hydrogen corresponds to transitions:
AEnding at $n = 1$, giving ultraviolet lines on the chart
BEnding at $n = 3$, giving infrared lines on the spectrum
CStarting at $n = 2$, going up to higher levels in absorption
DEnding at $n = 2$, giving visible spectral lines on chart
Answer & Solution
Correct answer: D. Ending at $n = 2$, giving visible spectral lines on chart
Balmer: transitions to $n = 2$ from higher $n$, visible region.
Related questions
A photon of wavelength $\lambda = 102.6\,\text{nm}$ is incident on a ground-state hydrogenAccording to de Broglie's interpretation of Bohr's quantisation, the circumference of the In the Bohr model, the velocity of an electron in the $n^\text{th}$ orbit of hydrogen is gIn the Bohr model, an electron transitions from $n = 3$ to $n = 2$ in a hydrogen atom (theThe ratio of the first excitation energy of a hydrogen atom ($E_2 - E_1$) to its ionisatioAn $\alpha$-particle of energy $7.7\,\text{MeV}$ is directed head-on at a stationary gold In the Bohr model, the radius of the $n^\text{th}$ orbit of a hydrogen-LIKE atom of atomicWhen the electron in a hydrogen atom makes a transition from $n = 2$ (first excited state)