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
The ionisation energy of the hydrogen atom is about:The lowest energy state of an atom is called the:The energy of the emitted photon equals the difference between the:By Bohr's third postulate, a transition to lower energy emits a:Allowed angular momenta are integral multiples of h divided by:Bohr's second postulate quantises which quantity?Bohr called the stable non-radiating orbits the:By Bohr's first postulate, an electron in a stable orbit emits: