The diagram shows the energy level transitions in a hydrogen atom that result in the emission of a visible photon. An il

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The diagram shows the energy level transitions in a hydrogen
atom that result in the emission of a visible photon.
An illustration of energy levels shows the colors of the lines
of the Balmer series. The bottom energy level in the diagram
is n = 2, and an upward arrow indicates that
energy increases with higher energy levels, labeled up
to n = ∞, where E = 0.00 eV. The energy
of n = 2 is −3.401
eV, n = 3 is −1.512
eV, n = 4 is −0.8504 eV,
and n = 5 is −0.5442 eV. Balmer lines are
produced when an electron jumps to n =
2 from any higher level. Red color is emitted during
transition from n = 3, green color during
transition from n = 4, blue color during
transition from n = 5, and violet color
during transition from n = 6.
Consider the photon that appears blue in the figure.
(a) Determine its energy.
eV

(b) Determine its wavelength.
nm
Consider the photon emission that appears red in the
diagram.
(c) Find its photon energy.
eV

(d) Find its wavelength.
nm