Scientists can analyze metals using the emission spectrum produced when the sample is introduced into the flame of an emission

Question

Scientists can analyze metals using the emission
spectrum produced when the sample is introduced
into the flame of an emission spectrometer. The
flame provides the energy to excite the electrons of
the metal atoms to higher energy states. When the
electrons return to the ground state, lines of
characteristic wavelengths are produced. The lines
in the emission spectrum are characteristic of the
metal because each atom's ground-state electron
configuration is unique.
The emission line used for zinc determinations in atomic emission spectroscopy is 214 nm. If there are 9.00x10¹0 atoms
of zinc emitting light in the instrument flame at any given instant, what energy (in joules) must the flame continuously
supply to achieve this level of emission?
Express your answer numerically in joules.
During an emission, electrons move from a higher energy orbital to a lower energy orbital. Which of the following are valid
transitions that produce lines in the emission spectrum of Zn?

Kunduz · Accepted Answer

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