The metals that are likely to be present in the steel sample according to the hypothetical emission spectrum should be determined. Concept introduction: Hypothetical emission spectrum In a real spectrum, the photographic images of the spectral lines would differ in depth and thickness depending on the strengths of the emissions producing them. Some of the spectral lines would not be seen because of their faintness. In principle, we obtain exactly the same information about the quantizedenergy levels of a system by using either emission spectroscopy or absorption spectroscopy. The choice of which technique to use is influenced byother considerations. If the sample contains a relatively small number ofatoms, emission spectroscopy might be the preferred technique because ithas a higher sensitivity. (It is easier to detect a very dim line on a dark background than to detect a faint dark line on a bright background.) If sensitivity is not a concern, then perhaps absorption spectroscopy might be thepreferred technique. Absorption spectra are often less complicated thanemissionspectra. An excited sample will contain atoms in a variety ofstates, each being able to drop down to any of several lower states. Anabsorbing sample generally is cool and transitions are possible only fromthe ground state. The Balmer series is not seen, for example, in absorptionfrom cold hydrogen atoms.

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Chapter 8, Problem 113FP

Interpretation Introduction

Interpretation:

The metals that are likely to be present in the steel sample according to the hypothetical emission spectrum should be determined.

Concept introduction:

Hypothetical emission spectrum

In a real spectrum, the photographic images of the spectral lines would differ in depth and thickness depending on the strengths of the emissions producing them. Some of the spectral lines would not be seen because of their faintness.

In principle, we obtain exactly the same information about the quantizedenergy levels of a system by using either emission spectroscopy or absorption spectroscopy. The choice of which technique to use is influenced byother considerations. If the sample contains a relatively small number ofatoms, emission spectroscopy might be the preferred technique because ithas a higher sensitivity. (It is easier to detect a very dim line on a dark background than to detect a faint dark line on a bright background.) If sensitivity is not a concern, then perhaps absorption spectroscopy might be thepreferred technique. Absorption spectra are often less complicated thanemissionspectra. An excited sample will contain atoms in a variety ofstates, each being able to drop down to any of several lower states. Anabsorbing sample generally is cool and transitions are possible only fromthe ground state. The Balmer series is not seen, for example, in absorptionfrom cold hydrogen atoms.

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