![]() The colour can be used to identify the metal or its compounds (eg sodium vapour in a street lamp). Certain bright lines in these spectra cause the characteristic flame colour. When the electrons fall back to lower energy levels, they emit light of various specific wavelengths (the atomic emission spectrum). The electrons in the metal ions are excited to higher energy levels by the heat. calcium – orange-red (probably the least spectacular).potassium – purple-pink, traditionally referred to as ‘lilac’ (often contaminated with small amounts of sodium).sodium – yellow-orange (typical ‘street lamp’ yellow).A better way to produce a steady source of light is to use discharge tubes from the Physics Department – with a suitable risk assessment.) As an extension, students can view the flames through hand-held spectroscopes or diffraction gratings in order to see the line spectrum of the element.The colour of the flame depends on the metal in the salt used. ![]()
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