Metal salts emit different characteristic colors when heated due to electrons in their atoms being excited to higher energy levels and emitting light as they fall back down. Spectroscopy can be used to analyze the light emitted, showing unique "fingerprint" atomic spectra for each element. This relates to Bohr's model of the atom, which describes electrons occupying fixed energy levels and emitting light as they change levels.

1. Flame Test
JOHN FLORENTINO E. ECHON

2. OBJECTIVES
determine the characteristic
colors that metal salts emit;
and
relate the colors emitted by
metal salts to the structure of
the atom.

6. Q1. Why do you think
are there different
colors emitted?

8. Q2. What particles in the heated
compounds are responsible for
the production of the colored
light?

11. Q3. How did the scientists explain
the relationship between the
colors observed and the structure
of the atom?

12. These colors given off by the vapors of elements
can be analyzed with an instrument called
spectroscope
An atomic spectroscope

14. We call this series of lines the atomic
spectrum of the element. The color, numbe
and position of lines produced is called the
“fingerprint” of an element. These are all
constant for a given element.

15. Q4. Explain how your observation in
Activity 1 relates to Bohr’s model of the
atom. You can explain using an illustration

16. n = energy level
Excited state of an electron

17. Q5. Which illustration below represents the
energy of the electron as described by
Bohr? Explain your answer.

19. Conclusion
In the Bohr model, electrons are described as
occupying fixed energy levels at a certain
distance from the nucleus of an atom.