The document discusses the flame test experiment to determine the characteristic colors emitted by metal salts when heated. It explains that the colors are related to the structure of the atom and energy levels of electrons. When metal salts are heated in a flame, electrons absorb energy and move to higher orbits. They then emit energy in the form of visible light as they fall back to lower orbits, producing distinct colors characteristic of each metal. The Bohr model is described, in which electrons exist at specific energy levels, and absorb or emit photons as they transition between these levels.

2. Objectives
• Find out the characteristic colors
that metal salts emit
• Relate the colors emitted by metal
salts to the structure of the atom

4. 1. Is the fireworks display fascinating to watch?
2. What makes the fireworks display fascinating to
watch?
3. What causes the fireworks display different
colors?
4. What do you think is responsible for the emission
of color during a firework display?

5. What are fireworks made up?
-G_n_o_d_r
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7. Activity No. 1
Flame Test
Objectives:
1. Determine the characteristic colors that metal
salts emit; and
2. Relate the colors emitted by metal salts to the
structure of the atom.

9. Calcium chloride
Iron (III) chloride
Sodium chloride
Lithium chloride
Copper chloride
Strontium chloride
Potassium chloride

10. 1. Calcium chloride Calcium

15. GUIDE QUESTIONS
1. Why do you think are there different colors
emitted?
Metal salts emitted different colors
because of the absorption of heat
from the flame.

16. GUIDE QUESTIONS
2. What particles in the heated compounds are
responsible for the production of the colored light?
The outermost particles in the
metallic element are responsible for
the production of colored light.

17. GUIDE QUESTIONS
3. How did the scientists explain the relationship
between the colors observed and the structure of the
atom?
The colors observed is an indication that
definite energy transformations occurs inside
the atom emitting light. It follows that
electrons must occupy orbits of fixed energy.

21. Ernest Rutherford

22. Rutherford Atomic Model
1. The positive charge and most of the mass of an
atom is concentrated in an extremely small volume.
He called this region of the atom as a nucleus.
2. Rutherford’s model proposed that the negatively
charged electrons surround the nucleus of an atom.
He also claimed that the electrons surrounding the
nucleus revolve around it with very high speed in
circular paths. He named these circular paths as
orbits.
3. Electrons being negatively charged and nucleus
being a densely concentrated mass of positively
charged particles are held together by a strong
electrostatic force of attraction.

23. Niels Bohr

24. Niels Bohr
The Bohr model postulates that
electrons orbit the nucleus at
fixed energy levels.
Orbits further from the nucleus
exist at higher energy levels.
When electrons return to a lower
energy level, they emit energy in
the form of light.

27. --The electrons can move from one energy level to
another by absorbing or releasing energy. Energy
levels in an atom are not equally spaced which
means that the amount of energy are not the same.
The higher energy levels are closer together. If an
electron occupies a higher energy level, it will take
less energy for it to move to the next higher energy
level. As a result of the Bohr model, electrons are
described as occupying fixed energy levels at a
certain distance from the nucleus of an atom.

28. Key
Concepts
The electrons are moving around the nucleus in
circular orbits. When an electron absorbed extra
energy from an outside source (flame), the
electron moves to a higher orbit. Colored light is
emitted when the electron falls back to a lower
orbit. This light is the difference between the
energies of the two orbits involved.

29. Key
Concepts
The energy levels (orbits) of electrons are like the steps of a ladder.
The lowest step of the ladder corresponds to the lowest energy
level. A person can climb up and down by going from step to step.
Similarly, the electrons can move from one energy level to another
by absorbing or releasing energy. Energy levels in an atom are not
equally spaced which means that the amounts of energy are not
the same. The higher energy levels are closer together. The higher
energy level occupied by an electron, the less energy it takes to
move from that energy level to the next higher energy level.

30. What is the difference between Rutherford and
Bohr Atomic modepogi ni landicho?
The Rutherford Model shows an atom with electrons
orbiting a fixed, positively charged nucleus in set,
predictable paths. The Bohr model shows electrons
travel in defined circular orbits around the nucleus.

31. 1.Which combination describes the flame
color of the compound when heated is
CORRECT?
A. Sodium chloride – red
B. Copper (II) sulfate – violet
C. Potassium chloride – blue
D. Calcium chloride-orange
ASSIMILATION

32. 2. Which statement is incorrect?
A. Orbital is a region in an atom where an electron can be found.
B. An electron can emit energy when it jumps to a higher energy
level.
C. An electron can absorb energy when it jumps to a higher energy
level.
D. Filling of electrons in an atom starts from a low energy level to the
highest energy level.

33. 3. Which explain the spectral line given off by an
atom of a substance when heat is applied directly
to it?
A. The electron is removed from the atom.
B. The electron moves faster around its orbit.
C. The electron absorbs energy and jumps to a
higher energy states.
D. The electrons which jumped to a higher
energy state returns to a lower energy state.

34. 4. What do the atomic spectra of elements prove
about the atom?
A. That atom is charged
B. That atom contains a nucleus
C. That atom has electrons that are negatively
charged.
D. That atom has electrons that are found in definite
energy
Levels.

35. 5. Which requires absorption of energy?
A. an electron coming nearer the nucleus
B. The electron going farther to the nucleus
C. an electron moving around the nucleus in its
normal path.
D. None of the above.