1. Flame Tests

2. Colors We can see white light when?
All colored light reaches our eyes at the same time
Only a small portion of the electromagnetic spectrum is visible by the human eye

3. Bohr’s model Electrons orbit the nucleus in “shells”
An electron can travel indefinitely within an energy level without losing energy
The greater the distance between the nucleus and the energy level, the greater the energy level
An electron cannot exist between energy levels, but can move to a higher, unfilled shell if it absorbs a specific quantity of energy, or to a lower, unfilled shell if it loses energy
When all the electrons in an atom are in the lowest possible energy levels, it is in its ground state.

4. Light
An atom becomes excited when one of its electrons absorb energy in the form of photons
If enough energy is absorbed then the electron can make a quantum leap to the next energy level, if there is room
When the electron returns to a lower energy state the energy is released in the form of a photon, which we see as visible light
The energy of the photon determines its wavelength or color
Each element has its own frequencies of color, so it emits its own distinctive glow

5. Spectroscope
An instrument used to observe the color components of any light source
When an element is burned and the flame looked at with a spectroscope, the color is revealed to consist of a pattern of distinct frequencies

6. Spectroscope

7. The Flame Test
The flame test is used to visually determine the identity of an unknown metal in a compound
Elements heated by a flame will glow their characteristic color
Eg. Fire Works
Eg.Sodium headlamps

8. Burning Elements
Calcium, Lithium, Rubidium, Sodium, Potassium