Flame Test Experiment
Purpose:
To measure the energy of the
photons released by specific
elements
Map the position of the electrons of
the elements of specific compounds
Flame Test Experiment
You will test different
elements by placing
them in the flame
The fire serves as
energy that excites
the electrons and
creates a colored
flame.
Flame Test Experiment
What you see inside is the atomic spectra
The numbers above the spectral lines
represent their wavelengths (λ)
The wavelengths are measured in 100 nm (i.e. the middle green line has a λ of 550nm)
Flame Test Experiment
During the lab, you will collect data and
record it in the table below:
Sample Color of
Flame
Spectral line
COLORS
Wavelengths, λ of
the spectral line
(in 100nm units)
Example A Blue 500nm, 550nm, 650nm Blue, Green, Red
Safety
Wear apron, goggles & gloves at all times
Hair tied back
No loose clothing
NEVER leave your station unattended
After you’re done with a wooden splint, put
in beaker of water
Extra Credit - Instagram Picture collage of all flame colors
Explain how the flame changes colors in
the caption
Include all group member first names &
class period
Add #thelaralaboratory to caption
Or tag thelaralaboratory in the picture (if
you follow the class insta)
Make sure it’s a public account
(or screenshot it and email it [email protected])
Clean Up
All materials need to be put in one
cupboard under the lab station
Lab station needs to be cleared off
Clean Up Stamp needs to be
received before you leave: worth 5
pts
After the Experiment
AFTER the lab is done, you will have
LOTS of Calculations. Here are the
formulas and constants
= c / λ E = h = frequency c = speed of light (3.0 x 108 m/s)
λ = wavelength (in m)
h = Plank’s constant (6.626 x 10-34 J·s)
E = energy (in J)
Wavelengths
NOTE:
Make sure to change the wavelength to
meters
550 nm = 550 x 10-9 m
What would the other wavelengths be in m?
Your Calculator
To do this math, you need to
locate the scientific notation
button (2nd x-1)
It is either EE or EXP or 10x
Lets type in 550 x 10-9
Type 550
Press 2ND then EE/EXP the X-1 button
Type -9
Calculations Sample Wavelengths, l Frequencies, Energies, E
Example
A
= c = 3.0 x 108 m/s
550x10-9 m
l λ
Calculations Sample Wavelengths, l Frequencies, Energies, E
Example
A
= 3.0 x 108 m/s =
550x10-9m
5.45x1014 1/s
550x10-9 m
Calculations
These two numbers will help
calculate the Energy of the photon
E= h
Sample Wavelengths, l Frequencies, Energies, E
Example
A 550 x 10-9m 5.45 x 1014 1/s
Calculations
= hν =
( 5.45 x 1014 1/s)
(6.626 x 10-34J·s)
3.61 x 10-19 J
Sample Wavelengths, l Frequencies, Energies, E
Example
A 550 x 10-9m 5.45 x 1014 1/s
How to draw the Electron Jumps
A part of your Post-Lab includes drawing a
Bohr atom showing possible the electron
jumps for the observed spectral lines.
REMEMBER:
R O Y G. B I V
Low Energy High Energy
Low energy produces Small electron jumps and
releases waves with Low frequencies, and Vice
Versa
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