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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

Using a spectroscope, you will observe

the spectra from the 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?

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

Ground level

Energy Level Diagrams

e- will jump

to a higher

level and

then fall

down

releasing a

photon of

light

Energy Level Diagrams