1. Light emission by Atoms
Chemistry of Art
Light emission by Atoms

3. colours & fires Stage 6 Chemistry Syllabus – Chemistry of Art (Option)
Identify Na+, K+, Ca2+, Ba2+, Sr2+, and Cu2+ by their flame colour
Perform first-hand investigations to observe the flame colour of Na+, K+, Ca2+, Ba2+, Sr2+, and Cu2+ (Demo only this lesson)
Explain the flame colour in terms of electrons releasing energy as they move to a lower energy level
Explain why excited atoms only emit certain frequencies of radiation
Explain what is meant by n, the principal quantum number
Identify that, as electrons return to lower energy levels, they emit quanta of energy which humans may detect as a specific colour

4. What’re those colours?
The colours of all glowing substances have the same starting point.
They come from atoms and molecules that have been excited to states of energy.
Atoms in burning fireworks and stars have become excited by absorbing energy as heat; then convert that energy into coloured light which is emitted.
The colours shown by an atom depend on how it’s electrons are configured.
Thus, by investigating the colours an atoms of an element emit, we can determine its atomic structure and work out which element it is.

5. Activity 1

6. Activity 2
Specific metal ions are used in fireworks to show different colours
Metal ions can be identified by the unique colours of their flames.

7. Activity 2
Specific metal ions are used in fireworks to show different colours
Metal ions can be identified by the unique colours of their flames.

8. How are these colours emitted at an atomic level?
Meetal Kumar

9. Atomic Emission SPECTRA in the electromagnetic spectrum
Electromagnetic spectrum: range of all wavelengths of electromagnetic radiation
Atomic Emission Spectra: Set of wavelengths of the electromagnetic spectrum emitted by excited electrons of an atom

10. What happens when white light passes through a prism?
Instructions:
Turn on the ray box
Place the prism flat on the paper in front of the ray box so that the beam of light passes through it
Turn off the lights
Observe the beam of light as it enters and exits the prism
What do u see?

11. What happens when white light passes through a prism?
The light is separated and dispersed into the full visible spectrum

12. For example:
Sunlight passes through a raindrop the light is dispersed into a visible rainbow

13. QUESTION
What happens when we hold a prism in front of light emitted from these specific burning elements? Would we see the entire visible spectrum?
A: Yes, we would see the entire visible spectrum
B: No, we would see bands of light broken up
C: No, we would see the colours refracting back into its white light form
Answer:

14. For example, Na+ light is broken up into bands within the spectrum - Notice each element has a unique spectrum that is emitted, referred to as its ‘Fingerprint’ and allows us to determine which element is becoming excited

15. First lets look at the electron configuration of an atom
Quantum numbers = energies of electrons in atoms or ‘shells’
They are like the ‘address’ of the electron
No two electrons can occupy the same address
N is called Principal energy level
It is always a whole number

16. Question:
If these energy levels or ‘shells’ are not occupied by electrons, are the shells still present? Yes or no?
Answer:
YES! The energy levels are always present

17. How do flame tests work

18. What causes the electron to become excited?
1) Electron begins in Ground State (electron in n=1)
2) Energy eg. heat is absorbed by electron
3) Electron bounces to higher energy level  enters Excited State (eg N=2,3,4)
4) Electron releases Photon (light energy)  moves back down to lower level energy
N=1 – UV rays ( not visible)
N=2 – Visible
N=3+ - IR rays (not visible)

19. How do flame tests work

20. Using all this information allows us to observe colours emitted from fireworks or outer space for example and determine which elements are becoming excited and emitting that colour of light

21. Emission Spectra Pembe Hussain Objective:
To explain the quantum concept.
Objectives:
To describe the Bohr model of the atom.
To explain the relationship between energy levels in an atom and lines in an emission spectrum.

22. Mars
Pale yellow patches
Dark red patches

23. Chemical composition of Mars
Pale yellow/white patches = hydrogen, helium, sulfur and sodium.
Iron oxide and small traces of calcium
Canyons = shadows

24. Jupiter
Pale grey
Orange

25. Jupiter’s composition
Hydrogen, helium with ammonium
Phosurphous, sulfur and hydrocarbons

26. Naturally white with slight blue tinge
Sun when in space
Naturally white with slight blue tinge

27. Sun when in space
Helium and hydrogen

28. Colour of the sun when it is up during the day

29. No interfering wavelengths
Sun when in space
Helium and hydrogen
No interfering wavelengths

30. SO WHAT ARE WE TALKING ABOUT?

31. The only electromagnetic waves detectable by human eyes
Visible light
The only electromagnetic waves detectable by human eyes

32. Put meetals picture here

33. It is from one “bump” to another.
What is a wavelength?
It is from one “bump” to another.
The technical term for a “bump” is a crest 

34. Each colour has its own wavelength that sets it apart so we can see it

35. Within the visible light section, we have a break down of colours
so that means: Visible light has its own spectrum`

36. Riddle:
What does a fingerprint belonging to a human being, and the electron configuration of an element have in common???

37. So: each element has its own unique visible wavelength and colour
They are both unique to the individual and element
Different electron configurations
Different electrons being different energy levels (n)
different photons released
Put flow chart/diagram here
different wavelengths
So: each element has its own unique visible wavelength and colour

38. Does an element emits only one colour?
Question:
Does an element emits only one colour?
Yes and no.
We see only one colour but, as electrons travel between different energy levels, they release different photons and wavelengths. We just see the most dominant wavelength.
My dot point:
Explain why excited atoms only emit certain frequencies of radiation
Identify that as electrons return to lower energy levels, they emit quanta of energy which humans may detect as a specific colour

39. Potassium - K+ Flame colour is lilac YET:
the potassium wavelength is a mixture of nm and blue @475 nm.
From
4000 A o
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An atom actually emits all of the colours, but the only colour detected by the human eye is that wavelength most dominant in the emission spectrum

40. So…. It is the dominant wavelength
Potassium when heated emits a lilac flame because:
It is the dominant wavelength
4000 A o
5000
6000
7000

41. Each emission spectrum is unique to on particular element
shows the electron configuration of a specific atom
Each emission spectrum is unique to on particular element
4000 A o
5000
6000
7000
Why?
Because it is like a finger print

42. Applications:
Identify different chemicals in a solution/substance for art restoration and chemical analysis
Fireworks
Astronomers use telescopes with detection devices that are sensitive to wavelengths  Determine composition

43. Flame test colours
Sodium, Na
Calcium, Ca

45. Next lesson:
You will perform a first-hand investigation into observing the flame colours. You will be given unknown solutions and from this lesson, you will be expected to indentify them.

46. FIREWORKS
Fireworks

48. How do flame tests work