Chemistry of Art

Light emission by AtomsChemistry of Art

colours & firesStage 6 Chemistry Syllabus Chemistry of Art (Option)

Identify Na+, K+, Ca2+, Ba2+, Sr2+, and Cu2+ by their flame colourPerform 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 levelExplain why excited atoms only emit certain frequencies of radiationExplain what is meant by n, the principal quantum numberIdentify that, as electrons return to lower energy levels, they emit quanta of energy which humans may detect as a specific colourWhatre 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 its 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.

Activity 1Activity 2

Metal ions can be identified by the unique colours of their flames.

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

Specific metal ions are used in fireworks to show different coloursMeetal KumarHow are these colours emitted at an atomic level?Atomic Emission SPECTRA in the electromagnetic spectrum Electromagnetic spectrum: range of all wavelengths of electromagnetic radiationAtomic Emission Spectra: Set of wavelengths of the electromagnetic spectrum emitted by excited electrons of an atom

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?

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

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

QUESTIONWhat 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:B: No, we would see bands of light broken up

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

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

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

How do flame tests workWhat 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)

How do flame tests workUsing 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

Pembe HussainEmission SpectraObjective: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.

21Mars

Pale yellow patchesDark red patchesChemical composition of Mars

Pale yellow/white patches = hydrogen, helium, sulfur and sodium.Iron oxide and small traces of calciumCanyons = shadowsJupiter

Pale greyOrange Jupiters composition

Hydrogen, helium with ammonium Phosurphous, sulfur and hydrocarbonsSun when in space

Naturally white with slight blue tinge26Sun when in space

Helium and hydrogen 27

Colour of the sun when it is up during the day Sun when in space

Helium and hydrogen No interfering wavelengths29SO WHAT ARE WE TALKING ABOUT?

Visible lightThe only electromagnetic waves detectable by human eyes

Put meetals picture here

32What is a wavelength?It is from one bump to another.

The technical term for a bump is a crest

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

34Within the visible light section, we have a break down of colours

so that means: Visible light has its own spectrum`

Riddle:What does a fingerprint belonging to a human being, and the electron configuration of an element have in common???So: each element has its own unique visible wavelength and colourThey are both unique to the individual and element Different electron configurationsDifferent electrons being excited @ different energy levels (n) different photons releaseddifferent wavelengthsPut flow chart/diagram here37Question: 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

38Potassium - K+Flame colour is lilacYET: the potassium wavelength is a mixture of red @650 nm and blue @475 nm.

4000 Ao500060007000An atom actually emits all of the colours, but the only colour detected by the human eye is that wavelength most dominant in the emission spectrumFrom http://webmineral.com/help/FlameTest.shtml39So.Potassium when heated emits a lilac flame because:

4000 Ao500060007000It is the dominant wavelength Each emission spectrum is unique to on particular element

Why?

Because it is like a finger printEmission spectrum shows the electron configuration of a specific atom

4000 Ao500060007000Applications:Identify different chemicals in a solution/substance for art restoration and chemical analysisFireworksAstronomers use telescopes with detection devices that are sensitive to wavelengths Determine compositionFlame test colours

Sodium, NaCalcium, Ca

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.

FIREWORKS Fireworks

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How do flame tests work