• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Flame test

Extracts from this document...


THE FLAME TEST The flame test is a procedure used in chemistry to detect the presence of certain metal ions based on each element's characteristic emission spectrum. The test involves introducing a sample of the element or compound to a hot, non-luminous bunsen flame, and observing the colour that results. Samples are usually held on a platinum wire cleaned repeatedly with hydrochloric acid to remove traces of previous analytes.1 Assessment: This work can be assessed for Data Collection and Conclusion & Evaluation Data Collection: The appearance of compounds, which will be introduced in the flame test: Compound Appearance sodium chloride (NaCl) white, very small crystals potassium chloride (KCl) white, crystalline solid boric acid (H3BO3) white, crystalline solid calcium chloride (CaCl2) ...read more.


violet unknown orange Data processing and presentation: * Determining the identity of the unknown salt As I was asked to state the unknown salt on the basis of flame test I checked the colour of the flame. Results: Physical appearance white, crystalline solid Flame colour orange On the basis of results provided I can state that my unknown salt was sodium chloride (NaCl) because it produced orange flame and it was white with small crystals. * What particles found in the chemicals are responsible for the production of coloured light? Since all the salts used in the experiment contained the chlorine anion and produced different colours of light, I can state that only metal cations presented in salts are responsible for change of light colour. ...read more.


* Why the chemicals have to be heated in the flame first before the coloured light is emitted? Chemicals have to be heated first to make the atoms jump onto higher energy levels where their emission spectrum is visible for our eyes. * Characteristic colour of flame. Color Element Red Lithium, Strontium Orange Calcium Yellow Sodium Yellowish-green Boron Green Barium, Copper ( CuSO4) Blue Copper (CuO), Halides Purple-violet Potassium White-silver Aluminum, Magnesium, Titanium The colours are different because of different emission spectra causing different colours to appear. * Colourful light emissions are applicable to everyday life. Where else you observed colourful light emissions. Are these light emission applications related? Colourful light emissions can be observed in everyday life in the case of fireworks. As they contain different metal cations, when heated different emission spectra resulting in different colours. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Classifying Materials section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Classifying Materials essays

  1. Marked by a teacher

    Identifying an Ionic Compound. Objectives: To learn and test for metal ions ...

    5 star(s)

    a green and blue flame. For part 2 of the experiment, I had hypothesized that if I was given test tube number nine with an unknown compound, then the compound will be formed by Na+ and SO42- (Sodium Sulfate). I hypothesized this because I knew that sulfur had a yellow colour (thinking this was the color of sulfate)

  2. Ions - a qualitative analysis on our chemicals by flame testing.

    with in your body just by inhaling the vapour through the air. One way of preventing this is by closing lids on all chemicals after use by closing the lid you are also preventing spillages so if the container is dropped the chemical remains inside the container.

  1. Rate of reaction of hydrochloric acid on magnesium.

    The experiment was held at room temperature so there was not an exact fixed temperature that had surrounded the solution. The room temperature must have varied time-to-time this may have been caused by body heat lost to the surroundings by students in the class.

  2. Identification of an unknown compound.

    The peak at 2.1 is split into a doublet, which suggests it is adjacent to a carbon atom with 1 proton. Chemical shift Type of proton 2.1 -CH3 9.8 Taking all the information from the NMR spectrum, I suggest that the displayed formula of compound B is: Ethanal (aldehyde)

  1. Identifying unknown substances. The test that we did was a flame test, negative ion ...

    B C Obesavation It stayed orange It stayed orange The sample turned Orange to green Flame test: A B Obesavation It turned light purple It turned orange Why I did not test for sample C? I did not test for sample C because we had found out the sample was

  2. Rate of reaction of different concentrations of sodium thiosulphate.

    slow, this is why in higher concentrations of sodium thiosulphate the time for the cross to disappear was quicker. This is because if there is a lot of particles in a solution then there will be a greater probability of those particles overcoming the activation energy.

  1. Elements of life.

    The more delocalised electrons and the better it is at packing together due to the size of individual atoms, the stronger the bond. Transitional metals are unusual in that they can delocalise electrons from inner and outer shells. Atomic Structure Electrons are structured 2.8.8 they have a negative charge of -1 and weigh about 1/1837ths of a proton.

  2. Our experiment consisted of two samples of water containing unknown substances, and our objective ...

    now since it has been heated for a couple of minutes in blue flame. The evaporation process takes place when the liquid molecules gain enough kinetic energy to overcome intermolecular forces (forces between molecules). 7. When there is nothing on the scales, it should display '0.00g'.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work