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Analytical Instruments. Area Study 1 Unit 3 2010. Key Terms. Spectroscopy – energy is used. Energy can be absorbed or emitted. When atoms or molecules absorb energy, can move to higher energy level. Radiation is emitted when returning to original energy level (falling to lower energy level). - PowerPoint PPT Presentation
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Area Study 1 Unit 3 2010
Spectroscopy – energy is used. Energy can be absorbed or emitted. When atoms or molecules absorb energy, can move to higher energy level. Radiation is emitted when returning to original energy level (falling to lower energy level).
Emission – this occurs when excited electrons return to their ground states and radiate energy of fixed wavelengths. Emission spectra have sets of coloured lines on a black background.
Absorption – molecules can absorb energy of certain wavelengths. In the visible and UV spectrum, electrons surrounding the atoms may gain energy. If no energy is absorbed, the substance appears white. If coloured, then it has absorbed light complementary to that being seen. Absorption spectra are the opposite of emission spectra, the wavelengths of light absorbed by the electrons appear as dark lines on a rainbow spectra.
Molecules can also absorb energy from the infrared region of the electromagnetic spectrum. This energy is insufficient to disrupt electrons but functional groups, C-H bonds, double and triple bonds can absorb energy, stretch, bend and can be measured.
In Nuclear Magnetic Radiation spectrometry, protons or 13C nuclei absorb energy from the radio frequency,
UV visible spectroscopy makes use of the UV visible region, IR spectroscopy the IR region and NMR the radio wave region.
UV = short wavelength, high energy
Radio = long wavelength, low energy
Each spectrometric techniques, the atom or molecules absorbs a specific amount of energy which causes a move to a higher energy level. For atoms, this is the movement of electrons where in molecules as well as electrons moving to higher energy levels we can also observe the movement of molecules in term of their spin, vibration or rotations.
Used to identify certain metal cations that after excitation emit light within the visible region of the electromagnetic spectrum.
Expected colours for common metal cations:
Metal cation Flame colour
Lithium Crimson
Sodium Golden Yellow
Potassium Lilac
Calcium Brick Red
Strontium Scarlet
Barium Yellow Green
Copper Green Blue
Inexpensive Very fast to perform but unreliable because colours
can be masked Used to identify metal ion in some salts Qualitative only Limited to few metals. Many common metals like Al
and Mg do not colour flame (only some of group 1 & 2) Other limitations: colours can be alike and therefore
hard to identify unknown, also samples can be impure and mask colours of component
Emission spectroscopy Can be observed by the naked eye More qualitative result: use a prism, hotter flame –
called atomic emission spectroscopy
Expensive, costs thousands of dollars. Lamps themselves are very expensive.
Fast, once standard solutions made up Quantitative, a hollow cathode lamp for the
metal being measured must be available Can be used for all metals and metalloids – can
identify & measure a much wider range of metals
Calibration curve constructed, absorbance vs. concentration – dilution is likely to be required
Visible spectrum
Australian invention, sample sprayed into flame
Very sensitive -ppm Used to detect amount of mercury in shellfish
(0.5ppm), lead in soil, trace metals in mineral water, forensic analysis of hair samples from heavy metal poisoning
Absorption spectroscopy – light absorbs indicates quantity of element in sample
p.83Example 7.3Lead in oystersppm = one millionth gram8.3 ppm- i.e. there are 8.3 g in 1.0 x 106 g of solution
2.5ppm = 2.5 µg per g of sample2.5mg per kg
2.5ppm =2.5 µg per mLOr 2.5 mg per L
Simple UV visible spectrophotometers are available from $1000 to $5000
Fast once a set of standard solutions set up Qualitative and Quantitative – mainly used
quantitatively to determine concentration of substance in a sample
Used for coloured solutions or organic molecules that absorb in the UV region – energy emitted is not in visible region therefore cannot be seen with the naked eye!
Absorption spectroscopy Wavelength of light selected for maximum
absorbance and a calibration curve constructed of absorbance plotted against concentration
Used to find concentration of food colourings, analysis of aspirin and paracetamol, concentration of some coloured pharmaceuticals in blood
Expensive, but simple are available at lower cost
Similar to UV spectrophotometer but operates in IR region – lower energy than UV light
Not enough energy to promote electrons to higher level, but causes changes in bond
Fast once sample is prepared Gases, liquids & solids can be used Absorption spectroscopy Qualitative, rarely quantitative Plot of transmittance against wave number
Transmittance: measures how much light has been transmitted. 100% transmittance means no energy has been absorbed. Absorbance is the intensity of light remaining after some has been absorbed.
Used to identify organic compounds, in particular functional groups, design of new drugs, protein analysis, checking quality of wine products, tea leaves that have a smell, forensic identification of oils, fibres, paint flakes
Expensive Hazardous because of the strong magnetic
field Operates in the radio region Very fast (milliseconds) Qualitative Absorption spectrum Spectra can be low resolution or high
resolution
Used for fossil fuel analysis, identification of organic molecules, protein & nucleic acid structures, forensic analysis (this type of analysis in non destructive of the sample)
MRI – medical diagnosis. Detects differences in water balance of tumour abnormalities.
Simple calorimeters are available for $100 Fast once standard solutions made up Qualitative and Quantitative Limited to coloured solutions or compounds Absorption spectroscopy Calibration curve constructed, absorbance
vs. concentration Used to find copper (II) sulfate in garden
sprays, any other coloured solution
Expensive, but portable models are cheaper Very sensitive – uses µg samples Qualitative and Quantitative Operates at low pressures Sample is vaporised and high energy
electrons knock off electrons of molecules & cause fragmentation. The different species are separated on passing though an electric field and a magnetic field.
Used to determine relative atomic mass on periodic table!!
Also used to identify organic molecules, qualitative and quantitative analysis of proteins, determine protein structure
We will study organic families first before talking reading these spectra. However it is important to remember that we have not had the opportunity to work with each instrument in the time given for Unit 3, so the exam may only test broad structural features. You should be able to identify the type of chemical to be identified by the instrument. You do not need to know all of the uses.
With chromatography, you will need to refer to the peak areas, retention times and perhaps which substance would emerge first. You may to construct a calibration curve of area against concentration, then use the graph to determine the concentration of an unknown sample.
With UV and AAS, you are often required to plot a calibration curve of absorbance against concentration. You would then be asked to determine the concentration of an unknown in the correct figures.
IR, NMR & MS – you are likely to be given a spectrum and asked to determine the molecule it represents. The necessary data will be in your data book. They should be a simple molecule like propanol or ethanoic acid. We are going to come back to interpreting spectra.
For MS you may also have to find the relative atomic mass if given the relative isotopic masses.
Wet methods: Slow but necessary. Used in remote areas or
labs that do not have expensive equipment. These methods rely on a chemical reaction.
Acid-base volumetric analysis Preparation of standard solutions to
determine concentration in consumer product
Redox volumetric analysis Gravimetric analysis: a) Analysis of water
content b) Analysis of content using precipitation, filtering and drying
Instrumental methods: Are fast and able to accurately determine
very small quantities in small samples They play a large role in identification of
compounds in forensics, IR NMR and MS are powerful tools in protein analysis and development of new medicines. Although some machines are very expensive, the labs can save labour costs with the speed of analysis and are therefore justifiable. With the exception of MS, they rely on absorbance.
AAS – used to determine metals UV & Colorimetry – used to determine
coloured metal complexes as well as coloured organic compounds.
Difference: IR & NMR – Identification of organic
compounds Difference: MS – Calculation of relative atomic mass
and identification of organic compounds USE p.120, Table 8.1 –Great for revision!!!