Biological Metals
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Transcript of Biological Metals
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BIOLOGICAL METALS: A BRIEF
INTRODUCTION INTO ATOMIC
SPECTROSCOPY 7
BSc Forensic Science ProgramForensic Toxicology
Ildi Fenyvesi
2013
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Beginning, Middle and End!
Metals and Us
The theoretical basics
Samples pretreatment and preservation Instrumentation
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ELEMENTS AND THE BODY
The mineral elements constitute a small amount of total bodytissues however they are essential to many vital processes.
The animal body requires 7 main mineral elements: calcium,magnesium, sodium, potassium, phosphorous, sulphur andchlorine.
60-80% of all inorganic material in the body. What is meant byinorganic??
An inorganic compound which contains a metal are thoseelements in the periodic table that when ionized, loseelectrons and form cations.
At least 7 other minerals are important in trace levels: Iron,
copper, iodine, manganese, cobalt, zinc and molybdenum. Other elements also play a role, but exact nature is still not
fully understood: fluorine, aluminium, boron, selenium,cadmium, chromium.
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ELEMENTS & BIOLOGICAL MOLECULES
Important roles in various biological activities
Metalloporphyrins: iron containing biological complex in the transport ofoxygen and the mediation in electron transfer chains. Heme groupassociated with a protein (hemoglobin, myoglobin, cytochromes, catalase,peroxidase).
Cobalt containing biological molecules: Vitamin B12 coenzymes(cobalamins).
Metalloenzymes and metal activated enzymes ~ M incorporated intoenzyme: carbonic anhydrase and carboxypeptidase (Zn) as well as ascorbicacid oxidase and various tyrosinases (Cu).
Iron (Fe) in hemoglobin.
Zinc in insulin.
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METAL IMBALANCES?
1. Metal toxicity occurs more often than one would expect. We are exposedto toxic metals on a day-to-day basis in our environment. Whether heavymetal poisoning comes from pollution, cooking utensils, exposures towaste contaminations, deodorants, pesticides, food sources etc., all havean effect on the human body.
2. Disease states: Rickets which is characterized by a faulty calcification ofbones due to low Vit D content in the body and deficiency of calcium andphosphorous in diet (deficiency of Ca = serum levels are low and P=low);Wilsons disease associated with large amounts of copper accumulationin the body (excessive urinary excretion and increased absorption ofcopper from the intestine and hence accumulation occurs).
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ARSENIC: PHARMACODYNAMICS
Elemental Arsenic (As ) isrelatively non toxic.
Arsenate (As +5) and Arsenite(As+3) are common forms ofarsenic with arsenite being
more toxic of the three. Arsine gas (most toxic) is AsH3
is a gas formed whenhydrogen is generated in thepresence of trivalent arsenic industrial organic synthesis
and in lead storage batterymanufacture
Arsenic compounds areprimarily absorbed with therespiratory and GI tracts.
Breathing (workplaceexposure) and percutaneous
exposure. >90% of orally consumed
arsenic is absorbed (organicarsenic compounds inseafoods are readily absorbedafter ingestion)
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ARSENIC: PHARMACODYNAMICS
Arsenic is absorbed bydiffusion, enters theportal system, circulatesto the liver and entersgeneral circulation.
The half life of inorganicarsenic = 10hrs andmethylated arsenic =30hrs
Arsenic binds tosulfhydryl groups andconcentrates in the hairand nails
Excreted to a minordegree in sweat and skin.
Nails and hair accumulatethe metal.
Trivalent arsenic isoxidized in vivo to thepentavalent species andthe reverse also applies.
Urine is the major
elimination pathway andaccounts for approx 60%absorbed
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ARSENIC: TOXICITY
Poisonings are lesscommon but still occurdue to the availability ofthe arsenic containing
herbicides and pesticides. Arsine poisonings may
occur in occupationalsettings and poisonings
may occur as a by-product of a chemicalreaction.
Acute symptoms: GIsymptoms including pain,vomiting, discomfort,diarrhea. Skeletal muscle
pain and severe thirst iscommon and in highconcentrations results inspasms, stupor andconvulsions.
Chronic symptoms:muscle weakness, garlicbreath and neuropathy.
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ARSENIC: APPLICATION
1. Daisy De Melker Case: poisonedher husbands with Strychnine and
her son with Arsenic.
http://www.africacrime-
mystery.co.za/books/fsac/chp6.htm
1. Arsenic cases are not that
common locally2. International cases:
3. http://www.localhistories.org/ars
enic.html
4. Not that popular anymore!
http://www.iol.co.za/sport/arsenic-victim-had-similar-symptoms-1.71748
http://www.africacrime-mystery.co.za/books/fsac/chp6.htmhttp://www.africacrime-mystery.co.za/books/fsac/chp6.htmhttp://www.localhistories.org/arsenic.htmlhttp://www.localhistories.org/arsenic.htmlhttp://www.localhistories.org/arsenic.htmlhttp://www.localhistories.org/arsenic.htmlhttp://www.africacrime-mystery.co.za/books/fsac/chp6.htmhttp://www.africacrime-mystery.co.za/books/fsac/chp6.htmhttp://www.africacrime-mystery.co.za/books/fsac/chp6.htmhttp://www.africacrime-mystery.co.za/books/fsac/chp6.htm -
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MERCURY
Exposure from environment, industrial
processes (dry cell batteries and lamps and
wiring and production of chlorine etc),
thermometers, pigments, lubricating oils andat one stage dental amalgams.
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MERCURY: PHARMACODYNAMICS
Mercury vapor inhaled and inorganic salts of mercuryis readily absorbed and transported to other organs inthe body.
80% of the inhaled dose is absorbed into the
circulation with only 2% absorbed percutaneously. The majority of the taken up erythrocytes and is
oxidized to the divalent mercuric ion. This thencombines with sulfhydryl residues in plasma proteins.
80% of mercury is deposited in the proximal tubules inthe kidneys and free mercury crosses the blood brainbarrier hence a large proportion of the metal isdeposited mainly in the kidney and the brain.
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MERCURY: PHARMACODYNAMICS
AND TOXICITY Routes of elimination include faeces (biliary excretion and intestinal
secretion) and urine (50%).
The half life is 3-5 days as well longer elimination of up to 45 days.(2 compartment model with a rapid and slow phase).
Orally (and inhalation) consumed Mercury poses more risks than
dermal exposure. Acute toxicity: inhalation of high vapor or dust. Flu-like symptoms
and symptoms of interstitial pneumonitis and bronchitis; GIsymptoms(burning mouth and throat, nausea, vomiting).
Chronic poisoning: neurological symptoms with tremors or the arms
and hands (lower concentrations) as well as lower limb involvement(high concentrations). Chronic effects lead to renal tubular injury,loss of memory and tremors.
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MERCURY APPLICATIONS
1. Occupational and environmentalexposure concerns.
2. Some forensic cases are still
reported.
3. Mercury is not routinely tested
for however in a forensic workup
it must be suspected and
requested specifically.
http://www.guardian.co.uk/commentisfree/2013/jan/10/mercury-poisoning-global-
menace-treaty
http://www.ncbi.nlm.nih.gov/pubmed/21646904
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LITHIUM
Lightest of metals andwas discovered in 1817 byJ. Arfuedson (Swedishchemist).
Small amounts found inmeteorites, soils, tobacco,grains, coffee and milk.
Therapeutically: since the19th century as an
anticonvulsant, a sedative(manic patients) and atreatment for gout.
1949 Cade discoveredthat Lithium carbonatewas useful in thetreatment of mania. Isused as ongoingtreatment for manicdepressive disorders.
Industry (LithiumHydride): source of
hydrogen, highperformance desiccantand a condensing agent inorganic synthesis.
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LITHIUM: PHARMACODYNAMICS
Rapid and completeabsorption of lithiumfrom the GI tract anddistribution to the
organs.
The concentration inCSF is 40-50% of plasmaconcentration.
Approximately 95% iseliminated in the urine(half life 20-24 hrs).
80% of lithium isreabsorbed in theproximal renal tubules.
Less than 1% iseliminated in the fecesand 4-5% in sweat.
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LITHIUM TOXICITY
Lithium hydride is intensively corrosive and
can produce skin burns.
Inhalation of dust causes strictures of the
larynx, bronchi and trachea.
Patients taking lithium may develop thyroid
enlargement. Acute exposure may produce
polyuria, sedation, polydipsia, confusion and
coma.
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LITHIUM APPLICATIONS
Lithium overdose cases since lithium isprescribed as medication.
http://www.ncbi.nlm.nih.gov/pubmed/20515402
http://www.bipolar-lives.com/lithium-toxicity-symptoms.html
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QUESTIONS:
1. What is it? Describe its abundance in nature andwhere it can be found?
2. How are we exposed to it? Give examples.
3. Describe its absorption, distribution,metabolism and elimination in the human body.
4. What is its toxicity? What are the medical effects
of over exposure?5. Explain a case or case study involving the metal
of interest.
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ANALYTICAL PROCESS
SAMPLE PREPARATION
SAMPLE PRESERVATION
INSTRUMENTS
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THE BASICS
Atomic Spectroscopy is the technique of analyzing the energy emitted byatoms.
All atoms have electrons existing in a most stable state = the ground state= also the lowest energy state.
Certain processes can change the energy of the state e.g. adding heat cancause the electrons of an atom to move to a higher energy state or theexcited state.
The transition from ground to excited state requires the absorption of aunique packet or quanta of energy.
When the excited electron returns to the ground state, it emits radiationof a specific wavelength.
Each element in the periodic table will absorb and emit light at a specificwavelength.
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THE BASICS cont
The energy or wavelength is UNIQUE to anelement and hence one wavelength = oneelement which gives a selective technique.
Volatilization of atoms in a flame will cause themto emit or absorb light of specific wavelengths.
Basic premise: is that with increasingconcentration of metal ions you will increase the
amount of energy produced. This energy iselectronically transferred into a digital signalwhich is measured.
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SAMPLE PREPARATION
Need some form of pretreatment to bring the sampleinto solution: slowest and most labour intensive.
Method: sample type; element, concentration,analytical technique.
Preliminary pretreatment: drying of compound in anoven to get rid of the water content; grinding forhomogeneity.
Dissolution: no interfering substances must beintroduced and usually dissolve into acids or water.
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SAMPLE PREPARATION
Cold vapour generation ~ Hg where mercury in sample isconverted to Hg2+ with HNO3 and H2SO4 and then reduced toelemental Hg with SnCl2 .
Ion Exchange ~ metal ion pre-concentrated on cationexchange resin and then desorbed using acid (removal of
metal ion from matrix).
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SAMPLE PREPARTION
Solvent Extraction ~ chelate used for the transfer ofmetal aqueous phase to organic phase eg.Ammonium pyrrolidine dithiocarbamate + methylisobutyl ketone.
Solids ~ electrothermal vaporization into the graphitefurnace oven.
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SAMPLE PRESERVATION
Issues: adsorption of trace metals ontoglassware.
Laboratory ware contamination of samples
e.g. airborne Pb and Cu from polythene. Keep acid concentrations of samples high.
Use plastic ware.
Store in fridge.
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HOW DO MEASURE THE AMOUNTS OF
ELEMENTS?
ATOMICABSORPTION-FLAME
ATOMICABSORPTION FLAMELESS(FURNACE)
INDUCTIVELY COUPLEDPLASMA (ICP)-ATOMICEMISSIONSPECTROSCOPY
ICP-MASSSPECTROMETRY
(MS)
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FLAME ATOMIC ABSORPTION
SPECTROMETRY (FAAS)
SOURCE: hollow cathode lamp
PRE-MIX BURNER SYSTEM ~NEBULISERLISER
ATOMISER: convert all chemical
forms of element in the samplesolution into free atoms in agaseous state. All analyte atomsshould be converted to freeatoms.
Absorption depends on density of
atoms and absorption pathlength.
2 types of flame in which atomsare generated: Air/Acetylene(2400C) or a NitrousOxide/Acetylene (2600C)generated in a single slot burnerhead.
AA spectrometers usemonochromators anddetectors for UV and visiblelight. The main purpose of themonochromator is to isolate
the absorption line frombackground light due tointerferences .
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FAAS
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FLAME PROPERTIES
Critical aspect because theflame must be sufficient tobreak down compounds ofthese elements and provideefficient atomisation ofanalyte element.
Ability to tolerate wide varietyof solvents.
Low level of backgroundemission and absorption.
Low noise and suitable
reproducibility. Convenient and safe.
Inexpensive operation.
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FLAME OBJECTIVE
FACTORS AFFECTING ATOMISATIONEFFICIENCY ~
Temperature: greater temp,greater dissociation.
Chemical environment in flame(oxidising or reducing).
Aspiration rate:spl uptake.
Ionisation: high temp causesthermal ionisation (red # neutralatoms=red sensitivity)
Physical effects: viscosity, surfacetension.
INTERCONAL ZONE: hottest,
lowest noise = analytical zone.
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INTERFERENCES: what can interfere in the
analysis
MATRIX
CHEMICAL
MATRIX PHYSICAL SPECTRAL
Element forms thermally
stable compound with
molecular or ionic
species in solution e.g.phosphate
Transport of sample
solution to flame
Due to atomic or
molecular fine structure in
the spectrum
Species combine with
analyte to give more
volatile compounds e.g.
EDTA with Ca
Viscosity, surface tension
of solution
Spectral line overlap e.g.
553.55nm calcium
hydroxide + barium
Occlude analyte into
volatile matrix particles
Aspiration, nebulisation
or atomisation efficiency
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STRENGTHS v WEAKNESSES
STRENGTHS ~ Easy to use
Fast
Low cost
Few interferences overcomeby matrix matching
Most elements areatomised
Automated
Good precision reasonablesensitivity
WEAKNESSES ~ Require large volume of
solutions
Require solution form
Chemical interferences Low atom concentrations
due to dilution effects
Safety precautions(explosive gases)
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GRAPHITE FURNACE ATOMIC ABSORPTION
SPECTROMETRY (GFAAS)
Proposed by Lvov
Commercial since 1969
Flameless; replaced by small electrically
heated graphite tube/cuvette which is heatedto 3000C to generate a cloud of atoms.
The higher atom density and longer residence
time in the tube improve detection limits.
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FLAMELESS
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FURNACE PROGRAM
DRY: remove sample solvent, isothermal/rampheating; do not want spluttering.
ASHING: remove sample matrix to leave analyte in aform to atomize efficiently and reproducible; remove
organic matter; analyte must be thermally stable toallow for high ash temp (matrix modifier).
ATOMISATION: atomize sample as fast as possible toproduce sharp reproducible profiles.
CLEAN: removal of residual analyte.
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FURNACE PROGRAM
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INTERFERENCES: MATRIX & SPECTRAL
EFFECTS
CHEMICAL PHYSICAL SPECTRALPyrolsis loss (elemental
form in matrix is more
volatile than in standards)
Micro-droplet delivery Background absorption
from molecular species
present in the furnace
atmosphere e.g. NaCl.
Atomisation interference-
chemical speciation (Se
species differs in nature
vs. stds)
Viscosity, surface tension
of solution (soaking into
the furnace carbon
surface)
Background correction
(Zeeman)
Vapour phase
condensation reactions-
recombination of free
atoms in vapour phase to
molecular species
Wetting and spreading of
sample in the furnace
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INTERFERENCES: MATRIX EFFECTS
INTERVENTIONS
Matrix matching of standards.
Standard addition in calibration.
Isothermal atomization.
Matrix Modification (makes analyte less volatile OR makes
the matrix more volatile) ~ Palladium Nitrate modifier (volatileanalyte less volatile) and Magnesium Nitrate which acts asoxidant to remove organic matter.
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STRENGTHS v WEAKNESSES
STRENGTHS ~
Better detection limits
Small sample size
Few spectralinterferences
WEAKNESSES ~
Slower analysis time
Major chemical
interferences Element limitations
Limited dynamic range
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ICP-AES
Inductively coupled plasma atomic emission spectrometry.
Multi-element technique that uses an inductively coupledplasma source (argon).
Plasma reaches temperature of 10000C (break molecular
bonds high atomization). Plasma configuration can be radial or axial.
The sample dissociates into the constituent atoms, excitingthem to a level where they emit light of a characteristicwavelength.
A detector measures the light emitted specific for atom andintensity indicates concentration.
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ICP-AES
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SPECTRAL INTERFERENCES
Common
Line rich spectra produced by hot plasma
source (high resolution spectrometers or use
alternate line).
Background effects.
Physical: nebulizer (viscosity and surface
tension effects) and spray chamber.
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STRENGTHS v WEAKNESSES
STRENGTHS ~
Easy to use
Multi-elements in 1 sample in 1min and no compromise onprecision or detection limit
Few chemical interferences Excellent screening abilities, high
productivity
Solid and organic samples
WEAKNESSES ~ Moderate to low detection
Spectral interferences
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ICP-MS
Inductively coupled plasma mass spectrometry.
Multi-element technique
Uses a plasma source to dissociate the sample into itsconstituent positively charged ions.
The ions themselves are detected whereby they are passedthrough a mass spectrometer and are separated by their massto charge ratio.
Utilize mostly quadrupole mass spectrometers.
Isotope detection of elements is possible e.g. Cu (63 and 65).
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ICP-MS SETUP
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Interferences
SPECTRAL: species have same or similar mass as the
analyte (isobaric interferences) e.g. Cr (52) vs.
ArC(40+12) or ClOH(35+16).
Overcome by using collision cell technology to breakmolecules.
CHEMICAL: presence of argon gas and also solvents
used.
PHYSICAL: viscosity and surface tension.
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STRENGTHS v WEAKNESSES
STRENGTHS ~
Excellent detectionlimit.
Multi-element High productivity
Wide dynamic range
Isotopic measurements
WEAKNESSES ~
High cost
Some spectral
interferences Method development
skill
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SUMMARY OF ELEMENTAL ANALYSIS
TECHNIQUES
FAAS GFAAS ICP ICPMS
DETECTION LIMIT SUB PPM SUB-PPB 1-10PPB 1-10PPT
SAMPLE
THROUGHPUT10-15s per
element
3-4min per
element
1-60
elements permin
All elements
per min
DYNAMIC RANGE 103 102 106 108
PRECISION(SHORT
AND LONG TERM)0.1-10% 0.5-10% 0.1-5% 0.5-4%
INTERFERENCES Manychemical
Manychemical
Manyspectral
Few spectral,some matrix
SAMPLE VOLUMES
REQUIREDLarge Small Medium small
CAPITAL AND
RUNNING COSTSLow Medium-
high
High High
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CALIBRATION
Signal caused by the detection of the element in a sample iscompared with a set of calibration samples of known content.
External calibration is utilized with suitable matrix matchingprecautions taken and the range of concern taken intoaccount.
Quality Assurance: procedures covering the sampling andstorage; contamination possibilities and treatment of samplesduring analytical phase.
Sources of Error: unsuitable methodology, contamination,interferences, calibration errors, losses and degradation,
incompetence and lack of care.