Chemical Oceanography - 19 Introduction to isotopic tracers Gitai Yahel The School of Marine...
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Chemical Oceanography - 19 Introduction to isotopic tracers Gitai Yahel The School of Marine Sciences Ruppin Academic Center Gitai Yahel ([email protected]),
Chemical Oceanography - 19 Introduction to isotopic tracers
Gitai Yahel The School of Marine Sciences Ruppin Academic Center
Gitai Yahel ([email protected]), Tel.(052)291 8007, Skype
gitaiyahel, Web http://Moodle.Ruppin.ac.il Partly after Schmidt,
Heip, Hungate,Johnson, & Middelburg
Slide 2
Isotopic tracers are a widely used in oceanography Radioactive
vs. stable isotopes Stable isotopes are used to: Trace the sources
and sinks of material in the environment Determine the extent and
type of biogeochmical processes which have acted on materials
Provide information on paleooceanographic conditions Experimentally
trace specific elements using stable isotope tracers (e.g., 15 N).
Radioactive active isotopes are used for most of the above + dating
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(2)
Slide 3
Isotopes Isotopes are atoms that contain the same number of
protons but differ in the number of neutrons. Wednesday, 9 January
2013 Chemical Oceanography, [email protected] (3) 6 protons 6
neutrons 6 protons 7 neutrons protons electrons neutrons
Carbon-12Carbon-13
Slide 4
Radioactive Isotopes Some isotopes are stable, while others are
unstable, or radioactive. (6P + 6N) (6P + 7N) (6P + 8N) Stable
isotopes Radioactive isotope Carbon-12Carbon-13Carbon-14 R. Doucett
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(4)
Slide 5
Radioisotopes Radioisotopes provide the clocks that are used to
measure rates of ocean processes oPresent in a variety of elements
with different chemistry oHave a variety of half lives, and a
variety of sources oCan be measured at very low concentration and
extremely accurately oRadioisotope tracers are both natural ( 10
Be, 14 C, 238 U, 230 Th) and anthropogenic ( 14 C, 90 Sr, 240 Pu
steady state tracers transient tracers Usage in chemical
oceanography oAge of water and sediment oRates of scavenging and
production oRates of gas exchange * Very important as tracers in
biological oceanography (primary production, nitrogen sources, etc)
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(5)
Slide 6
Nuclear Radiation Radioactivity 1896: Antoine Henri Becquerel
found that uranium salts would fog photographic film plates Marie
and Pierre Curie showed the uranium caused the fog on the plates.
Marie named this radioactivity. The penetrating rays/particles were
called radiation. Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (6)
Slide 7
Nuclear Radiation First scientist to win 2 Nobel Prizes Only
scientist to win Nobel Prizes in 2 sciences *Physics (1903) "in
recognition of the extraordinary services they have rendered by
their joint researches on the radiation phenomena discovered by
Professor Henri Becquerel *Chemistry (1911) "for her discovery of
radium and polonium Died in 1934 from leukemia due high exposure to
radioactive elements Marie Curie Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (7)
Slide 8
Nuclear Reactions Nuclei of unstable isotopes gain stability by
undergoing changes. These changes release a lot of energy! Not
affected by temperature, pressure, or catalysts. Not affected by
the compounds that they are present in. Cannot alter the rate of
chemical reactions* * Not entirely true We will return to this
issue later Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (8)
Slide 9
Nuclear Reactions Disproves Daltons theory that atoms are
indivisible. Radioisotopes: Unstable isotopes Too many or too few
neutrons relative to the number of protons in a nucleus make a
nucleus unstable. Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (9)
Slide 10
Nuclear Radiation - Nuclear Decay Three types of Radiation:
1)Alpha: a He nucleus (2 protons and 2 neutrons) Atomic number
reduced by 2 and atomic mass reduced by 4 Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (10)
Slide 11
2) Beta: an electron (a neutron is transformed into a proton)
Nuclear Radiation - Nuclear Decay Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (11)
Slide 12
3) Gamma: high energy photon (no mass and no charge) *Often
emitted with alpha or beta particles *Extremely penetrating and
very dangerous! Nuclear Radiation - Nuclear Decay Wednesday, 9
January 2013 Chemical Oceanography, [email protected] (12)
Slide 13
Nuclear Stability and Decay About 17% of known nuclei are
stable and do not change Stability: depends on proton-to-neutron
ratio Higher atomic numbers demand more neutrons per proton for
stability 12 C 1:1 206 Pb 1.5:1 Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (13)
Slide 14
Nuclear Transformations Nuclear Stability and Decay
Neutron-to-proton ratio determines the type of decay that occurs!
*Beta emission: nuclei with too many neutrons per proton *The
result is a decrease in the # of neutrons and an increase in the #
of protons Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (14)
Slide 15
Nuclear Transformations Nuclear Stability and Decay
Neutron-to-proton ratio determines the type of decay that occurs!
*Positron emission: nuclei with too few neutrons per proton
Positron: particle with the mass of an electron, but a positive
charge *The result is an increased # of neutrons and a decrease in
the # of protons Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (15)
Slide 16
Nuclear Transformations Nuclear Stability and Decay All
elements with atomic numbers greater than 83 are radioactive!
*Alpha emission: nuclei with too many neutrons and protons *The
result is a more stable (increased) neutron-to-proton ratio
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(16)
Slide 17
Half-Life The time required for one-half of the nuclei of a
radioisotope to decay 1005025 13 Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (17)
Slide 18
Half-Life Half lives can be fractions of seconds or billions of
years Calcium-37: 175 ms Radon-222: 3.8 days Carbon-14: 5.73 x 10 3
years Uranium-238: 4.46 x 10 9 years Thus Radioisotopes can be
useful as clocks Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (18)
Slide 19
The uranium series Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (19)
Slide 20
Carbon-14 ( 14 C) dating half-life = 5730 years Exponential
decay Spallation- cosmic rays constantly produce 14 C in the
atmosphere 14 C is consumed by plants Nearly constant amounts
throughout history Compares 14 C levels in sample to the current
atmospheric levels where 14 C is the quantity and is the decay
constant: The solution to this equation is: Where, for a given
sample of carbonaceous matter: o 14 C 0 = number of radiocarbon
atoms at t = 0, i.e. the origin of the disintegration time o 14 C =
number of radiocarbon atoms remaining after radioactive decay
during the time t o = radiocarbon decay or disintegration constant
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(20)
Slide 21
Radiocarbon dating Raw (not calibrated) radiocarbon age: t 1/2
= 5568 years Methods: oNumber of disintegration per time
Scintillation counting Gas proportional counting oDirect counting
Accelerated Mass Spectroscopy (AMS) Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (21) F Years 1/2 Drops to
0.5 in 5730 years ( 1/2 ) Drops to 0.25 in 2* 1/2 years
Slide 22
Nuclear Transformations Transmutation Reactions Transmutation:
conversion of an atom of one element into another Two instances of
transmutation: 1) Radioactive Decay 2) Particles bombard the
nucleus of an atom Ernest Rutherford (1919): first artificial
transmutation Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (22)
Slide 23
Nuclear Transformations Transmutation Reactions Trans uranium
Elements: Atomic numbers above 92 *All are artificial and
radioactive *Produced in nuclear reactors and accelerators *Np and
Pu first synthesized in 1940 *More than 20 elements synthesized
since Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (23)
Slide 24
Nuclear Transformations Nuclear Fission Splitting of the
nucleus into smaller fragments U-235 and Pu-239 are the only
fissionable isotopes 1 kg of U-235 releases the energy of 20,000
tons of dynamite Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (24)
Slide 25
Nuclear Transformations Nuclear Fission Chain Reaction:
neutrons produced react with other fissionable atoms Bombs are
uncontrolled chain reactions Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (25)
Slide 26
Nuclear Transformations Nuclear Fission Reactors use controlled
fission to produce energy Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (26)
Slide 27
Chemical Oceanography, [email protected] (27) Stable isotopes
Most elements in the periodic table have more than one stable
isotope. 12 C 13 C 2H2H 1H1H 36 S 32 S 33 S 34 S 14 N 15 N R.
Doucett Wednesday, 9 January 2013
Slide 28
Chemical Oceanography, [email protected] (28) One isotope is
always more common than the others The mass ratio difference is
more pronounced for lighter elements ElementIsotopesAbundance Mass
ratio Hydrogen 1 H, 2 H 1 H = 99.985% 2 H = 0.015% 2 Carbon 12 C,
13 C 12 C = 98.89% 13 C = 1.11% 1.083 Nitrogen 14 N, 15 N 14 N =
99.633% 15 N = 0.366% 1.071 Oxygen 16 O, 17 O, 18 O 16 O = 99.759%
17 O = 0.037% 18 O = 0.204% 1.125 1.058 Sulfur 32 S, 33 S, 34 S, 36
S 32 S = 95.00% 33 S = 0.76% 34 S = 4.22% 36 S = 0.014% 1.125 1.062
1.031 R. Doucett Commonly used stable isotopes Wednesday, 9 January
2013
Slide 29
Chemical Oceanography, [email protected] (29) Measurement
Stable isotope ratios (e.g., 13 C/ 12 C) are measured using a mass
spectrometer. Three masses of CO 2 (44/45/46) are measured to
determine the amount of 13 C and 12 C in a sample. 12 C+ 16 O+ 16 O
= 44 13 C+ 16 O+ 16 O = 45 12 C+ 18 O+ 16 O = 46 R. Doucett
Wednesday, 9 January 2013 o Convert element of interest into a
stable gas. o Purify/separate gas analyte from contaminants
(off-line or on-line) o Measure isotopic ratios on an isotope ratio
mass spectrometer (IRMS )
Slide 30
13 C/ 12 C = 0.011225 13 C/ 12 C = 0.011071 13 C/ 12 C =
0.010918 Raw ratios are converted into delta ( ) permil values:
Chemical Oceanography, [email protected] (30) Mass spectrometers
can measure very small differences in isotope ratios. 13 C sample =
x 1000 13 C/ 12 C sample - 13 C/ 12 C standard 13 C/ 12 C standard
R. Doucett Wednesday, 9 January 2013
Slide 31
Standards Vary Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (31)
Slide 32
Manipulating units o The units are not the same as molarity or
Atom % notation, but are ratios. o The units must be used only for
comparison. o Many mathematical calculations should be made by
converting units to atom %. o The units must be on exactly the same
scale to be comparable (e.g., V-SMOW for 18 O). Wednesday, 9
January 2013 Chemical Oceanography, [email protected] (32)
Slide 33
Natural ranges of isotope ratio values -8 Wednesday, 9 January
2013 Chemical Oceanography, [email protected] (33)
Slide 34
Isotopic Fractionation Two types of isotopic fractionation that
cause changes in isotopic ratios: Kinetic isotope fractionation:
oOne isotope reacts, diffuses, or evaporates faster than the other
oCan be due to chemical, physical, or biological processes
oUsually, the lighter isotope reacts or diffuses faster oMagnitude
of the isotopic fractionation effect is temperature, reaction rate,
and species dependent oe.g., 13 C in photosynthesis Equilibrium
isotope fractionation: oExchange reactions in which a single atom
is exchanged between 2 species (with isotopic preference)
oBidirectional (reversible) chemical reactions oTemperature
dependent oE.g., 18 O in water and air Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (34)
Slide 35
Stable C isotope 13 C Stable isotope ( 13 C) Fractionation:
Kinetic effects: 13 C reacts more slowly than 12 C 13 CO 2 diffuses
more slowly than 12 CO 2 Equilibrium effects: 12 CO 2 + 13 CO 3 2-
+H 2 O = 13 CO 2 + 12 CO 3 2- +H 2 O 13 C will partition into the
species where overall energy is lowest Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (35)
Slide 36
Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (36) Availability of substrate affects
fractionation Beggars cant be choosers If substrate is non-limiting
(and constantly renewed) maximum fractionation will take place. If
substrate is limiting (and virtually all is used, with slow
replacement), fractionation will be low Examples CO 2 limitation of
phytoplankton affects 13 C Nitrate availability affects
phytoplankton 15 N
Slide 37
Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (37) NO 3 - concentration (M) 15 N of plankton
biomass (o/oo) 0 +5 +10 +15 5 10 High N availability significant
fractionation Low N availability Little fractionation N-fixing
organisms Seawater NO 3 - 15 N value 15 N values of plankton depend
on the source of N (e.g NO 3 - vs. N 2 ) and availability of the
nutrient.
Slide 38
Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (38) Isotopes in food web studies You are what
you eat! Consumer isotopic composition reflects the isotope
composition of the food source. Little fractionation along trophic
levels for Carbon or Sulfur Some trophic enrichment of 15 N with
higher trophic levels (+3 to +4 o/oo per trophic level) due to
preferential excretion of light isotope.
Slide 39
Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (39) Typical values for del 13 C Sea water DIC
+2 o/oo Atmospheric CO 2 -7 o/oo Marine POC-20 to -22 o/oo
Terrestrial plants -27 o/oo Marsh grasses (C4)-14 o/oo Benthic
algae -17 o/oo Values for biogenic materials are approximate, and
subject to variation depending on factors such as temperature and
availability of substrates (e.g. CO 2 ) New data are emerging all
the time!
Slide 40
Unlike stable isotopes, radiocarbon is constantly created and
destroyed Total number of 14 C atoms (N) Production in the
stratosphere Loss by radioactive decay - N Total amount of
radiocarbon on Earth can (and does) vary Wednesday, 9 January 2013
Chemical Oceanography, [email protected] (40)
Slide 41
http://www.iup.uni-heidelberg.de/institut/forschung/groups/kk/14co2.html
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(41)
Slide 42
Application: calculating the ocean ventilation time Radiocarbon
concentrations in per mille deviation from a reference value
approximately equal to atmospheric radiocarbon before the
industrial revolution. The upper ocean waters are contaminated with
bomb radiocarbon. Data are from the Western Atlantic and Pacific
GEOSECS sections. Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (42)
Slide 43
Application: calculating the ocean ventilation time Wednesday,
9 January 2013 Chemical Oceanography, [email protected] (43)
Figure 2.5.6 Radiocarbon concentrations along the core of the deep
waters in the three ocean basins and Antarctic (Stuiver et al.
[1983]).
Slide 44
Temperature proxy Preserved air- bubbles Annual layers Rapid
changes can be studied Specific events can be investigated and
links to other climate systems established ice cores
Slide 45
Example: Core S100 from coastal Antarctica. Sseasonal peaks in
the 18 O, DEP and ECM records between 70-80 m depth used for
establishing an annual chronology. Dating - annual if accumulation
is high Kaczmarska, M., Isaksson, E., Karlf, K., Winther, J-G,
Kohler, J., Godtliebsen, F., Ringstad Olsen, L., Hofstede, C M.,
van den Broeke, M.R., Van De Wal, R. S.W., and Gundestrup, N. 2004.
Accumulation variability derived from an ice core from coastal
Dronning Maud Land, Antarctica. Annals of Glaciology, 39,
339-345.
Slide 46
Application: Using 18 O from ice cores to reconstruct past air
temperature Evaporation: lighter 16 O evaporates more easily from a
water body resulting atmospheric H 2 O vapor is poorer in 18 O than
oceanic water Condensation: heavier 18 O are precipitated faster
than lighter 16 O Precipitation will be depleted in 18 O relative
to the standard (ocean water) Negative 18 O Coldest snow is
lightest (less heavy 18 O isotopes, more lighter 16 O isotopes)
Wednesday, 9 January 2013 Chemical Oceanography, [email protected]
(46)
Slide 47
Temperature affects on air 18 O/ 16 O ratio: colder
temperatures more negative values for the 18 O warmer temperatures
18 O values that are less negative (closer to the standard ratio of
ocean water) Wednesday, 9 January 2013 Chemical Oceanography,
[email protected] (47)
Slide 48
Application: reconstructing past air temperature General rule
of thumb: the heavy isotope will be concentrated in the phase in
which it is most strongly bound (or lowest energy state).
Solid>liquid>water, covalent>ionic, etc. Ex: 18 O in
carbonates - heavily enriched in carbonate because O tightly bonded
to small, highly charged C 4+, vs. weaker H + - so 18 O cal-water =
18 Ocarb- 18 Owater = 30 Wednesday, 9 January 2013 Chemical
Oceanography, [email protected] (48)
Slide 49
Using specific events for dating ice cores Using specific
events for dating ice cores Examples from Svalbard ice cores
Kekonen and others, 2002Pinglot and others, 2003 Nuclear weapon
tests Laki 1783 Volcanic eruptions
Slide 50
Depthage relationship Ice cores have layer thinning due to pure
shear which means that if sample size is consistant the number per
time unit will decrease with depth
Slide 51
Ice cores as climatic indicators Trapped air bubbles in the ice
can provide us with information on the atmospheric greenhouse
content 18 O as an air temp. proxy