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Lecture 6 Radioactive Isotopes

Lecture 6 Radioactive Isotopes. Decay Equations Half Lives Useful Radiotracers in Oceanography Secular Equilibrium. E & H Chpt 5. Radioisotopes and decay Definitions and Units Parent – Original Radioactive Atom Daughter – The Product of Decay Decay Chain – A Series of Decays.

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Lecture 6 Radioactive Isotopes

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  1. Lecture 6 Radioactive Isotopes Decay Equations Half Lives Useful Radiotracers in Oceanography Secular Equilibrium E & H Chpt 5

  2. Radioisotopes and decay Definitions and Units Parent – Original Radioactive Atom Daughter – The Product of Decay Decay Chain – A Series of Decays Types of Decay DP DN DAtomic Wt. Alpha a He2+ -2 -2 -4 Beta b e- + 1 -1 0 (n → P+ + e-) Gamma g “excess energy” Decay is independent of chemistry and T and P. Decay is only a property of the nucleus (see Chart of Nuclides)

  3. The chart of the nuclides - decay b decay X X a decay

  4. Mathematical Formulation of Decay Decay Activity (A) = decays per time (dpm or dps) A = l N l = decay constant (t-1) N = # of atoms or concentration (atoms l-1) Units: Becquerel (Bq) = 1 dps Curie = 3.7 x 1010 Bq = Activity of 1 gram of 226Ra

  5. Decay Equations Decay is proportional to the # of atoms present (first order) dN/dt = - N = AN where N = the number of atoms of the radioactive substance present at time t  = the first order decay constant (time-1) The number of parent atoms at any time t can be calculated as follows. The decay equation can be rearranged and integrated over a time interval. where No is the number of parent atoms present at time zero. Integration leads to or or

  6. Decay Curve Both N and A decrease exponentially

  7. Half Life The half life is defined as the time required for half of the atoms initially present to decay. After one half life: Thus =  t1/2 ln (2) =  t1/2 0.693 =  t1/2 so Math note: -ln(1/2) = - (ln 1 – ln 2) = - ( 0 – ln 2) = + ln2 = 0.693

  8. Mean Life = Average Life of an Atom t = 1 / l t = 1.44 t1/2 Q. Why is the mean life longer than the half life?

  9. Isotopes used in Oceanography steady state transient U-Th series are shown on the next page. These tracers have a range of chemistries and half lives. Very useful for applications in oceanography.

  10. 238U decay products in the ocean

  11. Parent-Daughter Relationships Radioactive Parent (A) Stable Daughter (B) A → B e.g. 14C → 15N (stable) Production of Daughter = Decay of Parent 2-box model l A A B Example: 14C → 15N (stable) t1/2 = 5730 years

  12. Radioactive Parent (A) Radioactive Daughter (B) 2-box model A → B → lA lB A lA B l B source sink mass balance for B solution: solution after assuming NB = 0 at t = 0

  13. Three Limiting Cases 1) t1/2(A) > t1/2(B) or lA < lB one important case 2) t1/2(A) = t1/2(B) or lA = lB e.g. 226Ra → 222Rn 3) t1/2(A) < t1/2(B) or lA > lB 1600yrs 3.8 days Case #1: long half life of parent = small decay constant of parent SECULAR EQUILIBRIUM Activity of daughter equals activity of parent! Are concentrations also equal???

  14. Secular equilibrium t1/2 daughter = 0.8 hr t1/2 parent =  Total Activity parent Activity of parent and daughter at secular equilibrium daughter Activity (log scale) ! Daughter grows in with half life of the daughter! t1/2 time (hr)

  15. Example: Grow in of 222Rn from 226Ra After 5 half lives activity of daughter = 95% of activity of parent

  16. Example: Rate of grow in Assume we have a really big wind storm over the ocean so that all the inert gas 222Rn is stripped out of the surface ocean by gas exchange. The activity of the parent of 222Rn, 226Ra, is not affected by the wind. Then the wind stops and 222Rn starts to increase (grows in) due to decay. How many half lives will it take for the activity of 222Rn to equal 50% (and then 95%) of the 226Ra present? Answer: Use the following equation:

  17. There is considerable exposure due to artificially produced sources! Possibly largest contributor is tobacco which contains radioactive 210Po which emits 5.3 MeV aparticles with an half life of T1/2=138.4days.

  18. Was Litvinenko (a former Russian spy) killed by 210Po?? A case study of 210Po Toxicity of Polonium 210 Weight-for-weight, polonium's toxicity is around 106 times greater than hydrogen cyanide (50 ng for Po-210 vs 50 mg for hydrogen cyanide). The main hazard is its intense radioactivity (as an alpha emitter), which makes it very difficult to handle safely - one gram of Po will self-heat to a temperature of around 500°C. It is also chemically toxic (with poisoning effects analogous with tellurium). Even in microgram amounts, handling 210Po is extremely dangerous, requiring specialized equipment and strict handling procedures. Alpha particles emitted by polonium will damage organic tissue easily if polonium is ingested, inhaled, or absorbed (though they do not penetrate the epidermis and hence are not hazardous if the polonium is outside the body).Acute effectsThe lethal dose (LD50) for acute radiation exposure is generally about 4.5 Sv. (Sv = Sievert which is a unit of dose equivalent). The committed effective dose equivalent 210Po is 0.51 µSv/Bq if ingested, and 2.5 µSv/Bq if inhaled. Since 210Po has an activity of 166 TBq per gram (1 gram produces 166×1012 decays per second), a fatal 4-Sv dose can be caused by ingesting 8.8 MBq (238 microcurie), about 50 nanograms (ng), or inhaling 1.8 MBq (48 microcurie), about 10 ng. One gram of 210Po could thus in theory poison 100 million people of which 50 million would die (LD50).

  19. Body burden limitThe maximum allowable body burden for ingested polonium is only 1,100 Bq (0.03 microcurie), which is equivalent to a particle weighing only 6.8 picograms. The maximum permissible concentration for airborne soluble polonium compounds is about 10 Bq/m3 (2.7 × 10-10 µCi/cm3). The biological half-life of polonium in humans is 30 to 50 days. The target organs for polonium in humans are the spleen and liver. As the spleen (150 g) and the liver (1.3 to 3 kg) are much smaller than the rest of the body, if the polonium is concentrated in these vital organs, it is a greater threat to life than the dose which would be suffered (on average) by the whole body if it were spread evenly throughout the body, in the same way as cesium or tritium.Notably, the murder of Alexander Litvinenko in 2006 was announced as due to 210Po poisoning. Generally, 210Po is most lethal when it is ingested. Litvinenko was probably the first person ever to die of the acute α-radiation effects of 210Po , although Irene Joliot-Curie was actually the first person ever to die from the radiation effects of polonium (due to a single intake) in the late 1950s. It is reasonable to assume that many people have died as a result of lung cancer caused by the alpha emission of polonium present in their lungs, either as a radon daughter or from tobacco smoke.

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