Showing posts with label radiochemistry. Show all posts
Showing posts with label radiochemistry. Show all posts

Wednesday, May 11, 2022

Australian Curriculum and Year 9 "Science"

 Last year I was writing questions for an Australian Years 9-10 Science textbook when I first came across the "gamma decay" problem.

The textbook authors stated that there are 3 types  of radioactive decay: alpha, beta and gamma (which is kind of OK for Year 9 or 10 science). They wanted to provide an isolated example of each type, that is, an example of alpha decay, an example of beta decay, and an example of gamma decay. Which is where the problem lies. Giving an example of alpha or beta decay is easy, just ignore any other possible radiations when you do it, which is the "traditional" method for teaching nuclear decay to Years 9 or 10, or indeed Year 11 chemistry (and yes, physics teachers are probably horrified, and rightly so, IMHO). But, you can't do this for gamma decay unless you want to talk about "excited states".

Which brings us to version 9 of the Australian Curriculum for Year 9 Science which states,

"describing in simple terms how different unstable isotopes decay such as radon-222 releasing an alpha particle, iodine-131 releasing a beta particle and cobalt-60 releasing gamma radiation to form stable atoms"

Alpha decay of radon-222 and beta decay of iodine-131 ... OK, can do.

Gamma decay of cobalt-60 ? Problem! Cobalt-60 decays by emitting a beta particle to produce an excited state nickel-60 atom. Excited state nickel-60 loses energy by emitting high energy gamma ray and relaxing back to a ground-state nickel-60 atom. But, we can't use this as an explanation because the introduction to excited states won't occur 'til, possibly, year 10 (when they do flame tests).

Has the Australian Curriculum been proof-read?

I think not. Further evidence of the writer's (or writers') slipshod approach to "science" is evidenced in this "interesting" extract (also for Year 9)

"investigating how radiocarbon and other dating methods have been used to establish that First Peoples of Australia have been present on the Australian continent for more than 60,000 years"

Problem 1: radiocarbon dating is pretty useless for anything older than about 40,000 years old, so it would be worse than useless for artifacts said to be 60,000 years old. 

Problem 2: where is the SCIENTIFIC evidence that Australia has been inhabited by humans for "more than 60,000 years"? Surely if you are going to make a statement like this, and force SCIENCE teachers to teach it, you need to support the statement, just a link a two, some references, to some SCIENTIFIC studies would be useful. 

So, here's what I think I know ... Mungo man/mungo woman are thought to be about 40,000 years old (give or take a few thousand). Blackened rocks at Moyjil are thought to be about 125,000 years old, but not linked to human habitation (that I'm aware of). The Pilbara petroglyphs have a wide range of dates depending on who provides them, but they also seem to be scientifically dated between 40,000 and 50,000 years. 

My problem is that I'm not an anthropologist, I know a little bit about chemistry (Chemical Sciences), a bit less about geology (sorry, Earth Sciences), even less about physics (AKA physical sciences), and practically nothing about biology (sometimes called a science), and hence I am NOT in a position to either a) know how long Australia has been inhabited for, or

b) to teach anything about this 

... and I suspect most SCIENCE teachers in Australia would fall into the same category.

AC: Australian Curriculum or Australian C_ _ p?



Saturday, November 25, 2017

Ruthenium-106 Cloud

In October 2017 the German Federal Office for Radiation Protection detected a radioactive cloud containing ruthenium-106 wafting over Europe. They identified the Southern Ural Mountains in Russia or Kazakhstan as the most likely source of the cloud. In November 2017 Roshydromet, the authority responsible for monitoring radiation in Russia, finally admitted that it had found extremely high levels of ruthenium-106 at two monitoring stations in this region in late September and early October.

Ruthenium is a transition metal element with the chemical symbol Ru and an atomic number of 44.
 Naturally occurring ruthenium has 7 stable isotopes: 96Ru, 98Ru, 99Ru, 100Ru, 101Ru, 102Ru, and, 104Ru. The abundance of each isotope in naturally occurring ruthenium is given in the table below:

isotopeabundance %
ruthenium-965.54
ruthenium-981.87
ruthenium-9912.76
ruthenium-10012.60
ruthenium-10117.06
ruthenium-10231.55
ruthenium-10418.62

In addition to these naturally occurring stable isotopes, about 30 unstable, or radioactive, isotopes have also been identified. The most stable of these radioisotopes is ruthenium-106 which has a half-life of  359 73.days. It decays by emitting a beta particle to produce rhodium-106:
106Ru→ 0e+ 106Rh
44-145

Ruthenium-106 is produced in a nuclear reactor as a product of the nuclear fission of uranium-235. Ruthenium-106 can be extracted from spent nuclear fuel and then it can be used in medicine to treat eye tumors.

The radioactive cloud wafting across Europe is most likely to be due to a spill of ruthenium-106 rather than a nuclear reactor accident since this would have released other radioisotopes which would have been detected in the cloud. France's nuclear safety agency has estimated the amount of radiation released at the source as between 100 and 300 billion becquerels.
A becquerel (Bq) is the SI unit for measuring radioactivity. It is equivalent to the radioactive decay of 1 nucleus in 1 second.
We can use this to estimate the mass of ruthenium-106 spilled:
ABq =       mass      
atomic weight
x NA x ln(2)
t½

ABq = activity in becquerels = 200 x 109 Bq (averaged)
mass = ? grams
atomic weight = 106 g/mol (from the Periodic Table)
NA = 6 x 1023 mol-1 (Avogadro's number)
t½ =  373.59 days = 373.59 days x 24 hours/day x 60 minutes/hour x 60 seconds/minute = 3.22 x 107 seconds
200 x 109 =       mass      
106
x 6 x 1023 x 0.6931
3.22 x 107
200 x 109 =       mass      
106
x 6 x 1023 x 2.15 x 10-8
200 x 109 =       mass      
106
x 1.29 x 1016
mass = 200 x 109 x 106
1.29 x 1016
mass = 1.64 x 10-3 g

If the source of this ruthenium-106 was an accident involving spent fuel rods, then we can calculate the mass of spent fuel involved since 1.9 kg of ruthenium-106 can be extracted from 1 ton (or 1000 kg) of used fuel.
1.9 kg = 1.9 kg x 1000 g/kg  =  1900 g
1900 g of ruthenium-106 can be extracted from 1000 kg (1 000 000 g) of spent nuclear fuel.
1 g of ruthenium-106 can be extracted from 1 000 000 g/1900 g =  526 g of spent fuel
1.64 x 10-3 g ruthenium-106 would be produced from 1.64 x 10-3 x 526  = 0.86 g of spent fuel

A typical nuclear power plant produces 20 tons (2 x 107 g) of  used nuclear fuel per year, about 0.6 grams per second!

Reference:
http://www.smh.com.au/world/with-a-radiation-cloud-comes-a-mystery-from-russia-20171123-gzrvtf.html 

Further Reading:
Isotopes 
Atomic Number (number of protons) 
Mass Number (number of nucleons) 
Calculating Relative Atomic Mass (atomic weight)
Nuclear Half-life 


Suggested Study Questions
  1.  What does the term "isotope" mean?
  2.  Give the atomic number of each of the following species:
    • ruthenium-96
    • ruthenium-98
    • ruthenium-100
    • ruthenium-102
    • ruthenium-104
    • ruthenium-106
  3. Give the mass number (or nuclear number) of each of the following species:
    • ruthenium-96
    • ruthenium-98
    • ruthenium-100
    • ruthenium-102
    • ruthenium-104
    • ruthenium-106
  4. Determine the number of protons in the nucleus of an atom of each of the following:
    • ruthenium-96
    • ruthenium-98
    • ruthenium-100
    • ruthenium-102
    • ruthenium-104
    • ruthenium-106
  5. Determine the number of neutrons in the nucleus of an atom of each of the following:
    • ruthenium-96
    • ruthenium-98
    • ruthenium-100
    • ruthenium-102
    • ruthenium-104
    • ruthenium-106
  6. Use the information in the article to calculate the relative atomic mass (atomic weight) of ruthenium.
  7. Explain what is meant by the term "unstable isotope".
  8. Explain what is meant by the term "beta decay".
  9. A number of unstable isotopes of ruthenium undergo beta decay. Write balanced nuclear decay equations for the beta decay of the following ruthenium isotopes:
    • ruthenium-103
    • ruthenium-105
    • ruthenium-106
    • ruthenium-107
    • ruthenium-108
    • ruthenium-109
  10. Explain what is meant by nuclear "half-life"?
  11. Ruthenium-106 has a half-life of of  359 73.days. Calculate the percentage of ruthenium-106 remaining after:
    • 359.73 days
    • 719.46 days
    • 1079.19 days
    • 3597.3 days
  12. If the mass of ruthenium-106 in the cloud over Europe is currently 1.64 x 10-3 g, calculate the mass of ruthenium-106 remaining in the cloud after:
    • 1 year
    • 2 years
    • 10 years

Thursday, September 10, 2015

Uranium Glass

Uranium compounds have been used to colour glass since ancient times. A mosaic found in a Roman villa dated to about 79 AD used yellow glass containing 1% uranium oxide. Between 1880 and the 1920s, uranium glass was quite popular, not only because of its interesting yellow-green colour, but because it fluoresces in ultra-violet light as shown in the image of a vase below.
The image on the left hand side shows the vase under normal daylight, while the image on the right shows the same vase in the dark exposed to UV light.

Why does uranium glass glow green in the dark like this?
Well, it has nothing to do with the radioactivity of uranium isotopes. The green glow does not occur because of changes within the nucleus of uranium atoms, it occurs because of changes in the energy of electrons surrounding the nucleus.
A ground state electron in a uranium atom absorbs the energy of a photon  of ultra-violet light causing the electron to jump to a higher energy level known as the excited state. This new excited state electron configuration is not stable, so, the electron falls back down to to the ground state energy level, which is a lower energy state, by losing energy which it does by emitting a photon of light. Some of the energy of the original photon used to excite an electron is dispersed as molecular vibration and heat, so the energy of the photon emitted when the excited electron falls back to the ground state is less than the energy originally absorbed.
That is: E = hν/λ
where E = energy, h = Planck's constant, ν = speed of light , λ = wavelength of light
If the speed of light is a constant, then E ∝ 1/λ or Eλ = a constant
in other words, the more energy the photon of light has the shorter its wavelength is.
In the case of uranium glass, the absorbed photon of ultra-violet light has a wavelength of about 300 nm, while the emitted photon of green light has a wavelength of about 550 nm.
The wavelength of the emitted photon of light corresponds to the green part of the visible spectrum.
The emission of visible light in this way is known as fluorescence.

Further Reading:
Isotopes
Radioactivity: Properties and Uses
Emission Spectra
Flame Tests

Suggested Study Questions

  1. Uranium is found in nature as one of three isotopes, uranium-234, uranium-235 and uranium-238. Explain how atoms of each isotope are:
    • the same
    • different
  2. Atoms of neptunium-234, neptunium-235 and neptunium-238 have been synthesized. Explain the similarities and differences between each of the following pairs of atoms:
    • neptunium-234 and uranium-234
    • neptunium-235 and uranium-235
    • neptunium-238 and uranium-238
    1. The value for Planck's constant is 6.626 070 040 x 10-34 J s and the speed of light is given as 300 000 000 m / s. Calculate the energy of each of the following photons of light:
      • ultra-violet light, λ = 300 nm
      • green light, λ = 550 nm
    2. Using the results of question 3, compare the energy of the photons used to excite uranium atoms and the energy of the photons emitted by uranium atoms and explain the difference.
    3. Explain why the same wavelength of light is always emitted when these uranium atoms are exposed to ultra-violet light.
    4. Would you expect the uranium glass to fluoresce if it is exposed to infra-red light rather than to ultra-violet light? Explain your answer.
    5. Optical brighteners are often used in laundry detergents to make your old, yellowy-looking white clothes look whiter. Typically these compounds absorb ultra-violet light with a wavelength of around 300 nm and emit light with a wavelength of around 450 nm.
      • What colour is the light emitted?
      • What is the energy of the emitted light?
      • Why is the energy of the light emitted not the same as the energy absorbed when the incoming photon hits the "optical brightening compound"?
      • Would you expect a laundry detergent containing "optical brightening compounds" to glow in the dark when exposed to UV light? Explain your answer.

    Thursday, May 16, 2013

    Astatine's Ionization Energy

    Astatine is the product of the radioactive decay of some heavier elements and is the rarest naturally occurring element on Earth, only a few grams of astatine is estimated be present in the whole of the Earth's crust at any one time. All of astatine's isotopes are short-lived, with astatine-210 having the longest half-life of all its isotopes, 8.1 hours. As a result, astatine was unknown until 1940, when scientists bombarded bismuth-209 with alpha particles and produced astatine.
    Even today we don't know very much about astatine, but estimates about its properties have been made based on its position in the Periodic Table, right under iodine in Group 17 (halogens). The first ionization energy of astatine has been estimated to be between 849.11 and 926.29 kJ/mol (8.8 and 9.6 eV).

    The ionization energy, the energy required to remove an electron from the valence shell of an atom, is one of the most important properties that influences the chemical behaviour of an element.

    In May 2013 an international team of researchers announced that they had measured the first ionization energy of astatine using laser ionization spectroscopy and found it be be 9.31751 eV (899.02 kJ/mol)

    Reference:
    Rothe, S. et al. Measurement of the first ionization potential of astatine by laser ionization spectroscopy. Nat. Commun. 4:1835 doi: 10.1038/ncomms2819 (2013).

    Further Reading:
    http://www.ausetute.com.au/pertable.html

    http://www.ausetute.com.au/trendgp7.html 
    http://www.ausetute.com.au/trendie.html 
    http://www.ausetute.com.au/isotopes.html
    http://www.ausetute.com.au/nucledec.html
    http://www.ausetute.com.au/halflife.html

    Suggested Study Questions:
    1. Use the Periodic Table to find the following:
      • astatine's chemical symbol
      • astatine's atomic number
    2.  Use the Periodic Table to find the
      • The group astatine belongs to
      • the period astatine belongs to
    3. How many valence electrons does an atom of astatine have? Explain your answer.
    4. Describe the trend in melting points as you go down astatine's group in the periodic table, then estimate the melting point of astatine.
    5. Describe what you think astatine would look like at room temperature and justify your answer on the basis of trends in the periodic table. 
    6. How does astatine-207 differ from astatine-210? 
    7. Astatine-211 and 2 neutrons are produced when bismuth-209 is bombarded with alpha particles.  Write a nuclear equation for this reaction.
    8. Imagine working in a laboratory. You have been given 100 μg of astatine-210 at 9 am for your experiment. Assuming the half-life of astatine is 8 hours, how much astatine-210 would you have left when you leave the lab at 5 pm?
    9. The half-life of astatine-219 is about 1 minute. If you had 100 μg of astatine-219 at 9 am, how much astatine-219 would you have 5 minutes later at 9:05 am ?
    10. Use the information in the article above to estimate the conversion factor between electronvolts (eV) and kJ/mol. 
    11. Why do we not have an accurate measure of how much astatine is found in the Earth's crust?
    12. Suggest a way that scientists can estimate the amount of astatine in existence in the Earth's crust.  

    Sunday, June 3, 2012

    Element 118

    In 1998, Robert Smolanczuk published some calculations which suggested that it could be possible to produce element 118 by fusing lead with krypton. In 1999, Lawrence Berkeley National Laboratory (LBNL) scientists reported the successful production of element 118 (given the temporary name ununoctium and temporary chemical symbol Uuo) by fusing lead-208 and krypton-86: 


    86
    36
    Kr
    + 208
    82
    Pb
    → 293
    118
    Uuo
    + n

    Unfortunately, researchers, including LBNL scientists, were unable to duplicate theses results, and in 2002 the director of the laboratory announced that the original claim of the discovery of element 118 (ununoctium) had been based on data that was fabricated by a researcher and was not based on the results of a scientific investigation.

    In 2006, researchers at the Joint Institute for Nuclear Research (JINR) and Lawrence Livermore National Laboratory of California announced that they had indirectly detected several nuclei of ununoctium-294, produced by colliding californium-249 atoms and calcium-48 atoms:

    249
    98
    Cf
    + 48
    20
    Ca
    → 294
    118
    Uuo
    + 3n

    However, in 2011 the International Union of Pure and Applied Chemistry (IUPAC) said the results did not meet the criteria for the announcement of the discovery of a new element.

    Further Reading
    Isotopes 
    History of the Periodic Table

    Suggested Study Questions
    1. Give the atomic number for each of the following isotopes:
      • calcium-48
      • krypton-86
      • lead-208 
      • californium-249
      • ununoctium-294
    2. Give the mass number for each of the following isotopes:
      • calcium-48
      • krypton-86
      • lead-208 
      • californium-249
      • ununoctium-294
    3. Give the number of protons in the nucleus of each of the following isotopes:
      • calcium-48
      • krypton-86
      • lead-208 
      • californium-249
      • ununoctium-294
    4. Give the number of neutrons in the nucleus of each of the following isotopes:
      • calcium-48
      • krypton-86
      • lead-208 
      • californium-249
      • ununoctium-294
    5. It has been suggested that element 120 with a mass number of 302, and the temporary name unbinilium and temporary symbol Ubn, could be produced by bombarding plutonium-244 with iron-58. Write a possible equation for this reaction.
    6. It has also been suggested that element 120 (unbinilium, Ubn) with a mass number of 302 could be produced by fusing uranium-238 and nickel-64. Write a possible equation for this reaction.
    7. If unbinilium-302 were to be produced by fusing californium-248 with another atom, what would be the most likely element to use? Justify your answer by writing an equation for the equation.
    8. What is the most likely product of the reaction in which californium-249 atoms are fused with titanium-50 atoms? Justify your answer by writing an equation for this reaction.
    9. Based on your understanding of the arrangements of elements within the Periodic Table, which group do you think ununoctium would belong to? What would you predict the physical and chemical properties of ununoctium to be?
    10. Before 1979, element 118 had been known as eka-emanation or eka-radon because radium "emanation" is an old name for the element radon, so-called because Friedrich Ernst Dorn first noticed that radium compounds emanate, or emit, a radioactive gas, and "eka" was the prefix used by mendeleev when constructing his Periodic Table to denote an unknown element 1 place down in the same Group. Give the current names for the elements which were originally known as:
      • eka-caesium
      • eka-iodine
      • eka-boron
      • eka-aluminium
      • eka-manganese
      • eka-silicon

    Saturday, April 21, 2012

    Bismuth-209

    Until recently, bismuth-209 was considered to be a stable isotope, in fact, it was thought to be the heaviest stable isotope, but scientists weren't very happy about the "stable" designation. Measurements of atomic mass and nuclear decay schemes since the 1940's indicated that bismuth-209 should be just a bit too heavy to be truly stable. Then, during the night of March 14-15 2002, a team of scientists from the Institut d’Astrophysique Spatiale d’Orsay (IAS - CNRS, Université Paris XI) stumbled across the alpha decay products of bismuth-209. 

    The half-life for the decay of bismuth-209 to  thallium-205 has been reported as 1.9 x 1019 years. 
    In comparison, the estimated age of the universe, starting  from the time of the Big Bang, is just  13.75 x 109 years. Bismuth-209 is therefore a primordial isotope, one that has existed in its current form since before the Earth was formed. 288 primordial isotopes are known, including the 255 stable isotopes plus 33 unstable isotopes with exceptionally long half-lives like bismuth-209.

    Reference
    http://www.cnrs.fr/cw/en/pres/compress/bismuth.htm 

    Further Reading 
    Isotopes
    Properties & Uses of Radiation
    Nuclear Decay
    Half-life Calculations

    Suggested Study Questions
    1. For an atom of bismuth-209, give the
      • symbol
      • atomic number
      • mass number
      • number of protons in the nucleus
      • number of neutrons in the nucleus
    2. For bismuth-209,
      • Calculate the ratio of neutrons to protons
      • If the nucleus of a heavy metal atom is considered to be stable of the neutron to proton ratio is 1.5:1, would bismuth-209 be predicted to be stable or unstable? Explain your answer.
    3. For an atom of thallium-205, give the
      • symbol
      • atomic number
      • mass number
      • number of protons in the nucleus
      • number of neutrons in the nucleus
    4. Give the symbol for an alpha particle.
    5. Write an equation for the nuclear decay of bismuth-209 to thalium-205.
    6. Current predictions are that the Earth will be demolished during the death of the Sun in about 7 x 109 years. Assuming you had 1 tonne of bismuth-209 today,
      • How much bismuth-209 would remain in 7 x 109 years?
      • How much thallium-205 would have been produced as a result of bismuth-209 decay?
    7. Bismuth-209 is produced on earth when lead-209 undergoes beta decay. Write an equation to represent this nuclear reaction.
    8. The half-life of lead-209 is about 3.25 hours. If you had isolated 60 grams of lead-209, how long would it take for you to have less than about 1 gram left?

    Thursday, June 9, 2011

    Nickel Isotopes

    Atoms of an element with the same number of protons but a different number of neutrons are known as isotopes. Nickel, atomic number (Z) = 28, has 28 protons in its nucleus. There are at least 30 isotopes of nickel, including the stable isotopes nickel-58, nickel-60, nickel-61, nickel-62 and nickel-64, and the radioactive isotopes nickel-56 and nickel-59.
    Nickel-56 is produced in some supernovae in which nickel-56 then decays to cobalt-56 and then to iron-56. The half-life of nickel-56 is about 6 days.
    Nickel-59 has been used to date the age of meteorites because it has a long half-life of 76,000 years.

    Scientists from the Nuclear Spectroscopy Division at the Institute of Experimental Physics (IFD) of the Faculty of Physics, University of Warsaw (FUW) have undertaken research into nickel-48, a highly peculiar isotope which was only discovered in 1999. It has 28 protons and only 20 neutrons in its nucleus.

    Nickel-48 is the most neutron deficient nucleus ever studied. Such an isotope "lives" only 2 thousandths of a second and then decays. The research by the Polish scientists from FUW has shown that the most frequent decay mode of nickel-48 is two-proton emission in which 2 protons are emitted from the nucleus. This simultaneous two-proton emission is a very rare phenomenon. So far it has only been observed in three other atomic nuclei: magnesium-19, zinc-54 and iron-45.

    Reference
    University of Faculty of Physics Warsaw (2011, June 9). Unique Polish detector can observe rare decays of nickel nuclei. ScienceDaily. Retrieved June 10, 2011, from http://www.sciencedaily.com­ /releases/2011/06/110609084811.htm

    Further Reading
    Isotopes
    Nuclear Decay
    Half-Life

    Study Questions

    1. What is the mass number of each of the following isotopes?
      • nickel-58
      • nickel-62
      • magnesium-19
      • zinc-54
      • iron-45
    2. What is the atomic number of each of the following isotopes ?
      • nickel-58
      • nickel-62
      • magnesium-19
      • zinc-54
      • iron-45
    3. How many protons are present in an atom of each of the following isotopes?
      • nickel-58
      • nickel-62
      • magnesium-19
      • zinc-54
      • iron-45
    4. How many neutrons are present in an atom of each of the following isotopes?
      • nickel-58
      • nickel-62
      • magnesium-19
      • zinc-54
      • iron-45
    5. Write nuclear decay equations for each of the following:
      • nickel-56 decays to cobalt-56
      • cobalt-56 decays to iron-56
      • nickel-48 decays by emitting 2 protons from the nucleus
      • magnesium-19 decays by emitting 2 protons from the nucleus
    6. Using a half-life of 76,000 years for nickel-59, calculate how much nickel-59 will remain in a 50g pure sample in:
      • 38,000 years
      • 152,000 years
    7. If a meteorite is approximately 1.2 million years old, what percentage of the original nickel-59 would remain?
    8. If a meteorite has a mass of 600kg and contains 10% nickel-59, what mass of nickel-59 will remain in 380,000 years?

    Friday, March 25, 2011

    Fukushima Radiochemistry

    On the 11th March 2011 at 14:46 Japan Standard Time, a category 9 earthquake was recorded off the northeast coast of Japan. The epicenter was approximately 72 kilometers east of the Oshika Peninsula of Tohoku. The earthquake moved Honshu 2.4 m east and shifted the Earth on its axis by almost 10 cm. The earthquake was recorded as an upper 6 at the prefecture of Fukushima.

    6 separate boiling water nuclear reactors make up the Fukushima I power plant. Nuclear reactors numbers 4, 5 and 6 had already been shut down prior to the earthquake for routine maintenance. Nuclear reactors 1, 2 and 3 were shut down after the earthquake but the subsequent tsunami flooded the plant and incapacitated the emergency generators which ran the pumps to cool the reactors. Reactors 1, 2 and 3 suffered partial nuclear meltdowns (melting of the core of the nuclear reactor), hydrogen explosions destroyed parts of the buildings housing reactors 1 and 3, an explosion damaged reactor 2's containment which is designed to prevent the release of radioactivity into the environment, and several fires broke out in reactor 4. As the water levels in spent fuel pools dropped, the spent fuel rods began to overheat.
    On 25th March, Japan's nuclear regulator announced a likely breach of Number 3's containment vessel. World wide measurements of wind-born radioactive iodine and caesium vented from reactors suggested a massive increase in these substances which led to bans on the sale of food grown within a 100km radius of the Fukushima I plant

    Cesium-137 is a radioactive isotope of cesium that is formed during the nuclear fission of uranium. It has a half-life of 30.17 years and decays by beta emission to metastable barium-137. Cesium-137 is soluble in water, and its behaviour in living things is similar to that of potassium. The biological half-life of cesium is about 70 days. Experiments with dogs have shown that a dose of 44μg/kg of cesium-137 is lethal within 3 weeks. Prussian blue, Fe7(CN)18.14H2O, chemically binds cesium-137 and speeds up its expulsion from the body, so it can be used to treat ingestion of cesium-137.

    Iodine-131, also called radioiodine, makes up about 3% of the products of uranium fission. It undergoes beta decay and has a half-life of about 8.02 days. High doses of iodine-131 can be less dangerous than low doses since high doses tend to kill thyroid tissues which could otherwise become cancerous as a result of the radiation. Ingestion of iodine-131 is treated by taking iodine supplements containing non-radioactive iodine-127 as iodide ions. This raises the total amount of iodine in the body and therefore reduce the uptake and retention of radioactive iodine-131.

    Reference:
    http://www.newsdaily.com/stories/tre72l501-us-japan-contaminants/


    Further Reading:
    Isotopes
    Nuclear Decay
    Half-life

    Study Questions:
    1. Explain what is meant by the term nuclear fission.
    2. Give the atomic number and mass number for each of the following:
      • uranium-235
      • uranium-238
      • cesium-137
      • iodine-131
    3. How many protons and neutrons are contained within the nucleus of each of these atoms:
      • uranium-235
      • uranium-238
      • cesium-137
      • iodine-131
    4. Explain what is meant by beta decay.
    5. Write balanced chemical equations for the beta decay of each of the following:
      • cesium-137
      • iodine-131
    6. What does a Chemist mean by the term half-life?
    7. If a 20kg dog ingests 880μg of cesium-137, how much cesium-137 will remain after 3 weeks? (The half-life of cesium-137 is about 30.17 years)
    8. "The biological half-life of cesium is about 70 days". What do you think this means?
    9. If a 20kg dog ingests 880μg of cesium-137, how much cesium-137 will remain in the dog's body after 70 days?
    10. Iodine pills were distributed to people living around the Fukushima power plants on 12th March. A typical emergency dose is 130 milligrams of potassium iodide. What mass of iodine is contained in each dose?
    11. The iodine dose contained in the emergency pills is about 700 times larger than the normal nutritional daily need of an adult. What is the approximate mass of iodine is required per adult daily?

    Wednesday, September 8, 2010

    Magic Numbers

    Scientists who study the nuclei of atoms apply the "magic" moniker to elements with a certain number of protons or combinations of protons and neutrons. At the magic numbers of 2, 8, 20, 28, 50, 82 and 126 the protons and neutrons are tightly bound together, giving many "magic" elements a high degree of nuclear stability.

    Rutgers scientists have been studying an isotope of tin that is "doubly magic", it contains 50 protons and 82 neutrons. Unlike other magic nuclei that are stable, this isotope of tin is very unstable with a half-life of 40 seconds.

    The scientists believe that this isotope of tin may be formed in supernova explosions or collisions of neutron stars, and could be part of the process that forms heavier elements.

    Reference:
    K. L. Jones, A. S. Adekola, D. W. Bardayan, J. C. Blackmon, K. Y. Chae, K. A. Chipps, J. A. Cizewski, L. Erikson, C. Harlin, R. Hatarik, R. Kapler, R. L. Kozub, J. F. Liang, R. Livesay, Z. Ma, B. H. Moazen, C. D. Nesaraja, F. M. Nunes, S. D. Pain, N. P. Patterson, D. Shapira, J. F. Shriner, M. S. Smith, T. P. Swan, J. S. Thomas. The magic nature of 132Sn explored through the single-particle states of 133Sn. Nature, 2010; 465 (7297): 454 DOI: 10.1038/nature09048


    Further Reading
    Isotopes
    Nuclear Decay
    Half-life

    Study Questions

    1. Explain what is meant by the term isotope.
    2. What is the atomic number for the tin isotope described in the article above?
    3. What is the mass number for the tin isotope described in the article above?
    4. What are the names of the elements that have a nucleus containing the following "magic" numbers of protons:
      • 2
      • 8
      • 20
      • 28
      • 50
      • 82
    5. Explain what is meant by the term half-life.
    6. The half-life of the tin isotope described above is 40 seconds.
      • If the original sample had a mass of 0.1g, what mass of tin isotope would be present in the sample after 2 minutes?
      • What percentage of the mass of the original sample would be present after 80 seconds?




    Sunday, May 16, 2010

    Silver Isotopes to Date the Earth

    The Earth is depleted in some elements, such as hydrogen, carbon, nitrogen and silver, compared to the Solar System as a whole. What scientists can not tell us is when this depletion occurred. Carnegie Institute scientists have used the isotopic ratios of silver in primitive meteorites and rocks from the Earth's mantle to determine the history of Earth's volatiles relative to the formation of Earth's iron core.

    Silver has two stable isotopes of which silver-107 was produced in the early Solar System by the rapid nuclear decay of palladium-107, which is so unstable that virtually all of it decayed within the first 30 million years. Silver is more volatile than palladium, while palladium is more likely to bond with iron. The silver isotope evidence suggests that the core formed between 5 and 10 million years after the origin of the Solar System.

    Studies using hafnium and tungsten isotopes indicate that the core formed between 30 and 100 million years after the origin of the Solar System.

    These apparently contradictory results support the "Heterogeneous Accretion" model of planetary growth in which the Earth's building block's changed composition as the planet accreted. So, at first the Earth accreted volatile-depleted material until it reached about 85% of its final mass and then accreted volatile-rich material in the last stages of its formation, about 26 million years after the Solar System's origin.

    Reference:
    Carnegie Institution (2010, May 14). Water was present during birth of Earth, study of silver suggests. ScienceDaily. Retrieved May 17, 2010, from http://www.sciencedaily.com­ /releases/2010/05/100513143457.htm