Showing posts with label nuclear decay. Show all posts
Showing posts with label nuclear decay. 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:
106Ru0e+ 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

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?

Saturday, December 10, 2011

Flerovium and Livermorium?

Elements 114 and 116 are the latest additions to the Periodic Table of the elements,
created by smashing calcium ions into a curium target to create element 116. Element 116 decayed almost immediately into element 114. The scientists also created element 114 separately by replacing curium with a plutonium target.
Both elements were first produced at the Joint Institute for Nuclear Reasearch, Dubna, Russia, and Lawrence Livermore chemists. Element 114 was first produced in 1998 and element 116 in 2000. The proposed name for element 114 is flerovium with the symbol Fl, and, the proposed name for element 116 is livermorium with the symbol Lv.

Flerovium was chosen to honour the Flerov Laboratory of Nuclear Reactions where element 114 was synthesized. The laboratory itself is named after Georgiy N. Flerov (1913-1990) , a renowned physicist who discovered the spontaneous fission of uranium and was a pioneer in heavy-ion physics. He is the founder of the Joint Institute for Nuclear Research.

Livermorium was chosen to honour Lawrence Livermore National Laboratory (LLNL) and the city of Livermore, California. A group of researchers from the Laboratory, along with scientists at the Flerov Laboratory of Nuclear Reactions, participated in the work carried out in Dubna on the synthesis of superheavy elements, including element 116. The element lawrencium, element 103, was named after LLNL's founder E.O. Lawrence.

The new names were submitted to the IUPAC in October 2011 and now remain in the public domain. The new names will not be official until about March 2012 when the public comment period is over.

Reference
DOE/Lawrence Livermore National Laboratory (2011, December 1). Scientists propose new names for elements 114 and 116. ScienceDaily. Retrieved December 11, 2011, from http://www.sciencedaily.com­ /releases/2011/12/111201125400.htm


Further Reading
History of the Elements
Periodic Table of the Elements
Isotopes
Nuclear Decay

Suggested Study Questions
  1. What is the atomic number of each of the following elements?
    • calcium
    • curium
    • plutonium
    • uranium
    • lawrencium
    • flerovium
    • livermorium
  2. How many protons are in the nucleus of an atom of each of the following elements?
    • calcium
    • curium
    • plutonium
    • uranium
    • lawrencium
    • flerovium
    • livermorium
  3. Calculate the number of electrons present in an atom of each of the following elements:
    • calcium
    • curium
    • plutonium
    • uranium
    • lawrencium
    • flerovium
    • livermorium
  4. For each of the elements above, state whether it is found in nature or whether it is man-made.
  5. Assuming each of the elements above forms an ion with a charge of +2 then
    • how many electrons will be present in each ion?
    • how many protons will be present in each ion?
  6. Write a possible nuclear equation to show the production of livermorium from calcium ions and curium atoms.

  7. Write a possible nuclear equation to show the production of flerovium from plutonium atoms and calcium atoms.

  8. Write a possible nuclear decay equation to show how livermorium could decay to produce flerovium.

  9. The suggested symbol for Flerovium is Fl. List all other elements that have a symbol which includes the letter F.

  10. The suggested symbol for Livermorium is Lv. List all the other elements that have a symbol which includes the letter L.


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?

Tuesday, June 22, 2010

Element 114

About 10 years ago, scientists in Dubna, Russia, reported the observation of element 114. Scientists at Berkeley, USA, and GSI Helmholtzzentrum für Schwerionenforschung in Darmstadt Germany have also reported observations of element 114.

In the most recent GSI experiment using the 120 meter long GSI particle accelerator, the scientists fired calcium ions onto a plutonium coated foil. The nuclei undergo fusion to form the nucleus of the new element. The atoms of element 114 were then separated from the other products of the reaction and identified on the basis of the radiation emitted during their decay. Two different isotopes of element 114 were identified with mass numbers 288 and 289. The measured half-lives are of the order of one second.

Russian reports on the creation of elements up to atomic number 118 are yet to be confirmed.

Reference:
Helmholtz Association of German Research Centres (2010, June 22). Chemical element 114: One of heaviest elements created. ScienceDaily. Retrieved June 23, 2010, from http://www.sciencedaily.com­ /releases/2010/06/100622102347.htm


Study Questions
  1. What is the atomic number of the element 114?
  2. What are the atomic numbers of calcium and plutonium?
  3. Define the term atomic number.
  4. Write an equation to represent the fusion of calcium and plutonium.
  5. What is meant by the term isotope?
  6. For each of the isotopes of element 114 in the article above, give the atomic number, mass number, number of protons, number of neutrons, and number of electrons in an atom of each isotope.
  7. Write a nuclear equation for the decay of each isotope of element 114 assuming it undergoes beta decay.
  8. Write a nuclear decay equation for the decay of each isotope of element 114 assuming it undergoes alpha decay.
  9. What is meant by the term half life?
  10. If the half-life an isotope of element 114 is assumed to be 1 second, what percentage of the original isotope will be present after 10 seconds?