Nuclear chemistry
This presentation is the property of its rightful owner.
Sponsored Links
1 / 117

Nuclear Chemistry PowerPoint PPT Presentation


  • 173 Views
  • Uploaded on
  • Presentation posted in: General

Nuclear Chemistry. Brief history of nuclear related discoveries Electron, proton, neutron Nuclear transformations Natural radioactivity Half Life, carbon dating Nuclear chemistry equations Chain reaction, atom bomb Applications Nuclear reactors Radioisotopes Personl Exposure

Download Presentation

Nuclear Chemistry

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


Nuclear chemistry

Nuclear Chemistry

  • Brief history of nuclear related discoveries

    • Electron, proton, neutron

  • Nuclear transformations

    • Natural radioactivity

    • Half Life, carbon dating

    • Nuclear chemistry equations

    • Chain reaction, atom bomb

  • Applications

    • Nuclear reactors

    • Radioisotopes

  • Personl Exposure

    • Radon, other natural sources

    • 3-mile Island (USA), Chernobyl (USSR), Japan

      • Potassium Iodide protection


Atomic versus nuclear what s the difference

Atomic versus NuclearWhat’s the Difference?

  • Atomic properties are those of an atom

    • Chemical reactions (gain/loss of electrons)

    • Emission of light (electron orbit jumps)

    • Bonds between elements (covalent, ionic)

  • Nuclear properties are within the atom

    • Construction of nucleus (electrons, protons)

    • Radioactive disintegration

    • Fission/fusion of nuclei, element conversion


Atomic number

Atomic number

  • Atomic Number (and element number)

    • Number protons = number electrons = “Z”

  • Atomic Mass Number

    • Total Number of Protons defining the element = Z

    • Total number of Neutrons in element nucleus = N

    • Total mass of nucleus = A = Z + N

    • Electron mass is ignored 1/1836 =0.054% (negligible)

  • Isotopes

    • Same atomic number, different number of neutrons

    • Large variations of isotopes between elements

    • Isotope significance (e.g. U-235 vs U-238, C-14 vs C-12)

  • Atomic Weight (most often used)

    • Weighted average of isotope masses

    • What’s on the periodic chart


Weighted atomic mass natural values

Weighted Atomic Mass (natural values)

  • Lots of isotopes of Uranium exist, all different masses

    • Most prevalent isotope is U-238 at 99.283%

    • Most useful isotope is U-235 at 0.711%

    • Other isotopes rather rare, relatively insignificant

  • “Weighted Average” recognizes quantity

    • Sum of mass contributions = the weighted average value

    • This is what we see on the periodic charts.


Nuclear changes

Nuclear reaction: A reaction that changes an atomic nucleus, usually causing the change of one element into another. A chemical reaction never changes the nucleus.

Different isotopes of an element have essentially the same behavior in chemical reactions but often have completely different behavior in nuclear reactions.

The rate of a nuclear reaction is unaffected by a change in temperature or pressure (within the range found on earth) or by the addition of a catalyst.

The nuclear reaction of an atom is essentially the same whether it is in a chemical compound or in an uncombined, elemental form.

The energy change accompanying a nuclear reaction can be up to several million times greater than that accompanying a chemical reaction.

Nuclear Changes


Nuclear nomenclature

Nuclear Nomenclature

  • The atomic number, written below and to the left of the element symbol, gives the number of protons in the nucleus and identifies the element.

  • The mass number, written above and to the left of the element symbol, gives the total number of nucleons, a general term for both protons (p) and neutrons (n).

  • The most common isotope of carbon, for example, has 12 nucleons: 6 protons and 6 neutrons:


Writing nuclear reactions

Writing Nuclear Reactions

  • “stacked” numbers difficult to write

    • Possible but difficult using a word processor

  • Alternative is “front and back” values

    • Carbon 14 = 6C14

    • Front value is atomic number Z

    • Back value is atomic mass A


60 years of discoveries

60 years of discoveries

  • 1884 - Chemistry theories, 56 theses, Arrhenius

  • 1888 - Proton Discovery, Goldstein

  • 1895 – X-Ray discovery, Roentgen

  • 1896 - Radioactivity Discovery, Baquerel

  • 1897 - Electron Discovery, J.J. Thompson

  • 1905 - Radioactive Element separation, Curie

  • 1905 - Equivalence of mass & energy E=mC2, relativity, photoelectric effect, A. Einstein

  • 1916 - general relativity, proven in 1919, A. Einstein

  • 1932 - Neutron Discovery, Chadwick

  • 1933 - Nuclear chain reaction proposed, Szilard

  • 1938 - Nuclear fission discovered

  • 1942 - First operational nuclear reactor, Fermi

  • 1945 - First warfare use of nuclear energy


Nuclear chemistry

Cathode Rays (electrons)first demonstrated by Crookes in1895Early investigator of radiation inside electrical discharge tubes, eventually leading to CRT (Television) tubes. He was one of the first to experiment with radioactivity and its ability to make certain minerals glow. He also invented the ”radiometer” still in use as an educational toy.


Nuclear chemistry

ELECTRON - J.J. Thompson 1897found a new particle “boiling off” a heated filament which had <1/1000 mass of hydrogen. It had a negative charge by its magnetic and/or electrostatic deflection. Using similar apparatus he discovered isotopes of the same element with different mass, which led to science of mass spectrometry


Nuclear chemistry

PROTON, Goldstein in1888Used high voltage to ionize gases, accelerating particles through holes in cathode, causing “canal rays” (trails looked like canals). Particles were positive. Hydrogen particles later identified as protons by Rutherford in 1919


Nuclear chemistry

NEUTRON, Chadwick 1932observed a new form of penetrating radiation, which had no charge (not protons or electrons)


Nuclear chemistry

NEUTRINOPredicted by Wolfgang Pauli in 1930, based on conservation discrepancies. the “little neutron” Indirectly observed in 1942 and1946 via interactions with other particles, directly observed in 1972 “bubble chamber”


Discovery and nature of radioactivity

Discovery and Nature of Radioactivity

  • In 1896, the French physicist Henri Becquerel noticed a uranium-containing mineral exposed a photographic plate that had been wrapped in paper.

  • Marie and Pierre Curie investigated this new phenomenon, which they termed radioactivity: The spontaneous emission of radiation from a nucleus.

  • Ernest Rutherford established that there were at least two types of radiation, which he named alphaand beta. Shortly thereafter, a third type of radiation was found and named for the third Greek letter, gamma.


Nuclear chemistry

Baquerel – observed radioactivity 1896Photographic plate accidentally exposed by Uranium Baquerel is SI unit of radiation, Bq = disintegrations/sec1 Curie = radiation from 1 gram of Radium = 3.7*10^10 Bq


Radioactivity

Radioactivity

Emissions from Pitchblende (uranium ore)

Found to expose photographic film

We will measure pitchblende today

3 common types of nuclear radiation

Alpha (α), helium nuclei particle, 2He4 = 2p+2n

Very strong but not very penetrating

Beta (β), an electron particle, -1e0

Mildly penetrating, stopped by thick paper

Gamma (γ), radiation similar to X-Ray

Very penetrating, used for imaging


Stable and unstable isotopes

Stable and Unstable Isotopes

  • Every element in the periodic table has at least one radioactive isotope, or radioisotope, and more than 3300radioactive isotopes are known.

  • Their radioactivity is the result of having unstable nuclei. Radiation is emitted when an unstable radioactive nucleus, or radionuclide, spontaneously changes into a more stable one.

  • There are only 264 stable isotopes among all the elements.

  • All isotopes of elements with atomic numbers higher than that of bismuth (83) are radioactive.


Radioactivity1

Radioactivity

  • Results from unstable elements

  • Heavy elements formed inside stars

    • Formed and stable at extreme temperatures

    • Unstable and disintegrate at earth temperatures

  • Half-Life

    • Time it takes for ½ of material to disintegrate

    • Uranium 238 is 4.5 billion years, same as earth’s age

      • There was twice as much uranium when earth formed

      • A non-linear scale (e.g ½ of ½, etc)

      • A natural nuclear reactor happened in Okla, Africa


Nuclear chemistry

Marie & Pierre Curie, 1905Separated tons of mineral pitchblende to discover and isolate Radium, and polonium (named for Poland). The standard measure for radioactivity is the Curie = Ci


Nuclear chemistry

  • For elements in the first few rows of the periodic table, stability is associated with a roughly equal number of neutrons and protons.

  • As elements get heavier, the number of neutrons relative to protons in stable nuclei increases.

  • Lead-208, for example, the most abundant stable isotope of lead, has 126 neutrons and 82 protons in its nuclei.


Nuclear chemistry

  • Alpha rays move about ~0.1c and can be stopped by a few sheets of paper or by the top layer of skin.

  • Beta rays move at up to 0.9c and have about 100 times the penetrating power of a particles. A block of wood or heavy clothing is necessary to stop b rays.

  • Gamma rays move at c and have about 1000 times the penetrating power of a rays. A lead block several inches thick is needed to stop g rays.


Nuclear chemistry

When passed between two charged plates:

  • Alpha rays, helium nuclei (He+2 ), bend toward the negative plate because they have a positive charge.

  • Beta rays, electrons (e- ), bend toward the positive plate because they have a negative charge.

  • Gamma rays, photons (g), do not bend toward either plate because they have no charge.


Nuclear decay

Nuclear Decay

  • Nuclear decay: The spontaneous emission of a particle from an unstable nucleus.

  • Transmutation: The change of one element into another.

  • The equation for a nuclear reaction is not balanced in the usual chemical sense because the kinds of atoms are not the same on both sides of the arrow. A nuclear equation is balanced when the number of nucleons and the sums of the charges are the same on both sides.


Nuclear decay1

Nuclear Decay

  • Decrease in atomic number

    • Loss of alpha particle with positive charge

      • Mass of 2 protons and 2 neutrons

      • Loss of 2 protons reduces element # by 2

        • Uranium 92U238 into Thorium 90Th234 + 2He4

  • Increase in atomic number

    • Loss of electron with negative charge

      • Charge of nucleus increases by 1

      • Next higher element formed

        • Thorium 90Th234 Proactinium 91Pa234 + -1 e0

        • Proactinium 91Pa234 Uranium 92U234 + -1 e0


Nuclear chemistry

  • During alpha emission, the nucleus loses two protons and two neutrons.

  • Emission of an a particle from an atom of uranium-238 produces an atom of thorium-234.


Nuclear chemistry

  • Beta emission involves the decompositionof a neutron to yield an electron and a proton.

  • Iodine-131, a radioisotope used in detecting thyroid problems, undergoes nuclear decay by b emission to yield xenon-131.


Anti particles

Anti-Particles

  • In 1928 Paul Dirac predicted that all particles should have opposites called anti-particles.

  • The first of these was discovered in 1932 by Carl Anderson. This was an electron with a positive electric charge (+1). This particle is the anti-electron (also called a positron). It is identical in every respect to the electron apart from its electric charge.

  • When an electron and positron come into contact, they mutually annihilate each other producing a flood of energy in accordance with Einstein's famous equation, E=mC2


Anti matter

Anti-matter

  • Anti-particles making up atoms are same as conventional particles except for charge

    • Electron (e-)  Positron (e+), 2008-LNL

    • Proton (p+)  Anti-Proton (p-), 1955-UCB

    • Hydrogen  Anti-Hydrogen; 1995-CERN

  • Matter+Antimatter  pure energy

    • Antimatter engines in Star Trek !

  • Parts of universe could be “anti-matter”

    • Same properties, light emission, etc.

    • Matter + Antimatter  pure energy

    • Something to avoid ….


Nuclear chemistry

  • Positron emission involves the conversion of a proton in the nucleus into a neutron plus an ejected positron.

  • A positron has the same mass as an electron but a positive charge.

  • Potassium-40 undergoes positron emission to yield argon-40, this hppens in your body which contains tiny amounts of K-40.


Radioactive half life

Radioactive Half-Life

  • Rates of nuclear decay are measured in units of half-life , defined as the amount of time required for one-half of the radioactive sample to decay.

  • Each passage of a half-life causes the decay of one half of whatever sample remains. The half-life is the same no matter what the size of the sample, the temperature, or any other external conditions.


Nuclear chemistry

All nuclear decays follow the same curve, 50% of the sample remains after one half-life, 25% after two half-lives, 12.5% after three half-lives, and so on.


Carbon 14

Carbon-14

  • Carbon14 discovered 1940 at UC Berkeley

    • Formed in upper atmosphere from nitrogen

    • Solar neutrons convert nitrogen to carbon-14

    • Carbon-14 becomes carbon dioxide

    • Carbon-14 dioxide absorbed by plant life

    • Animal life eats the plant life, absorbs C-14

    • Steady state evolves … until object dies

    • After death, the decay rate reduces C-14


Nuclear chemistry

Decay of Carbon-14Neutron turns into proton + electron (beta particle)Mass remains at 14, but carbon becomes nitrogenintensity of electron emission indicates object’s age


Nuclear chemistry

14C is continually produced in the atmosphere and incorporated into life cycles, so 14C amount in living things is constant. Upon death, no more 14C is absorbed, so concentration decreases. Measuring the remaining radioactivity provides an age estimate. The half life of 14C is 5730 years. The method is good for estimating age of objects 500 to 50,000 years old.


Carbon dating methodology counts min versus age of sample assumes c 14 formation at a constant rate

Carbon dating methodologycounts/min versus age of sample, assumes C-14 formation at a constant rate


Half life calculations

Half Life calculations

  • Reduction in material is non-linear

    • original½ at half-life¼ at 2 half-lives

  • General equation:

    • n1/n0 = (0.5)^(#of half lives)

    • n1/n0 = (0.5)^1  50% remaining

    • n1/n0 = (0.5)^2  25% remaining

    • n1/n0 = (0.5)^3  12.5% remaining


Half life calculations1

Half Life calculations

  • Carbon dating example: (reverse example)

    • old object has 12.79% normal C14

    • Half life of C14 is 5730 years

  • n1/n0 = (0.5)^(number of half lives)

    • Take natural logs to eliminate exponents:

  • Ln(n1/n0)= Ln(0.5)*(t / 5730)

  • Ln(0.1279/1.00)= Ln(0.5)*(t / 5730)

    • Ln(0.1279)= -.6931(t / 5730)

    • -2.0565 = -0.6931 * (t / 5730)

    • t = (-2.0565)*(5730 years)/-0.69314 = 17,002 years


K 40 is part of your body

K-40 is part of your body

  • K-40 is the largest radiation source in you

    • Human body has ≈160 grams of Potassium

    • 0.0117% K-40*160 grams  0.0187g K-40

    • This produces 4,400 disintegrations/sec

    • Emission mostly β (beta ray or electrons)

  • We will look at a potassium sample today


Nuclear chemistry

Radioisotopes used internally for medical applications will have short half-lives so that they decay rapidly and do not remain in the body for prolonged periods (Tc-99, ½=6hrs)


Ionizing radiation

Ionizing Radiation

  • A large dose of ionizing radiation can destroy living cells, causing death.

  • A small dose of ionizing radiation may not cause visible symptoms but might lead to a genetic mutation or cancer.


What s an mev

What’s an “MeV”?

  • Alternative energy unit used in physics

    • Equals 1 electron passing through 1 volt field

    • Same as 1.6*10-19Joule

    • Convenience is simple numbers, fewer zeros

    • Energy of visible light in eV in diagram below

    • Nuclear particles & rays >106 times light energy

      • 1 MeV = 10^6 eV


Light energy in electron volts

Light energy in electron volts


Radiation intensity

Health professionals who work with X rays or other kinds of ionizing radiation protect themselves by surrounding the source with a thick layer of lead or other dense material.

Protection is also afforded by controlling the distance between the worker and the radiation source because radiation intensity (I) decreases with the square of the distance from the source. We will demonstrate inverse square law this week in lab.

The intensities (I) of radiation at two different distances (d) are given by the equation:

I1d12 = I2d22

Radiation Intensity


Inverse square law

Inverse Square Law


Inverse square law1

Inverse square law

  • Intensity of radiation falls with distance

  • A non-linear relationship

    • Twice as far  ¼ the intensity

    • Works with all forms of point source radiation

    • Why planet Mercury is so hot, Venus so cold


Inverse square example

Inverse Square Example

  • Radiation intensity is 2250 at 2 meters, what is intensity at 3 meters?

  • I1 * d12 = I2 * d22

  • 2250 * 22 = I2 * 32

  • I2 = 2250*4/9 = 1000

  • Moving away by 1 meter cuts radiation by more than half


Mass into energy

Mass into Energy

Enormous ratio between mass & Energy

c = 3*10^8 meters/sec

c2 = 9*10^16 meters2/sec2

How much energy is that ?

1 gram U235 converts to 3.4*10^8 kcal

Hiroshima bomb converted only a few grams


Equivalence of mass energy albert einstein s famous equation e mc 2

Equivalence of Mass & EnergyAlbert Einstein’s famous equation E=mc2


Nuclear chemistry

E=mc2, so light has mass E=mc2, E= hc/λ, so m=h/(c*λ)= 3.4E-36 kg/photonThis is about 1 millionth the mass of an electron(Although very tiny, mass of light has important consequences


Nuclear chemistry

Space distortion due to massGeneral Relativity predicted light deflection by mass in 1916, proven by experiment in 1919


Nuclear chemistry

Gravity Well or “Black Hole”space is so distorted that light cannot pass nearby without falling in … a consequence of general relativity


Chain reaction

Chain Reaction

  • Postulated in 1930’s

    • Fission induces more fission, an avalanche

    • “critical mass” required to sustain reaction

    • Only certain isotopes sustain the reaction

      • Uranium 235 and Plutonium 239 most common

      • Show You-Tube simulation

  • First atomic reactor University of Chicago

    • Concentrated U235 required

    • The critical mass for lower-grade uranium depends strongly on the grade:

    • 20% U235 requires over 400 kg

    • 15% U235 requires over 600 kg.


Critical mass

A chain reaction requires a minimum amount of material for to be self sustaining

Plutonium-239 the size of a softball is enough to make a nuclear weapon.

Critical Mass


U 235

U235 %

  • Natural 0.711% U235 cannot sustain a chain reaction. Too much distance & shielding between fissionable atoms.

  • Minimal enrichment OK for reactors

  • High enrichment for weapons, reduces minimum mass and increases reaction rate.


First nuclear fission bomb

First Nuclear Fission Bomb


Nuclear fusion

Nuclear Fusion

  • Nuclear fusion: The joining together of light nuclei.

  • Light nuclei such as the isotopes of hydrogen release enormous amounts of energy when they undergo fusion. It is fusion reactions of hydrogen nuclei to produce helium that powers our sun and other stars.

  • The necessary conditions for nuclear fusion are not easily created on earth.

  • In stars the temperature is on the order of 2 x 107 K and pressures approach 1 x 105 atmospheres. At these extremes, nuclei are stripped of all their electrons and have enough kinetic energy that nuclear fusion readily occurs.


Fusion is primary energy source

Fusion is primary energy source

  • Universe is mostly Hydrogen

    • 75% by mass, 90% of all atoms

    • Hydrogen fuses at high temperature to Helium

      • Helium mass less that Hydrogen starting material

      • Balance of mass converted to energy

      • Fusion reaction powers the sun

      • Sun is a continuously operating Hydrogen bomb

    • Sun is also our primary light source

      • Fundamental basis for life on earth

      • Numerous energy conversion processes


Nuclear fusion in the sun

Nuclear Fusion in the Sun


Nuclear chemistry

Nuclear FusionPrinciple source of energy in stars from fusing hydrogenatom of helium weighs slightly less than 4 hydrogen, balance is energy


Heavier elements formed in stars formation due extreme temperatures pressures inside star

Heavier elements formed in starsformation due extreme temperatures & pressures inside star


Nuclear fusion hydrogen bomb

Nuclear Fusion (Hydrogen) Bomb


Medical issues

Medical Issues

  • Radiation poisoning

    • Bad if uncontrolled fallout (Chernobyl)

    • Good if controlled attack on tumors

    • Same idea in chemotherapy, selective poison

  • Radiation protection

    • Radioactive iodine from nuclear accidents

    • Thyroid collects & concentrates iodine

    • Use of potassium iodide to saturate thyroid prevents uptake of radioactive fallout iodine


Thyroid cancer

Thyroid Cancer


Nuclear chemistry

Polonium PoisoningsAlexander Litvenenko ex-KGB agent and critic of Russian politics. At lunch in London with ”friends” he ingested 10 micrograms Po-210, 200x a lethal dose of extremely radioactive alpha-emitter, and died 3 weeks later. There is some suspicion Yasser Arafat may have been similarly poisoned


Polonium 210 poisoning

Polonium-210 poisoning


Chernobyl reactor meltdown 2 3 radiation increase world wide

Chernobyl reactor meltdown2.3% radiation increase world-wide


Chernoble fallout victims

Chernoblefallout victims


Detecting radiation

Detecting Radiation

The simplest device for detecting exposure to radiation is the photographic film badge.

The film is protected from exposure to light, but any other radiation striking the badge causes the film to fog.

  • We cannot see, hear, smell, touch, or taste radiation, no matter how high the dose. We can, however, detect radiation by taking advantage of its ionizing properties.

70


Nuclear chemistry

The Geiger counter is an argon-filled tube. The inner walls are given a negative charge, and a wire in the center is given a positive charge.

Radiation ionizes the argon atoms, which briefly conduct a current between the walls and the center electrode.

The current is detected, amplified, and used to produce a clicking sound or to register on a meter.

71


Nuclear chemistry

When Ionizing radiation strikes certain crystals or plastics, a small flash of light results, which can be measured


Nuclear chemistry

Scintillation, emission of lightObserved by Crooks in 1895, using luminescence of ZnS, whichbecame basis of “picture tubes” in television. Radiation generating a single photon of light can be amplified108 by “photomultiplier” tube.


Large scale lab scintillator

Large Scale Lab Scintillator

The most versatile method for measuring radiation in the laboratory is the scintillation counter.

In this device, a substance called a phosphoremits a flash of light when struck by radiation.

The number of flashes are counted electronically and converted into an electrical signal.

74


Scintillator we will use in lab

Scintillator we will use in Lab


Sources of natural radiation

Sources of Natural Radiation

  • Radon

    • A natural decay product of Uranium

  • Cosmic radiation

    • From the sun and outside the solar system

    • Altitude increases exposure, less air protection

    • Similar to X-Rays

  • Food

    • Carbon-14, Potassium-40 are naturally radioactive

    • A few other elements in trace amounts (e.g. Polonium)

  • From Earth itself

    • Uranium, thorium, other natural radioactive elements


Radon

Radon

  • Alpha emitter, the most ionizing radiation

    • Short range but very dangerous internally

  • Radon decay products also radioactive

    • Solids, not gases …stay on lung tissues


Deaths per year including radon http elitehomeinspections net radon

Deaths per year, including Radonhttp://elitehomeinspections.net/radon


Http discoveringsomethingneweveryday blogspot com 2013 08 why is radon hazard html

http://discoveringsomethingneweveryday.blogspot.com/2013/08/why-is-radon-hazard.html


Nuclear chemistry

How Radon enters your homehttp://www6.montgomerycountymd.gov/dectmpl.asp?url=/content/dep/air/radon.asp


Radon exposure in usa http www tjernlund com radonvac htm

Radon exposure in USAhttp://www.tjernlund.com/radonvac.htm


Worldwide radon distribution http www fixradon com maps pages d 01 world radon by country htm

Worldwide Radon distributionhttp://www.fixradon.com/maps/pages/D_01_world_radon_by_country.htm


Http www omfi hu cejoem volume13 vol13no1 ce07 1 01 html

http://www.omfi.hu/cejoem/Volume13/Vol13No1/CE07_1-01.html


Source of radon danger http www grundyhealth org newsite radon shtml

Source of Radon Dangerhttp://www.grundyhealth.org/newsite/radon.shtml


Smoking is greatest cancer risk radon is 2

Smoking is greatest cancer risk, Radon is #2


Internal external radiation

Internal & External Radiation

  • Eating food involves internal exposure

    • C-14, K-40 in food, cannot be avoided

  • Cosmic rays from space hard to avoid

    • Greater risk at higher altitudes, aircraft rides

  • Ground radiation, radioactive elements

    • Uranium, Thorium, other natural materials

  • Radiation is everywhere!

    • From above, below, and in our food & water


X rays from below the earth

X-rays from below the Earth


Radiation units of measure

Radiation Units of Measure


Differences between radiation units

Differences between radiation units


Activity versus dosage not all radiation absorbed different units used

Activity versus dosagenot all radiation absorbed … different units used


Today s experiment

Today’s Experiment

  • We will have 3 stations for 3 tests

    • (1) Effect of shielding

    • (2) Isotope half-life

    • (3) Radiation from household objects

  • 3 or 4 groups of students circulate

    • Run each test, one after another (any order)

  • Allocate 20 minutes per test

    • Pre and post lab questions also included


Today s experiment part 1

Today’s Experiment, part 1

  • Effectiveness of Shields

    • Different radiation has differing penetration

      • Alpha is comparatively massive, low penetration

      • Beta is low mass, modest penetration

      • Gamma has zero mass, high penetration

    • Intensity reduced by mass of shield

      • We will use paper, plastic, aluminum, lead,etc.

      • Distinguish radiation by influence of shields


Today s experiment part 2

Today’s Experiment, part 2

  • Half life of an isotope

    • Intensity of radiation decreases with time

    • We prepare an isotope with ½ life of few min.

    • Measure radiation over period of 7 minutes

    • Plot radiation versus time

      • We will find half life experimentally


Today s experiment part 3

Today’s Experiment, part 3

  • Radiation from common objects

    • Natural and manufactured items

  • Radiation sources allaround us

    • Rocks, minerals, natural objects

    • Pottery, Smoke detectors

    • Power plant disasters (Russia, Japan, USA)

    • Nuclear testing fallout

  • We will measure several objects

    • Compare radiation types and amounts


Your personal exposure profile

Your personal exposure profile

  • Last part of experiment, done at home

  • Your assessment of radiation exposure

    • Medical x-rays (scans, dental, bone density)

    • Where you live influences exposure

      • California better than most other places

    • How often to you use airlines


To the benches

To the Benches!

  • Choose groups of 3-4

  • Run one station (any order)

  • Move to next station

  • Last station … and you’re done.


Los alamos national laboratory s periodic table

Los Alamos National Laboratory's Periodic Table


Nuclear chemistry

Marie & Pierre Curie, 1905Separated tons of mineral pitchblende to discover and isolate Radium, and polonium (named for Poland). The standard measure for radioactivity is the Curie = Ci


Nuclear chemistry

14C is continually produced in the atmosphere and incorporated into life cycles, so 14C amount in living things is constant. Upon death, no more 14C is absorbed, so concentration decreases. Measuring the remaining radioactivity provides an age estimate. The half life of 14C is 5730 years. The method is good for estimating age of objects 500 to 50,000 years old.


Nuclear chemistry

14C is continually produced in the atmosphere and incorporated into life cycles, so 14C amount in living things is constant. Upon death, no more 14C is absorbed, so concentration decreases. Measuring the remaining radioactivity provides an age estimate. The half life of 14C is 5730 years. The method is good for estimating age ofobjects 500 to 50,000 years old.


Radiation exposure http enhs umn edu hazards hazardssite radon radonintro html

Radiation exposurehttp://enhs.umn.edu/hazards/hazardssite/radon/radonintro.html


Radon radiation density in usa http en wikipedia org wiki health effects of radon

Radon radiation density in USAhttp://en.wikipedia.org/wiki/Health_effects_of_radon


Nuclear chemistry

Beta ParticleUnstable isotope emits electron having negative charge, nucleus of parent changes charge in the other direction, creating a new element. Example is Carbon-14 used for dating historical objects. Note another particle with zero mass and charge, the “Neutrino” … more about that later


Nuclear chemistry

Positron EmissionUnstable nuclei can also emit a positive electron, a form of “anti-matter” which turns into energy upon meeting it’s opposite. Mass and charge must balance


Today s experiment part 11

Today’s Experiment, part 1

  • Radiation versus Distance

    • Intensity falls off as square of distance

    • Assumes a “point source” (e.g. sun in sky)

    • Our source is not exactly a point

    • Falloff will be approximately linear

    • You will plot radiation versus distance

      • A non-linear relationship

    • Replot with inverse distance

      • Approximately linear relationship


Radiation units of measure original definition of curie was radiation from one gram of radium

Radiation units of measureOriginal definition of “curie” was radiation from one gram of radium


Nuclear chemistry

Emission of g rays causes no change in mass or atomic number.

g emission usually accompanies emission of other rays but it is often omitted from nuclear equations.

Their penetrating power makes them both dangerous to humans and useful in medical applications.

114


Proton emission loss of positive charge reduces atomic number by 1

Proton Emissionloss of positive charge reduces atomic number by 1


Neutron emission element stays the same but new isotope weighs less

Neutron EmissionElement stays the same, but new isotope weighs less


Nuclear chemistry

Atomic Bomb ExplosionAutomatic Camera situated 7 miles from blast with 10 foot lens. Shutter speed 1/100,000,000 second. Joshua tree’s near base vaporized in microseconds.


  • Login