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Transcript of Nuclear Stability & Radioactive Decay. Notation for a nuclide (specific atom) 12 C 6 The left...
![Page 1: Nuclear Stability & Radioactive Decay. Notation for a nuclide (specific atom) 12 C 6 The left superscript is the mass number = number of protons + neutrons.The.](https://reader035.fdocuments.net/reader035/viewer/2022062404/551c5693550346a5458b4fcf/html5/thumbnails/1.jpg)
Nuclear Stability & Radioactive Decay
![Page 2: Nuclear Stability & Radioactive Decay. Notation for a nuclide (specific atom) 12 C 6 The left superscript is the mass number = number of protons + neutrons.The.](https://reader035.fdocuments.net/reader035/viewer/2022062404/551c5693550346a5458b4fcf/html5/thumbnails/2.jpg)
Notation for a nuclide (specific atom)
12C
6
•The left superscript is the mass number = number of protons + neutrons.
•The left subscript is the atomic number = number of protons.
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Isotopes
• Atoms with identical atomic numbers but different mass numbers.
• (Two nuclides can have different atomic numbers and different mass numbers.)
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Nuclear Stability
• Determined by neutron/proton ratio.– All nuclides with 84 or more protons are
unstable.– Light elements (up to atomic number 20): like
a neutron/proton ratio of 1.– For heavier elements, the neutron/proton ratio
required for stability > 1, and increases as atomic number increases.
– Of 2000 known nuclides, only 279 are stable with respect to radioactive decay.
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Zone of Stability
Beta
decay
Positron emission or
electron capture
Alpha decay: heavy elements.
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Radioactive Decay
• Represented by equations
• 14C 14N + 0e6 7 -1
Original nuclide Decay Mode
Decay Product
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Decay Modes
• Alpha – common decay mode for heavy nuclides. Mass # by 4, atomic # by 2. Tends to slightly increase n/p ratio.
• Beta – mass # remains constant.– Net effect: neutron changed to proton. So this
is a likely decay mode for nuclides whose n/p ratio is too high – decreases n/p ratio.
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Decay Modes
• Positron production: net effect: change a proton to a neutron.– Important decay mode for nuclides whose n/p
ratio is low – it increases the n/p ratio!
• Electron capture: inner-orbital electron is captured by the nucleus– Increases neutron-proton ratio
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Decay series
• Some radioactive nuclides must go through several decay events to reach a stable (nonradioactive) state.
• 235U 207Pb
• 238U 206Pb
92 82
92 82
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Kinetics of Radioactive Decay
• Can never predict exactly when a specific nuclide will decay.
• N = # of nuclides
• Rate = - (N/t) = kN
• i.e., the rate is directly proportional to the # of nuclides in the sample.
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Rate = - (N/t) = kN
• ln(N/N0) = -kt
• N = # of nuclides remaining at time t• N0 = # of nuclides at t = 0.
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Half-Life, t½
• Half-life of a sample = time required for the number of nuclides to reach half the original value, N0/2.
• t½ = 0.693/k
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Nuclear Transformations
• Change of one nuclide into another• Target nucleus is bombarded by a “bullet”• “Bullet” may be a positive ion or a neutron
– Particle accelerators used for + ions– Positive ions must be accelerated to high KE
to overcome electrostatic repulsions• Cyclotron
– Neutrons quite different experimentally. Not repelled by target nuclei.
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Transuranium Elements
• Elements 93 – 1** have been synthesized.
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Uses of Radioisotopes
• Ratioactive Dating
• 14C 0e + 14N6 -1 7
Continuously produced
in atm by:
14N +
1n
14C +
1H
7 0 6 1
So, C-14 is incorporated into living plants.
As long as it is alive,
C-14 to C-12 ratio is constant.
When plant dies, 14
C/12
C ratio starts to
decrease.
t½ = 5730 yrs
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Geologic History
• 238U 206Pb92 82
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Medical Applications
• Radiotracers/Diagnosis– Radioactive nuclide whose pathway in an
organism can be traced by monitoring its radioactivity.
– I-131 thyroid– Th-201 heart
• Treatment
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Thermodynamic Stability of Nucleus
• Mass of a nucleus is always less than the sum of the masses of the protons and neutrons that make up the nucleus.
• This difference is a measure of the binding energy
• Binding energy = energy released when nucleus is formed.
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Chemical Potential Well
Pot
entia
l Ene
rgy
Separate Nucleons
Stable Nucleus
Green Arrow represents binding energy:
Energy RELEASED when nucleus is
formed.
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Mass Defect for O-16
• 8p: (8 X 1.007276 amu) = 8.058208 amu• 8n: (8 X 1.008665 amu) = 8.06932 amu• 8e: (8 X 0.0005486 amu) = 0.004389 amu
• Total combined mass = 16.125789• Atomic mass of 0-16 = 15.994915 amu• m = 0.130874 amu• Use 1 amu = 1.66054 X 10-27 kg
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Mass Defect for O-16
• m = 0.130874 amu• Use 1 amu = 1.66054 X 10-27 kg• m = 2.1732 X 10-28 kg• mc2 = E = 1.9559 X 10-11 kgm2s-2
• E = 1.9559 X 10-11 J per O-16 atom & 1.22 X 10-12 J per nucleon
• In kJ/mol: 7.4 X 108 kJ per nucleon per mol
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Binding Energy/Nucleon vs. Mass #
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Units of binding energy
• Chemists use kJ/(molnucleon)• Physics uses a different unit: Mev
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Nuclear Fission
• Splitting a heavy nucleus into two smaller nuclei.
• U-235 and Pu-239 are fissionable fuels• Reaction initiated by a neutron
• Many, many possible products
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Nuclear Fusion
• Two light nuclei combine to form a heavier, more stable nucleus.
• Occurs in the stars.• Sun: 73% H, 26% He, and 1% other• Protons fuse to form He
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Sun
• 1H + 1H 2H + 0e + energy
• 1H + 2H 3He + energy
• Then • 3He + 3He 4He + 2 1H + energy
• 3He + 1H 4He + 0e + energy
1 1 1 1
1 1 2
2 2 2 1
2 1 2 1
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Fusion vs. Fission as Energy Source
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Nuclear vs. Ordinary Chemical & Physical Change
• Nuclear transformations involve much larger energy changes than ordinary chemical & physical changes– Orders of magnitude larger
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Risks of radionuclides
• Somatic damage = damage to the organism itself, resulting in sickness or death
• Genetic damage = damage to genes